k+ ion is smaller in size
Zeff = Z - S Zeff is the effective nuclear charge on an
electron; Z is the nuclear charge and S is the screening of that
charge on the electron by all the other electrons.
Assume core electrons S = 1, valence electrons S = 0
Cl^- 1s^2 2s^2p^6 3s^2 3p^6 1s^2 2s^2p^6 S = 10; 3s^2 3p^6 S =
0
Zeff = Z-S = 17- 10 =7
K^+ 1s^2 2s^2p^6 3s^2 3p^6; 1s^2 2s^2p^6 S = 10; 3s^2 3p^6 S =
0
Zeff = Z-S = 19- 10 = 9
Firstly, the electrons are arranged in to a sequence of groups
in order of increasing principal quantum number n, and for equal n
in order of increasing azimuthal quantum number l, except that s-
and p- orbitals are kept together. Well ignore 3d electrons etc:
don’t apply
[1s] [2s,2p] [3s,3p] Each group is given a different shielding
constant which depends upon the number and types of electrons in
those groups preceding it.
The shielding constant for each group is formed as the sum of the
following contributions:
An amount of 0.35 from each other electron within the same group
except for the [1s] group, where the other electron contributes
only 0.30.
If the group is of the [s p] type, an amount of 0.85 from each
electron with principal quantum number (n) one less and an amount
of 1.00 for each electron with an even smaller principal quantum
number
Cl^- 1s^2 2s^2p^6 3s^2 3p^6; 1s^2 S = 2; 2s^2p^6 S = 8×0.85; 3s^2
3p^6 S = 7×0.35 (don’t count the electron under
consideration)
S = 2 + 6.8 + 2.45 = 11.25
Zeff(Cl^-) = 17 – 11.25 = 5.75
K^+ 1s^2 2s^2p^6 3s^2 3p^6 same S as for Cl^- but Z increases by 2
hence
Zeff(K^+) = 19 - 11.25 = 7.75
Z effective of K+ ion is 19-11.75= 7.75
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