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Electron affinity



The electron affinity, Eea, of an atom or molecule is the energy required to detach an electron from a singly charged negative ion, i.e., the energy change for the process

X- → X + e

An equivalent definition is the energy released (Einitial − Efinal) when an electron is attached to a neutral atom or molecule. It should be noted that the sign convention for Eea is the opposite to most thermodynamic quantities: a positive electron affinity indicates that energy is released on going from atom to anion.

All elements whose EA have been measured using modern methods have a positive electron affinity, but older texts mistakenly report that some elements such as alkaline earth metals have negative Eea, meaning they would repel electrons. This is not recognized by modern chemists. The electron affinity of the noble gases have not been conclusively measured, so they may or may not have slightly negative EAs. Atoms whose anions are relatively more stable than neutral atoms have a greater Eea. Chlorine most strongly attracts extra electrons; mercury most weakly attracts an extra electron. Eea of noble gases are close to 0.

Although Eea vary in a chaotic manner across the table, some patterns emerge. Generally, nonmetals have more positive Eea than metals.

Additional recommended knowledge

Contents

Values for the elements

The following data are quoted in kJ/mol. Elements marked with an asterisk are expected to have electron affinities close to zero on quantum mechanical grounds. Elements marked with a dotted box are synthetically made elements - elements not found naturally in the environment.

Group → 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
↓ Period
1 H
73

He
*
2 Li
60
Be
*

B
27
C
122
N
*
O
141
F
328
Ne
*
3 Na
53
Mg
*

Al
42
Si
134
P
72
S
200
Cl
349
Ar
*
4 K
48
Ca
2
Sc
18
Ti
8
V
51
Cr
65
Mn
*
Fe
15
Co
64
Ni
112
Cu
119
Zn
*
Ga
41
Ge
119
As
79
Se
195
Br
343
Kr
*
5 Rb
47
Sr
5
Y
30
Zr
41
Nb
86
Mo
72
Tc
*
Ru
101
Rh
110
Pd
54
Ag
126
Cd
*
In
39
Sn
107
Sb
101
Te
190
I
295
Xe
*
6 Cs
46
Ba
14
*
Hf
 
Ta
31
W
79
Re
*
Os
104
Ir
150
Pt
205
Au
223
Hg
*
Tl
36
Pb
35
Bi
91
Po
 
At
 
Rn
*
7 Fr
 
Ra
 
**
Rf
 
Db
 
Sg
 
Bh
 
Hs
 
Mt
 
Ds
 
Rg
 
Uub
 
Uut
 
Uuq
 
Uup
 
Uuh
 
Uus
 
Uuo
 

* Lanthanides La
45
Ce
92
Pr
 
Nd
 
Pm
 
Sm
 
Eu
 
Gd
 
Tb
 
Dy
 
Ho
 
Er
 
Tm
99
Yb
 
Lu
33
** Actinides Ac
 
Th
 
Pa
 
U
 
Np
 
Pu
 
Am
 
Cm
 
Bk
 
Cf
 
Es
 
Fm
 
Md
 
No
 
Lr
 
Chemical series of the periodic table
Alkali metals Alkaline earth metals Lanthanides Actinides Transition metals
Poor metals Metalloids Nonmetals Halogens Noble gases

Periodic trends

Eea generally increases across a period (row) in the periodic table. This is caused by the filling of the valence shell of the atom; a group 7A atom releases more energy than a group 1A atom on gaining an electron because it obtains a filled valence shell.

A trend of decreasing Eea going down the groups in the periodic table would be expected. The additional electron will be entering an orbital farther away from the nucleus, and thus would experience a lesser effective nuclear charge. However, a clear counterexample to this trend can be found in group 2A, and this trend only applies to group 1A atoms.

Molecular electron affinities

Eea is not limited to the elements but also applies to molecules. For instance the electron affinity for benzene is negative, as is that of naphthalene, while those of anthracene,phenanthrene and pyrene are positive. In silico experiments show that the electron affinity of hexacyanobenzene surpasses that of fullerene [1].

See also

References

  • Tro, Nivaldo J. (2008). Chemistry: A Molecular Approach (2nd Edn.). New Jersey: Pearson Prentice Hall. ISBN 0-13-100065-9. pp. 348–349.
 
This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Electron_affinity". A list of authors is available in Wikipedia.
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