Question

# In aqueous solution, $${ Cr }^{ 2+ }$$ is a stronger reducing agent than $${ Fe }^{ 2+ }$$. This is because:

A
Cr2+ ion is more stable than Fe2+.
B
Cr3+ ion with d3 configuration has favourable crystal field stabilisation energy.
C
Cr3+ has half-filled configuration and hence more stable
D
Fe3+ in aqueous solution is more stable than Cr3+.
E
Fe2+ ion with d6 configuration has favourable crystal field stabilisation energy.

Solution

## The correct option is B $${ Cr }^{ 3+ }$$ ion with $${ d }^{ 3 }$$ configuration has favourable crystal field stabilisation energy.$$\because { Cr }^{ 3+ }$$ ion has $${ d }^{ 3 }$$ configuration $$\left( { t }_{ 2g }^{ 3 }{ e }_{ g }^{ 0 } \right)$$, which makes $${ Cr }^{ 3+ }$$ stable by providing crystal field stabilisation energy.Thus, $${ Cr }^{ 2+ }$$ ion can easily changes to $${ Cr }^{ 3+ }$$ (i.e. get oxidised) and acts as a strong reducing agent.$${ Cr }^{ 2+ }\rightarrow { Cr }^{ 3+ }+{ e }^{ - }$$Chemistry

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