Chemical Forums
Chemistry Forums for Students => Inorganic Chemistry Forum => Topic started by: harini_5 on April 23, 2008, 04:49:22 AM
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I recently learnt about the SLATER rules for the calculation of effective nuclear charge In that I learnt that, in case of d and f electrons the inner electrons need not be divided into subgroups and different values like 0.85 and 1 need not be applied and uniformly for all electrons the number of electrons may be multiplied by 1.Why is it so in case of d and f electrons and not s and p electrons?
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Slater's Rules:
1. Write out the electron configuration of the element in the following order and groupings: (1s) (2s,2p) (3s,3p) (3d) (4s, 4p) (4f) (5s, 5p), etc.
2. Electrons in any group to the right of the (ns, np) group contribute nothing to the shielding constant.
3. All of the other electrons in the (ns, np) group shield the valence electron to an extent of 0.35 each.
4. All electrons in the n-1 shell shield to an extent of 0.85 each.
5. All electrons in the n-2 or lower shells shield completely (shielding = 1).
6. When the outer electrons are in either an f or a d subshell, all electrons to the left shield completely (shielding = 1)
In order to specifically adress your question:
This is best done by example. Please see the attached word document ;)
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thanks