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Physical Properties of Boron Family

Why are Mn 2+...

Question

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

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Solution

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 3d⁶ configuration and by losing one electron, its configuration changes to a more stable 3d⁵ configuration. Therefore, Fe²⁺ easily gets oxidized to Fe⁺³ oxidation state.

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

M n^{2 +}

compounds are more stable than

F e^{2 +}

compounds towards oxidation to their

+ 3

state, because :

M n_{+ 2}

compounds more stable than

F e_{2 +}

towards oxidation to their +3 state?
(b)

[T i (H_{2} 0)_{6}]^{3 +}

gives violet coloured aqueous solution but

[M g (H_{2} 0)_{6}]^{2 +}

solution is colourless, why?

Q. Explain why:

M n^{2 +}

is more stable than

F e^{2 +}

towards oxidation to +3 state.
(At. no. of Mn = 25, Fe = 26)

M n^{2 +}

is much more resistant than

F e^{2 +}

towards oxidation. Give reason.

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