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In aqueous solution, Cr^(2+) is a strong...

In aqueous solution, `Cr^(2+)` is a stronger reducing agent than `Fe^(2+)`. This is because

A

`Cr^(2+)` ion is more stable than `Fe^(2+)`

B

`Cr^(3+)` ion with `d^(3)` configuration has favourable crystal field stabilisation energy

C

`Cr^(3+)` has half-filled configuration and hence more stable

D

`Fe^(3+)` in aqueous solution is more stable than `Cr^(3+)`

Text Solution

Verified by Experts

The correct Answer is:
B
`because Cr^(3+)` ion has `d^(3)` configuration `(t_(2g)^(3) e_(g)^(0))`, which makes `Cr^(3+)` stable by providing crystalfield stabilisation energy. Thus, `Cr^(2+)` ion can easily changes to `Cr^(3+)` (i.e. get oxidised) and acts as a strong reducing agent.
`Cr^(2+) rarr Cr^(3+) + e^(-)`
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