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Slater's rule for calculation of effective nuclear charge

Slater's rule for calculation of effective nuclear charge

Grade:12th pass

1 Answers

Arun
25750 Points
5 years ago
Dear student
 
Here are the Slater's rules to calculate an approximate value for the effective nuclear charge "felt" by an electron in a particular orbital of an atom. 

1 - Write the electronic configuration for the atom using the following grouping, called Slater electron configuration:

(1s) (2s,2p) (3s,3p) (3d) (4s,4p) (4d) (4f) (5s,5p) ... , 

2 - Any electron to the right of the considered electron of interest do not contribute to shielding, 

3 - All other electrons in the same group of the considered electron shield by 0.35 nuclear charge units each; except for 1s, the screening is reduced to 0.30, 

4 - If the considered electron is an s or p electron in the shell of principal quantum number n, all electrons with one less value n-1 shield by 0.85 units of nuclear charge each; and all electrons with two less values n-2 shield by 1.00 units. The n-3, n-4, ... shield by 1.00 units each as well. 

5 - If the considered electron is an d or f electron: all electrons to the left shield by 1.00 units of nuclear charge each. 

6 - Sum all the shielding amounts for each group. To obtain the effective charge for each group, subtract from the nuclear charge value the corresponding shielding. 

7 - For larger principal quantum numbers, n is corrected as follows:
n = 1, 2, 3, 4, 5, 6 
n* = 1, 2, 3, 3.7, 4.0, 4.2

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