Electron affinity (data page)

This page deals with the electron affinity as a property of isolated atoms or molecules (i.e. in the gas phase). Solid state electron affinities are not listed here.

Elements

Electron affinity can be defined in two equivalent ways. First, as the energy that is released by adding an electron to an isolated gaseous atom. The second (reverse) definition is that electron affinity is the energy required to remove an electron from a singly charged gaseous negative ion. The latter can be regarded as the ionization energy of the –1 ion or the zeroth ionization energy.[1] Either convention can be used.[2]

Negative electron affinities can be used in those cases where electron capture requires energy, i.e. when capture can occur only if the impinging electron has a kinetic energy large enough to excite a resonance of the atom-plus-electron system. Conversely electron removal from the anion formed in this way releases energy, which is carried out by the freed electron as kinetic energy. Negative ions formed in these cases are always unstable. They may have lifetimes of the order of microseconds to milliseconds, and invariably autodetach after some time.

Z	Element	Name	Electron affinity (eV)	Electron affinity (kJ/mol)	References
1	¹H	Hydrogen	0.754 195(19)	72.769(2)	[3]
1	²H	Deuterium	0.754 67(4)	72.814(4)	[4]
2	He	Helium	−0.5(2)	−48(20)	est.[5]
3	Li	Lithium	0.618 049(22)	59.632 6(21)	[6]
4	Be	Beryllium	−0.5(2)	−48(20)	est.[5]
5	B	Boron	0.279 723(25)	26.989(3)	[7]
6	¹²C	Carbon	1.262 122 6(11)	121.776 3(1)	[8]
6	¹³C	Carbon	1.262 113 6(12)	121.775 5(2)	[8]
7	N	Nitrogen	−0.07	−6.8	[5]
8	¹⁶O	Oxygen	1.461 112 97(9)	140.975 970(9)	[9]
8	¹⁷O	Oxygen	1.461 108(4)	140.975 5(3)	[10]
8	¹⁸O	Oxygen	1.461 105(3)	140.975 2(3)	[10]
9	F	Fluorine	3.401 189 8(24)	328.164 9(3)	[11][12]
10	Ne	Neon	−1.2(2)	−116(19)	est.[5]
11	Na	Sodium	0.547 926(25)	52.867(3)	[13]
12	Mg	Magnesium	−0.4(2)	−40(19)	est.[5]
13	Al	Aluminium	0.432 83(5)	41.762(5)	[14]
14	Si	Silicon	1.389 521 2(8)	134.068 4(1)	[15]
15	P	Phosphorus	0.746 609(11)	72.037(1)	[16]
16	³²S	Sulfur	2.077 104 2(6)	200.410 1(1)	[15]
16	³⁴S	Sulfur	2.077 104 5(12)	200.410 1(2)	[17]
17	Cl	Chlorine	3.612 725(28)	348.575(3)	[18]
18	Ar	Argon	−1.0(2)	−96(20)	est.[5]
19	K	Potassium	0.501 459(13)	48.383(2)	[19]
20	Ca	Calcium	0.024 55(10)	2.37(1)	[20]
21	Sc	Scandium	0.179 380(23)	17.307 6(22)	[21]
22	Ti	Titanium	0.075 54(5)	7.289(5)	[22]
23	V	Vanadium	0.527 66(20)	50.911(20)	[23]
24	Cr	Chromium	0.675 928(27)	65.217 2(26)	[21]
25	Mn	Manganese	−0.5(2)	−50(19)	est.[5]
26	Fe	Iron	0.153 236(35)	14.785(4)	[24]
27	Co	Cobalt	0.662 255(47)	63.897 9(45)	[25]
28	Ni	Nickel	1.157 16(12)	111.65(2)	[26]
29	Cu	Copper	1.235 78(4)	119.235(4)	[27]
30	Zn	Zinc	−0.6(2)	−58(20)	est.[5]
31	Ga	Gallium	0.301 166(15)	29.058 1(15)	[28]
32	Ge	Germanium	1.232 676 4(13)	118.935 2(2)	[29]
33	As	Arsenic	0.804 8(2)	77.65(2)	[30]
34	Se	Selenium	2.020 604 7(12)	194.958 7(2)	[31]
35	Br	Bromine	3.363 588(3)	324.536 9(3)	[11]
36	Kr	Krypton	−1.0(2)	−96(20)	est.[5]
37	Rb	Rubidium	0.485 916(21)	46.884(3)	[32]
38	Sr	Strontium	0.052 06(6)	5.023(6)	[33]
39	Y	Yttrium	0.311 29(22)	30.035(21)	[21]
40	Zr	Zirconium	0.433 28(9)	41.806(9)	[34]
41	Nb	Niobium	0.917 40(7)	88.516(7)	[35]
42	Mo	Molybdenum	0.747 23(8)	72.097(8)	[21]
43	Tc	Technetium	0.55(20)	53(20)	est.[36]
44	Ru	Ruthenium	1.046 27(2)	100.950(3)	[21]
45	Rh	Rhodium	1.142 89(20)	110.27(2)	[26]
46	Pd	Palladium	0.562 14(12)	54.24(2)	[26]
47	Ag	Silver	1.304 47(3)	125.862(3)	[27]
48	Cd	Cadmium	−0.7(2)	−68(20)	est.[5]
49	In	Indium	0.383 92(6)	37.043(6)	[37]
50	Sn	Tin	1.112 070(2)	107.298 4(3)	[38]
51	Sb	Antimony	1.047 401(19)	101.059(2)	[39]
52	Te	Tellurium	1.970 875(7)	190.161(1)	[40]
53	¹²⁷I	Iodine	3.059 046 5(37)	295.153 1(4)	[41]
53	¹²⁸I	Iodine	3.059 052(38)	295.154(4)	[42]
54	Xe	Xenon	−0.8(2)	−77(20)	est.[5]
55	Cs	Caesium	0.4715983(38)	45.5023(4)	[43]
56	Ba	Barium	0.144 62(6)	13.954(6)	[44]
57	La	Lanthanum	0.557 546(20)	53.795(2)	[45]
58	Ce	Cerium	0.600 160(27)	57.906 7(26)	[46]
59	Pr	Praseodymium	0.109 23(46)	10.539(45)	[47]
60	Nd	Neodymium	0.097 49(33)	9.406(32)	[47]
61	Pm	Promethium	0.129	12.45	[48]
62	Sm	Samarium	0.162	15.63	[48]
63	Eu	Europium	0.116(13)	11.2(13)	[49]
64	Gd	Gadolinium	0.212(30)	20.5(29)	[21]
65	Tb	Terbium	0.131 31(80)	12.670(77)	[47]
66	Dy	Dysprosium	0.015(3)	1.45(30)	[50]
67	Ho	Holmium	0.338	32.61	[48]
68	Er	Erbium	0.312	30.10	[48]
69	Tm	Thulium	1.029(22)	99(3)	[51]
70	Yb	Ytterbium	−0.02	−1.93	est.[36]
71	Lu	Lutetium	0.238 8(7)	23.04(7)	[52]
72	Hf	Hafnium	0.178 0(7)	17.18(7)	[53]
73	Ta	Tantalum	0.328 859(23)	31.730 1(22)	[21]
74	W	Tungsten	0.816 26(8)	78.76(1)	[54]
75	Re	Rhenium	0.060 396(64)	5.827 3(62)	[55]
76	Os	Osmium	1.077 661(24)	103.978 5(24)	[21]
77	Ir	Iridium	1.564 057(12)	150.908 6(12)	[56]
78	Pt	Platinum	2.125 10(5)	205.041(5)	[57]
79	Au	Gold	2.308 610(25)	222.747(3)	[58]
80	Hg	Mercury	−0.5(2)	−48(20)	est.[5]
81	Tl	Thallium	0.320 053(19)	30.880 4(19)	[59]
82	Pb	Lead	0.356 721(2)	34.418 3(3)	[60]
83	Bi	Bismuth	0.942 362(13)	90.924(2)	[61]
84	Po	Polonium	1.40(7)	136(7)	calc.[62]
85	At	Astatine	2.415 78(7)	233.087(8)	[63]
86	Rn	Radon	−0.7(2)	−68(20)	est.[5]
87	Fr	Francium	0.486	46.89	est.[64][36]
88	Ra	Radium	0.10	9.648 5	est.[65][36]
89	Ac	Actinium	0.35	33.77	est.[36]
90	Th	Thorium	0.607 69(6)	58.633(6)	[66]
91	Pa	Protactinium	0.55	53.03	est.[67]
92	U	Uranium	0.314 97(9)	30.390(9)	[68]
93	Np	Neptunium	0.48	45.85	est.[67]
94	Pu	Plutonium	−0.50	−48.33	est.[67]
95	Am	Americium	0.10	9.93	est.[67]
96	Cm	Curium	0.28	27.17	est.[67]
97	Bk	Berkelium	−1.72	−165.24	est.[67]
98	Cf	Californium	−1.01	−97.31	est.[67]
99	Es	Einsteinium	−0.30	−28.60	est.[67]
100	Fm	Fermium	0.35	33.96	est.[67]
101	Md	Mendelevium	0.98	93.91	est.[67]
102	No	Nobelium	−2.33	−223.22	est.[67]
103	Lr	Lawrencium	−0.31	−30.04	est.[67]
111	Rg	Roentgenium	1.565	151.0	calc.[69]
113	Nh	Nihonium	0.69	66.6	calc.[70]
115	Mc	Moscovium	0.366	35.3	calc.[70]
116	Lv	Livermorium	0.776	74.9	calc.[70]
117	Ts	Tennessine	1.719	165.9	calc.[70]
118	Og	Oganesson	0.080(6)	7.72(58)	calc.[71]
119	Uue	Ununennium	0.662	63.87	calc.[64]
120	Ubn	Unbinilium	0.021	2.03	calc.[72]
121	Ubu	Unbiunium	0.57	55	calc.[36]

Molecules

The electron affinities E_ea of some molecules are given in the table below, from the lightest to the heaviest. Many more have been listed by Rienstra-Kiracofe et al. (2002). The electron affinities of the radicals OH and SH are the most precisely known of all molecular electron affinities.

Molecule	Name	E_ea (eV)	E_ea (kJ/mol)	References
Diatomics
¹⁶OH	Hydroxyl	1.827 6488(11)	176.3413(2)	Goldfarb et al. (2005)
¹⁶OD		1.825 53(4)	176.137(5)	Schulz et al. (1982)
C₂	Dicarbon	3.269(6)	315.4(6)	Ervin & Lineberger (1991)
BO	Boron oxide	2.508(8)	242.0(8)	Wenthold et al. (1997)
NO	Nitric oxide	0.026(5)	2.5(5)	Travers, Cowles & Ellison (1989)
O₂	Dioxygen	0.450(2)	43.42(20)	Schiedt & Weinkauf (1995)
³²SH	Sulfhydryl	2.314 7283(17)	223.3373(2)	Chaibi et al. (2006)
F₂	Difluorine	3.08(10)	297(10)	Janousek & Brauman (1979)
Cl₂	Dichlorine	2.35(8)	227(8)	Janousek & Brauman (1979)
Br₂	Dibromine	2.53(8)	244(8)	Janousek & Brauman (1979)
I₂	Diiodine	2.524(5)	243.5(5)	Zanni et al. (1997)
IBr	Iodine bromide	2.512(3)	242.4(4)	Sheps, Miller & Lineberger (2009)
LiCl	Lithium chloride	0.593(10)	57.2(10)	Miller et al. (1986)
FeO	Iron(II) oxide	1.4950(5)	144.25(6)	Kim, Weichman & Neumark (2015)
CN	Cyano radical	3.862(4)		[73]
Triatomics
NO₂	Nitrogen dioxide	2.273(5)	219.3(5)	Ervin, Ho & Lineberger (1988)
O₃	Ozone	2.1028(25)	202.89(25)	Novick et al. (1979)
SO₂	Sulfur dioxide	1.107(8)	106.8(8)	Nimlos & Ellison (1986)
Larger polyatomics
CH₂CHO	Vinyloxy	1.8248(+2-6)	176.07(+3-7)	Rienstra-Kiracofe et al. (2002) after Mead et al. (1984)
C₆H₆	Benzene	−0.70(14)	−68(14)	Ruoff et al. (1995)
C₆H₄O₂	p-Benzoquinone	1.860(5)	179.5(6)	Schiedt & Weinkauf (1999)
BF₃	Boron trifluoride	2.65(10)	256(10)	Page & Goode (1969)
HNO₃	Nitric acid	0.57(15)	55(14)	Janousek & Brauman (1979)
CH₃NO₂	Nitromethane	0.172(6)	16.6(6)	Adams et al. (2009)
POCl₃	Phosphoryl chloride	1.41(20)	136(20)	Mathur et al. (1976)
SF₆	Sulfur hexafluoride	1.03(5)	99.4(49)	Troe, Miller & Viggiano (2012)
C₂(CN)₄	Tetracyanoethylene	3.17(20)	306(20)	Chowdhury & Kebarle (1986)
WF₆	Tungsten hexafluoride	3.5(1)	338(10)	George & Beauchamp (1979)
UF₆	Uranium hexafluoride	5.06(20)	488(20)	NIST chemistry webbook after Borshchevskii et al. (1988)
C₆₀	Buckminsterfullerene	2.6835(6)	258.92(6)	Huang et al. (2014)

Second and third electron affinity

Z	Element	Name	Electron affinity (eV)	Electron affinity (kJ/mol)	References
7	N⁻	Nitrogen	−6.98	−673	[74]
7	N²⁻	Nitrogen	−11.09	−1070	[74]
8	O⁻	Oxygen	−7.71	−744	[74]
15	P⁻	Phosphorus	−4.85	−468	[74]
15	P²⁻	Phosphorus	−9.18	−886	[74]

Bibliography

Janousek, Bruce K.; Brauman, John I. (1979), "Electron affinities", in Bowers, M. T. (ed.), Gas Phase Ion Chemistry, vol. 2, New York: Academic Press, p. 53.
Rienstra-Kiracofe, J.C.; Tschumper, G.S.; Schaefer, H.F.; Nandi, S.; Ellison, G.B. (2002), "Atomic and molecular electron affinities: Photoelectron experiments and theoretical computations", Chem. Rev., vol. 102, no. 1, pp. 231–282, doi:10.1021/cr990044u, PMID 11782134.
Updated values can be found in the NIST chemistry webbook for around three dozen elements and close to 400 compounds.

Specific molecules

Adams, C.L.; Schneider, H.; Ervin, K.M.; Weber, J.M. (2009), "Low-energy photoelectron imaging spectroscopy of nitromethane anions: Electron affinity, vibrational features, anisotropies, and the dipole-bound state", J. Chem. Phys., 130 (7): 074307, Bibcode:2009JChPh.130g4307A, doi:10.1063/1.3076892, PMID 19239294
Borshchevskii, A.Ya.; Boltalina, O.V.; Sorokin, I.D.; Sidorov, L.N. (1988), "Thermochemical quantities for gas-phase iron, uranium, and molybdenum fluorides, and their negative ions", J. Chem. Thermodyn., 20 (5): 523, doi:10.1016/0021-9614(88)90080-8
Chaibi, W.; Delsart, C.; Drag, C.; Blondel, C. (2006), "High precision measurement of the ³²SH electron affinity by laser detachment microscopy", J. Mol. Spectrosc., 239 (1): 11, Bibcode:2006JMoSp.239...11C, doi:10.1016/j.jms.2006.05.012
Chowdhury, S.; Kebarle, P. (1986), "Electron affinities of di- and tetracyanoethylene and cyanobenzenes based on measurements of gas-phase electron-transfer equilibria", J. Am. Chem. Soc., 108 (18): 5453, doi:10.1021/ja00278a014
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George, P.M.; Beauchamp, J.L. (1979), "The electron and fluoride affinities of tungsten hexafluoride by ion cyclotron resonance spectroscopy", Chem. Phys., 36 (3): 345, Bibcode:1979CP.....36..345G, doi:10.1016/0301-0104(79)85018-1
Goldfarb, F.; Drag, C.; Chaibi, W.; Kröger, S.; Blondel, C.; Delsart, C. (2005), "Photodetachment microscopy of the P, Q, and R branches of the OH⁻(v=0) to OH(v=0) detachment threshold", J. Chem. Phys., 122 (1): 014308, Bibcode:2005JChPh.122a4308G, doi:10.1063/1.1824904, PMID 15638660
Huang, Dao-Ling; Dau, Phuong Diem; Liu, Hong-Tao; Wang, Lai-Sheng (2014), "High-resolution photoelectron imaging of cold C⁻
₆₀ anions and accurate determination of the electron affinity of C₆₀", J. Chem. Phys., 140 (22): 224315, Bibcode:2014JChPh.140v4315H, doi:10.1063/1.4881421, PMID 24929396, S2CID 1061364
Kim, J.B.; Weichman, M.L.; Neumark, D.M. (2015), "Low-lying states of FeO and FeO⁻ by slow photoelectron spectroscopy", Mol. Phys., 113 (15–16): 2105, Bibcode:2015MolPh.113.2105K, doi:10.1080/00268976.2015.1005706, S2CID 13868986
Mathur, B.P.; Rothe, E.W.; Tang, S.Y.; Reck, G.P. (1976), "Negative ions from phosphorus halides due to cesium charge exchange", J. Chem. Phys., 65 (2): 565, Bibcode:1976JChPh..65..565M, doi:10.1063/1.433109
Mead, R.D.; Lykke, K.R.; Lineberger, W.C.; Marks, J.; Brauman, J.I. (1984), "Spectroscopy and dynamics of the dipole-bound state of acetaldehyde enolate", J. Chem. Phys., 81 (11): 4883, Bibcode:1984JChPh..81.4883M, doi:10.1063/1.447515
Miller, T.M.; Leopold, D.G.; Murray, K.K.; Lineberger, W.C. (1986), "Electron affinities of the alkali halides and the structure of their negative ions", J. Chem. Phys., 85 (5): 2368, Bibcode:1986JChPh..85.2368M, doi:10.1063/1.451091
Nimlos, Mark R.; Ellison, G. Barney (1986), "Photoelectron spectroscopy of sulfur-containing anions (SO⁻
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Novick, S.E.; Engelking, P.C.; Jones, P.L.; Futrell, J.H.; Lineberger, W.C. (1979), "Laser photoelectron, photodetachment, and photodestruction spectra of O⁻
₃", J. Chem. Phys., 70 (6): 2652, Bibcode:1979JChPh..70.2652N, doi:10.1063/1.437842
Page, F. M.; Goode, G. C. (1969), Negative ions and the magnetron, John Wiley & Sons[75]
Ruoff, R.S.; Kadish, K.M.; Boulas, P.; Chen, E.C.M. (1995), "Relationship between the Electron Affinities and Half-Wave Reduction Potentials of Fullerenes, Aromatic Hydrocarbons, and Metal Complexes", J. Phys. Chem., 99 (21): 8843, doi:10.1021/j100021a060
Schiedt, J.; Weinkauf, R. (1995), "Spin-orbit coupling in the O⁻
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Schiedt, J.; Weinkauf, R. (1999), "Resonant photodetachment via shape and Feshbach resonances: p-benzoquinone anions as a model system", J. Chem. Phys., 110 (1): 304, Bibcode:1999JChPh.110..304S, doi:10.1063/1.478066
Schulz, P.A.; Mead, R.D.; Jones, P.L.; Lineberger, W.C. (1982), "OH⁻ and OD⁻ threshold photodetachment", J. Chem. Phys., 77 (3): 1153, Bibcode:1982JChPh..77.1153S, doi:10.1063/1.443980
Sheps, L.; Miller, E.M.; Lineberger, W.C. (2009), "Photoelectron spectroscopy of small IBr⁻(CO₂)_n(n=0–3) cluster anions", J. Chem. Phys., 131 (6): 064304, Bibcode:2009JChPh.131f4304S, doi:10.1063/1.3200941, PMID 19691385
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According to NIST as concerns Boron trifluoride, the Magnetron method, lacking mass analysis, is not considered reliable.