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Date: 6-7-2017
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One set of estimates for the effective nuclear charge (Zeff ) we described Zeff as being less than the actual nuclear charge (Z) because of the repulsive interaction between core and valence electrons. We can quantitatively represent this difference between Z and Zeff as follows:
Rearranging this formula to solve for Zeff we obtain:
We can then substitute the shielding constant obtained using Equation 2 to calculate an estimate of Zeff for the corresponding atomic electron.
Example 1 : The Effective Charge of p Electrons of Boron Atoms What is the effective nuclear charge experienced by a valence p- electron in boron?
Given: Boron (B)
Asked for: Zeff for a valence p- electron
Strategy:
Solution:
A B: 1s2 2s2 2p1 . The valence p- electron in boron resides in the 2p subshell.
B (1s2)(2s2 2p1)
B S[2p] = 1.00(0) + 0.85(2) + 0.35(2) = 2.40
C Z = 5
D Zeff=2.60
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