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Using slater's rules, the effective nuclear charge for a valence electron in Co2+
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Using Slater's rules, the effective nuclear charge (Zeff) for a valence electron in Co2+ is calculated as follows:
1. Electron Configuration: Co2+ has the electron configuration [Ar]3d7. Valence electrons are in the 3d orbitals.
2. Slater's Rules:
Electrons in the same group (n): Each electron contributes 0.35 to the shielding constant (S) except for the 1s electrons, which contribute 0.30.
Electrons in the (n-1) shell: Each electron contributes 0.85 to S.
Electrons in the (n-2) or lower shells: Each electron contributes 1.00 to S.
3. Shielding Constant (S) Calculation:
There are 7 3d electrons (same group as valence), so they each contribute 0.35, giving 7
0.35 = 2.45.
There are 18 electrons in the (n-1) shell (3s and 3p), each contributing 0.85, giving 18
0.85 = 15.30.
There are 10 electrons in the (n-2) shell (2s and 2p), each contributing 1.00, giving 10
1.00 = 10.00.
Total Shielding Constant (S) = 2.45 + 15.30 + 10.00 = 27.75
4. Effective Nuclear Charge (Zeff):
Zeff = Z - S, where Z is the atomic number of Cobalt (27)
Zeff = 27 - 27.75 = -0.75
This negative Zeff indicates that Slater's rules are not accurate for transition metals. The actual Zeff for Co2+ is positive due to the complex electronic interactions in transition metals. More sophisticated methods are needed for accurate Zeff calculations in these cases.
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