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Table of electron affinity of elements
Table shows electronic affinity (i.e. the amount of energy released when an electron is added to atom) for most of chemical elements.

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Electron affinity

Atomic numberElement nameElement symbolElectron affinity [eV]
1HydrogenH0.754
2HeliumHe-0.52
3LithiumLi0.618
4BerylliumBe-0.52
5BoronB0.279
6CarbonC1.2621136
7NitrogenN-11.09
8OxygenO-7.711
9FluorineF3.401
10NeonNe-1.2
11SodiumNa0.547
12MagnesiumMg-0.415
13AluminiumAl0.432
14SiliconSi1.389
15PhosphorousP-9.183
16SulfurS-4.726
17ChlorineCl3.612
18ArgonAr-1
19PotassiumK0.501
20CalciumCa0.024
21ScandiumSc0.188
22TitaniumTi0.084
23VanadiumV0.527
24ChromiumCr0.675
25ManganeseMn-0.52
26IronFe0.153
27CobaltCo0.662
28NickelNi1.157
29CopperCu1.235
30ZincZn-0.62
31GalliumGa0.43
32GermaniumGe1.232
33ArsenicAs0.804
34SeleniumSe2.02
35BromineBr3.363
36KryptonKr-0.62
37RubidiumRb0.485
38StrontiumSr0.052
39YttriumY0.307
40ZirconiumZr0.433
41NiobiumNb0.917
42MolybdeniumMo0.747
43TechnetiumTc0.55
44RutheniumRu1.046
45RhodiumRh1.142
46PalladiumPd0.562
47SilverAg1.304
48CadmiumCd-0.725
49IndiumIn0.3
50TinSn1.112
51AntimonySb1.047
52TelluriumTe1.97
53IodineI3.059
54XenonXe-0.83
55CesiumCs0.471
56BariumBa0.144
57LanthanumLa0.47
58CeriumCe0.65
59PraseodymiumPr0.962
60NeodymiumNd1.916
61PromethiumPm0.129
62SamariumSm0.162
63EuropiumEu0.864
64GadoliniumGd0.137
65TerbiumTb1.165
66DysprosiumDy0.352
67HolmiumHo0.338
68ErbiumEr0.312
69ThuliumTm1.029
70YtterbiumYb-0.02
71LutetiumLu0.346
72HafniumHf0.017
73TantalumTa0.323
74TungstenW0.816
75RheniumRe0.06
76OsmiumOs1.1
77IridiumIr1.564
78PlatinumPt2.125
79GoldAu2.308
80MercuryHg-0.52
81ThaliumTl0.377
82LeadPb0.356
83BismuthBi0.942
84PoloniumPo1.9
85AstatineAt2.3
86RadonRn-0.725
87FranciumFr0.486
88RadiumRa0.1
89ActiniumAc0.35
90ThoriumTh1.17
91ProtactiniumPa0.55
92UraniumU0.53
93NeptuniumNp0.48
94PlutoniumPu-0.5
95AmericiumAm0.1
96CuriumCm0.28
97BerkeliumBk-1.72
98CaliforniumCf-1.01
99EinsteiniumEs-0.3
100FermiumFm0.35
101MendeleviumMd0.98
102NobeliumNo-2.33

Some facts

  • The electronic affinity is amount of energy, that is released during the attachment of the electron to the neutral atom. As a result of such attachment, a negative ion (anion) is formed.
  • Electron affinity is related to electronegativity of elements. Simply speaking, the greater the affinity of electrons, the more eagerly the atoms of a given element join electrons to form ions (anions).
  • The electronic affinity is most often given in electron volts (eV) or in kilojoules per mole (kJ / mol).
  • Theoretically, the value of the electron affinity can be approximated using Koopmans theorem as energy of lowest unocuppied orbital. Such calculations can be made using quantum chemistry methods.
  • Electronic affinity is a property specific to a given element. However, it may be slightly different for individual isotopes.
  • When two atoms form a chemical compound, the electron cloud is shifted towards the element with a higher electron affinity. When this difference is large enough, the electron is virtually transferred from one atom to the other creating an ionic bond. This is the case, for example, in the case of sodium-chlorine (Na-Cl) bonding in sodium chloride.
  • Electronic affinity is measured (or calculated theoretically) for isolated atoms in gaseous state.
  • Analogically, it is possible to define the electron affinity for chemical compounds (molecules).


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