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प्रश्न
Use Hund’s rule to derive the electronic configuration of Ce3+ ion and calculate its magnetic moment on the basis of ‘spin-only’ formula.
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उत्तर
The electronic configuration of Ce and Ce3+ ions is as follows:
Ce (Z = 58): 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 4f1 5s2 5p6 5d1 6s2
or, [Xe] 4f1 5d1 6s2
Ce3+ (Z = 55): [Xe] 4f1
Thus, Ce3+ has only one unpaired electron, i.e., n = 1
∴ μs = `sqrt(n(n + 2))` BM
= `sqrt(1 xx (1 + 2))` BM
= `sqrt3` BM
= 1.732 BM
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संबंधित प्रश्न
Complete the following chemical equations:
`(i) Cr_2O_7^(2-)+6Fe^(2+)+14H^+ ->`
`(ii) 2CrO_4^(2-)+2H^+ ->`
`(iii) 2MnO_4^-+5C_2O_4^(2-)+16H^+ ->`
Account for the following:
Cr2+ is a strong reducing agent.
For M2+/M and M3+/M2+ systems, the EΘ values for some metals are as follows:
| Cr2+/Cr | −0.9 V |
| Mn2+/Mn | −1.2 V |
| Fe2+/Fe | −0.4 V |
| Cr3/Cr2+ | −0.4 V |
| Mn3+/Mn2+ | +1.5 V |
| Fe3+/Fe2+ | +0.8 V |
Use this data to comment upon:
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