Code
from elements import fGT, Elements, DensityEstimator, Plotter
# quality graphics
%config InlineBackend.figure_formats = ['svg']
= Elements.df() df
Stephen J. Mildenhall
2025-08-10
2025-08-18
The periodic table is more than a static grid of symbols and numbers. It is a compact map of how the elements behave, interact, and differ. In this post I have assembled charts and tables that bring those patterns into view: crystal structures, densities, melting and boiling points, ionization energies, and more. The aim is to let familiar trends sharpen into focus, highlight anomalies that challenge expectations, and uncover relationships that become clear only when the whole landscape is seen at once.
Some of these features are striking. The rise and fall of ionization energy across each period is sharply defined, with the noble gases forming regular peaks and the alkali metals deep troughs. Mercury stands apart from its neighbors, a liquid metal at room temperature with melting and boiling points far lower than the metals around it. Silver, copper, and gold combine high electrical and thermal conductivities in a way that reflects the Wiedemann-Franz law, showing a clear link between the movement of electrons and the transfer of heat. These examples are not isolated curiosities but part of a connected picture that emerges from the data as a whole.
The charts and tables use data from the Mendeleev
Python package, see Section 15. All the data used is shown in Section 16
There is also an old version using the Vertex spreadsheet template data.
Atomic weight (more precisely, relative atomic mass) is the weighted average mass of an element’s naturally occurring isotopes, measured relative to one-twelfth of the mass of a carbon-12 atom. It is dimensionless (a ratio), but in practice often written in unified atomic mass units (u), where 1 u ≈ 1.660 539 × 10⁻²⁷ kg. The value reflects both the number of protons and neutrons in the nucleus and the proportions of each isotope found in nature, which means it can vary slightly depending on the source of the element—chlorine, for example, has an atomic weight of about 35.45 because it is roughly 75 % chlorine-35 and 25 % chlorine-37. Some elements, especially those with only one stable isotope (e.g., fluorine-19, beryllium-9), have atomic weights that are essentially fixed, while others with large isotope variations (e.g., lithium, boron) may be given as ranges by the International Union of Pure and Applied Chemistry (IUPAC). For radioactive elements with no stable isotopes, an atomic weight is not fixed and is often based on the most stable isotope or the isotope most commonly used in research.
In all bar charts color each element by its block (s, p, d, f). Paler colors are used for higher periods. Vertical lines separate the blocks.
Density is the mass per unit volume of a substance, typically expressed for elements in kilograms per cubic metre (kg·m⁻³) or grams per cubic centimetre (g·cm⁻³) which are used here. For solids and liquids, density depends on both the mass of individual atoms and how closely they are packed in the crystal or molecular structure. In the periodic table, metals tend to have higher densities than nonmetals because their atoms are both heavier and packed tightly in metallic lattices. Osmium and iridium are the densest known elements under standard conditions (both around 22.6 g·cm⁻³), while lithium, the least dense metal, has a density of just 0.534 g·cm⁻³, making it light enough to float on water. Nonmetals vary widely: solid carbon (graphite) is about 2.27 g·cm⁻³, while gaseous elements like helium have densities in the thousandths of a g·cm⁻³ at room temperature. Density can also change significantly with temperature and pressure; for example, metals expand slightly when heated, lowering their density, while gases follow the ideal gas law and decrease in density more sharply with rising temperature at constant pressure.
See Section 13 for estimates of density based on atomic weight, crystal structure and atomic radius.
When plotted across the periodic table, melting and boiling points reveal distinct trends and striking anomalies. Metals in the middle of the transition series, such as tungsten, have exceptionally high melting points (tungsten’s is the highest of all, 3422 °C), while noble gases like helium remain liquefied only near absolute zero (helium’s boiling point is the lowest known, −268.93 °C). Carbon is unusual in that at atmospheric pressure it does not melt but sublimates directly to gas at about 3900 K, giving it one of the highest sublimation points of any element. Gallium is another oddity—its melting point is just 29.76 °C, meaning it can melt in the palm of your hand, yet its boiling point is a much higher 2400 °C, an unusually wide liquid range for a metal. The alkali metals show a steady increase in both melting and boiling points up a group, while the halogens progress from gases to solids with rising boiling points as atomic mass increases. Mercury is a notable liquid metal at room temperature, with a melting point of −38.83 °C and a relatively low boiling point of 356.73 °C. These extremes—whether in refractory metals, cryogenic gases, or unusual phase behavior—mark the boundaries of elemental physical properties.
These are complementary measures, but not strict opposites.
High ionization energy usually goes with a strongly negative electron affinity (atoms both hold on to electrons tightly and want more—e.g., fluorine, chlorine). Low ionization energy often accompanies small or even positive electron affinity (atoms lose electrons easily and don’t strongly attract extras—e.g., alkali metals, noble gases). The relationship isn’t perfectly mirrored because the processes involve different initial and final states, and subshell structure can skew the trends.
Ionization energy is the amount of energy required to remove the most loosely bound electron from a neutral atom in its gaseous state, producing a singly charged positive ion. It is usually expressed in electronvolts (eV, shown here) or kilojoules per mole (kJ·mol⁻¹). When plotted by element, first ionization energy shows a strong periodic trend: it generally increases across a period from left to right, reflecting the growing nuclear charge that holds electrons more tightly, and decreases down a group as outer electrons are farther from the nucleus and more shielded by inner shells. The noble gases sit at the top of each period, with helium having the highest value of all (24.59 eV, 2372 kJ·mol⁻¹), while alkali metals like cesium and francium have the lowest, reflecting how easily they lose their single valence electron. Notable irregularities occur in elements like boron and oxygen, where subshell structure slightly lowers the expected value. These variations reflect the interplay of nuclear charge, electron shielding, and subshell stability.
Electron affinity is the change in energy when a neutral atom in the gaseous state gains an electron to form a negative ion. It is usually expressed in electronvolts (eV, shown here) or kilojoules per mole (kJ·mol⁻¹); by convention, a negative value means energy is released (exothermic), while a positive value means energy is required (endothermic). Across a period from left to right, electron affinity generally becomes more negative as atoms have a stronger tendency to complete their valence shell—halogens are the most extreme, with chlorine releasing about −3.6 eV (−349 kJ·mol⁻¹) when gaining an electron. Noble gases have positive electron affinities because adding an electron would start a new shell, which is energetically unfavorable. Down a group, the trend is less regular than for ionization energy: while increasing atomic size generally makes electron gain less favorable, subshell configurations cause exceptions, such as oxygen’s slightly less negative value than sulfur’s, due to electron–electron repulsion in its compact 2p shell. These variations highlight the balance between nuclear attraction, electron shielding, and subshell stability in determining how readily an atom will accept an extra electron.
Radius is measured in pm, picometers or \(10^{-12}\)m. An element’s radius can be defined in several different ways, depending on how the atom is bonded or measured, and each definition captures a different aspect of its size.
When plotted across the periodic table, all radii decrease from left to right within a period due to increasing nuclear charge, and increase down a group as additional electron shells are added. Differences between these four radii reflect the type of interaction being measured—tightly bound in covalent bonds, more spread out in metallic lattices, and most expansive when only weak van der Waals forces act.
Electronegativity is a dimensionless measure of how strongly an atom attracts shared electrons in a chemical bond. It is not a directly measurable physical quantity but is derived from other data, most famously by Linus Pauling, whose Pauling scale remains the most widely used. Other scales, like Mulliken or Allred–Rochow, use ionization energy and electron affinity or electrostatic arguments to produce similar trends. On the Pauling scale, values range from about 0.7 (cesium and francium, very weak attraction) to 4.0 (fluorine, the strongest). Across a period from left to right, electronegativity increases due to rising nuclear charge and smaller atomic radii, making the nucleus’s pull on bonding electrons stronger. Down a group, it decreases as added electron shells increase shielding and distance from the nucleus. Noble gases are usually omitted because they rarely form covalent bonds, though some heavier ones can. Extremes include fluorine (highest), oxygen (second highest), and cesium/francium (lowest). Electronegativity is related to both ionization energy and electron affinity—atoms with high values for both tend to have high electronegativity—but because it deals with shared electrons in bonds rather than isolated atoms, the correlation is not exact.
Thermal conductivity is a measure of how efficiently a material transfers heat, usually expressed in watts per meter per kelvin (W·m⁻¹·K⁻¹). For elements, it largely depends on how mobile the electrons or lattice vibrations (phonons) are in carrying thermal energy. Metals, with their “sea” of delocalized electrons, generally have the highest thermal conductivities—silver holds the record at about 429 W·m⁻¹·K⁻¹, closely followed by copper and gold—while nonmetals vary widely depending on structure. Diamond (a form of carbon) is exceptional, with the highest known thermal conductivity of any bulk material (~2200 W·m⁻¹·K⁻¹) due to its rigid, perfectly ordered covalent lattice and strong covalent bonds. At the other extreme, elements like sulfur, phosphorus, and the noble gases have extremely low conductivities, as they rely solely on phonon transport through relatively weakly bound structures. Trends in the periodic table are less regular than for properties like ionization energy, since conductivity depends not only on bonding type but also on crystal structure, defects, and isotopic composition.
Electrical resistivity measures how strongly a material opposes the flow of electric current, with units of ohm-meters (Ω·m). It is the inverse of electrical conductivity, so low resistivity means high conductivity. Among the elements, silver has the lowest resistivity (~1.59 × 10⁻⁸ Ω·m), followed closely by copper and gold, which is why these metals dominate in electrical wiring and contacts. Most metals have low resistivities because their delocalized conduction electrons can move freely through the metallic lattice. In contrast, nonmetals and metalloids such as sulfur, phosphorus, and silicon have much higher resistivities—ranging from semiconducting values in silicon (~10⁻³ to 10³ Ω·m, depending on doping) to extremely high, effectively insulating values in materials like sulfur or diamond (>10¹² Ω·m). Temperature strongly affects resistivity: in pure metals it increases with temperature due to greater scattering of electrons by lattice vibrations, while in semiconductors it decreases as more charge carriers become available. Extreme cases include superconductors, which have effectively zero resistivity below their critical temperature. The mendeleev
package does not include electrical resistivity. Table 1 includes some values.
Element and form | Resistivity \(\rho\) (\(\Omega\cdot\text{m}\)) |
---|---|
Ag | \(1.59\times 10^{-8}\) |
Cu | \(1.68\times 10^{-8}\) |
Au | \(2.44\times 10^{-8}\) |
Al | \(2.65\text{–}2.82\times 10^{-8}\) |
W | \(5.6\times 10^{-8}\) |
Fe | \(\sim 1.0\times 10^{-7}\) |
Pb | \(\sim 2.2\times 10^{-7}\) |
Graphite (basal plane) | \(\sim 10^{-5}\) (anisotropic) |
Si (intrinsic, 300 K) | \(\sim 10^{3}\) (order of \(10^{2}\text{–}10^{3}\)) |
Ge (intrinsic, 300 K) | \(\sim 0.4\text{–}0.5\) |
Diamond | \(10^{11} ext{–}10^{18}\) (insulator) |
Name | Symbol | Atomic Number | Phase | Type | Group | Group Symbol | Block | Electron Configuration | Crystal Structure |
---|---|---|---|---|---|---|---|---|---|
Hydrogen | H | 1 | Gas | Nonmetals | 1 | IA | s | 1s | HEX |
Helium | He | 2 | Gas | Noble gases | 18 | VIIIA | s | 1s2 | HEX |
Lithium | Li | 3 | Solid | Alkali metals | 1 | IA | s | [He] 2s | BCC |
Beryllium | Be | 4 | Solid | Alkaline earth metals | 2 | IIA | s | [He] 2s2 | HEX |
Boron | B | 5 | Solid | Metalloids | 13 | IIIA | p | [He] 2s2 2p | TET |
Carbon | C | 6 | Gas | Nonmetals | 14 | IVA | p | [He] 2s2 2p2 | DIA |
Nitrogen | N | 7 | Gas | Nonmetals | 15 | VA | p | [He] 2s2 2p3 | HEX |
Oxygen | O | 8 | Gas | Nonmetals | 16 | VIA | p | [He] 2s2 2p4 | CUB |
Fluorine | F | 9 | Gas | Halogens | 17 | VIIA | p | [He] 2s2 2p5 | MCL |
Neon | Ne | 10 | Gas | Noble gases | 18 | VIIIA | p | [He] 2s2 2p6 | FCC |
Sodium | Na | 11 | Solid | Alkali metals | 1 | IA | s | [Ne] 3s | BCC |
Magnesium | Mg | 12 | Solid | Alkaline earth metals | 2 | IIA | s | [Ne] 3s2 | HEX |
Aluminum | Al | 13 | Solid | Poor metals | 13 | IIIA | p | [Ne] 3s2 3p | FCC |
Silicon | Si | 14 | Solid | Metalloids | 14 | IVA | p | [Ne] 3s2 3p2 | DIA |
Phosphorus | P | 15 | Solid | Nonmetals | 15 | VA | p | [Ne] 3s2 3p3 | CUB |
Sulfur | S | 16 | Solid | Nonmetals | 16 | VIA | p | [Ne] 3s2 3p4 | ORC |
Chlorine | Cl | 17 | Gas | Halogens | 17 | VIIA | p | [Ne] 3s2 3p5 | ORC |
Argon | Ar | 18 | Gas | Noble gases | 18 | VIIIA | p | [Ne] 3s2 3p6 | FCC |
Potassium | K | 19 | Solid | Alkali metals | 1 | IA | s | [Ar] 4s | BCC |
Calcium | Ca | 20 | Solid | Alkaline earth metals | 2 | IIA | s | [Ar] 4s2 | FCC |
Scandium | Sc | 21 | Solid | Transition metals | 3 | IIIB | d | [Ar] 3d 4s2 | HEX |
Titanium | Ti | 22 | Solid | Transition metals | 4 | IVB | d | [Ar] 3d2 4s2 | HEX |
Vanadium | V | 23 | Solid | Transition metals | 5 | VB | d | [Ar] 3d3 4s2 | BCC |
Chromium | Cr | 24 | Solid | Transition metals | 6 | VIB | d | [Ar] 3d5 4s | BCC |
Manganese | Mn | 25 | Solid | Transition metals | 7 | VIIB | d | [Ar] 3d5 4s2 | CUB |
Iron | Fe | 26 | Solid | Transition metals | 8 | VIIIB | d | [Ar] 3d6 4s2 | BCC |
Cobalt | Co | 27 | Solid | Transition metals | 9 | VIIIB | d | [Ar] 3d7 4s2 | HEX |
Nickel | Ni | 28 | Solid | Transition metals | 10 | VIIIB | d | [Ar] 3d8 4s2 | FCC |
Copper | Cu | 29 | Solid | Transition metals | 11 | IB | d | [Ar] 3d10 4s | FCC |
Zinc | Zn | 30 | Solid | Transition metals | 12 | IIB | d | [Ar] 3d10 4s2 | HEX |
Gallium | Ga | 31 | Solid | Poor metals | 13 | IIIA | p | [Ar] 3d10 4s2 4p | ORC |
Germanium | Ge | 32 | Solid | Metalloids | 14 | IVA | p | [Ar] 3d10 4s2 4p2 | DIA |
Arsenic | As | 33 | Solid | Metalloids | 15 | VA | p | [Ar] 3d10 4s2 4p3 | RHL |
Selenium | Se | 34 | Solid | Nonmetals | 16 | VIA | p | [Ar] 3d10 4s2 4p4 | HEX |
Bromine | Br | 35 | Liquid | Halogens | 17 | VIIA | p | [Ar] 3d10 4s2 4p5 | ORC |
Krypton | Kr | 36 | Gas | Noble gases | 18 | VIIIA | p | [Ar] 3d10 4s2 4p6 | FCC |
Rubidium | Rb | 37 | Solid | Alkali metals | 1 | IA | s | [Kr] 5s | BCC |
Strontium | Sr | 38 | Solid | Alkaline earth metals | 2 | IIA | s | [Kr] 5s2 | FCC |
Yttrium | Y | 39 | Solid | Transition metals | 3 | IIIB | d | [Kr] 4d 5s2 | HEX |
Zirconium | Zr | 40 | Solid | Transition metals | 4 | IVB | d | [Kr] 4d2 5s2 | HEX |
Niobium | Nb | 41 | Solid | Transition metals | 5 | VB | d | [Kr] 4d4 5s | BCC |
Molybdenum | Mo | 42 | Solid | Transition metals | 6 | VIB | d | [Kr] 4d5 5s | BCC |
Technetium | Tc | 43 | Solid | Transition metals | 7 | VIIB | d | [Kr] 4d5 5s2 | HEX |
Ruthenium | Ru | 44 | Solid | Transition metals | 8 | VIIIB | d | [Kr] 4d7 5s | HEX |
Rhodium | Rh | 45 | Solid | Transition metals | 9 | VIIIB | d | [Kr] 4d8 5s | FCC |
Palladium | Pd | 46 | Solid | Transition metals | 10 | VIIIB | d | [Kr] 4d10 | FCC |
Silver | Ag | 47 | Solid | Transition metals | 11 | IB | d | [Kr] 4d10 5s | FCC |
Cadmium | Cd | 48 | Solid | Transition metals | 12 | IIB | d | [Kr] 4d10 5s2 | HEX |
Indium | In | 49 | Solid | Poor metals | 13 | IIIA | p | [Kr] 4d10 5s2 5p | TET |
Tin | Sn | 50 | Solid | Poor metals | 14 | IVA | p | [Kr] 4d10 5s2 5p2 | TET |
Antimony | Sb | 51 | Solid | Metalloids | 15 | VA | p | [Kr] 4d10 5s2 5p3 | RHL |
Tellurium | Te | 52 | Solid | Metalloids | 16 | VIA | p | [Kr] 4d10 5s2 5p4 | HEX |
Iodine | I | 53 | Solid | Halogens | 17 | VIIA | p | [Kr] 4d10 5s2 5p5 | ORC |
Xenon | Xe | 54 | Gas | Noble gases | 18 | VIIIA | p | [Kr] 4d10 5s2 5p6 | FCC |
Cesium | Cs | 55 | Solid | Alkali metals | 1 | IA | s | [Xe] 6s | BCC |
Barium | Ba | 56 | Solid | Alkaline earth metals | 2 | IIA | s | [Xe] 6s2 | BCC |
Lanthanum | La | 57 | Solid | Lanthanides | 3 | IIIB | d | [Xe] 5d 6s2 | HEX |
Cerium | Ce | 58 | Solid | Lanthanides | nan | None | f | [Xe] 4f 5d 6s2 | FCC |
Praseodymium | Pr | 59 | Solid | Lanthanides | nan | None | f | [Xe] 4f3 6s2 | HEX |
Neodymium | Nd | 60 | Solid | Lanthanides | nan | None | f | [Xe] 4f4 6s2 | HEX |
Promethium | Pm | 61 | Solid | Lanthanides | nan | None | f | [Xe] 4f5 6s2 | None |
Samarium | Sm | 62 | Solid | Lanthanides | nan | None | f | [Xe] 4f6 6s2 | RHL |
Europium | Eu | 63 | Solid | Lanthanides | nan | None | f | [Xe] 4f7 6s2 | BCC |
Gadolinium | Gd | 64 | Solid | Lanthanides | nan | None | f | [Xe] 4f7 5d 6s2 | HEX |
Terbium | Tb | 65 | Solid | Lanthanides | nan | None | f | [Xe] 4f9 6s2 | HEX |
Dysprosium | Dy | 66 | Solid | Lanthanides | nan | None | f | [Xe] 4f10 6s2 | HEX |
Holmium | Ho | 67 | Solid | Lanthanides | nan | None | f | [Xe] 4f11 6s2 | HEX |
Erbium | Er | 68 | Solid | Lanthanides | nan | None | f | [Xe] 4f12 6s2 | HEX |
Thulium | Tm | 69 | Solid | Lanthanides | nan | None | f | [Xe] 4f13 6s2 | HEX |
Ytterbium | Yb | 70 | Solid | Lanthanides | nan | None | f | [Xe] 4f14 6s2 | FCC |
Lutetium | Lu | 71 | Solid | Transition metals | nan | None | f | [Xe] 4f14 5d 6s2 | HEX |
Hafnium | Hf | 72 | Solid | Transition metals | 4 | IVB | d | [Xe] 4f14 5d2 6s2 | HEX |
Tantalum | Ta | 73 | Solid | Transition metals | 5 | VB | d | [Xe] 4f14 5d3 6s2 | BCC |
Tungsten | W | 74 | Solid | Transition metals | 6 | VIB | d | [Xe] 4f14 5d4 6s2 | BCC |
Rhenium | Re | 75 | Solid | Transition metals | 7 | VIIB | d | [Xe] 4f14 5d5 6s2 | HEX |
Osmium | Os | 76 | Solid | Transition metals | 8 | VIIIB | d | [Xe] 4f14 5d6 6s2 | HEX |
Iridium | Ir | 77 | Solid | Transition metals | 9 | VIIIB | d | [Xe] 4f14 5d7 6s2 | FCC |
Platinum | Pt | 78 | Solid | Transition metals | 10 | VIIIB | d | [Xe] 4f14 5d9 6s | FCC |
Gold | Au | 79 | Solid | Transition metals | 11 | IB | d | [Xe] 4f14 5d10 6s | FCC |
Mercury | Hg | 80 | Liquid | Transition metals | 12 | IIB | d | [Xe] 4f14 5d10 6s2 | RHL |
Thallium | Tl | 81 | Solid | Poor metals | 13 | IIIA | p | [Xe] 4f14 5d10 6s2 6p | HEX |
Lead | Pb | 82 | Solid | Poor metals | 14 | IVA | p | [Xe] 4f14 5d10 6s2 6p2 | FCC |
Bismuth | Bi | 83 | Solid | Poor metals | 15 | VA | p | [Xe] 4f14 5d10 6s2 6p3 | RHL |
Polonium | Po | 84 | Solid | Metalloids | 16 | VIA | p | [Xe] 4f14 5d10 6s2 6p4 | SC |
Astatine | At | 85 | Solid | Halogens | 17 | VIIA | p | [Xe] 4f14 5d10 6s2 6p5 | None |
Radon | Rn | 86 | Gas | Noble gases | 18 | VIIIA | p | [Xe] 4f14 5d10 6s2 6p6 | FCC |
Francium | Fr | 87 | Gas | Alkali metals | 1 | IA | s | [Rn] 7s | BCC |
Radium | Ra | 88 | Solid | Alkaline earth metals | 2 | IIA | s | [Rn] 7s2 | None |
Actinium | Ac | 89 | Solid | Actinides | 3 | IIIB | d | [Rn] 6d 7s2 | FCC |
Thorium | Th | 90 | Solid | Actinides | nan | None | f | [Rn] 6d2 7s2 | FCC |
Protactinium | Pa | 91 | Solid | Actinides | nan | None | f | [Rn] 5f2 6d 7s2 | TET |
Uranium | U | 92 | Solid | Actinides | nan | None | f | [Rn] 5f3 6d 7s2 | ORC |
Neptunium | Np | 93 | Solid | Actinides | nan | None | f | [Rn] 5f4 6d 7s2 | ORC |
Plutonium | Pu | 94 | Solid | Actinides | nan | None | f | [Rn] 5f6 7s2 | MCL |
Americium | Am | 95 | Solid | Actinides | nan | None | f | [Rn] 5f7 7s2 | None |
Curium | Cm | 96 | Solid | Actinides | nan | None | f | [Rn] 5f7 6d 7s2 | None |
Berkelium | Bk | 97 | Solid | Actinides | nan | None | f | [Rn] 5f9 7s2 | None |
Californium | Cf | 98 | Solid | Actinides | nan | None | f | [Rn] 5f10 7s2 | None |
Einsteinium | Es | 99 | Solid | Actinides | nan | None | f | [Rn] 5f11 7s2 | None |
Fermium | Fm | 100 | Solid | Actinides | nan | None | f | [Rn] 5f12 7s2 | None |
Mendelevium | Md | 101 | Solid | Actinides | nan | None | f | [Rn] 5f13 7s2 | None |
Nobelium | No | 102 | Solid | Actinides | nan | None | f | [Rn] 5f14 7s2 | None |
Lawrencium | Lr | 103 | Solid | Transition metals | nan | None | f | [Rn] 5f14 7s2 7p1 | None |
Rutherfordium | Rf | 104 | Gas | Transition metals | 4 | IVB | d | [Rn] 5f14 6d2 7s2 | None |
Dubnium | Db | 105 | Gas | Transition metals | 5 | VB | d | [Rn] 5f14 6d3 7s2 | None |
Seaborgium | Sg | 106 | Gas | Transition metals | 6 | VIB | d | [Rn] 5f14 6d4 7s2 | None |
Bohrium | Bh | 107 | Gas | Transition metals | 7 | VIIB | d | [Rn] 5f14 6d5 7s2 | None |
Hassium | Hs | 108 | Gas | Transition metals | 8 | VIIIB | d | [Rn] 5f14 6d6 7s2 | None |
Meitnerium | Mt | 109 | Gas | Transition metals | 9 | VIIIB | d | [Rn] 5f14 6d7 7s2 | None |
Darmstadtium | Ds | 110 | Gas | Transition metals | 10 | VIIIB | d | [Rn] 5f14 6d9 7s1 | None |
Roentgenium | Rg | 111 | Gas | Transition metals | 11 | IB | d | [Rn] 5f14 6d10 7s1 | None |
Copernicium | Cn | 112 | Gas | Transition metals | 12 | IIB | d | [Rn] 5f14 6d10 7s2 | None |
Nihonium | Nh | 113 | Gas | Poor metals | 13 | IIIA | p | [Rn] 5f14 6d10 7s2 7p1 | None |
Flerovium | Fl | 114 | Gas | Poor metals | 14 | IVA | p | [Rn] 5f14 6d10 7s2 7p2 | None |
Moscovium | Mc | 115 | Gas | Poor metals | 15 | VA | p | [Rn] 5f14 6d10 7s2 7p3 | None |
Livermorium | Lv | 116 | Gas | Poor metals | 16 | VIA | p | [Rn] 5f14 6d10 7s2 7p4 | None |
Tennessine | Ts | 117 | Gas | Halogens | 17 | VIIA | p | [Rn] 5f14 6d10 7s2 7p5 | None |
Oganesson | Og | 118 | Gas | Noble gases | 18 | VIIIA | p | [Rn] 5f14 6d10 7s2 7p6 | None |
Type is a broad chemical classification of elements, grouping them by their general physical and chemical properties. It is a way of labeling an element according to where it sits in the periodic table and the kind of bonding and reactivity it usually shows.
A metal is an element that tends to lose electrons to form positive ions and whose atoms in the solid state are bound by metallic bonding—a lattice of positive atomic cores surrounded by a “sea” of delocalised electrons. This electron cloud gives metals their characteristic properties: high electrical and thermal conductivity, malleability, ductility, and metallic lustre. Most metals have only one to three electrons in their outermost shell, which are relatively weakly bound and easily delocalised; these configurations are common in the s-block (alkali and alkaline earth metals), d-block (transition metals), and lower p-block (post-transition metals). The periodic table position is a strong guide, with metals dominating the left and centre, nonmetals at the upper right, and metalloids along the boundary between them. While outer-shell electron count is a good predictor of metallic behaviour, the decisive factor is the electronic band structure—specifically, whether the valence and conduction bands overlap to allow electrons to move freely. Edge cases exist, such as metalloids that can act metallic under some conditions, or nonmetals like hydrogen that become metallic only at high pressures.
Metals (e.g., iron, copper, aluminum) are generally good conductors of heat and electricity, malleable, and form positive ions (cations) in compounds.
Nonmetals (e.g., oxygen, sulfur, chlorine) are poor conductors, often brittle in solid form, and tend to form negative ions (anions) or covalent bonds.
Metalloids (e.g., boron, silicon, arsenic) have properties intermediate between metals and nonmetals, often depending on the chemical environment.
These are based mostly on position in the periodic table.
Alkali metals — Group 1 (except hydrogen): Li, Na, K, Rb, Cs, Fr. Very reactive metals with one valence electron, low melting points, form strong bases with water.
Alkaline earth metals — Group 2: Be, Mg, Ca, Sr, Ba, Ra. Reactive metals with two valence electrons, form basic oxides.
Transition metals — Groups 3–12 in the “d-block” of the periodic table. Variable oxidation states, form coloured compounds, often good catalysts. The “Transition Metal ?” label in your list likely means uncertain classification, perhaps due to inconsistent data source mapping.
Rare earth metals — The lanthanides (La to Lu) and sometimes Sc and Y. Similar reactivity and electron configurations (4f-block), often used in magnets, alloys, and phosphors.
Poor metals / Post-transition metals — Metals in the p-block that are softer, lower melting, and poorer conductors than transition metals (e.g., Al, Ga, In, Sn, Tl, Pb, Bi). “Post-transition” is essentially the same concept; the difference in your list may come from merging multiple data sources.
Noble gases — Group 18: He, Ne, Ar, Kr, Xe, Rn, Og. Chemically inert under most conditions, full valence shell. “Noble Gas ?” means an uncertain flag in the source data.
Halogens — Group 17: F, Cl, Br, I, At, Ts. Reactive nonmetals with seven valence electrons, form salts with metals.
Most elements crystallize at ambient conditions into a small set of common crystal structures, each defined by how atoms are arranged in three-dimensional space. These arrangements determine packing density, nearest-neighbour distances, and many physical properties such as density, strength, and conductivity. The most relevant for elemental solids are:
Face-centred cubic (FCC) — Atoms are located at each corner of a cube and at the centres of all cube faces. This structure is close-packed (packing fraction 0.74) and each atom has 12 nearest neighbours. Many ductile metals adopt FCC at room temperature, including aluminium, copper, silver, and gold.
Body-centred cubic (BCC) — Atoms are located at each cube corner and one atom at the cube’s body centre. This is not close-packed (packing fraction 0.68) and has 8 nearest neighbours. BCC metals such as iron (at room temperature), chromium, and tungsten are typically stronger and harder but less ductile than FCC metals.
Hexagonal (HEX) — A family of hexagonal lattices, including hexagonal close-packed (HCP) and related variants. Layers of atoms form a hexagonal lattice, often with 12 nearest neighbours. Close-packed forms have a packing fraction of 0.74, but some variants differ in stacking sequence or bonding. Magnesium, titanium, zinc, and cobalt adopt hexagonal forms at ambient conditions.
Diamond cubic (DIA) — A variation of the FCC lattice where each atom is covalently bonded to four others in a tetrahedral arrangement. This open structure has a low packing fraction (~0.34) and is characteristic of covalently bonded elements such as carbon (diamond form), silicon, and germanium.
Orthorhombic (ORC) — A rectangular lattice with three unequal axes at right angles. Found in elements such as sulfur and the halogens (Cl, Br, I), often reflecting molecular or complex bonding arrangements rather than close-packed spheres.
Rhombohedral (RHL) — A lattice with equal-length axes inclined at the same angle (not 90°). Examples include bismuth, antimony, and α-mercury.
Tetragonal (TET) — A cube stretched or compressed along one axis. Indium and tin adopt tetragonal forms.
Cubic (unspecified, CUB) — Cubic symmetry without a specific close-packed or diamond arrangement, often for molecular solids or high-temperature phases.
Monoclinic (MCL) — A skewed lattice with three unequal axes, two at right angles and the third inclined. Examples include plutonium at ambient temperature.
Simple cubic (SC) — Atoms occupy only the cube corners, each with 6 nearest neighbours. This has a low packing fraction (0.52) and is rare among elements; polonium is the only one that adopts it at ambient conditions.
These are the principal model structures used in elemental crystallography. Some elements adopt more complex or low-symmetry forms, which generally require experimental lattice constants for accurate property calculations.
Abbrev. | Meaning | Number | Examples |
---|---|---|---|
HEX | Hexagonal (includes HCP, dhcp, other variants) | 30 | Be, Mg, Ti, Zn |
FCC | Face-centred cubic | 21 | Al, Cu, Ag, Au |
BCC | Body-centred cubic | 15 | Li, Fe, W |
ORC | Orthorhombic | 7 | S, Cl, Br |
RHL | Rhombohedral | 5 | Sb, Bi, Hg |
TET | Tetragonal | 4 | In, Sn |
DIA | Diamond cubic | 3 | C (diamond), Si, Ge |
CUB | Cubic (unspecified type) | 3 | O, F, Po |
MCL | Monoclinic | 2 | Se, Pu |
SC | Simple cubic | 1 | Po |
Name | Symbol | Atomic Number | Atomic Weight | Melting Point | Boiling Point | Density | Electron Affinity | Thermal Conductivity |
---|---|---|---|---|---|---|---|---|
Hydrogen | H | 1 | 1.01 | 13.99 | 20.27 | 0.00 | 0.75 | 0.18 |
Helium | He | 2 | 4.00 | 4.22 | 0.00 | -19.70 | 0.15 | |
Lithium | Li | 3 | 6.94 | 453.65 | 1,615.15 | 0.53 | 0.62 | 84.80 |
Beryllium | Be | 4 | 9.01 | 1,560.15 | 2,741.15 | 1.85 | -2.40 | 201.00 |
Boron | B | 5 | 10.81 | 2,350.15 | 4,273.15 | 2.34 | 0.28 | 27.40 |
Carbon | C | 6 | 12.01 | 4,098.15 | 2.20 | 1.26 | 1.59 | |
Nitrogen | N | 7 | 14.01 | 63.15 | 77.35 | 0.00 | -1.40 | 0.03 |
Oxygen | O | 8 | 16.00 | 54.36 | 90.19 | 0.00 | 1.46 | 0.03 |
Fluorine | F | 9 | 19.00 | 53.48 | 85.04 | 0.00 | 3.40 | 0.03 |
Neon | Ne | 10 | 20.18 | 24.56 | 27.10 | 0.00 | ||
Sodium | Na | 11 | 22.99 | 370.94 | 1,156.09 | 0.97 | 0.55 | 142.00 |
Magnesium | Mg | 12 | 24.30 | 923.15 | 1,363.15 | 1.74 | 156.00 | |
Aluminum | Al | 13 | 26.98 | 933.47 | 2,792.15 | 2.70 | 0.43 | 237.00 |
Silicon | Si | 14 | 28.09 | 1,687.15 | 3,538.15 | 2.33 | 1.39 | 149.00 |
Phosphorus | P | 15 | 30.97 | 852.35 | 704.15 | 1.82 | 0.75 | |
Sulfur | S | 16 | 32.06 | 388.36 | 717.76 | 2.07 | 2.08 | 0.27 |
Chlorine | Cl | 17 | 35.45 | 171.65 | 239.11 | 0.00 | 3.61 | 0.01 |
Argon | Ar | 18 | 39.95 | 83.81 | 87.30 | 0.00 | -11.50 | 0.02 |
Potassium | K | 19 | 39.10 | 336.65 | 1,032.15 | 0.89 | 0.50 | 79.00 |
Calcium | Ca | 20 | 40.08 | 1,115.15 | 1,757.15 | 1.54 | 0.02 | |
Scandium | Sc | 21 | 44.96 | 1,814.15 | 3,109.15 | 2.99 | 0.19 | 15.80 |
Titanium | Ti | 22 | 47.87 | 1,943.15 | 3,560.15 | 4.51 | 0.08 | 21.90 |
Vanadium | V | 23 | 50.94 | 2,183.15 | 3,680.15 | 6.00 | 0.53 | 30.70 |
Chromium | Cr | 24 | 52.00 | 2,180.15 | 2,944.15 | 7.15 | 0.67 | 93.90 |
Manganese | Mn | 25 | 54.94 | 1,519.15 | 2,334.15 | 7.30 | ||
Iron | Fe | 26 | 55.84 | 1,811.15 | 3,134.15 | 7.87 | 0.15 | 80.40 |
Cobalt | Co | 27 | 58.93 | 1,768.15 | 3,200.15 | 8.86 | 0.66 | 100.00 |
Nickel | Ni | 28 | 58.69 | 1,728.15 | 3,186.15 | 8.90 | 1.16 | 90.90 |
Copper | Cu | 29 | 63.55 | 1,357.77 | 2,833.15 | 8.96 | 1.24 | 401.00 |
Zinc | Zn | 30 | 65.38 | 692.68 | 1,180.15 | 7.13 | 116.00 | |
Gallium | Ga | 31 | 69.72 | 302.91 | 2,502.15 | 5.91 | 0.43 | 28.10 |
Germanium | Ge | 32 | 72.63 | 1,211.40 | 3,106.15 | 5.32 | 1.23 | 60.20 |
Arsenic | As | 33 | 74.92 | 1,090.15 | 889.15 | 5.75 | 0.80 | |
Selenium | Se | 34 | 78.97 | 493.95 | 958.15 | 4.81 | 2.02 | 0.52 |
Bromine | Br | 35 | 79.90 | 265.95 | 331.95 | 3.10 | 3.36 | 0.01 |
Krypton | Kr | 36 | 83.80 | 115.78 | 119.73 | 0.00 | 0.01 | |
Rubidium | Rb | 37 | 85.47 | 312.45 | 961.15 | 1.53 | 0.49 | 58.20 |
Strontium | Sr | 38 | 87.62 | 1,050.15 | 1,650.15 | 2.64 | 0.05 | |
Yttrium | Y | 39 | 88.91 | 1,795.15 | 3,618.15 | 4.47 | 0.31 | |
Zirconium | Zr | 40 | 91.22 | 2,127.15 | 4,679.15 | 6.52 | 0.43 | 22.70 |
Niobium | Nb | 41 | 92.91 | 2,750.15 | 5,014.15 | 8.57 | 0.92 | 53.70 |
Molybdenum | Mo | 42 | 95.95 | 2,895.15 | 4,912.15 | 10.20 | 0.75 | |
Technetium | Tc | 43 | 97.91 | 2,430.15 | 4,535.15 | 11.00 | 0.55 | 50.60 |
Ruthenium | Ru | 44 | 101.07 | 2,606.15 | 4,420.15 | 12.10 | 1.05 | 117.00 |
Rhodium | Rh | 45 | 102.91 | 2,236.15 | 3,968.15 | 12.40 | 1.14 | 150.00 |
Palladium | Pd | 46 | 106.42 | 1,827.95 | 3,236.15 | 12.00 | 0.56 | 71.80 |
Silver | Ag | 47 | 107.87 | 1,234.93 | 2,435.15 | 10.50 | 1.30 | 429.00 |
Cadmium | Cd | 48 | 112.41 | 594.22 | 1,040.15 | 8.69 | 96.90 | |
Indium | In | 49 | 114.82 | 429.75 | 2,300.15 | 7.31 | 0.30 | 81.80 |
Tin | Sn | 50 | 118.71 | 505.08 | 2,859.15 | 7.29 | 1.11 | 66.80 |
Antimony | Sb | 51 | 121.76 | 903.78 | 1,860.15 | 6.68 | 1.05 | 24.43 |
Tellurium | Te | 52 | 127.60 | 722.66 | 1,261.15 | 6.23 | 1.97 | 14.30 |
Iodine | I | 53 | 126.90 | 386.85 | 457.55 | 4.93 | 3.06 | |
Xenon | Xe | 54 | 131.29 | 161.40 | 165.05 | 0.01 | -0.06 | 0.01 |
Cesium | Cs | 55 | 132.91 | 301.65 | 944.15 | 1.87 | 0.47 | 35.90 |
Barium | Ba | 56 | 137.33 | 1,000.15 | 2,118.15 | 3.62 | 0.14 | |
Lanthanum | La | 57 | 138.91 | 1,193.15 | 3,737.15 | 6.15 | 0.47 | 13.40 |
Cerium | Ce | 58 | 140.12 | 1,072.15 | 3,716.15 | 6.77 | 0.65 | 11.30 |
Praseodymium | Pr | 59 | 140.91 | 1,204.15 | 3,793.15 | 6.77 | 0.96 | 12.50 |
Neodymium | Nd | 60 | 144.24 | 1,289.15 | 3,347.15 | 7.01 | 1.92 | |
Promethium | Pm | 61 | 144.91 | 1,315.15 | 7.26 | 17.90 | ||
Samarium | Sm | 62 | 150.36 | 1,345.15 | 2,067.15 | 7.52 | ||
Europium | Eu | 63 | 151.96 | 1,095.15 | 1,802.15 | 5.24 | 0.86 | 13.90 |
Gadolinium | Gd | 64 | 157.25 | 1,586.15 | 3,546.15 | 7.90 | ||
Terbium | Tb | 65 | 158.93 | 1,632.15 | 3,503.15 | 8.23 | 1.17 | 11.10 |
Dysprosium | Dy | 66 | 162.50 | 1,685.15 | 2,840.15 | 8.55 | 0.35 | 10.70 |
Holmium | Ho | 67 | 164.93 | 1,745.15 | 2,973.15 | 8.80 | ||
Erbium | Er | 68 | 167.26 | 1,802.15 | 3,141.15 | 9.07 | ||
Thulium | Tm | 69 | 168.93 | 1,818.15 | 2,223.15 | 9.32 | 1.03 | |
Ytterbium | Yb | 70 | 173.04 | 1,097.15 | 1,469.15 | 6.90 | -0.02 | |
Lutetium | Lu | 71 | 174.97 | 1,936.15 | 3,675.15 | 9.84 | 0.34 | |
Hafnium | Hf | 72 | 178.49 | 2,506.15 | 4,873.15 | 13.30 | 0.01 | 23.00 |
Tantalum | Ta | 73 | 180.95 | 3,290.15 | 5,728.15 | 16.40 | 0.32 | 57.50 |
Tungsten | W | 74 | 183.84 | 3,687.15 | 5,828.15 | 19.30 | 0.82 | 173.00 |
Rhenium | Re | 75 | 186.21 | 3,458.15 | 5,863.15 | 20.80 | 0.15 | 48.00 |
Osmium | Os | 76 | 190.23 | 3,306.15 | 5,281.15 | 22.59 | 1.10 | |
Iridium | Ir | 77 | 192.22 | 2,719.15 | 4,701.15 | 22.56 | 1.56 | 147.00 |
Platinum | Pt | 78 | 195.08 | 2,041.35 | 4,098.15 | 21.50 | 2.13 | 71.60 |
Gold | Au | 79 | 196.97 | 1,337.33 | 3,109.15 | 19.30 | 2.31 | 318.00 |
Mercury | Hg | 80 | 200.59 | 234.32 | 629.77 | 13.53 | 8.30 | |
Thallium | Tl | 81 | 204.38 | 577.15 | 1,746.15 | 11.80 | 0.38 | 46.10 |
Lead | Pb | 82 | 207.20 | 600.61 | 2,022.15 | 11.30 | 0.36 | 35.30 |
Bismuth | Bi | 83 | 208.98 | 544.55 | 1,837.15 | 9.79 | 0.94 | 7.90 |
Polonium | Po | 84 | 209.00 | 527.15 | 1,235.15 | 9.20 | 1.90 | |
Astatine | At | 85 | 210.00 | 575.15 | 7.00 | 2.80 | ||
Radon | Rn | 86 | 222.00 | 202.15 | 211.45 | 0.01 | 0.00 | |
Francium | Fr | 87 | 223.00 | 294.15 | 1.87 | 0.49 | ||
Radium | Ra | 88 | 226.00 | 969.15 | 5.00 | 0.10 | ||
Actinium | Ac | 89 | 227.00 | 1,323.15 | 3,473.15 | 10.00 | 0.35 | |
Thorium | Th | 90 | 232.04 | 2,023.15 | 5,058.15 | 11.70 | ||
Protactinium | Pa | 91 | 231.04 | 1,845.15 | 15.40 | |||
Uranium | U | 92 | 238.03 | 1,408.15 | 4,404.15 | 19.10 | 27.50 | |
Neptunium | Np | 93 | 237.00 | 917.15 | 20.20 | |||
Plutonium | Pu | 94 | 244.00 | 913.15 | 3,501.15 | 19.70 | ||
Americium | Am | 95 | 243.00 | 1,449.15 | 12.00 | |||
Curium | Cm | 96 | 247.00 | 1,618.15 | 13.51 | |||
Berkelium | Bk | 97 | 247.00 | 1,259.15 | 14.78 | |||
Californium | Cf | 98 | 251.00 | 1,173.15 | 15.10 | |||
Einsteinium | Es | 99 | 252.00 | 1,133.15 | 8.84 | |||
Fermium | Fm | 100 | 257.00 | 1,800.15 | 9.70 | |||
Mendelevium | Md | 101 | 258.00 | 1,100.15 | 10.30 | |||
Nobelium | No | 102 | 259.00 | 1,100.15 | 9.90 | |||
Lawrencium | Lr | 103 | 262.00 | 1,900.15 | 15.60 | |||
Rutherfordium | Rf | 104 | 267.00 | 23.30 | ||||
Dubnium | Db | 105 | 268.00 | 29.30 | ||||
Seaborgium | Sg | 106 | 271.00 | 35.00 | ||||
Bohrium | Bh | 107 | 274.00 | 37.10 | ||||
Hassium | Hs | 108 | 269.00 | 40.70 | ||||
Meitnerium | Mt | 109 | 276.00 | 37.40 | ||||
Darmstadtium | Ds | 110 | 281.00 | 34.80 | ||||
Roentgenium | Rg | 111 | 281.00 | 28.70 | ||||
Copernicium | Cn | 112 | 285.00 | 14.00 | ||||
Nihonium | Nh | 113 | 286.00 | 16.00 | ||||
Flerovium | Fl | 114 | 289.00 | 9.93 | ||||
Moscovium | Mc | 115 | 288.00 | 13.50 | ||||
Livermorium | Lv | 116 | 293.00 | 12.90 | ||||
Tennessine | Ts | 117 | 294.00 | 7.20 | ||||
Oganesson | Og | 118 | 294.00 | 7.00 | 0.06 |
Thermal conductivity measures how effectively a material conducts heat, with units of watts per metre–kelvin (W·m⁻¹·K⁻¹). In metals, heat is carried primarily by conduction electrons, so good electrical conductors like copper, silver, and aluminum are also excellent thermal conductors. In nonmetals, heat is carried mainly by lattice vibrations (phonons), and conductivity depends on atomic bonding and crystal structure—diamond, for example, has extremely high thermal conductivity due to its strong covalent bonds and stiff lattice. Temperature, impurities, and structural defects can significantly affect a material’s thermal conductivity.
Name | Symbol | Atomic Number | Discoverers | Year |
---|---|---|---|---|
Hydrogen | H | 1 | Henry Cavendish | 1766 |
Helium | He | 2 | Sir William Ramsey, Nils Langet, P.T.Cleve | 1895 |
Lithium | Li | 3 | Johann Arfwedson | 1817 |
Beryllium | Be | 4 | Fredrich Wöhler, A.A.Bussy | 1798 |
Boron | B | 5 | Sir H. Davy, J.L. Gay-Lussac, L.J. Thénard | 1808 |
Carbon | C | 6 | Known to the ancients | ancient |
Nitrogen | N | 7 | Daniel Rutherford | 1772 |
Oxygen | O | 8 | Joseph Priestly, Carl Wilhelm Scheele | 1774 |
Fluorine | F | 9 | Henri Moissan | 1886 |
Neon | Ne | 10 | Sir William Ramsey, M.W. Travers | 1898 |
Sodium | Na | 11 | Sir Humphrey Davy | 1807 |
Magnesium | Mg | 12 | Sir Humphrey Davy | 1808 |
Aluminum | Al | 13 | Hans Christian Oersted | 1825 |
Silicon | Si | 14 | Jöns Berzelius | 1824 |
Phosphorus | P | 15 | Hennig Brand | 1669 |
Sulfur | S | 16 | Known to the ancients. | ancient |
Chlorine | Cl | 17 | Carl Wilhelm Scheele | 1774 |
Argon | Ar | 18 | Sir William Ramsey, Baron Rayleigh | 1894 |
Potassium | K | 19 | Sir Humphrey Davy | 1807 |
Calcium | Ca | 20 | Sir Humphrey Davy | 1808 |
Scandium | Sc | 21 | Lars Nilson | 1879 |
Titanium | Ti | 22 | William Gregor | 1791 |
Vanadium | V | 23 | Nils Sefström | 1830 |
Chromium | Cr | 24 | Louis Vauquelin | 1797 |
Manganese | Mn | 25 | Johann Gahn | 1774 |
Iron | Fe | 26 | Known to the ancients. | ancient |
Cobalt | Co | 27 | George Brandt | 1739 |
Nickel | Ni | 28 | Axel Cronstedt | 1751 |
Copper | Cu | 29 | Known to the ancients. | ancient |
Zinc | Zn | 30 | Known to the ancients. | ancient |
Gallium | Ga | 31 | Paul Émile Lecoq de Boisbaudran | 1875 |
Germanium | Ge | 32 | Clemens Winkler | 1886 |
Arsenic | As | 33 | Known to the ancients. | ancient |
Selenium | Se | 34 | Jöns Berzelius | 1818 |
Bromine | Br | 35 | Antoine J. Balard | 1826 |
Krypton | Kr | 36 | Sir William Ramsey, M.W. Travers | 1898 |
Rubidium | Rb | 37 | R. Bunsen, G. Kirchoff | 1861 |
Strontium | Sr | 38 | A. Crawford | 1790 |
Yttrium | Y | 39 | Johann Gadolin | 1789 |
Zirconium | Zr | 40 | Martin Klaproth | 1789 |
Niobium | Nb | 41 | Charles Hatchet | 1801 |
Molybdenum | Mo | 42 | Carl Wilhelm Scheele | 1778 |
Technetium | Tc | 43 | Carlo Perrier, Émillo Segrè | 1937 |
Ruthenium | Ru | 44 | Karl Klaus | 1844 |
Rhodium | Rh | 45 | William Wollaston | 1803 |
Palladium | Pd | 46 | William Wollaston | 1803 |
Silver | Ag | 47 | Known to the ancients. | ancient |
Cadmium | Cd | 48 | Fredrich Stromeyer | 1817 |
Indium | In | 49 | Ferdinand Reich, T. Richter | 1863 |
Tin | Sn | 50 | Known to the ancients. | ancient |
Antimony | Sb | 51 | Known to the ancients. | ancient |
Tellurium | Te | 52 | Franz Müller von Reichenstein | 1782 |
Iodine | I | 53 | Bernard Courtois | 1811 |
Xenon | Xe | 54 | Sir William Ramsay; M. W. Travers | 1898 |
Cesium | Cs | 55 | Gustov Kirchoff, Robert Bunsen | 1860 |
Barium | Ba | 56 | Sir Humphrey Davy | 1808 |
Lanthanum | La | 57 | Carl Mosander | 1839 |
Cerium | Ce | 58 | W. von Hisinger, J. Berzelius, M. Klaproth | 1803 |
Praseodymium | Pr | 59 | C.F. Aver von Welsbach | 1885 |
Neodymium | Nd | 60 | C.F. Aver von Welsbach | 1925 |
Promethium | Pm | 61 | J.A. Marinsky, L.E. Glendenin, C.D. Coryell | 1945 |
Samarium | Sm | 62 | Paul Émile Lecoq de Boisbaudran | 1879 |
Europium | Eu | 63 | Eugène Demarçay | 1901 |
Gadolinium | Gd | 64 | Jean de Marignac | 1880 |
Terbium | Tb | 65 | Carl Mosander | 1843 |
Dysprosium | Dy | 66 | Paul Émile Lecoq de Boisbaudran | 1886 |
Holmium | Ho | 67 | J.L. Soret | 1878 |
Erbium | Er | 68 | Carl Mosander | 1843 |
Thulium | Tm | 69 | Per Theodor Cleve | 1879 |
Ytterbium | Yb | 70 | Jean de Marignac | 1878 |
Lutetium | Lu | 71 | Georges Urbain | 1907 |
Hafnium | Hf | 72 | Dirk Coster, Georg von Hevesy | 1923 |
Tantalum | Ta | 73 | Anders Ekeberg | 1802 |
Tungsten | W | 74 | Fausto and Juan José de Elhuyar | 1783 |
Rhenium | Re | 75 | Walter Noddack, Ida Tacke, Otto Berg | 1925 |
Osmium | Os | 76 | Smithson Tenant | 1804 |
Iridium | Ir | 77 | S.Tenant, A.F.Fourcory, L.N.Vauquelin, H.V.Collet-Descoltils | 1804 |
Platinum | Pt | 78 | Julius Scaliger | 1735 |
Gold | Au | 79 | Known to the ancients. | ancient |
Mercury | Hg | 80 | Known to the ancients. | ancient |
Thallium | Tl | 81 | Sir William Crookes | 1861 |
Lead | Pb | 82 | Known to the ancients. | ancient |
Bismuth | Bi | 83 | Known to the ancients. | ancient |
Polonium | Po | 84 | Pierre and Marie Curie | 1898 |
Astatine | At | 85 | D.R.Corson, K.R.MacKenzie, E.Segré | 1940 |
Radon | Rn | 86 | Fredrich Ernst Dorn | 1898 |
Francium | Fr | 87 | Marguerite Derey | 1939 |
Radium | Ra | 88 | Pierre and Marie Curie | 1898 |
Actinium | Ac | 89 | André Debierne | 1899 |
Thorium | Th | 90 | Jöns Berzelius | 1828 |
Protactinium | Pa | 91 | Fredrich Soddy, John Cranston, Otto Hahn, Lise Meitner | 1917 |
Uranium | U | 92 | Martin Klaproth | 1789 |
Neptunium | Np | 93 | E.M. McMillan, P.H. Abelson | 1940 |
Plutonium | Pu | 94 | G.T.Seaborg, J.W.Kennedy, E.M.McMillan, A.C.Wohl | 1940 |
Americium | Am | 95 | G.T.Seaborg, R.A.James, L.O.Morgan, A.Ghiorso | 1945 |
Curium | Cm | 96 | G.T.Seaborg, R.A.James, A.Ghiorso | 1944 |
Berkelium | Bk | 97 | G.T.Seaborg, S.G.Tompson, A.Ghiorso | 1949 |
Californium | Cf | 98 | G.T.Seaborg, S.G.Tompson, A.Ghiorso, K.Street Jr. | 1950 |
Einsteinium | Es | 99 | Argonne, Los Alamos, U of Calif | 1952 |
Fermium | Fm | 100 | Argonne, Los Alamos, U of Calif | 1953 |
Mendelevium | Md | 101 | G.T.Seaborg, S.G.Tompson, A.Ghiorso, K.Street Jr. | 1955 |
Nobelium | No | 102 | Nobel Institute for Physics | 1957 |
Lawrencium | Lr | 103 | A.Ghiorso, T.Sikkeland, A.E.Larsh, R.M.Latimer | 1961 |
Rutherfordium | Rf | 104 | A. Ghiorso, et al | 1969 |
Dubnium | Db | 105 | A. Ghiorso, et al | 1970 |
Seaborgium | Sg | 106 | Soviet Nuclear Research/ U. of Cal at Berkeley | 1974 |
Bohrium | Bh | 107 | Heavy Ion Research Laboratory (HIRL) | 1976 |
Hassium | Hs | 108 | Heavy Ion Research Laboratory (HIRL) | 1984 |
Meitnerium | Mt | 109 | Heavy Ion Research Laboratory (HIRL) | 1982 |
Darmstadtium | Ds | 110 | Heavy Ion Research Laboratory (HIRL) | 1994 |
Roentgenium | Rg | 111 | Heavy Ion Research Laboratory (HIRL) | 1994 |
Copernicium | Cn | 112 | GSI Helmholtz Centre for Heavy Ion Research | 1996 |
Nihonium | Nh | 113 | RIKEN | 2015 |
Flerovium | Fl | 114 | Joint Institute for Nuclear Research | 1998 |
Moscovium | Mc | 115 | Joint Institute for Nuclear Research | 2003 |
Livermorium | Lv | 116 | Lawrence Livermore National Laboratory | 2000 |
Oganesson | Og | 118 | Joint Institute for Nuclear Research | 2002 |
This estimation method uses basic crystallographic geometry to approximate an element’s bulk density from its atomic weight, metallic radius, and crystal structure (Section 10.2). The key idea is that, if you know how atoms are arranged in a solid and how big they are, you can calculate the size of the repeating unit cell in the crystal lattice. By combining the unit cell’s volume with the number of atoms it contains and the mass per atom (derived from the atomic weight), you get an estimate of the density. Different crystal structures—face-centred cubic (FCC), body-centred cubic (BCC), hexagonal close-packed (HCP), simple cubic (SC), or diamond cubic—have characteristic relationships between the lattice parameter and the atomic radius, as well as fixed numbers of atoms per unit cell. For close-packed metals, a metallic radius and an idealised \(c/a\) ratio are used; for more accurate work, element-specific \(c/a\) values can be substituted for non-ideal structures such as zinc and cadmium.
This is a first-order physical model and, while it works reasonably well for close-packed metals, it is less reliable for elements with non-metallic bonding, low-symmetry structures, or significant open space in the crystal lattice. In such cases—noble gases, molecular solids, graphite, or unusual hcp variants—the actual packing fraction can deviate substantially from the ideal, leading to large errors. The method also depends on using the correct type of radius (metallic, covalent, or van der Waals) for the structure in question. When applied carefully with appropriate inputs, it can match tabulated densities within about 5–10 % for many metals, while providing a clear, geometry-based link between microscopic atomic parameters and macroscopic material properties.
bit = df[['Symbol', 'Atomic Number', 'Atomic Weight', 'Density', 'Crystal Structure', 'Metallic Radius']].copy()
bit.columns = ['Symbol', 'Z', 'Atomic Weight', 'Density', 'Crystal Structure', 'Radius']
bit["Crystal"] = bit["Symbol"].map(DensityEstimator.CRYSTAL).fillna("")
bit["Radius_pm"] = bit["Symbol"].map(
DensityEstimator.RADIUS_PM).astype("Float64")
bit["Density_est"] = [
DensityEstimator._estimate_density_one(sym, aw)
for sym, aw in zip(bit["Symbol"], bit["Atomic Weight"])
]
bit['Error'] = bit.Density_est / bit.Density - 1
fGT(bit.query('Density_est > 0').set_index(['Symbol', 'Z']), year_cols='Z', ratio_cols='Error')
Symbol | Z | Atomic Weight | Density | Crystal Structure | Radius | Crystal | Radius_pm | Density_est | Error |
---|---|---|---|---|---|---|---|---|---|
Li | 3 | 6.94 | 0.534 | BCC | 123.00 | bcc | 167.00 | 0.402 | -24.8% |
Be | 4 | 9.01 | 1.850 | HEX | 89.00 | hcp | 112.00 | 1.883 | 1.8% |
C | 6 | 12.01 | 2.200 | DIA | nan | diamond | 77.00 | 3.547 | 61.2% |
Na | 11 | 22.99 | 0.970 | BCC | 157.00 | bcc | 190.00 | 0.904 | -6.8% |
Mg | 12 | 24.30 | 1.740 | HEX | 136.00 | hcp | 160.00 | 1.742 | 0.1% |
Al | 13 | 26.98 | 2.700 | FCC | 125.00 | fcc | 143.00 | 2.709 | 0.3% |
Si | 14 | 28.09 | 2.330 | DIA | 117.00 | diamond | 111.00 | 2.769 | 18.8% |
K | 19 | 39.10 | 0.890 | BCC | 203.00 | bcc | 243.00 | 0.735 | -17.4% |
Ca | 20 | 40.08 | 1.540 | FCC | 174.00 | fcc | 197.00 | 1.539 | -0.1% |
Ti | 22 | 47.87 | 4.506 | HEX | 132.00 | hcp | 147.00 | 4.423 | -1.8% |
V | 23 | 50.94 | 6.000 | BCC | 122.00 | bcc | 134.00 | 5.709 | -4.9% |
Cr | 24 | 52.00 | 7.150 | BCC | 119.00 | bcc | 128.00 | 6.685 | -6.5% |
Mn | 25 | 54.94 | 7.300 | CUB | 118.00 | bcc | 127.00 | 7.232 | -0.9% |
Fe | 26 | 55.84 | 7.870 | BCC | 117.00 | bcc | 126.00 | 7.528 | -4.4% |
Co | 27 | 58.93 | 8.860 | HEX | 116.00 | hcp | 125.00 | 8.857 | -0.0% |
Ni | 28 | 58.69 | 8.900 | FCC | 115.00 | fcc | 124.00 | 9.036 | 1.5% |
Cu | 29 | 63.55 | 8.960 | FCC | 118.00 | fcc | 128.00 | 8.895 | -0.7% |
Zn | 30 | 65.38 | 7.134 | HEX | 121.00 | hcp | 134.00 | 7.018 | -1.6% |
Ge | 32 | 72.63 | 5.323 | DIA | 124.00 | diamond | 122.00 | 5.392 | 1.3% |
Rb | 37 | 85.47 | 1.530 | BCC | 216.00 | bcc | 265.00 | 1.238 | -19.1% |
Sr | 38 | 87.62 | 2.640 | FCC | 191.00 | fcc | 215.00 | 2.588 | -2.0% |
Y | 39 | 88.91 | 4.470 | HEX | 162.00 | hcp | 180.00 | 4.475 | 0.1% |
Zr | 40 | 91.22 | 6.520 | HEX | 145.00 | hcp | 160.00 | 6.538 | 0.3% |
Nb | 41 | 92.91 | 8.570 | BCC | 134.00 | bcc | 146.00 | 8.049 | -6.1% |
Mo | 42 | 95.95 | 10.200 | BCC | 130.00 | bcc | 139.00 | 9.633 | -5.6% |
Tc | 43 | 97.91 | 11.000 | HEX | 127.00 | hcp | 136.00 | 11.425 | 3.9% |
Ru | 44 | 101.07 | 12.100 | HEX | 125.00 | hcp | 134.00 | 12.331 | 1.9% |
Ag | 47 | 107.87 | 10.500 | FCC | 134.00 | fcc | 144.00 | 10.604 | 1.0% |
Cd | 48 | 112.41 | 8.690 | HEX | 138.00 | hcp | 151.00 | 8.299 | -4.5% |
Cs | 55 | 132.91 | 1.873 | BCC | 235.00 | bcc | 298.00 | 1.354 | -27.7% |
Ba | 56 | 137.33 | 3.620 | BCC | 198.00 | bcc | 217.00 | 3.624 | 0.1% |
La | 57 | 138.91 | 6.150 | HEX | 169.00 | hcp | 187.00 | 6.235 | 1.4% |
Eu | 63 | 151.96 | 5.240 | BCC | nan | bcc | 199.00 | 5.200 | -0.8% |
Gd | 64 | 157.25 | 7.900 | HEX | nan | hcp | 180.00 | 7.915 | 0.2% |
Tb | 65 | 158.93 | 8.230 | HEX | nan | hcp | 177.00 | 8.413 | 2.2% |
Dy | 66 | 162.50 | 8.550 | HEX | nan | hcp | 178.00 | 8.458 | -1.1% |
Ho | 67 | 164.93 | 8.800 | HEX | nan | hcp | 176.00 | 8.880 | 0.9% |
Er | 68 | 167.26 | 9.070 | HEX | nan | hcp | 176.00 | 9.006 | -0.7% |
Tm | 69 | 168.93 | 9.321 | HEX | nan | hcp | 175.00 | 9.253 | -0.7% |
Yb | 70 | 173.04 | 6.900 | FCC | nan | fcc | 194.00 | 6.957 | 0.8% |
Lu | 71 | 174.97 | 9.840 | HEX | nan | hcp | 174.00 | 9.749 | -0.9% |
Hf | 72 | 178.49 | 13.300 | HEX | 144.00 | hcp | 159.00 | 13.035 | -2.0% |
Ta | 73 | 180.95 | 16.400 | BCC | 134.00 | bcc | 146.00 | 15.677 | -4.4% |
W | 74 | 183.84 | 19.300 | BCC | 130.00 | bcc | 139.00 | 18.458 | -4.4% |
Re | 75 | 186.21 | 20.800 | HEX | 128.00 | hcp | 137.00 | 21.257 | 2.2% |
Os | 76 | 190.23 | 22.587 | HEX | 126.00 | hcp | 135.00 | 22.696 | 0.5% |
Au | 79 | 196.97 | 19.300 | FCC | 134.00 | fcc | 144.00 | 19.363 | 0.3% |
Pb | 82 | 207.20 | 11.300 | FCC | 150.00 | fcc | 175.00 | 11.349 | 0.4% |
Po | 84 | 209.00 | 9.200 | SC | nan | sc | 167.00 | 9.314 | 1.2% |
import matplotlib.pyplot as plt
bitm = bit.query("Density_est > 0").copy()
# color map per crystal type
crystal_colors = {
"fcc": "tab:blue",
"bcc": "tab:orange",
"hcp": "tab:green",
"diamond": "tab:red",
"sc": "tab:purple",
"": "gray", # fallback
}
fig, ax = plt.subplots(1, 1, figsize=(5, 5))
# 1:1 reference line
ax.plot(bitm.Density, bitm.Density, lw=0.5, c="k", alpha=0.5)
# plot by crystal type
for struct, group in bitm.groupby("Crystal"):
ax.scatter(
group.Density,
group.Density_est,
marker="o",
s=10,
c=crystal_colors.get(struct, "gray"),
label=struct if struct else "unknown",
alpha=0.8,
)
ax.set(
xlabel="Density (g cm$^{-3}$)",
ylabel="Estimated density (g cm$^{-3}$)",
aspect="equal",
)
ax.legend(title="Crystal structure", markerscale=2, fontsize=8)
for n, r in bit.query('abs(Error) > 0.2').iterrows():
if r.Error > 0:
ax.text(r.Density, r.Density_est + 0.2, r.Symbol, ha='center', va='bottom', fontsize=10)
else:
ax.text(r.Density, r.Density_est - 0.2, r.Symbol, ha='center', va='top', fontsize=10)
Here are some other relationships between observables.
Molar volume \(V_m\) — the volume occupied by one mole of a substance. Formula: \(V_m = M / \rho\), where \(M\) is molar mass in g·mol⁻¹ (mass of one mole of atoms), and \(\rho\) is density in g·cm⁻³. Units are usually cm³·mol⁻¹.
Packing fraction — the fraction of space inside a crystal lattice that is actually filled by atoms. Formula: \(f = V_{\text{atoms}} / V_{\text{cell}}\), where \(V_{\text{atoms}}\) is the combined volume of all atoms in the unit cell (from atomic radius), and \(V_{\text{cell}}\) is the volume of the unit cell (from lattice parameters). Ideal close-packed values are 0.74 (FCC, HCP), 0.68 (BCC), and 0.52 (simple cubic).
Nearest-neighbor distance \(d_{\text{NN}}\) — the distance between the centers of two atoms that are directly bonded (or touching in the metallic sense). Calculated from the lattice parameter \(a\) and structure: for FCC, \(d_{\text{NN}} = a / \sqrt{2}\); for BCC, \(d_{\text{NN}} = \sqrt{3}a / 2\); for HCP, \(d_{\text{NN}} = a\).
Number density \(n\) — the number of atoms per unit volume of the solid. Formula: \(n = N_A \rho / M\), where \(N_A\) is Avogadro’s number (6.022×10²³ mol⁻¹), \(\rho\) is density (kg·m⁻³ or g·cm⁻³), and \(M\) is molar mass in kg·mol⁻¹ or g·mol⁻¹.
Melting point \(T_m\) — the temperature at which the solid and liquid phases of a substance are in equilibrium. While exact values require experiment, trends can be estimated from atomic number, radius, and bonding type: small-radius transition metals tend to have high \(T_m\), alkali metals low \(T_m\).
Boiling point \(T_b\) — the temperature at which the vapor pressure equals the external pressure (often 1 atm). Similar empirical modeling to melting points: strong metallic or covalent bonding → high \(T_b\); weak van der Waals interactions → low \(T_b\).
Hardness — resistance of a material to deformation, usually given on the Mohs or Vickers scale. For elements, hardness correlates with bond strength (short bonds, high electronegativity differences, or covalent networks tend to be hardest).
Electrical conductivity \(\sigma\) — the ability of a material to carry electric current, measured in siemens per metre (S·m⁻¹). For metals, \(\sigma\) can be estimated from crystal structure, valence electron count, and resistivity data; low resistivity corresponds to high \(\sigma\).
Thermal conductivity \(k\) — the ability of a material to conduct heat, measured in watts per metre per kelvin (W·m⁻¹·K⁻¹). For metals, \(k\) is related to electrical conductivity via the Wiedemann–Franz law: \(k / \sigma T \approx L\), where \(L\) is the Lorenz number (~2.45×10⁻⁸ W·Ω·K⁻²).
Bulk modulus \(K\) — a measure of resistance to uniform compression, in pascals (Pa). Roughly scales with bond strength and inversely with atomic volume (\(K \propto 1 / V_m\)); highest in dense covalent solids and close-packed transition metals.
Speed of sound \(v\) — the velocity of mechanical waves through the solid, in m·s⁻¹. Formula: \(v = \sqrt{K / \rho}\) for longitudinal waves in a simple isotropic model, where \(K\) is bulk modulus and \(\rho\) is density.
Cohesive energy \(E_c\) — the energy required to separate a solid into isolated atoms, usually in eV per atom. Correlates with bonding type, crystal structure, and atomic radius: covalent networks and dense metals have the highest \(E_c\).
Surface energy \(\gamma\) — the energy per unit area to create a new surface, in J·m⁻². Related to cohesive energy and atomic packing: \(\gamma\) tends to be high for strongly bonded, close-packed solids and low for weakly bound molecular solids.
Mendeleev
packageMendeleev
is a Python package providing a comprehensive source of data with an easy Python interface, see the Documentation.
L. M. Mentel, mendeleev - A Python resource for properties of chemical elements, ions and isotopes. , 2014–present. Available at: https://github.com/lmmentel/mendeleev.
index | Hydrogen | Carbon | Nitrogen | Oxygen | Neon |
---|---|---|---|---|---|
atomic_number | 1 | 6 | 7 | 8 | 10 |
atomic_radius | 25 | 70 | 65 | 60 | 160 |
block | s | p | p | p | p |
density | 0.000 | 2.200 | 0.001 | 0.001 | 0.001 |
description | Colourless, odourless gaseous chemical element. Lightest and most abundant element in the universe. Present in water and in all organic compounds. Chemically reacts with most elements. Discovered by Henry Cavendish in 1776. | Carbon is a member of group 14 of the periodic table. It has three allotropic forms of it, diamonds, graphite and fullerite. Carbon-14 is commonly used in radioactive dating. Carbon occurs in all organic life and is the basis of organic chemistry. Carbon has the interesting chemical property of being able to bond with itself, and a wide variety of other elements. | Colourless, gaseous element which belongs to group 15 of the periodic table. Constitutes ~78% of the atmosphere and is an essential part of the ecosystem. Nitrogen for industrial purposes is acquired by the fractional distillation of liquid air. Chemically inactive, reactive generally only at high temperatures or in electrical discharges. It was discovered in 1772 by D. Rutherford. | A colourless, odourless gaseous element belonging to group 16 of the periodic table. It is the most abundant element present in the earth's crust. It also makes up 20.8% of the Earth's atmosphere. For industrial purposes, it is separated from liquid air by fractional distillation. It is used in high temperature welding, and in breathing. It commonly comes in the form of Oxygen, but is found as Ozone in the upper atmosphere. It was discovered by Priestley in 1774. | Colourless gaseous element of group 18 on the periodic table (noble gases). Neon occurs in the atmosphere, and comprises 0.0018% of the volume of the atmosphere. It has a distinct reddish glow when used in discharge tubes and neon based lamps. It forms almost no chemical compounds. Neon was discovered in 1898 by Sir William Ramsey and M.W. Travers. |
dipole_polarizability | 4.507 | 11.300 | 7.400 | 5.300 | 2.661 |
electron_affinity | 0.754 | 1.262 | -1.400 | 1.461 | nan |
electronic_configuration | 1s | [He] 2s2 2p2 | [He] 2s2 2p3 | [He] 2s2 2p4 | [He] 2s2 2p6 |
evaporation_heat | 0.904 | nan | nan | nan | 1.740 |
fusion_heat | 0.117 | nan | nan | nan | nan |
group_id | 1 | 14 | 15 | 16 | 18 |
lattice_constant | 3.750 | 3.570 | 4.039 | 6.830 | 4.430 |
lattice_structure | HEX | DIA | HEX | CUB | FCC |
period | 1 | 2 | 2 | 2 | 2 |
series_id | 1 | 1 | 1 | 1 | 2 |
specific_heat_capacity | 14.304 | 0.709 | 1.040 | 0.918 | 1.030 |
symbol | H | C | N | O | Ne |
thermal_conductivity | 0.181 | 1.590 | 0.026 | 0.027 | nan |
vdw_radius | 110.000 | 170 | 155 | 152 | 154 |
covalent_radius_cordero | 31 | 73 | 71 | 66 | 58.000 |
covalent_radius_pyykko | 32 | 75 | 71 | 63 | 67 |
en_pauling | 2.200 | 2.550 | 3.040 | 3.440 | nan |
en_allen | 13.610 | 15.050 | 18.130 | 21.360 | 28.310 |
jmol_color | #ffffff | #909090 | #3050f8 | #ff0d0d | #b3e3f5 |
cpk_color | #ffffff | #c8c8c8 | #8f8fff | #f00000 | #ff1493 |
proton_affinity | nan | nan | 342.200 | 485.200 | 198.800 |
gas_basicity | nan | nan | 318.700 | 459.600 | 174.400 |
heat_of_formation | 217.998 | 716.870 | 472.440 | 249.229 | nan |
c6 | 6.499 | 46.600 | 24.200 | 15.600 | 6.200 |
covalent_radius_bragg | nan | 77 | 65 | 65 | nan |
vdw_radius_bondi | 120 | 170 | 155 | 152 | 154 |
vdw_radius_truhlar | nan | nan | nan | nan | nan |
vdw_radius_rt | 110.000 | 177 | 164 | 158 | nan |
vdw_radius_batsanov | nan | 170 | 160 | 155 | nan |
vdw_radius_dreiding | 319.500 | 389.830 | 366.210 | 340.460 | nan |
vdw_radius_uff | 288.600 | 385.100 | 366 | 350 | 324.300 |
vdw_radius_mm3 | 162 | 204 | 193 | 182 | 160 |
abundance_crust | 1,400 | 200 | 19 | 461,000 | 0.005 |
abundance_sea | 108,000 | 28 | 0.500 | 857,000 | 0.000 |
molcas_gv_color | #f2f2f2 | #555555 | #3753bb | #f32e42 | #b3e3f5 |
en_ghosh | 0.264 | 0.225 | 0.265 | 0.305 | 0.384 |
vdw_radius_alvarez | 120 | 177 | 166 | 150 | 158 |
c6_gb | 6.510 | 47.900 | 25.700 | 16.700 | 6.910 |
atomic_weight | 1.008 | 12.011 | 14.007 | 15.999 | 20.180 |
atomic_weight_uncertainty | nan | nan | nan | nan | 0.001 |
is_monoisotopic | nan | nan | nan | nan | nan |
is_radioactive | 0 | 0 | 0 | 0 | 0 |
cas | 1333-74-0 | 7440-44-0 | 7727-37-9 | 7782-44-7 | 7440-01-9 |
atomic_radius_rahm | 154 | 190 | 179 | 171 | 156 |
geochemical_class | volatile | semi-volatile | volatile | major | volatile |
goldschmidt_class | atmophile | atmophile | atmophile | litophile | atmophile |
metallic_radius | nan | nan | nan | nan | nan |
metallic_radius_c12 | 78 | 86 | 53 | nan | nan |
covalent_radius_pyykko_double | nan | 67 | 60 | 57 | 96 |
covalent_radius_pyykko_triple | nan | 60 | 54 | 53 | nan |
discoverers | Henry Cavendish | Known to the ancients | Daniel Rutherford | Joseph Priestly, Carl Wilhelm Scheele | Sir William Ramsey, M.W. Travers |
discovery_year | 1,766 | nan | 1,772 | 1,774 | 1,898 |
discovery_location | England | None | Scotland | England/Sweden | England |
name_origin | Greek: hydro (water) and genes (generate) | Latin: carbo, (charcoal). | Greek: nitron and genes, (soda forming). | Greek: oxys and genes, (acid former). | Greek: neos (new). |
sources | Commercial quantities are produced by reacting superheated steam with methane or carbon. In lab work from reaction of metals with acid solutions or electrolysis. | Made by burning organic compounds with insufficient oxygen. | Obtained from liquid air by fractional distillation. | Obtained primarily from liquid air by fractional distillation. Small amounts are made in the laboratory by electrolysis of water or heating potassium chlorate (KClO3) with manganese dioxide (MnO2) catalyst. | Obtained from production of liquid air as a byproduct of producing liquid oxygen and nitrogen. |
uses | Most hydrogen is used in the production of ammonia. Also used in balloons and in metal refining. Also used as fuel in rockets. Its two heavier isotopes are: deuterium (D) and tritium (T) used respectively for nuclear fission and fusion. | For making steel, in filters, and many more uses. Radiocarbon dating uses the carbon-14 isotope to date old objects. | Primarily to produce ammonia and other fertilizers. Also used in making nitric acid, which is used in explosives. Also used in welding and enhanced oil recovery. | Used in steel making, welding, and supporting life. Naturally occuring ozone (O3) in the upper atmosphere shields the earth from ultraviolet radiation. | Primarily for lighting. |
mendeleev_number | 105 | 87 | 93 | 99 | 113 |
dipole_polarizability_unc | 0.000 | 0.400 | 0.200 | 0.200 | 0.000 |
pettifor_number | 103 | 95 | 100 | 101 | 2 |
glawe_number | 103 | 87 | 88 | 97 | 2 |
molar_heat_capacity | 28.836 | 8.517 | 29.124 | 29.378 | 20.786 |
en_miedema | 5.200 | 6.240 | 6.860 | nan | nan |
miedema_molar_volume | 1.700 | 3.260 | 4.100 | nan | nan |
miedema_electron_density | 3.380 | 5.550 | 4.490 | nan | nan |
en_gunnarsson_lundqvist | 5.740 | 6.520 | 6.670 | 7.670 | 6.960 |
en_robles_bartolotti | 5.270 | 6.390 | 5.780 | 6.450 | 6.600 |
production_concentration | nan | 46 | nan | nan | nan |
relative_supply_risk | nan | 4.500 | nan | nan | nan |
reserve_distribution | nan | 28 | nan | nan | nan |
political_stability_of_top_producer | nan | 24.100 | nan | nan | nan |
political_stability_of_top_reserve_holder | nan | 56.600 | nan | nan | nan |
top_3_producers | None | 1) China 2) USA 3) India | None | None | None |
top_3_reserve_holders | None | 1) USA 2) Russia 3) China | None | None | None |
recycling_rate | None | None | None | None | None |
substitutability | None | None | None | None | None |
price_per_kg | 1.390 | 0.122 | 0.140 | 0.154 | 240 |
en_mullay | 2.080 | 2.470 | 2.400 | 3.150 | nan |
mendeleev
includes other tables, e.g., isotope, radii, oxidation, phase and scattering. Here is a subset of the ionization energy data.
atomic_number | IE1 | IE2 | IE3 | IE4 | IE5 |
---|---|---|---|---|---|
1 | 13.60 | ||||
2 | 24.59 | 54.42 | |||
3 | 5.39 | 75.64 | 122.45 | ||
4 | 9.32 | 18.21 | 153.90 | 217.72 | |
5 | 8.30 | 25.15 | 37.93 | 259.37 | 340.23 |
6 | 11.26 | 24.38 | 47.89 | 64.49 | 392.09 |
7 | 14.53 | 29.60 | 47.45 | 77.47 | 97.89 |
8 | 13.62 | 35.12 | 54.94 | 77.41 | 113.90 |
9 | 17.42 | 34.97 | 62.71 | 87.17 | 114.25 |
10 | 21.56 | 40.96 | 63.42 | 97.19 | 126.25 |
11 | 5.14 | 47.29 | 71.62 | 98.94 | 138.40 |
12 | 7.65 | 15.04 | 80.14 | 109.27 | 141.33 |
13 | 5.99 | 18.83 | 28.45 | 119.99 | 153.83 |
14 | 8.15 | 16.35 | 33.49 | 45.14 | 166.77 |
15 | 10.49 | 19.77 | 30.20 | 51.44 | 65.03 |
16 | 10.36 | 23.34 | 34.86 | 47.22 | 72.59 |
17 | 12.97 | 23.81 | 39.80 | 53.24 | 67.68 |
18 | 15.76 | 27.63 | 40.73 | 59.58 | 74.84 |
Table 9 shows all the data extracted from mendeleev
used in this post.
index | Atomic Number | Name | Symbol | Atomic Weight | Group | Group Symbol | Block | Period | Electron Configuration | Crystal Structure | Lattice Constant | Atomic Radius | Metallic Radius | Covalent radius | Van der Waals Radius | Electro-negativity (Pauling) | Density | Electron Affinity | Thermal Conductivity | Discoverers | Year | Ionization Energy | Melting Point | Boiling Point | Type | Phase |
---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|
0 | 1 | Hydrogen | H | 1.01 | 1 | IA | s | 1 | 1s | HEX | 3.750 | 25.00 | nan | 32.00 | 110.00 | 2.200 | 0.000 | 0.754 | 0.18 | Henry Cavendish | 1766 | 13.598 | 13.99 | 20.27 | Nonmetals | Gas |
1 | 2 | Helium | He | 4.00 | 18 | VIIIA | s | 1 | 1s2 | HEX | 3.570 | 120.00 | nan | 46.00 | 140.00 | nan | 0.000 | -19.700 | 0.15 | Sir William Ramsey, Nils Langet, P.T.Cleve | 1895 | 24.587 | nan | 4.22 | Noble gases | Gas |
2 | 3 | Lithium | Li | 6.94 | 1 | IA | s | 2 | [He] 2s | BCC | 3.490 | 145.00 | 123.00 | 133.00 | 182.00 | 0.980 | 0.534 | 0.618 | 84.80 | Johann Arfwedson | 1817 | 5.392 | 453.65 | 1,615.15 | Alkali metals | Solid |
3 | 4 | Beryllium | Be | 9.01 | 2 | IIA | s | 2 | [He] 2s2 | HEX | 2.290 | 105.00 | 89.00 | 102.00 | 153.00 | 1.570 | 1.850 | -2.400 | 201.00 | Fredrich Wöhler, A.A.Bussy | 1798 | 9.323 | 1,560.15 | 2,741.15 | Alkaline earth metals | Solid |
4 | 5 | Boron | B | 10.81 | 13 | IIIA | p | 2 | [He] 2s2 2p | TET | 8.730 | 85.00 | 80.00 | 85.00 | 192.00 | 2.040 | 2.340 | 0.280 | 27.40 | Sir H. Davy, J.L. Gay-Lussac, L.J. Thénard | 1808 | 8.298 | 2,350.15 | 4,273.15 | Metalloids | Solid |
5 | 6 | Carbon | C | 12.01 | 14 | IVA | p | 2 | [He] 2s2 2p2 | DIA | 3.570 | 70.00 | nan | 75.00 | 170.00 | 2.550 | 2.200 | 1.262 | 1.59 | Known to the ancients | nan | 11.260 | nan | 4,098.15 | Nonmetals | Gas |
6 | 7 | Nitrogen | N | 14.01 | 15 | VA | p | 2 | [He] 2s2 2p3 | HEX | 4.039 | 65.00 | nan | 71.00 | 155.00 | 3.040 | 0.001 | -1.400 | 0.03 | Daniel Rutherford | 1772 | 14.534 | 63.15 | 77.35 | Nonmetals | Gas |
7 | 8 | Oxygen | O | 16.00 | 16 | VIA | p | 2 | [He] 2s2 2p4 | CUB | 6.830 | 60.00 | nan | 63.00 | 152.00 | 3.440 | 0.001 | 1.461 | 0.03 | Joseph Priestly, Carl Wilhelm Scheele | 1774 | 13.618 | 54.36 | 90.19 | Nonmetals | Gas |
8 | 9 | Fluorine | F | 19.00 | 17 | VIIA | p | 2 | [He] 2s2 2p5 | MCL | nan | 50.00 | nan | 64.00 | 147.00 | 3.980 | 0.002 | 3.401 | 0.03 | Henri Moissan | 1886 | 17.423 | 53.48 | 85.04 | Halogens | Gas |
9 | 10 | Neon | Ne | 20.18 | 18 | VIIIA | p | 2 | [He] 2s2 2p6 | FCC | 4.430 | 160.00 | nan | 67.00 | 154.00 | nan | 0.001 | nan | nan | Sir William Ramsey, M.W. Travers | 1898 | 21.565 | 24.56 | 27.10 | Noble gases | Gas |
10 | 11 | Sodium | Na | 22.99 | 1 | IA | s | 3 | [Ne] 3s | BCC | 4.230 | 180.00 | 157.00 | 155.00 | 227.00 | 0.930 | 0.970 | 0.548 | 142.00 | Sir Humphrey Davy | 1807 | 5.139 | 370.94 | 1,156.09 | Alkali metals | Solid |
11 | 12 | Magnesium | Mg | 24.30 | 2 | IIA | s | 3 | [Ne] 3s2 | HEX | 3.210 | 150.00 | 136.00 | 139.00 | 173.00 | 1.310 | 1.740 | nan | 156.00 | Sir Humphrey Davy | 1808 | 7.646 | 923.15 | 1,363.15 | Alkaline earth metals | Solid |
12 | 13 | Aluminum | Al | 26.98 | 13 | IIIA | p | 3 | [Ne] 3s2 3p | FCC | 4.050 | 125.00 | 125.00 | 126.00 | 184.00 | 1.610 | 2.700 | 0.433 | 237.00 | Hans Christian Oersted | 1825 | 5.986 | 933.47 | 2,792.15 | Poor metals | Solid |
13 | 14 | Silicon | Si | 28.09 | 14 | IVA | p | 3 | [Ne] 3s2 3p2 | DIA | 5.430 | 110.00 | 117.00 | 116.00 | 210.00 | 1.900 | 2.330 | 1.390 | 149.00 | Jöns Berzelius | 1824 | 8.152 | 1,687.15 | 3,538.15 | Metalloids | Solid |
14 | 15 | Phosphorus | P | 30.97 | 15 | VA | p | 3 | [Ne] 3s2 3p3 | CUB | 7.170 | 100.00 | 110.00 | 111.00 | 180.00 | 2.190 | 1.823 | 0.747 | nan | Hennig Brand | 1669 | 10.487 | 852.35 | 704.15 | Nonmetals | Solid |
15 | 16 | Sulfur | S | 32.06 | 16 | VIA | p | 3 | [Ne] 3s2 3p4 | ORC | 10.470 | 100.00 | 104.00 | 103.00 | 180.00 | 2.580 | 2.070 | 2.077 | 0.27 | Known to the ancients. | nan | 10.360 | 388.36 | 717.76 | Nonmetals | Solid |
16 | 17 | Chlorine | Cl | 35.45 | 17 | VIIA | p | 3 | [Ne] 3s2 3p5 | ORC | 6.240 | 100.00 | nan | 99.00 | 175.00 | 3.160 | 0.003 | 3.613 | 0.01 | Carl Wilhelm Scheele | 1774 | 12.968 | 171.65 | 239.11 | Halogens | Gas |
17 | 18 | Argon | Ar | 39.95 | 18 | VIIIA | p | 3 | [Ne] 3s2 3p6 | FCC | 5.260 | 71.00 | nan | 96.00 | 188.00 | nan | 0.002 | -11.500 | 0.02 | Sir William Ramsey, Baron Rayleigh | 1894 | 15.760 | 83.81 | 87.30 | Noble gases | Gas |
18 | 19 | Potassium | K | 39.10 | 1 | IA | s | 4 | [Ar] 4s | BCC | 5.230 | 220.00 | 203.00 | 196.00 | 275.00 | 0.820 | 0.890 | 0.501 | 79.00 | Sir Humphrey Davy | 1807 | 4.341 | 336.65 | 1,032.15 | Alkali metals | Solid |
19 | 20 | Calcium | Ca | 40.08 | 2 | IIA | s | 4 | [Ar] 4s2 | FCC | 5.580 | 180.00 | 174.00 | 171.00 | 231.00 | 1.000 | 1.540 | 0.025 | nan | Sir Humphrey Davy | 1808 | 6.113 | 1,115.15 | 1,757.15 | Alkaline earth metals | Solid |
20 | 21 | Scandium | Sc | 44.96 | 3 | IIIB | d | 4 | [Ar] 3d 4s2 | HEX | 3.310 | 160.00 | 144.00 | 148.00 | 215.00 | 1.360 | 2.990 | 0.188 | 15.80 | Lars Nilson | 1879 | 6.561 | 1,814.15 | 3,109.15 | Transition metals | Solid |
21 | 22 | Titanium | Ti | 47.87 | 4 | IVB | d | 4 | [Ar] 3d2 4s2 | HEX | 2.950 | 140.00 | 132.00 | 136.00 | 211.00 | 1.540 | 4.506 | 0.079 | 21.90 | William Gregor | 1791 | 6.828 | 1,943.15 | 3,560.15 | Transition metals | Solid |
22 | 23 | Vanadium | V | 50.94 | 5 | VB | d | 4 | [Ar] 3d3 4s2 | BCC | 3.020 | 135.00 | 122.00 | 134.00 | 207.00 | 1.630 | 6.000 | 0.525 | 30.70 | Nils Sefström | 1830 | 6.746 | 2,183.15 | 3,680.15 | Transition metals | Solid |
23 | 24 | Chromium | Cr | 52.00 | 6 | VIB | d | 4 | [Ar] 3d5 4s | BCC | 2.880 | 140.00 | 119.00 | 122.00 | 206.00 | 1.660 | 7.150 | 0.666 | 93.90 | Louis Vauquelin | 1797 | 6.767 | 2,180.15 | 2,944.15 | Transition metals | Solid |
24 | 25 | Manganese | Mn | 54.94 | 7 | VIIB | d | 4 | [Ar] 3d5 4s2 | CUB | 8.890 | 140.00 | 118.00 | 119.00 | 205.00 | 1.550 | 7.300 | nan | nan | Johann Gahn | 1774 | 7.434 | 1,519.15 | 2,334.15 | Transition metals | Solid |
25 | 26 | Iron | Fe | 55.84 | 8 | VIIIB | d | 4 | [Ar] 3d6 4s2 | BCC | 2.870 | 140.00 | 117.00 | 116.00 | 204.00 | 1.830 | 7.870 | 0.151 | 80.40 | Known to the ancients. | nan | 7.902 | 1,811.15 | 3,134.15 | Transition metals | Solid |
26 | 27 | Cobalt | Co | 58.93 | 9 | VIIIB | d | 4 | [Ar] 3d7 4s2 | HEX | 2.510 | 135.00 | 116.00 | 111.00 | 200.00 | 1.880 | 8.860 | 0.662 | 100.00 | George Brandt | 1739 | 7.881 | 1,768.15 | 3,200.15 | Transition metals | Solid |
27 | 28 | Nickel | Ni | 58.69 | 10 | VIIIB | d | 4 | [Ar] 3d8 4s2 | FCC | 3.520 | 135.00 | 115.00 | 110.00 | 197.00 | 1.910 | 8.900 | 1.156 | 90.90 | Axel Cronstedt | 1751 | 7.640 | 1,728.15 | 3,186.15 | Transition metals | Solid |
28 | 29 | Copper | Cu | 63.55 | 11 | IB | d | 4 | [Ar] 3d10 4s | FCC | 3.610 | 135.00 | 118.00 | 112.00 | 196.00 | 1.900 | 8.960 | 1.235 | 401.00 | Known to the ancients. | nan | 7.726 | 1,357.77 | 2,833.15 | Transition metals | Solid |
29 | 30 | Zinc | Zn | 65.38 | 12 | IIB | d | 4 | [Ar] 3d10 4s2 | HEX | 2.660 | 135.00 | 121.00 | 118.00 | 201.00 | 1.650 | 7.134 | nan | 116.00 | Known to the ancients. | nan | 9.394 | 692.68 | 1,180.15 | Transition metals | Solid |
30 | 31 | Gallium | Ga | 69.72 | 13 | IIIA | p | 4 | [Ar] 3d10 4s2 4p | ORC | 4.510 | 130.00 | 125.00 | 124.00 | 187.00 | 1.810 | 5.910 | 0.430 | 28.10 | Paul Émile Lecoq de Boisbaudran | 1875 | 5.999 | 302.91 | 2,502.15 | Poor metals | Solid |
31 | 32 | Germanium | Ge | 72.63 | 14 | IVA | p | 4 | [Ar] 3d10 4s2 4p2 | DIA | 5.660 | 125.00 | 124.00 | 121.00 | 211.00 | 2.010 | 5.323 | 1.233 | 60.20 | Clemens Winkler | 1886 | 7.899 | 1,211.40 | 3,106.15 | Metalloids | Solid |
32 | 33 | Arsenic | As | 74.92 | 15 | VA | p | 4 | [Ar] 3d10 4s2 4p3 | RHL | 4.130 | 115.00 | 121.00 | 121.00 | 185.00 | 2.180 | 5.750 | 0.804 | nan | Known to the ancients. | nan | 9.789 | 1,090.15 | 889.15 | Metalloids | Solid |
33 | 34 | Selenium | Se | 78.97 | 16 | VIA | p | 4 | [Ar] 3d10 4s2 4p4 | HEX | 4.360 | 115.00 | 117.00 | 116.00 | 190.00 | 2.550 | 4.809 | 2.021 | 0.52 | Jöns Berzelius | 1818 | 9.752 | 493.95 | 958.15 | Nonmetals | Solid |
34 | 35 | Bromine | Br | 79.90 | 17 | VIIA | p | 4 | [Ar] 3d10 4s2 4p5 | ORC | 6.670 | 115.00 | nan | 114.00 | 185.00 | 2.960 | 3.103 | 3.364 | 0.01 | Antoine J. Balard | 1826 | 11.814 | 265.95 | 331.95 | Halogens | Liquid |
35 | 36 | Krypton | Kr | 83.80 | 18 | VIIIA | p | 4 | [Ar] 3d10 4s2 4p6 | FCC | 5.720 | nan | nan | 117.00 | 202.00 | nan | 0.003 | nan | 0.01 | Sir William Ramsey, M.W. Travers | 1898 | 14.000 | 115.78 | 119.73 | Noble gases | Gas |
36 | 37 | Rubidium | Rb | 85.47 | 1 | IA | s | 5 | [Kr] 5s | BCC | 5.590 | 235.00 | 216.00 | 210.00 | 303.00 | 0.820 | 1.530 | 0.486 | 58.20 | R. Bunsen, G. Kirchoff | 1861 | 4.177 | 312.45 | 961.15 | Alkali metals | Solid |
37 | 38 | Strontium | Sr | 87.62 | 2 | IIA | s | 5 | [Kr] 5s2 | FCC | 6.080 | 200.00 | 191.00 | 185.00 | 249.00 | 0.950 | 2.640 | 0.048 | nan | A. Crawford | 1790 | 5.695 | 1,050.15 | 1,650.15 | Alkaline earth metals | Solid |
38 | 39 | Yttrium | Y | 88.91 | 3 | IIIB | d | 5 | [Kr] 4d 5s2 | HEX | 3.650 | 180.00 | 162.00 | 163.00 | 232.00 | 1.220 | 4.470 | 0.307 | nan | Johann Gadolin | 1789 | 6.217 | 1,795.15 | 3,618.15 | Transition metals | Solid |
39 | 40 | Zirconium | Zr | 91.22 | 4 | IVB | d | 5 | [Kr] 4d2 5s2 | HEX | 3.230 | 155.00 | 145.00 | 154.00 | 223.00 | 1.330 | 6.520 | 0.426 | 22.70 | Martin Klaproth | 1789 | 6.634 | 2,127.15 | 4,679.15 | Transition metals | Solid |
40 | 41 | Niobium | Nb | 92.91 | 5 | VB | d | 5 | [Kr] 4d4 5s | BCC | 3.300 | 145.00 | 134.00 | 147.00 | 218.00 | 1.600 | 8.570 | 0.917 | 53.70 | Charles Hatchet | 1801 | 6.759 | 2,750.15 | 5,014.15 | Transition metals | Solid |
41 | 42 | Molybdenum | Mo | 95.95 | 6 | VIB | d | 5 | [Kr] 4d5 5s | BCC | 3.150 | 145.00 | 130.00 | 138.00 | 217.00 | 2.160 | 10.200 | 0.748 | nan | Carl Wilhelm Scheele | 1778 | 7.092 | 2,895.15 | 4,912.15 | Transition metals | Solid |
42 | 43 | Technetium | Tc | 97.91 | 7 | VIIB | d | 5 | [Kr] 4d5 5s2 | HEX | 2.740 | 135.00 | 127.00 | 128.00 | 216.00 | 2.100 | 11.000 | 0.550 | 50.60 | Carlo Perrier, Émillo Segrè | 1937 | 7.119 | 2,430.15 | 4,535.15 | Transition metals | Solid |
43 | 44 | Ruthenium | Ru | 101.07 | 8 | VIIIB | d | 5 | [Kr] 4d7 5s | HEX | 2.700 | 130.00 | 125.00 | 125.00 | 213.00 | 2.200 | 12.100 | 1.050 | 117.00 | Karl Klaus | 1844 | 7.361 | 2,606.15 | 4,420.15 | Transition metals | Solid |
44 | 45 | Rhodium | Rh | 102.91 | 9 | VIIIB | d | 5 | [Kr] 4d8 5s | FCC | 3.800 | 135.00 | 125.00 | 125.00 | 210.00 | 2.280 | 12.400 | 1.137 | 150.00 | William Wollaston | 1803 | 7.459 | 2,236.15 | 3,968.15 | Transition metals | Solid |
45 | 46 | Palladium | Pd | 106.42 | 10 | VIIIB | d | 5 | [Kr] 4d10 | FCC | 3.890 | 140.00 | 128.00 | 120.00 | 210.00 | 2.200 | 12.000 | 0.562 | 71.80 | William Wollaston | 1803 | 8.337 | 1,827.95 | 3,236.15 | Transition metals | Solid |
46 | 47 | Silver | Ag | 107.87 | 11 | IB | d | 5 | [Kr] 4d10 5s | FCC | 4.090 | 160.00 | 134.00 | 128.00 | 211.00 | 1.930 | 10.500 | 1.302 | 429.00 | Known to the ancients. | nan | 7.576 | 1,234.93 | 2,435.15 | Transition metals | Solid |
47 | 48 | Cadmium | Cd | 112.41 | 12 | IIB | d | 5 | [Kr] 4d10 5s2 | HEX | 2.980 | 155.00 | 138.00 | 136.00 | 218.00 | 1.690 | 8.690 | nan | 96.90 | Fredrich Stromeyer | 1817 | 8.994 | 594.22 | 1,040.15 | Transition metals | Solid |
48 | 49 | Indium | In | 114.82 | 13 | IIIA | p | 5 | [Kr] 4d10 5s2 5p | TET | 4.590 | 155.00 | 142.00 | 142.00 | 193.00 | 1.780 | 7.310 | 0.300 | 81.80 | Ferdinand Reich, T. Richter | 1863 | 5.786 | 429.75 | 2,300.15 | Poor metals | Solid |
49 | 50 | Tin | Sn | 118.71 | 14 | IVA | p | 5 | [Kr] 4d10 5s2 5p2 | TET | 5.820 | 145.00 | 142.00 | 140.00 | 217.00 | 1.960 | 7.287 | 1.112 | 66.80 | Known to the ancients. | nan | 7.344 | 505.08 | 2,859.15 | Poor metals | Solid |
50 | 51 | Antimony | Sb | 121.76 | 15 | VA | p | 5 | [Kr] 4d10 5s2 5p3 | RHL | 4.510 | 145.00 | 139.00 | 140.00 | 206.00 | 2.050 | 6.680 | 1.046 | 24.43 | Known to the ancients. | nan | 8.608 | 903.78 | 1,860.15 | Metalloids | Solid |
51 | 52 | Tellurium | Te | 127.60 | 16 | VIA | p | 5 | [Kr] 4d10 5s2 5p4 | HEX | 4.450 | 140.00 | 137.00 | 136.00 | 206.00 | 2.100 | 6.232 | 1.971 | 14.30 | Franz Müller von Reichenstein | 1782 | 9.010 | 722.66 | 1,261.15 | Metalloids | Solid |
52 | 53 | Iodine | I | 126.90 | 17 | VIIA | p | 5 | [Kr] 4d10 5s2 5p5 | ORC | 7.720 | 140.00 | nan | 133.00 | 198.00 | 2.660 | 4.933 | 3.059 | nan | Bernard Courtois | 1811 | 10.451 | 386.85 | 457.55 | Halogens | Solid |
53 | 54 | Xenon | Xe | 131.29 | 18 | VIIIA | p | 5 | [Kr] 4d10 5s2 5p6 | FCC | 6.200 | nan | nan | 131.00 | 216.00 | 2.600 | 0.005 | -0.056 | 0.01 | Sir William Ramsay; M. W. Travers | 1898 | 12.130 | 161.40 | 165.05 | Noble gases | Gas |
54 | 55 | Cesium | Cs | 132.91 | 1 | IA | s | 6 | [Xe] 6s | BCC | 6.050 | 260.00 | 235.00 | 232.00 | 343.00 | 0.790 | 1.873 | 0.472 | 35.90 | Gustov Kirchoff, Robert Bunsen | 1860 | 3.894 | 301.65 | 944.15 | Alkali metals | Solid |
55 | 56 | Barium | Ba | 137.33 | 2 | IIA | s | 6 | [Xe] 6s2 | BCC | 5.020 | 215.00 | 198.00 | 196.00 | 268.00 | 0.890 | 3.620 | 0.145 | nan | Sir Humphrey Davy | 1808 | 5.212 | 1,000.15 | 2,118.15 | Alkaline earth metals | Solid |
56 | 57 | Lanthanum | La | 138.91 | 3 | IIIB | d | 6 | [Xe] 5d 6s2 | HEX | 3.750 | 195.00 | 169.00 | 180.00 | 243.00 | 1.100 | 6.150 | 0.470 | 13.40 | Carl Mosander | 1839 | 5.577 | 1,193.15 | 3,737.15 | Lanthanides | Solid |
57 | 58 | Cerium | Ce | 140.12 | nan | None | f | 6 | [Xe] 4f 5d 6s2 | FCC | 5.160 | 185.00 | nan | 163.00 | 242.00 | 1.120 | 6.770 | 0.650 | 11.30 | W. von Hisinger, J. Berzelius, M. Klaproth | 1803 | 5.539 | 1,072.15 | 3,716.15 | Lanthanides | Solid |
58 | 59 | Praseodymium | Pr | 140.91 | nan | None | f | 6 | [Xe] 4f3 6s2 | HEX | 3.670 | 185.00 | nan | 176.00 | 240.00 | 1.130 | 6.773 | 0.962 | 12.50 | C.F. Aver von Welsbach | 1885 | 5.470 | 1,204.15 | 3,793.15 | Lanthanides | Solid |
59 | 60 | Neodymium | Nd | 144.24 | nan | None | f | 6 | [Xe] 4f4 6s2 | HEX | 3.660 | 185.00 | nan | 174.00 | 239.00 | 1.140 | 7.010 | 1.916 | nan | C.F. Aver von Welsbach | 1925 | 5.525 | 1,289.15 | 3,347.15 | Lanthanides | Solid |
60 | 61 | Promethium | Pm | 144.91 | nan | None | f | 6 | [Xe] 4f5 6s2 | None | nan | 185.00 | nan | 173.00 | 238.00 | nan | 7.260 | nan | 17.90 | J.A. Marinsky, L.E. Glendenin, C.D. Coryell | 1945 | 5.582 | 1,315.15 | nan | Lanthanides | Solid |
61 | 62 | Samarium | Sm | 150.36 | nan | None | f | 6 | [Xe] 4f6 6s2 | RHL | 9.000 | 185.00 | nan | 172.00 | 236.00 | 1.170 | 7.520 | nan | nan | Paul Émile Lecoq de Boisbaudran | 1879 | 5.644 | 1,345.15 | 2,067.15 | Lanthanides | Solid |
62 | 63 | Europium | Eu | 151.96 | nan | None | f | 6 | [Xe] 4f7 6s2 | BCC | 4.610 | 185.00 | nan | 168.00 | 235.00 | nan | 5.240 | 0.864 | 13.90 | Eugène Demarçay | 1901 | 5.670 | 1,095.15 | 1,802.15 | Lanthanides | Solid |
63 | 64 | Gadolinium | Gd | 157.25 | nan | None | f | 6 | [Xe] 4f7 5d 6s2 | HEX | 3.640 | 180.00 | nan | 169.00 | 234.00 | 1.200 | 7.900 | nan | nan | Jean de Marignac | 1880 | 6.150 | 1,586.15 | 3,546.15 | Lanthanides | Solid |
64 | 65 | Terbium | Tb | 158.93 | nan | None | f | 6 | [Xe] 4f9 6s2 | HEX | 3.600 | 175.00 | nan | 168.00 | 233.00 | nan | 8.230 | 1.165 | 11.10 | Carl Mosander | 1843 | 5.864 | 1,632.15 | 3,503.15 | Lanthanides | Solid |
65 | 66 | Dysprosium | Dy | 162.50 | nan | None | f | 6 | [Xe] 4f10 6s2 | HEX | 3.590 | 175.00 | nan | 167.00 | 231.00 | 1.220 | 8.550 | 0.352 | 10.70 | Paul Émile Lecoq de Boisbaudran | 1886 | 5.939 | 1,685.15 | 2,840.15 | Lanthanides | Solid |
66 | 67 | Holmium | Ho | 164.93 | nan | None | f | 6 | [Xe] 4f11 6s2 | HEX | 3.580 | 175.00 | nan | 166.00 | 230.00 | 1.230 | 8.800 | nan | nan | J.L. Soret | 1878 | 6.021 | 1,745.15 | 2,973.15 | Lanthanides | Solid |
67 | 68 | Erbium | Er | 167.26 | nan | None | f | 6 | [Xe] 4f12 6s2 | HEX | 3.560 | 175.00 | nan | 165.00 | 229.00 | 1.240 | 9.070 | nan | nan | Carl Mosander | 1843 | 6.108 | 1,802.15 | 3,141.15 | Lanthanides | Solid |
68 | 69 | Thulium | Tm | 168.93 | nan | None | f | 6 | [Xe] 4f13 6s2 | HEX | 3.540 | 175.00 | nan | 164.00 | 227.00 | 1.250 | 9.321 | 1.029 | nan | Per Theodor Cleve | 1879 | 6.184 | 1,818.15 | 2,223.15 | Lanthanides | Solid |
69 | 70 | Ytterbium | Yb | 173.04 | nan | None | f | 6 | [Xe] 4f14 6s2 | FCC | 5.490 | 175.00 | nan | 170.00 | 226.00 | nan | 6.900 | -0.020 | nan | Jean de Marignac | 1878 | 6.254 | 1,097.15 | 1,469.15 | Lanthanides | Solid |
70 | 71 | Lutetium | Lu | 174.97 | nan | None | f | 6 | [Xe] 4f14 5d 6s2 | HEX | 3.510 | 175.00 | nan | 162.00 | 224.00 | 1.000 | 9.840 | 0.340 | nan | Georges Urbain | 1907 | 5.426 | 1,936.15 | 3,675.15 | Transition metals | Solid |
71 | 72 | Hafnium | Hf | 178.49 | 4 | IVB | d | 6 | [Xe] 4f14 5d2 6s2 | HEX | 3.200 | 155.00 | 144.00 | 152.00 | 223.00 | 1.300 | 13.300 | 0.014 | 23.00 | Dirk Coster, Georg von Hevesy | 1923 | 6.825 | 2,506.15 | 4,873.15 | Transition metals | Solid |
72 | 73 | Tantalum | Ta | 180.95 | 5 | VB | d | 6 | [Xe] 4f14 5d3 6s2 | BCC | 3.310 | 145.00 | 134.00 | 146.00 | 222.00 | 1.500 | 16.400 | 0.322 | 57.50 | Anders Ekeberg | 1802 | 7.550 | 3,290.15 | 5,728.15 | Transition metals | Solid |
73 | 74 | Tungsten | W | 183.84 | 6 | VIB | d | 6 | [Xe] 4f14 5d4 6s2 | BCC | 3.160 | 135.00 | 130.00 | 137.00 | 218.00 | 1.700 | 19.300 | 0.816 | 173.00 | Fausto and Juan José de Elhuyar | 1783 | 7.864 | 3,687.15 | 5,828.15 | Transition metals | Solid |
74 | 75 | Rhenium | Re | 186.21 | 7 | VIIB | d | 6 | [Xe] 4f14 5d5 6s2 | HEX | 2.760 | 135.00 | 128.00 | 131.00 | 216.00 | 1.900 | 20.800 | 0.150 | 48.00 | Walter Noddack, Ida Tacke, Otto Berg | 1925 | 7.834 | 3,458.15 | 5,863.15 | Transition metals | Solid |
75 | 76 | Osmium | Os | 190.23 | 8 | VIIIB | d | 6 | [Xe] 4f14 5d6 6s2 | HEX | 2.740 | 130.00 | 126.00 | 129.00 | 216.00 | 2.200 | 22.587 | 1.100 | nan | Smithson Tenant | 1804 | 8.438 | 3,306.15 | 5,281.15 | Transition metals | Solid |
76 | 77 | Iridium | Ir | 192.22 | 9 | VIIIB | d | 6 | [Xe] 4f14 5d7 6s2 | FCC | 3.840 | 135.00 | 127.00 | 122.00 | 213.00 | 2.200 | 22.562 | 1.564 | 147.00 | S.Tenant, A.F.Fourcory, L.N.Vauquelin, H.V.Collet-Descoltils | 1804 | 8.967 | 2,719.15 | 4,701.15 | Transition metals | Solid |
77 | 78 | Platinum | Pt | 195.08 | 10 | VIIIB | d | 6 | [Xe] 4f14 5d9 6s | FCC | 3.920 | 135.00 | 130.00 | 123.00 | 213.00 | 2.200 | 21.500 | 2.128 | 71.60 | Julius Scaliger | 1735 | 8.959 | 2,041.35 | 4,098.15 | Transition metals | Solid |
78 | 79 | Gold | Au | 196.97 | 11 | IB | d | 6 | [Xe] 4f14 5d10 6s | FCC | 4.080 | 135.00 | 134.00 | 124.00 | 214.00 | 2.400 | 19.300 | 2.309 | 318.00 | Known to the ancients. | nan | 9.226 | 1,337.33 | 3,109.15 | Transition metals | Solid |
79 | 80 | Mercury | Hg | 200.59 | 12 | IIB | d | 6 | [Xe] 4f14 5d10 6s2 | RHL | 2.990 | 150.00 | 139.00 | 133.00 | 223.00 | 1.900 | 13.534 | nan | 8.30 | Known to the ancients. | nan | 10.438 | 234.32 | 629.77 | Transition metals | Liquid |
80 | 81 | Thallium | Tl | 204.38 | 13 | IIIA | p | 6 | [Xe] 4f14 5d10 6s2 6p | HEX | 3.460 | 190.00 | 144.00 | 144.00 | 196.00 | 1.800 | 11.800 | 0.377 | 46.10 | Sir William Crookes | 1861 | 6.108 | 577.15 | 1,746.15 | Poor metals | Solid |
81 | 82 | Lead | Pb | 207.20 | 14 | IVA | p | 6 | [Xe] 4f14 5d10 6s2 6p2 | FCC | 4.950 | 180.00 | 150.00 | 144.00 | 202.00 | 1.800 | 11.300 | 0.357 | 35.30 | Known to the ancients. | nan | 7.417 | 600.61 | 2,022.15 | Poor metals | Solid |
82 | 83 | Bismuth | Bi | 208.98 | 15 | VA | p | 6 | [Xe] 4f14 5d10 6s2 6p3 | RHL | 4.750 | 160.00 | 151.00 | 151.00 | 207.00 | 1.900 | 9.790 | 0.942 | 7.90 | Known to the ancients. | nan | 7.286 | 544.55 | 1,837.15 | Poor metals | Solid |
83 | 84 | Polonium | Po | 209.00 | 16 | VIA | p | 6 | [Xe] 4f14 5d10 6s2 6p4 | SC | 3.350 | 190.00 | nan | 145.00 | 197.00 | 2.000 | 9.200 | 1.900 | nan | Pierre and Marie Curie | 1898 | 8.418 | 527.15 | 1,235.15 | Metalloids | Solid |
84 | 85 | Astatine | At | 210.00 | 17 | VIIA | p | 6 | [Xe] 4f14 5d10 6s2 6p5 | None | nan | nan | nan | 147.00 | 202.00 | 2.200 | 7.000 | 2.800 | nan | D.R.Corson, K.R.MacKenzie, E.Segré | 1940 | 9.318 | 575.15 | nan | Halogens | Solid |
85 | 86 | Radon | Rn | 222.00 | 18 | VIIIA | p | 6 | [Xe] 4f14 5d10 6s2 6p6 | FCC | nan | nan | nan | 142.00 | 220.00 | nan | 0.009 | nan | 0.00 | Fredrich Ernst Dorn | 1898 | 10.748 | 202.15 | 211.45 | Noble gases | Gas |
86 | 87 | Francium | Fr | 223.00 | 1 | IA | s | 7 | [Rn] 7s | BCC | nan | nan | nan | 223.00 | 348.00 | 0.700 | 1.870 | 0.486 | nan | Marguerite Derey | 1939 | 4.073 | 294.15 | nan | Alkali metals | Gas |
87 | 88 | Radium | Ra | 226.00 | 2 | IIA | s | 7 | [Rn] 7s2 | None | nan | 215.00 | nan | 201.00 | 283.00 | 0.900 | 5.000 | 0.100 | nan | Pierre and Marie Curie | 1898 | 5.278 | 969.15 | nan | Alkaline earth metals | Solid |
88 | 89 | Actinium | Ac | 227.00 | 3 | IIIB | d | 7 | [Rn] 6d 7s2 | FCC | 5.310 | 195.00 | nan | 186.00 | 247.00 | 1.100 | 10.000 | 0.350 | nan | André Debierne | 1899 | 5.380 | 1,323.15 | 3,473.15 | Actinides | Solid |
89 | 90 | Thorium | Th | 232.04 | nan | None | f | 7 | [Rn] 6d2 7s2 | FCC | 5.080 | 180.00 | nan | 175.00 | 245.00 | 1.300 | 11.700 | nan | nan | Jöns Berzelius | 1828 | 6.307 | 2,023.15 | 5,058.15 | Actinides | Solid |
90 | 91 | Protactinium | Pa | 231.04 | nan | None | f | 7 | [Rn] 5f2 6d 7s2 | TET | 3.920 | 180.00 | nan | 169.00 | 243.00 | 1.500 | 15.400 | nan | nan | Fredrich Soddy, John Cranston, Otto Hahn, Lise Meitner | 1917 | 5.890 | 1,845.15 | nan | Actinides | Solid |
91 | 92 | Uranium | U | 238.03 | nan | None | f | 7 | [Rn] 5f3 6d 7s2 | ORC | 2.850 | 175.00 | nan | 170.00 | 241.00 | 1.700 | 19.100 | nan | 27.50 | Martin Klaproth | 1789 | 6.194 | 1,408.15 | 4,404.15 | Actinides | Solid |
92 | 93 | Neptunium | Np | 237.00 | nan | None | f | 7 | [Rn] 5f4 6d 7s2 | ORC | 4.720 | 175.00 | nan | 171.00 | 239.00 | 1.300 | 20.200 | nan | nan | E.M. McMillan, P.H. Abelson | 1940 | 6.266 | 917.15 | nan | Actinides | Solid |
93 | 94 | Plutonium | Pu | 244.00 | nan | None | f | 7 | [Rn] 5f6 7s2 | MCL | nan | 175.00 | nan | 172.00 | 243.00 | 1.300 | 19.700 | nan | nan | G.T.Seaborg, J.W.Kennedy, E.M.McMillan, A.C.Wohl | 1940 | 6.026 | 913.15 | 3,501.15 | Actinides | Solid |
94 | 95 | Americium | Am | 243.00 | nan | None | f | 7 | [Rn] 5f7 7s2 | None | nan | 175.00 | nan | 166.00 | 244.00 | nan | 12.000 | nan | nan | G.T.Seaborg, R.A.James, L.O.Morgan, A.Ghiorso | 1945 | 5.974 | 1,449.15 | nan | Actinides | Solid |
95 | 96 | Curium | Cm | 247.00 | nan | None | f | 7 | [Rn] 5f7 6d 7s2 | None | nan | nan | nan | 166.00 | 245.00 | nan | 13.510 | nan | nan | G.T.Seaborg, R.A.James, A.Ghiorso | 1944 | 5.992 | 1,618.15 | nan | Actinides | Solid |
96 | 97 | Berkelium | Bk | 247.00 | nan | None | f | 7 | [Rn] 5f9 7s2 | None | nan | nan | nan | 168.00 | 244.00 | nan | 14.780 | nan | nan | G.T.Seaborg, S.G.Tompson, A.Ghiorso | 1949 | 6.198 | 1,259.15 | nan | Actinides | Solid |
97 | 98 | Californium | Cf | 251.00 | nan | None | f | 7 | [Rn] 5f10 7s2 | None | nan | nan | nan | 168.00 | 245.00 | nan | 15.100 | nan | nan | G.T.Seaborg, S.G.Tompson, A.Ghiorso, K.Street Jr. | 1950 | 6.282 | 1,173.15 | nan | Actinides | Solid |
98 | 99 | Einsteinium | Es | 252.00 | nan | None | f | 7 | [Rn] 5f11 7s2 | None | nan | nan | nan | 165.00 | 245.00 | nan | 8.840 | nan | nan | Argonne, Los Alamos, U of Calif | 1952 | 6.368 | 1,133.15 | nan | Actinides | Solid |
99 | 100 | Fermium | Fm | 257.00 | nan | None | f | 7 | [Rn] 5f12 7s2 | None | nan | nan | nan | 167.00 | 245.00 | nan | 9.700 | nan | nan | Argonne, Los Alamos, U of Calif | 1953 | 6.500 | 1,800.15 | nan | Actinides | Solid |
100 | 101 | Mendelevium | Md | 258.00 | nan | None | f | 7 | [Rn] 5f13 7s2 | None | nan | nan | nan | 173.00 | 246.00 | nan | 10.300 | nan | nan | G.T.Seaborg, S.G.Tompson, A.Ghiorso, K.Street Jr. | 1955 | 6.580 | 1,100.15 | nan | Actinides | Solid |
101 | 102 | Nobelium | No | 259.00 | nan | None | f | 7 | [Rn] 5f14 7s2 | None | nan | nan | nan | 176.00 | 246.00 | nan | 9.900 | nan | nan | Nobel Institute for Physics | 1957 | 6.626 | 1,100.15 | nan | Actinides | Solid |
102 | 103 | Lawrencium | Lr | 262.00 | nan | None | f | 7 | [Rn] 5f14 7s2 7p1 | None | nan | nan | nan | 161.00 | 246.00 | nan | 15.600 | nan | nan | A.Ghiorso, T.Sikkeland, A.E.Larsh, R.M.Latimer | 1961 | 4.960 | 1,900.15 | nan | Transition metals | Solid |
103 | 104 | Rutherfordium | Rf | 267.00 | 4 | IVB | d | 7 | [Rn] 5f14 6d2 7s2 | None | nan | nan | nan | 157.00 | nan | nan | 23.300 | nan | nan | A. Ghiorso, et al | 1969 | 6.020 | nan | nan | Transition metals | Gas |
104 | 105 | Dubnium | Db | 268.00 | 5 | VB | d | 7 | [Rn] 5f14 6d3 7s2 | None | nan | nan | nan | 149.00 | nan | nan | 29.300 | nan | nan | A. Ghiorso, et al | 1970 | 6.800 | nan | nan | Transition metals | Gas |
105 | 106 | Seaborgium | Sg | 271.00 | 6 | VIB | d | 7 | [Rn] 5f14 6d4 7s2 | None | nan | nan | nan | 143.00 | nan | nan | 35.000 | nan | nan | Soviet Nuclear Research/ U. of Cal at Berkeley | 1974 | 7.800 | nan | nan | Transition metals | Gas |
106 | 107 | Bohrium | Bh | 274.00 | 7 | VIIB | d | 7 | [Rn] 5f14 6d5 7s2 | None | nan | nan | nan | 141.00 | nan | nan | 37.100 | nan | nan | Heavy Ion Research Laboratory (HIRL) | 1976 | 7.700 | nan | nan | Transition metals | Gas |
107 | 108 | Hassium | Hs | 269.00 | 8 | VIIIB | d | 7 | [Rn] 5f14 6d6 7s2 | None | nan | nan | nan | 134.00 | nan | nan | 40.700 | nan | nan | Heavy Ion Research Laboratory (HIRL) | 1984 | 7.600 | nan | nan | Transition metals | Gas |
108 | 109 | Meitnerium | Mt | 276.00 | 9 | VIIIB | d | 7 | [Rn] 5f14 6d7 7s2 | None | nan | nan | nan | 129.00 | nan | nan | 37.400 | nan | nan | Heavy Ion Research Laboratory (HIRL) | 1982 | nan | nan | nan | Transition metals | Gas |
109 | 110 | Darmstadtium | Ds | 281.00 | 10 | VIIIB | d | 7 | [Rn] 5f14 6d9 7s1 | None | nan | nan | nan | 128.00 | nan | nan | 34.800 | nan | nan | Heavy Ion Research Laboratory (HIRL) | 1994 | nan | nan | nan | Transition metals | Gas |
110 | 111 | Roentgenium | Rg | 281.00 | 11 | IB | d | 7 | [Rn] 5f14 6d10 7s1 | None | nan | nan | nan | 121.00 | nan | nan | 28.700 | nan | nan | Heavy Ion Research Laboratory (HIRL) | 1994 | nan | nan | nan | Transition metals | Gas |
111 | 112 | Copernicium | Cn | 285.00 | 12 | IIB | d | 7 | [Rn] 5f14 6d10 7s2 | None | nan | nan | nan | 122.00 | nan | nan | 14.000 | nan | nan | GSI Helmholtz Centre for Heavy Ion Research | 1996 | nan | nan | nan | Transition metals | Gas |
112 | 113 | Nihonium | Nh | 286.00 | 13 | IIIA | p | 7 | [Rn] 5f14 6d10 7s2 7p1 | None | nan | nan | nan | 136.00 | nan | nan | 16.000 | nan | nan | RIKEN | 2015 | nan | nan | nan | Poor metals | Gas |
113 | 114 | Flerovium | Fl | 289.00 | 14 | IVA | p | 7 | [Rn] 5f14 6d10 7s2 7p2 | None | nan | nan | nan | 143.00 | nan | nan | 9.928 | nan | nan | Joint Institute for Nuclear Research | 1998 | nan | nan | nan | Poor metals | Gas |
114 | 115 | Moscovium | Mc | 288.00 | 15 | VA | p | 7 | [Rn] 5f14 6d10 7s2 7p3 | None | nan | nan | nan | 162.00 | nan | nan | 13.500 | nan | nan | Joint Institute for Nuclear Research | 2003 | nan | nan | nan | Poor metals | Gas |
115 | 116 | Livermorium | Lv | 293.00 | 16 | VIA | p | 7 | [Rn] 5f14 6d10 7s2 7p4 | None | nan | nan | nan | 175.00 | nan | nan | 12.900 | nan | nan | Lawrence Livermore National Laboratory | 2000 | nan | nan | nan | Poor metals | Gas |
116 | 117 | Tennessine | Ts | 294.00 | 17 | VIIA | p | 7 | [Rn] 5f14 6d10 7s2 7p5 | None | nan | nan | nan | 165.00 | nan | nan | 7.200 | nan | nan | Joint Institute for Nuclear Research/Oak Ridge National Laboratory | 2010 | nan | nan | nan | Halogens | Gas |
117 | 118 | Oganesson | Og | 294.00 | 18 | VIIIA | p | 7 | [Rn] 5f14 6d10 7s2 7p6 | None | nan | nan | nan | 157.00 | nan | nan | 7.000 | 0.056 | nan | Joint Institute for Nuclear Research | 2002 | nan | nan | nan | Noble gases | Gas |
---
author: Stephen J. Mildenhall
title: Elements
categories:
- notes
- science
- mathematics
- llm
- elements
date: '2025-08-10'
date-modified: last-modified
description: 'Properties of the elements in charts and tables.'
draft: false
toc: true
toc-depth: 2
toc-title: 'In this post:'
number-sections: true
number-depth: 2
image: img/banner.png
fig-format: svg
format:
html:
page-layout: full
code-tools: true
code-line-numbers: false
code-overflow: wrap
code-fold: true
code-copy: true
execute:
eval: true
echo: true
error: true
cache: true
cache-type: jupyter
freeze: false
kernel: python3
engine: jupyter
daemon: 1200
jupyter:
jupytext:
text_representation:
extension: .qmd
format_name: quarto
format_version: '1.0'
jupytext_version: 1.16.4
kernelspec:
display_name: Python 3 (ipykernel)
language: python
name: python
---
```{python}
#| echo: true
#| label: code-setup
from elements import fGT, Elements, DensityEstimator, Plotter
# quality graphics
%config InlineBackend.figure_formats = ['svg']
df = Elements.df()
```
{width=50%}
The periodic table is more than a static grid of symbols and numbers. It is a compact map of how the elements behave, interact, and differ. In this post I have assembled charts and tables that bring those patterns into view: crystal structures, densities, melting and boiling points, ionization energies, and more. The aim is to let familiar trends sharpen into focus, highlight anomalies that challenge expectations, and uncover relationships that become clear only when the whole landscape is seen at once.
Some of these features are striking. The rise and fall of ionization energy across each period is sharply defined, with the noble gases forming regular peaks and the alkali metals deep troughs. Mercury stands apart from its neighbors, a liquid metal at room temperature with melting and boiling points far lower than the metals around it. Silver, copper, and gold combine high electrical and thermal conductivities in a way that reflects the [Wiedemann-Franz law](https://en.wikipedia.org/wiki/Wiedemann%E2%80%93Franz_law), showing a clear link between the movement of electrons and the transfer of heat. These examples are not isolated curiosities but part of a connected picture that emerges from the data as a whole.
# Data source
The charts and tables use data from the `Mendeleev` Python package, see @sec-mend. All the data used is shown in @sec-appendix
There is also an [old version](index_old.qmd) using the [Vertex spreadsheet](https://www.vertex42.com/ExcelTemplates/periodic-table-of-elements.html) template data.
# Atomic weight
Atomic weight (more precisely, relative atomic mass) is the weighted average mass of an element’s naturally occurring isotopes, measured relative to one-twelfth of the mass of a carbon-12 atom. It is dimensionless (a ratio), but in practice often written in unified atomic mass units (u), where 1 u ≈ 1.660 539 × 10⁻²⁷ kg. The value reflects both the number of protons and neutrons in the nucleus and the proportions of each isotope found in nature, which means it can vary slightly depending on the source of the element—chlorine, for example, has an atomic weight of about 35.45 because it is roughly 75 % chlorine-35 and 25 % chlorine-37. Some elements, especially those with only one stable isotope (e.g., fluorine-19, beryllium-9), have atomic weights that are essentially fixed, while others with large isotope variations (e.g., lithium, boron) may be given as ranges by the International Union of Pure and Applied Chemistry (IUPAC). For radioactive elements with no stable isotopes, an atomic weight is not fixed and is often based on the most stable isotope or the isotope most commonly used in research.
In all bar charts color each element by its block (s, p, d, f). Paler colors are used for higher periods. Vertical lines separate the blocks.
```{python}
#| echo: true
#| label: fig-2
#| fig-cap: 'Atomic weight.'
plotter = Plotter(df)
plotter.plot('Atomic Weight')
```
# Density {.mt-5}
Density is the mass per unit volume of a substance, typically expressed for elements in kilograms per cubic metre (kg·m⁻³) or grams per cubic centimetre (g·cm⁻³) which are used here. For solids and liquids, density depends on both the mass of individual atoms and how closely they are packed in the crystal or molecular structure. In the periodic table, metals tend to have higher densities than nonmetals because their atoms are both heavier and packed tightly in metallic lattices. Osmium and iridium are the densest known elements under standard conditions (both around 22.6 g·cm⁻³), while lithium, the least dense metal, has a density of just 0.534 g·cm⁻³, making it light enough to float on water. Nonmetals vary widely: solid carbon (graphite) is about 2.27 g·cm⁻³, while gaseous elements like helium have densities in the thousandths of a g·cm⁻³ at room temperature. Density can also change significantly with temperature and pressure; for example, metals expand slightly when heated, lowering their density, while gases follow the ideal gas law and decrease in density more sharply with rising temperature at constant pressure.
See @sec-est-den for estimates of density based on atomic weight, crystal structure and atomic radius.
```{python}
#| echo: true
#| label: fig-23
#| fig-cap: 'Density in g/cm3.'
plotter.plot('Density')
```
# Melting and boiling points {.mt-5}
When plotted across the periodic table, melting and boiling points reveal distinct trends and striking anomalies. Metals in the middle of the transition series, such as tungsten, have exceptionally high melting points (tungsten’s is the highest of all, 3422 °C), while noble gases like helium remain liquefied only near absolute zero (helium’s boiling point is the lowest known, −268.93 °C). Carbon is unusual in that at atmospheric pressure it does not melt but sublimates directly to gas at about 3900 K, giving it one of the highest sublimation points of any element. Gallium is another oddity—its melting point is just 29.76 °C, meaning it can melt in the palm of your hand, yet its boiling point is a much higher 2400 °C, an unusually wide liquid range for a metal. The alkali metals show a steady increase in both melting and boiling points up a group, while the halogens progress from gases to solids with rising boiling points as atomic mass increases. Mercury is a notable liquid metal at room temperature, with a melting point of −38.83 °C and a relatively low boiling point of 356.73 °C. These extremes—whether in refractory metals, cryogenic gases, or unusual phase behavior—mark the boundaries of elemental physical properties.
```{python}
#| echo: true
#| label: fig-13
#| fig-cap: 'Melting point in °K.'
plotter.plot('Melting Point')
```
```{python}
#| echo: true
#| label: fig-15
#| fig-cap: 'Boiling point in °K.'
plotter.plot('Boiling Point')
```
# Ionization energy and electron affinity {.mt-5}
These are complementary measures, but not strict opposites.
* **Ionization energy**, @fig-12, measures how much energy you must put in to remove an electron from a neutral atom.
* **Electron affinity** @fig-24, measures how much energy is released (or absorbed) when you add an electron to a neutral atom.
High ionization energy usually goes with a strongly negative electron affinity (atoms both hold on to electrons tightly and want more—e.g., fluorine, chlorine). Low ionization energy often accompanies small or even positive electron affinity (atoms lose electrons easily and don’t strongly attract extras—e.g., alkali metals, noble gases). The relationship isn’t perfectly mirrored because the processes involve different initial and final states, and subshell structure can skew the trends.
## Ionization energy
Ionization energy is the amount of energy required to remove the most loosely bound electron from a neutral atom in its gaseous state, producing a singly charged positive ion. It is usually expressed in electronvolts (eV, shown here) or kilojoules per mole (kJ·mol⁻¹). When plotted by element, first ionization energy shows a strong periodic trend: it generally increases across a period from left to right, reflecting the growing nuclear charge that holds electrons more tightly, and decreases down a group as outer electrons are farther from the nucleus and more shielded by inner shells. The noble gases sit at the top of each period, with helium having the highest value of all (24.59 eV, 2372 kJ·mol⁻¹), while alkali metals like cesium and francium have the lowest, reflecting how easily they lose their single valence electron. Notable irregularities occur in elements like boron and oxygen, where subshell structure slightly lowers the expected value. These variations reflect the interplay of nuclear charge, electron shielding, and subshell stability.
```{python}
#| echo: true
#| label: fig-12
#| fig-cap: 'Ionization energy in eV.'
plotter.plot('Ionization Energy')
```
## Electron affinity
Electron affinity is the change in energy when a neutral atom in the gaseous state gains an electron to form a negative ion. It is usually expressed in electronvolts (eV, shown here) or kilojoules per mole (kJ·mol⁻¹); by convention, a negative value means energy is released (exothermic), while a positive value means energy is required (endothermic). Across a period from left to right, electron affinity generally becomes more negative as atoms have a stronger tendency to complete their valence shell—halogens are the most extreme, with chlorine releasing about −3.6 eV (−349 kJ·mol⁻¹) when gaining an electron. Noble gases have positive electron affinities because adding an electron would start a new shell, which is energetically unfavorable. Down a group, the trend is less regular than for ionization energy: while increasing atomic size generally makes electron gain less favorable, subshell configurations cause exceptions, such as oxygen’s slightly less negative value than sulfur’s, due to electron–electron repulsion in its compact 2p shell. These variations highlight the balance between nuclear attraction, electron shielding, and subshell stability in determining how readily an atom will accept an extra electron.
```{python}
#| echo: true
#| label: fig-24
#| fig-cap: 'Electron Affinity in kJ/mol.'
plotter.plot("Electron Affinity")
```
# Radii {.mt-5}
Radius is measured in pm, picometers or $10^{-12}$m. An element’s radius can be defined in several different ways, depending on how the atom is bonded or measured, and each definition captures a different aspect of its size.
* **Metallic radius** (@fig-18) is half the distance between the nuclei of two adjacent atoms in a pure metallic crystal; it is most relevant for metals and is typically larger than other definitions because metallic bonding allows atoms to be packed but still delocalized.
* **Covalent radius** (@fig-19) is half the distance between the nuclei of two atoms joined by a single covalent bond; it applies mainly to nonmetals and covalently bonded solids and tends to be smaller than the metallic radius for the same element.
* **Atomic radius** (@fig-20) is often a more general term—sometimes used for the covalent value, sometimes defined from theoretical models like the Bohr radius for hydrogen. @fig-20 shows the metallic radius for metals and the covalent radius otherwise.
* **Van der Waals radius** (@fig-21) measures half the distance between two non-bonded atoms when they are in closest contact (e.g., in neighboring molecules in a crystal or liquid); it is the largest of these radii, since it represents the “personal space” an atom keeps when no bond is present.
When plotted across the periodic table, all radii decrease from left to right within a period due to increasing nuclear charge, and increase down a group as additional electron shells are added. Differences between these four radii reflect the type of interaction being measured—tightly bound in covalent bonds, more spread out in metallic lattices, and most expansive when only weak van der Waals forces act.
```{python}
#| echo: true
#| label: fig-18
#| fig-cap: 'Metallic Radius (pm).'
plotter.plot('Metallic Radius')
```
```{python}
#| echo: true
#| label: fig-19
#| fig-cap: 'Covalent radius (pm).'
plotter.plot('Covalent radius')
```
```{python}
#| echo: true
#| label: fig-20
#| fig-cap: 'Atomic Radius (pm).'
plotter.plot('Atomic Radius')
```
```{python}
#| echo: true
#| label: fig-21
#| fig-cap: 'Van der Waals Radius (pm).'
plotter.plot('Van der Waals Radius')
```
# Electro-negativity {.mt-5}
Electronegativity is a dimensionless measure of how strongly an atom attracts shared electrons in a chemical bond. It is not a directly measurable physical quantity but is derived from other data, most famously by Linus Pauling, whose Pauling scale remains the most widely used. Other scales, like Mulliken or Allred–Rochow, use ionization energy and electron affinity or electrostatic arguments to produce similar trends. On the Pauling scale, values range from about 0.7 (cesium and francium, very weak attraction) to 4.0 (fluorine, the strongest). Across a period from left to right, electronegativity increases due to rising nuclear charge and smaller atomic radii, making the nucleus’s pull on bonding electrons stronger. Down a group, it decreases as added electron shells increase shielding and distance from the nucleus. Noble gases are usually omitted because they rarely form covalent bonds, though some heavier ones can. Extremes include fluorine (highest), oxygen (second highest), and cesium/francium (lowest). Electronegativity is related to both ionization energy and electron affinity—atoms with high values for both tend to have high electronegativity—but because it deals with shared electrons in bonds rather than isolated atoms, the correlation is not exact.
```{python}
#| echo: true
#| label: fig-22
#| fig-cap: 'Electro-negativity (Pauling).'
plotter.plot("Electro-negativity (Pauling)")
```
# Thermal conductivity {.mt-5}
Thermal conductivity is a measure of how efficiently a material transfers heat, usually expressed in watts per meter per kelvin (W·m⁻¹·K⁻¹). For elements, it largely depends on how mobile the electrons or lattice vibrations (phonons) are in carrying thermal energy. Metals, with their “sea” of delocalized electrons, generally have the highest thermal conductivities—silver holds the record at about 429 W·m⁻¹·K⁻¹, closely followed by copper and gold—while nonmetals vary widely depending on structure. Diamond (a form of carbon) is exceptional, with the highest known thermal conductivity of any bulk material (\~2200 W·m⁻¹·K⁻¹) due to its rigid, perfectly ordered covalent lattice and strong covalent bonds. At the other extreme, elements like sulfur, phosphorus, and the noble gases have extremely low conductivities, as they rely solely on phonon transport through relatively weakly bound structures. Trends in the periodic table are less regular than for properties like ionization energy, since conductivity depends not only on bonding type but also on crystal structure, defects, and isotopic composition.
```{python}
#| echo: true
#| label: fig-25
#| fig-cap: 'Thermal Conductivity, W/(m K)'
plotter.plot("Thermal Conductivity")
```
# Electrical resistivity {.mt-5}
Electrical resistivity measures how strongly a material opposes the flow of electric current, with units of ohm-meters (Ω·m). It is the inverse of electrical conductivity, so low resistivity means high conductivity. Among the elements, silver has the lowest resistivity (\~1.59 × 10⁻⁸ Ω·m), followed closely by copper and gold, which is why these metals dominate in electrical wiring and contacts. Most metals have low resistivities because their delocalized conduction electrons can move freely through the metallic lattice. In contrast, nonmetals and metalloids such as sulfur, phosphorus, and silicon have much higher resistivities—ranging from semiconducting values in silicon (\~10⁻³ to 10³ Ω·m, depending on doping) to extremely high, effectively insulating values in materials like sulfur or diamond (>10¹² Ω·m). Temperature strongly affects resistivity: in pure metals it increases with temperature due to greater scattering of electrons by lattice vibrations, while in semiconductors it decreases as more charge carriers become available. Extreme cases include superconductors, which have effectively zero resistivity below their critical temperature. The `mendeleev` package does not include electrical resistivity. @tbl-elect-resist includes some values.
```{python}
#| echo: false
#| label: tbl-elect-resist
#| tbl-cap: 'Electrical resistivity data for selected elements.'
fGT("""
| Element and form | Resistivity $\\rho$ ($\\Omega\\cdot\\text{m}$) |
|:-----------------------|:--------------------------------------------------|
| Ag | $1.59\\times 10^{-8}$ |
| Cu | $1.68\\times 10^{-8}$ |
| Au | $2.44\\times 10^{-8}$ |
| Al | $2.65\\text{–}2.82\\times 10^{-8}$ |
| W | $5.6\\times 10^{-8}$ |
| Fe | $\\sim 1.0\\times 10^{-7}$ |
| Pb | $\\sim 2.2\\times 10^{-7}$ |
| Graphite (basal plane) | $\\sim 10^{-5}$ (anisotropic) |
| Si (intrinsic, 300 K) | $\\sim 10^{3}$ (order of $10^{2}\\text{–}10^{3}$) |
| Ge (intrinsic, 300 K) | $\\sim 0.4\\text{–}0.5$ |
| Diamond | $10^{11}\text{–}10^{18}$ (insulator) |
""")
```
# Phase, type, group, block, electron configuration and crystal structure
```{python}
#| echo: true
#| label: tbl-basic-1
#| tbl-cap: 'Phase, type, electron configuration, group, and crystal structure by element.'
import numpy as np
fGT(df[Elements.base_cols_1].set_index('Name'), table_float_format=lambda x: '' if np.isnan(x) else f'{x:,.2f}')
```
## Details about Type
Type is a broad chemical classification of elements, grouping them by their general physical and chemical properties. It is a way of labeling an element according to where it sits in the periodic table *and* the kind of bonding and reactivity it usually shows.
### Metals
A metal is an element that tends to lose electrons to form positive ions and whose atoms in the solid state are bound by metallic bonding—a lattice of positive atomic cores surrounded by a “sea” of delocalised electrons. This electron cloud gives metals their characteristic properties: high electrical and thermal conductivity, malleability, ductility, and metallic lustre. Most metals have only one to three electrons in their outermost shell, which are relatively weakly bound and easily delocalised; these configurations are common in the s-block (alkali and alkaline earth metals), d-block (transition metals), and lower p-block (post-transition metals). The periodic table position is a strong guide, with metals dominating the left and centre, nonmetals at the upper right, and metalloids along the boundary between them. While outer-shell electron count is a good predictor of metallic behaviour, the decisive factor is the electronic band structure—specifically, whether the valence and conduction bands overlap to allow electrons to move freely. Edge cases exist, such as metalloids that can act metallic under some conditions, or nonmetals like hydrogen that become metallic only at high pressures.
### Metals vs. nonmetals vs. metalloids
* Metals (e.g., iron, copper, aluminum) are generally good conductors of heat and electricity, malleable, and form positive ions (cations) in compounds.
* Nonmetals (e.g., oxygen, sulfur, chlorine) are poor conductors, often brittle in solid form, and tend to form negative ions (anions) or covalent bonds.
* Metalloids (e.g., boron, silicon, arsenic) have properties intermediate between metals and nonmetals, often depending on the chemical environment.
### Specific subcategories
These are based mostly on position in the periodic table.
* Alkali metals — Group 1 (except hydrogen): Li, Na, K, Rb, Cs, Fr. Very reactive metals with one valence electron, low melting points, form strong bases with water.
* Alkaline earth metals — Group 2: Be, Mg, Ca, Sr, Ba, Ra. Reactive metals with two valence electrons, form basic oxides.
* Transition metals — Groups 3–12 in the “d-block” of the periodic table. Variable oxidation states, form coloured compounds, often good catalysts. The “Transition Metal ?” label in your list likely means uncertain classification, perhaps due to inconsistent data source mapping.
* Rare earth metals — The lanthanides (La to Lu) and sometimes Sc and Y. Similar reactivity and electron configurations (4f-block), often used in magnets, alloys, and phosphors.
* Poor metals / Post-transition metals — Metals in the p-block that are softer, lower melting, and poorer conductors than transition metals (e.g., Al, Ga, In, Sn, Tl, Pb, Bi). “Post-transition” is essentially the same concept; the difference in your list may come from merging multiple data sources.
* Noble gases — Group 18: He, Ne, Ar, Kr, Xe, Rn, Og. Chemically inert under most conditions, full valence shell. “Noble Gas ?” means an uncertain flag in the source data.
* Halogens — Group 17: F, Cl, Br, I, At, Ts. Reactive nonmetals with seven valence electrons, form salts with metals.
## Details about Crystal Structure {#sec-crystal}
Most elements crystallize at ambient conditions into a small set of common crystal structures, each defined by how atoms are arranged in three-dimensional space. These arrangements determine packing density, nearest-neighbour distances, and many physical properties such as density, strength, and conductivity. The most relevant for elemental solids are:
* Face-centred cubic (FCC) — Atoms are located at each corner of a cube and at the centres of all cube faces. This structure is close-packed (packing fraction 0.74) and each atom has 12 nearest neighbours. Many ductile metals adopt FCC at room temperature, including aluminium, copper, silver, and gold.
* Body-centred cubic (BCC) — Atoms are located at each cube corner and one atom at the cube’s body centre. This is not close-packed (packing fraction 0.68) and has 8 nearest neighbours. BCC metals such as iron (at room temperature), chromium, and tungsten are typically stronger and harder but less ductile than FCC metals.
* Hexagonal (HEX) — A family of hexagonal lattices, including hexagonal close-packed (HCP) and related variants. Layers of atoms form a hexagonal lattice, often with 12 nearest neighbours. Close-packed forms have a packing fraction of 0.74, but some variants differ in stacking sequence or bonding. Magnesium, titanium, zinc, and cobalt adopt hexagonal forms at ambient conditions.
* Diamond cubic (DIA) — A variation of the FCC lattice where each atom is covalently bonded to four others in a tetrahedral arrangement. This open structure has a low packing fraction (\~0.34) and is characteristic of covalently bonded elements such as carbon (diamond form), silicon, and germanium.
* Orthorhombic (ORC) — A rectangular lattice with three unequal axes at right angles. Found in elements such as sulfur and the halogens (Cl, Br, I), often reflecting molecular or complex bonding arrangements rather than close-packed spheres.
* Rhombohedral (RHL) — A lattice with equal-length axes inclined at the same angle (not 90°). Examples include bismuth, antimony, and α-mercury.
* Tetragonal (TET) — A cube stretched or compressed along one axis. Indium and tin adopt tetragonal forms.
* Cubic (unspecified, CUB) — Cubic symmetry without a specific close-packed or diamond arrangement, often for molecular solids or high-temperature phases.
* Monoclinic (MCL) — A skewed lattice with three unequal axes, two at right angles and the third inclined. Examples include plutonium at ambient temperature.
* Simple cubic (SC) — Atoms occupy only the cube corners, each with 6 nearest neighbours. This has a low packing fraction (0.52) and is rare among elements; polonium is the only one that adopts it at ambient conditions.
These are the principal model structures used in elemental crystallography. Some elements adopt more complex or low-symmetry forms, which generally require experimental lattice constants for accurate property calculations.
```{python}
#| echo: false
#| label: tbl-lattice-info
#| tbl-cap: 'Abbreviations for crystal structure, frequency, and typical elements.'
fGT("""
| Abbrev. | Meaning | Number | Examples |
|:--------|:-----------------------------------------------|-------:|:--------------------|
| HEX | Hexagonal (includes HCP, dhcp, other variants) | 30 | Be, Mg, Ti, Zn |
| FCC | Face-centred cubic | 21 | Al, Cu, Ag, Au |
| BCC | Body-centred cubic | 15 | Li, Fe, W |
| ORC | Orthorhombic | 7 | S, Cl, Br |
| RHL | Rhombohedral | 5 | Sb, Bi, Hg |
| TET | Tetragonal | 4 | In, Sn |
| DIA | Diamond cubic | 3 | C (diamond), Si, Ge |
| CUB | Cubic (unspecified type) | 3 | O, F, Po |
| MCL | Monoclinic | 2 | Se, Pu |
| SC | Simple cubic | 1 | Po |
""")
```
# Melting and boiling points, density, electron affinity, and thermal conductivity
```{python}
#| echo: true
#| label: tbl-basic-2
#| tbl-cap: 'Basic numerical characteristics by element.'
fGT(df[Elements.base_cols_2].set_index('Name'), table_float_format=lambda x: '' if np.isnan(x) else f'{x:,.2f}')
```
## Details about Thermal Conductivity
Thermal conductivity measures how effectively a material conducts heat, with units of watts per metre–kelvin (W·m⁻¹·K⁻¹). In metals, heat is carried primarily by conduction electrons, so good electrical conductors like copper, silver, and aluminum are also excellent thermal conductors. In nonmetals, heat is carried mainly by lattice vibrations (phonons), and conductivity depends on atomic bonding and crystal structure—diamond, for example, has extremely high thermal conductivity due to its strong covalent bonds and stiff lattice. Temperature, impurities, and structural defects can significantly affect a material’s thermal conductivity.
# Discoverers and year discovered
```{python}
#| echo: true
#| label: tbl-discovered
#| tbl-cap: 'Year discovered by element.'
fGT(df[Elements.prov_cols].set_index('Name').drop(index='Tennessine').fillna(0),
formatters={'Year': lambda x: 'ancient' if x==0 else f'{int(x):d}' })
```
# Estimating density from radius, crystal structure, and atomic weight {#sec-est-den}
This estimation method uses basic crystallographic geometry to approximate an element’s bulk density from its atomic weight, metallic radius, and crystal structure (@sec-crystal). The key idea is that, if you know how atoms are arranged in a solid and how big they are, you can calculate the size of the repeating unit cell in the crystal lattice. By combining the unit cell’s volume with the number of atoms it contains and the mass per atom (derived from the atomic weight), you get an estimate of the density. Different crystal structures—face-centred cubic (FCC), body-centred cubic (BCC), hexagonal close-packed (HCP), simple cubic (SC), or diamond cubic—have characteristic relationships between the lattice parameter and the atomic radius, as well as fixed numbers of atoms per unit cell. For close-packed metals, a metallic radius and an idealised $c/a$ ratio are used; for more accurate work, element-specific $c/a$ values can be substituted for non-ideal structures such as zinc and cadmium.
This is a first-order physical model and, while it works reasonably well for close-packed metals, it is less reliable for elements with non-metallic bonding, low-symmetry structures, or significant open space in the crystal lattice. In such cases—noble gases, molecular solids, graphite, or unusual hcp variants—the actual packing fraction can deviate substantially from the ideal, leading to large errors. The method also depends on using the correct type of radius (metallic, covalent, or van der Waals) for the structure in question. When applied carefully with appropriate inputs, it can match tabulated densities within about 5–10 % for many metals, while providing a clear, geometry-based link between microscopic atomic parameters and macroscopic material properties.
```{python}
#| echo: true
#| label: tbl-density-computed
#| tbl-cap: "Estimating density from atomic radius, crystal structure, and atomic weight."
bit = df[['Symbol', 'Atomic Number', 'Atomic Weight', 'Density', 'Crystal Structure', 'Metallic Radius']].copy()
bit.columns = ['Symbol', 'Z', 'Atomic Weight', 'Density', 'Crystal Structure', 'Radius']
bit["Crystal"] = bit["Symbol"].map(DensityEstimator.CRYSTAL).fillna("")
bit["Radius_pm"] = bit["Symbol"].map(
DensityEstimator.RADIUS_PM).astype("Float64")
bit["Density_est"] = [
DensityEstimator._estimate_density_one(sym, aw)
for sym, aw in zip(bit["Symbol"], bit["Atomic Weight"])
]
bit['Error'] = bit.Density_est / bit.Density - 1
fGT(bit.query('Density_est > 0').set_index(['Symbol', 'Z']), year_cols='Z', ratio_cols='Error')
```
```{python}
#| echo: true
#| label: fig-density-computed
#| fig-cap: "Estimating density from atomic radius, crystal structure, and atomic weight: estimated vs. actual. Diagonal line shows actual."
import matplotlib.pyplot as plt
bitm = bit.query("Density_est > 0").copy()
# color map per crystal type
crystal_colors = {
"fcc": "tab:blue",
"bcc": "tab:orange",
"hcp": "tab:green",
"diamond": "tab:red",
"sc": "tab:purple",
"": "gray", # fallback
}
fig, ax = plt.subplots(1, 1, figsize=(5, 5))
# 1:1 reference line
ax.plot(bitm.Density, bitm.Density, lw=0.5, c="k", alpha=0.5)
# plot by crystal type
for struct, group in bitm.groupby("Crystal"):
ax.scatter(
group.Density,
group.Density_est,
marker="o",
s=10,
c=crystal_colors.get(struct, "gray"),
label=struct if struct else "unknown",
alpha=0.8,
)
ax.set(
xlabel="Density (g cm$^{-3}$)",
ylabel="Estimated density (g cm$^{-3}$)",
aspect="equal",
)
ax.legend(title="Crystal structure", markerscale=2, fontsize=8)
for n, r in bit.query('abs(Error) > 0.2').iterrows():
if r.Error > 0:
ax.text(r.Density, r.Density_est + 0.2, r.Symbol, ha='center', va='bottom', fontsize=10)
else:
ax.text(r.Density, r.Density_est - 0.2, r.Symbol, ha='center', va='top', fontsize=10)
```
# Other relationships {.mt-5}
Here are some other relationships between observables.
## Directly from crystal geometry and atomic constants
* Molar volume $V_m$ — the volume occupied by one mole of a substance.
Formula: $V_m = M / \rho$, where $M$ is molar mass in g·mol⁻¹ (mass of one mole of atoms), and $\rho$ is density in g·cm⁻³. Units are usually cm³·mol⁻¹.
* Packing fraction — the fraction of space inside a crystal lattice that is actually filled by atoms.
Formula: $f = V_{\text{atoms}} / V_{\text{cell}}$, where $V_{\text{atoms}}$ is the combined volume of all atoms in the unit cell (from atomic radius), and $V_{\text{cell}}$ is the volume of the unit cell (from lattice parameters). Ideal close-packed values are 0.74 (FCC, HCP), 0.68 (BCC), and 0.52 (simple cubic).
* Nearest-neighbor distance $d_{\text{NN}}$ — the distance between the centers of two atoms that are directly bonded (or touching in the metallic sense).
Calculated from the lattice parameter $a$ and structure: for FCC, $d_{\text{NN}} = a / \sqrt{2}$; for BCC, $d_{\text{NN}} = \sqrt{3}a / 2$; for HCP, $d_{\text{NN}} = a$.
* Number density $n$ — the number of atoms per unit volume of the solid.
Formula: $n = N_A \rho / M$, where $N_A$ is Avogadro’s number (6.022×10²³ mol⁻¹), $\rho$ is density (kg·m⁻³ or g·cm⁻³), and $M$ is molar mass in kg·mol⁻¹ or g·mol⁻¹.
### From simple empirical rules & periodic trends
* Melting point $T_m$ — the temperature at which the solid and liquid phases of a substance are in equilibrium.
While exact values require experiment, trends can be estimated from atomic number, radius, and bonding type: small-radius transition metals tend to have high $T_m$, alkali metals low $T_m$.
* Boiling point $T_b$ — the temperature at which the vapor pressure equals the external pressure (often 1 atm).
Similar empirical modeling to melting points: strong metallic or covalent bonding → high $T_b$; weak van der Waals interactions → low $T_b$.
* Hardness — resistance of a material to deformation, usually given on the Mohs or Vickers scale.
For elements, hardness correlates with bond strength (short bonds, high electronegativity differences, or covalent networks tend to be hardest).
* Electrical conductivity $\sigma$ — the ability of a material to carry electric current, measured in siemens per metre (S·m⁻¹).
For metals, $\sigma$ can be estimated from crystal structure, valence electron count, and resistivity data; low resistivity corresponds to high $\sigma$.
* Thermal conductivity $k$ — the ability of a material to conduct heat, measured in watts per metre per kelvin (W·m⁻¹·K⁻¹).
For metals, $k$ is related to electrical conductivity via the Wiedemann–Franz law: $k / \sigma T \approx L$, where $L$ is the Lorenz number (\~2.45×10⁻⁸ W·Ω·K⁻²).
### Elastic properties
* Bulk modulus $K$ — a measure of resistance to uniform compression, in pascals (Pa).
Roughly scales with bond strength and inversely with atomic volume ($K \propto 1 / V_m$); highest in dense covalent solids and close-packed transition metals.
* Speed of sound $v$ — the velocity of mechanical waves through the solid, in m·s⁻¹.
Formula: $v = \sqrt{K / \rho}$ for longitudinal waves in a simple isotropic model, where $K$ is bulk modulus and $\rho$ is density.
### Derived from periodic table block & radius
* Cohesive energy $E_c$ — the energy required to separate a solid into isolated atoms, usually in eV per atom.
Correlates with bonding type, crystal structure, and atomic radius: covalent networks and dense metals have the highest $E_c$.
* Surface energy $\gamma$ — the energy per unit area to create a new surface, in J·m⁻².
Related to cohesive energy and atomic packing: $\gamma$ tends to be high for strongly bonded, close-packed solids and low for weakly bound molecular solids.
# The `Mendeleev` package {#sec-mend}
`Mendeleev` is a Python package providing a comprehensive source of data with an easy Python interface, see the [Documentation](https://mendeleev.readthedocs.io/en/stable/).
L. M. Mentel, mendeleev - A Python resource for properties of chemical elements, ions and isotopes. , 2014–present. Available at: https://github.com/lmmentel/mendeleev.
```{python}
#| echo: true
#| label: tbl-mend
#| tbl-cap: "Data available from Mendeleev."
from mendeleev.fetch import fetch_table
ptable = fetch_table("elements")
slist = ['H', 'C', 'N', 'O', 'Ne']
fGT(ptable.query('symbol in @slist').set_index('name').T)
```
## Ionization energies
`mendeleev` includes other tables, e.g., isotope, radii, oxidation, phase and scattering. Here is a subset of the ionization energy data.
```{python}
#| echo: true
#| label: tbl-ionization
#| tbl-cap: "Data available from Mendeleev."
from mendeleev.fetch import fetch_ionization_energies
ies_multiple = fetch_ionization_energies(degree=[1, 2, 3, 4, 5])
fGT(ies_multiple.head(18).fillna(0), table_float_format=lambda x: '' if x==0 else f'{x:.2f}')
```
# Appendix: All raw data {#sec-appendix}
@tbl-raw-data shows all the data extracted from `mendeleev` used in this post.
```{python}
#| echo: true
#| label: tbl-raw-data
#| tbl-cap: 'All raw data.'
fGT(df.drop(columns=['_label', '_color']), max_table_inch_width=20)
```