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Why Are Mn2+Compounds More Stable than Fe2+ Towards Oxidation to Their +3 State? - CBSE (Science) Class 12 - Chemistry

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Question

Why are Mn2+compounds more stable than Fe2+ towards oxidation to their +3 state?

Solution 1

Electronic configuration of Mn2+ is [Ar]18 3d5.

Electronic configuration of Fe2+ is [Ar]18 3d6.

It is known that half-filled and fully-filled orbitals are more stable. Therefore, Mn in (+2) state has a stabled5 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 3d5 configuration. Therefore, Fe2+ easily gets oxidized to Fe+3 oxidation state.

Solution 2

Electronic configuration of Mn2+ is 3d5. This is a half-filled configuration and hence stable. Therefore, third ionization enthalpy is’very high, i. e., third electron cannot be lost easily. Electronic configuration of Fe2+is 3d6. It can lose one electron easily to achieve a stable configuration 3d5.

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APPEARS IN

 NCERT Solution for Chemistry Textbook for Class 12 (2018 to Current)
Chapter 8: The d-block and f-block Elements
Q: 2 | Page no. 234

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Solution Why Are Mn2+Compounds More Stable than Fe2+ Towards Oxidation to Their +3 State? Concept: Electronic Configurations of the D-block Elements.
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