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Systematically outline the term symbols with the respective highest spin multiplicities for d 2 , d 3 , d 4 , d 5 electronic configurations of transition metals
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Here's a breakdown of the term symbols and highest spin multiplicities for d2, d3, d4, and d5 electronic configurations in transition metals:
Electronic Configuration | Term Symbols | Highest Spin Multiplicity
---|---|---
d2 | 3F, 1D, 1G, 3P | 3F (S = 1, 2S+1 = 3)
d3 | 4F, 4P, 2H, 2G, 2D, 2P | 4F (S = 3/2, 2S+1 = 4)
d4 (high spin) | 5D, 3H, 3G, 3F, 3P, 1I, 1G, 1S | 5D (S = 2, 2S+1 = 5)
d4 (low spin) | 3F, 1D, 1G, 3P | 3F (S = 1, 2S+1 = 3)
d5 (high spin) | 6S, 4G, 4F, 4D, 2I, 2H, 2G, 2F, 2D, 2P | 6S (S = 5/2, 2S+1 = 6)
d5 (low spin) | 2S, 2D, 2G | 2S (S = 1/2, 2S+1 = 2)
Explanation:
Term symbols represent the total angular momentum (L) and spin angular momentum (S) of an electronic configuration. They follow the format: 2S+1LJ, where:
2S+1: Spin multiplicity (number of unpaired electrons + 1)
L: Total orbital angular momentum (S = 0, P = 1, D = 2, F = 3, G = 4...)
J: Total angular momentum (L + S) or (L - S), depending on the coupling of the spin and orbital moments.
Highest spin multiplicity: The term symbol with the largest spin multiplicity (2S+1) corresponds to the ground state configuration.
High spin vs. low spin: These refer to the electronic configurations where electrons are distributed to maximize or minimize the number of unpaired electrons, respectively. This is influenced by factors like ligand field strength and Hund's rule.
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