Question

Fe2+ is easy oxsidised to Fe3+ but Mn2+ is not easy oxidised...why??

Answer 1

HEY DEAR.....!!!

1.Fe2+ is easy to oxidize to Fe3+ because removing the electron results in a half filled d subshell. 

2. Mn2+ is difficult to oxidize to Mn3+ because Mn2+ has a half filled d subshell and by removing an electron the d subshell of Mn3+ is not half filled. 

3. Fe2+ is easy to oxidize to Fe3+ because ions with an odd charge are most stable for atoms with an even atomic number. 

4. Mn2+ is difficult to oxidize to Mn3+ because ions with an even charge are most stable for atoms with an odd atomic number. 

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Answer 2

Explanation:

Fe2+ is easy oxsidised to Fe3+  because.....

• The oxidation of Fe to Fe2+is not as easy as the oxidation of Mn to Mn2+.
• Thus, these metals can be arranged in the increasing order of their ability to get oxidised as: Fe < Cr < Mn value for Fe3+/ Fe2+­­ is lower than that for Mn3+/Mn2+.
• The reduction of Fe3+to Fe2+is easier than the reduction of Mn3+to Mn2+, Hence, Fe3+is more stable than Mn3+.
• Fe2+ is easy to oxidize to Fe3+ because removing the electron results in a half filled d subshell.
• Mn2+ is difficult to oxidize to Mn3+ because Mn2+ has a half filled d subshell and by removing an electron the d subshell of Mn3+ is not half filled.
• Fe3+ is more stable than Fe2+.
• The electron configuration of Fe3+ is 3d5 whereas the electron configuration of Fe2+ is 3d6. 3d5 configuration is a half-filled configuration which is very stable. Thus Fe3+ is more stable than Fe2+.And Fe2+ is easy oxsidised to Fe3+ .

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