List of elements by atomic properties

Last updated November 17, 2024

This is a list of chemical elements and their atomic properties, ordered by atomic number (Z).

Since valence electrons are not clearly defined for the d-block and f-block elements, there not being a clear point at which further ionisation becomes unprofitable, a purely formal definition as number of electrons in the outermost shell has been used.

Table^[1]

Z	Name	Symbol	Average atomic mass	Electronegativity (Pauling)	First Ionization Energy (eV)	Radii (pm)			Valence electrons
Z	Name	Symbol	Average atomic mass	Electronegativity (Pauling)	First Ionization Energy (eV)	Atomic	Van der Waals	Covalent	Valence electrons
1	Hydrogen	H	1.008^[2]	2.2	13.59844	25	120	38	1
2	Helium	He	4.002602(2)	—	24.58741	31	140	32	2
3	Lithium	Li	6.941(2)	0.98	5.39172	145	182	134	1
4	Beryllium	Be	9.012182(3)	1.57	9.3227	105	—	90	2
5	Boron	B	10.811(7)	2.04	8.29803	85	—	82	3
6	Carbon	C	12.0107(8)	2.55	11.2603	70	170	77	4
7	Nitrogen	N	14.0067(2)	3.04	14.53414	65	155	75	5
8	Oxygen	O	15.9994(3)	3.44	13.61806	60	152	73	6
9	Fluorine	F	18.9984032(5)	3.98	17.42282	50	147	71	7
10	Neon	Ne	20.1797(6)	—	21.5646	38	154	69	8
11	Sodium	Na	22.98976928(2)	0.93	5.13908	180	227	154	1
12	Magnesium	Mg	24.3050(6)	1.31	7.64624	150	173	130	2
13	Aluminium	Al	26.9815386(8)	1.61	5.98577	125	—	118	3
14	Silicon	Si	28.0855(3)	1.9	8.15169	110	210	111	4
15	Phosphorus	P	30.973762(2)	2.19	10.48669	100	180	106	5
16	Sulfur	S	32.065(5)	2.58	10.36001	100	180	102	6
17	Chlorine	Cl	35.453(2)	3.16	12.96764	100	175	99	7
18	Argon	Ar	39.948(1)	—	15.75962	71	188	97	8
19	Potassium	K	39.0983(1)	0.82	4.34066	220	275	196	1
20	Calcium	Ca	40.078(4)	1	6.11316	180	—	174	2
21	Scandium	Sc	44.955912(6)	1.36	6.5615	160	—	144	2
22	Titanium	Ti	47.867(1)	1.54	6.8281	140	—	136	2
23	Vanadium	V	50.9415(1)	1.63	6.7462	135	—	125	2
24	Chromium	Cr	51.9961(6)	1.66	6.7665	140	—	127	1
25	Manganese	Mn	54.938045(5)	1.55	7.43402	140	—	139	2
26	Iron	Fe	55.845(2)	1.83	7.9024	140	—	125	2
27	Cobalt	Co	58.933195(5)	1.91	7.6398	135	163	121	2
28	Nickel	Ni	58.6934(4)	1.88	7.881	135	—	126	2
29	Copper	Cu	63.546(3)	1.9	7.72638	135	140	138	1
30	Zinc	Zn	65.38(2)	1.65	9.3942	135	139	131	2
31	Gallium	Ga	69.723(1)	1.81	5.9993	130	187	126	3
32	Germanium	Ge	72.63(1)	2.01	7.8994	125	—	122	4
33	Arsenic	As	74.92160(2)	2.18	9.7886	115	185	119	5
34	Selenium	Se	78.96(3)	2.55	9.75238	115	190	116	6
35	Bromine	Br	79.904(1)	2.96	11.81381	115	185	114	7
36	Krypton	Kr	83.798(2)	3	13.99961	88	202	110	8
37	Rubidium	Rb	85.4678(3)	0.82	4.17713	235	—	211	1
38	Strontium	Sr	87.62(1)	0.95	5.6949	200	—	192	2
39	Yttrium	Y	88.90585(2)	1.22	6.2171	180	—	162	2
40	Zirconium	Zr	91.224(2)	1.33	6.6339	155	—	148	2
41	Niobium	Nb	92.90638(2)	1.6	6.75885	145	—	137	1
42	Molybdenum	Mo	95.96(2)	2.16	7.09243	145	—	145	1
43	Technetium	Tc	[98]	1.9	7.28	135	—	156	1
44	Ruthenium	Ru	101.07(2)	2.2	7.3605	130	—	126	1
45	Rhodium	Rh	102.90550(2)	2.28	7.4589	135	—	135	1
46	Palladium	Pd	106.42(1)	2.2	8.3369	140	163	131
47	Silver	Ag	107.8682(2)	1.93	7.5762	160	172	153	1
48	Cadmium	Cd	112.411(8)	1.69	8.9938	155	158	148	2
49	Indium	In	114.818(3)	1.78	5.78636	155	193	144	3
50	Tin	Sn	118.710(7)	1.96	7.3439	145	217	141	4
51	Antimony	Sb	121.760(1)	2.05	8.6084	145	—	138	5
52	Tellurium	Te	127.60(3)	2.1	9.0096	140	206	135	6
53	Iodine	I	126.90447(3)	2.66	10.45126	140	198	133	7
54	Xenon	Xe	131.293(6)	2.6	12.1298	108	216	130	8
55	Caesium	Cs	132.9054519(2)	0.79	3.8939	260	—	225	1
56	Barium	Ba	137.327(7)	0.89	5.2117	215	—	198	2
57	Lanthanum	La	138.90547(7)	1.1	5.5769	195	—	169	2
58	Cerium	Ce	140.116(1)	1.12	5.5387	185	—	—	2
59	Praseodymium	Pr	140.90765(2)	1.13	5.473	185	—	—	2
60	Neodymium	Nd	144.242(3)	1.14	5.525	185	—	—	2
61	Promethium	Pm	[145]	—	5.582	185	—	—	2
62	Samarium	Sm	150.36(2)	1.17	5.6436	185	—	—	2
63	Europium	Eu	151.964(1)	—	5.6704	185	—	—	2
64	Gadolinium	Gd	157.25(3)	1.2	6.1501	180	—	—	2
65	Terbium	Tb	158.92535(2)	—	5.8638	175	—	—	2
66	Dysprosium	Dy	162.500(1)	1.22	5.9389	175	—	—	2
67	Holmium	Ho	164.93032(2)	1.23	6.0215	175	—	—	2
68	Erbium	Er	167.259(3)	1.24	6.1077	175	—	—	2
69	Thulium	Tm	168.93421(2)	1.25	6.18431	175	—	—	2
70	Ytterbium	Yb	173.054(5)	—	6.25416	175	—	—	2
71	Lutetium	Lu	174.9668(1)	1.27	5.4259	175	—	160	2
72	Hafnium	Hf	178.49(2)	1.3	6.82507	155	—	150	2
73	Tantalum	Ta	180.94788(2)	1.5	7.5496	145	—	138	2
74	Tungsten	W	183.84(1)	2.36	7.864	135	—	146	2
75	Rhenium	Re	186.207(1)	1.9	7.8335	135	—	159	2
76	Osmium	Os	190.23(3)	2.2	8.4382	130	—	128	2
77	Iridium	Ir	192.217(3)	2.2	8.967	135	—	137	2
78	Platinum	Pt	195.084(9)	2.28	8.9587	135	175	128	1
79	Gold	Au	196.966569(4)	2.54	9.2255	135	166	144	1
80	Mercury	Hg	200.59(2)	2	10.4375	150	155	149	2
81	Thallium	Tl	204.3833(2)	1.62	6.1082	190	196	148	3
82	Lead	Pb	207.2(1)	2.33	7.41666	180	202	147	4
83	Bismuth	Bi	208.98040(1)	2.02	7.2856	160	—	146	5
84	Polonium	Po	[209]	2	8.417	190	—	—	6
85	Astatine	At	[210]	2.2		—	—	—	7
86	Radon	Rn	[222]	—	10.7485	120	—	145	8
87	Francium	Fr	[223]	0.7	4.0727	—	—	—	1
88	Radium	Ra	[226]	0.9	5.2784	215	—	—	2
89	Actinium	Ac	[227]	1.1	5.17	195	—	—	2
90	Thorium	Th	232.03806(2)	1.3	6.3067	180	—	—	2
91	Protactinium	Pa	231.03588(2)	1.5	5.89	180	—	—	2
92	Uranium	U	238.02891(3)	1.38	6.19405	175	186	—	2
93	Neptunium	Np	[237]	1.36	6.2657	175	—	—	2
94	Plutonium	Pu	[244]	1.28	6.0262	175	—	—	2
95	Americium	Am	[243]	1.3	5.9738	175	—	—	2
96	Curium	Cm	[247]	1.3	5.9915				2
97	Berkelium	Bk	[247]	1.3	6.1979				2
98	Californium	Cf	[251]	1.3	6.2817				2
99	Einsteinium	Es	[252]	1.3	6.42				2
100	Fermium	Fm	[257]	1.3	6.5				2
101	Mendelevium	Md	[258]	1.3	6.58				2
102	Nobelium	No	[259]	1.3	6.65				2
103	Lawrencium	Lr	[266]	1.3	4.9				3
104	Rutherfordium	Rf	[267]		6				2
105	Dubnium	Db	[268]						2
106	Seaborgium	Sg	[269]						2
107	Bohrium	Bh	[270]						2
108	Hassium	Hs	[277]						2
109	Meitnerium	Mt	[278]
110	Darmstadtium	Ds	[281]
111	Roentgenium	Rg	[282]
112	Copernicium	Cn	[285]
113	Nihonium	Nh	[286]
114	Flerovium	Fl	[289]
115	Moscovium	Mc	[290]
116	Livermorium	Lv	[293]
117	Tennessine	Ts	[294]
118	Oganesson	Og	[294]

[*] a few atomic radii are calculated, not experimental

[—] a long dash marks properties for which there is no data available

[ ] a blank marks properties for which no data has been found

Related Research Articles

The alkali metals consist of the chemical elements lithium (Li), sodium (Na), potassium (K), rubidium (Rb), caesium (Cs), and francium (Fr). Together with hydrogen they constitute group 1, which lies in the s-block of the periodic table. All alkali metals have their outermost electron in an s-orbital: this shared electron configuration results in their having very similar characteristic properties. Indeed, the alkali metals provide the best example of group trends in properties in the periodic table, with elements exhibiting well-characterised homologous behaviour. This family of elements is also known as the lithium family after its leading element.

The atomic number or nuclear charge number of a chemical element is the charge number of its atomic nucleus. For ordinary nuclei composed of protons and neutrons, this is equal to the proton number (n_p) or the number of protons found in the nucleus of every atom of that element. The atomic number can be used to uniquely identify ordinary chemical elements. In an ordinary uncharged atom, the atomic number is also equal to the number of electrons.

Atoms are the basic particles of the chemical elements. An atom consists of a nucleus of protons and generally neutrons, surrounded by an electromagnetically bound swarm of electrons. The chemical elements are distinguished from each other by the number of protons that are in their atoms. For example, any atom that contains 11 protons is sodium, and any atom that contains 29 protons is copper. Atoms with the same number of protons but a different number of neutrons are called isotopes of the same element.

In quantum mechanics, an atomic orbital is a function describing the location and wave-like behavior of an electron in an atom. This function describes an electron's charge distribution around the atom's nucleus, and can be used to calculate the probability of finding an electron in a specific region around the nucleus.

Electronegativity, symbolized as χ, is the tendency for an atom of a given chemical element to attract shared electrons when forming a chemical bond. An atom's electronegativity is affected by both its atomic number and the distance at which its valence electrons reside from the charged nucleus. The higher the associated electronegativity, the more an atom or a substituent group attracts electrons. Electronegativity serves as a simple way to quantitatively estimate the bond energy, and the sign and magnitude of a bond's chemical polarity, which characterizes a bond along the continuous scale from covalent to ionic bonding. The loosely defined term electropositivity is the opposite of electronegativity: it characterizes an element's tendency to donate valence electrons.

The periodic table, also known as the periodic table of the elements, is an ordered arrangement of the chemical elements into rows ("periods") and columns ("groups"). It is an icon of chemistry and is widely used in physics and other sciences. It is a depiction of the periodic law, which states that when the elements are arranged in order of their atomic numbers an approximate recurrence of their properties is evident. The table is divided into four roughly rectangular areas called blocks. Elements in the same group tend to show similar chemical characteristics.

In chemistry, a transition metal is a chemical element in the d-block of the periodic table, though the elements of group 12 are sometimes excluded. The lanthanide and actinide elements are called inner transition metals and are sometimes considered to be transition metals as well.

The atomic radius of a chemical element is a measure of the size of its atom, usually the mean or typical distance from the center of the nucleus to the outermost isolated electron. Since the boundary is not a well-defined physical entity, there are various non-equivalent definitions of atomic radius. Four widely used definitions of atomic radius are: Van der Waals radius, ionic radius, metallic radius and covalent radius. Typically, because of the difficulty to isolate atoms in order to measure their radii separately, atomic radius is measured in a chemically bonded state; however theoretical calculations are simpler when considering atoms in isolation. The dependencies on environment, probe, and state lead to a multiplicity of definitions.

In physics and chemistry, ionization energy (IE) is the minimum energy required to remove the most loosely bound electron of an isolated gaseous atom, positive ion, or molecule. The first ionization energy is quantitatively expressed as

In atomic physics and quantum chemistry, the electron configuration is the distribution of electrons of an atom or molecule in atomic or molecular orbitals. For example, the electron configuration of the neon atom is 1s² 2s² 2p⁶, meaning that the 1s, 2s, and 2p subshells are occupied by two, two, and six electrons, respectively.

Moscovium is a synthetic chemical element; it has symbol Mc and atomic number 115. It was first synthesized in 2003 by a joint team of Russian and American scientists at the Joint Institute for Nuclear Research (JINR) in Dubna, Russia. In December 2015, it was recognized as one of four new elements by the Joint Working Party of international scientific bodies IUPAC and IUPAP. On 28 November 2016, it was officially named after the Moscow Oblast, in which the JINR is situated.

Tennessine is a synthetic chemical element; it has symbol Ts and atomic number 117. It has the second-highest atomic number and joint-highest atomic mass of all known elements and is the penultimate element of the 7th period of the periodic table. It is named after the U.S. state of Tennessee, where key research institutions involved in its discovery are located.

A period on the periodic table is a row of chemical elements. All elements in a row have the same number of electron shells. Each next element in a period has one more proton and is less metallic than its predecessor. Arranged this way, elements in the same group (column) have similar chemical and physical properties, reflecting the periodic law. For example, the halogens lie in the second-to-last group and share similar properties, such as high reactivity and the tendency to gain one electron to arrive at a noble-gas electronic configuration. As of 2022, a total of 118 elements have been discovered and confirmed.

A period 7 element is one of the chemical elements in the seventh row of the periodic table of the chemical elements. The periodic table is laid out in rows to illustrate recurring (periodic) trends in the chemical behavior of the elements as their atomic number increases: a new row is begun when chemical behavior begins to repeat, meaning that elements with similar behavior fall into the same vertical columns. The seventh period contains 32 elements, tied for the most with period 6, beginning with francium and ending with oganesson, the heaviest element currently discovered. As a rule, period 7 elements fill their 7s shells first, then their 5f, 6d, and 7p shells in that order, but there are exceptions, such as uranium.

In atomic physics and quantum chemistry, the Aufbau principle, also called the Aufbau rule, states that in the ground state of an atom or ion, electrons first fill subshells of the lowest available energy, then fill subshells of higher energy. For example, the 1s subshell is filled before the 2s subshell is occupied. In this way, the electrons of an atom or ion form the most stable electron configuration possible. An example is the configuration 1s² 2s² 2p⁶ 3s² 3p³ for the phosphorus atom, meaning that the 1s subshell has 2 electrons, the 2s subshell has 2 electrons, the 2p subshell has 6 electrons, and so on.

The lanthanide contraction is the greater-than-expected decrease in atomic radii and ionic radii of the elements in the lanthanide series, from left to right. It is caused by the poor shielding effect of nuclear charge by the 4f electrons along with the expected periodic trend of increasing electronegativity and nuclear charge on moving from left to right. About 10% of the lanthanide contraction has been attributed to relativistic effects.

In chemistry, periodic trends are specific patterns present in the periodic table that illustrate different aspects of certain elements when grouped by period and/or group. They were discovered by the Russian chemist Dmitri Mendeleev in 1863. Major periodic trends include atomic radius, ionization energy, electron affinity, electronegativity, valency and metallic character. These trends exist because of the similar electron configurations of the elements within their respective groups or periods; they reflect the periodic nature of the elements. These trends give a qualitative assessment of the properties of each element.

Periodic systems of molecules are charts of molecules similar to the periodic table of the elements. Construction of such charts was initiated in the early 20th century and is still ongoing.

A block of the periodic table is a set of elements unified by the atomic orbitals their valence electrons or vacancies lie in. The term seems to have been first used by Charles Janet. Each block is named after its characteristic orbital: s-block, p-block, d-block, f-block and g-block.

References

↑ PubChem. "Periodic Table of Elements". pubchem.ncbi.nlm.nih.gov. Retrieved 2024-05-31.
↑

This page is based on this Wikipedia article
Text is available under the CC BY-SA 4.0 license; additional terms may apply.
Images, videos and audio are available under their respective licenses.

[1] PubChem. "Periodic Table of Elements". pubchem.ncbi.nlm.nih.gov. Retrieved 2024-05-31.

[2] ↑

[1]

[2]

List of elements by atomic properties

Table [1]

Related Research Articles

References

Table^[1]