Give reason Mn2+ is more paramagnetic than fe2+
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Why are Mn2+compounds more stable than Fe2+ towards oxidation to their +3 state?
Answer
Electronic configuration of Mn2+ is [Ar]183d5.
Electronic configuration of Fe2+ is [Ar]183d6.
It is known that half-filled and fully-filled orbitals are more stable. Therefore, Mn in (+2) state has a stable d5 configuration. This is the reason Mn2+shows resistance to oxidation to Mn3+. Also, Fe2+has 3d6configuration and by losing one electron, its configuration changes to a more stable 3d5configuration. Therefore, Fe2+ easily gets oxidized to Fe+3 oxidation state.
Answer
Electronic configuration of Mn2+ is [Ar]183d5.
Electronic configuration of Fe2+ is [Ar]183d6.
It is known that half-filled and fully-filled orbitals are more stable. Therefore, Mn in (+2) state has a stable d5 configuration. This is the reason Mn2+shows resistance to oxidation to Mn3+. Also, Fe2+has 3d6configuration and by losing one electron, its configuration changes to a more stable 3d5configuration. Therefore, Fe2+ easily gets oxidized to Fe+3 oxidation state.
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Answer:
Explanation:
Mn2+ configuration is 4s0 3d5 ie 5 unpaired electrons in d subshell while Fe2+ contains only 4 unpaired electrons. More unpaired electrons more paramagnetic.
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