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Why the ionization energy of \mathrm{Fe^{2+}} is less than \mathrm{Mn^{2+}} although they have the same exchange energy?

a) Pairing energy compensates for the low ionization energy in \mathrm{Fe^{2+}}

b) Pairing energy compensates for the high ionization energy in \mathrm{Mn^{2+}}

c) Small size compensates for the low ionization energy in \mathrm{Fe^{2+}}

d) \mathrm{d^{5}} configuration is more stable than \mathrm{d^{6}}

Option: 1

A) and B)

 


Option: 2

A) and D)


Option: 3

C) and D)

 


Option: 4

B) and C) 


Answers (1)

best_answer

Half-filled orbitals are more stable than partly-filled orbitals. Also, pairing electrons require energy due to repulsion between the two electrons. So, unpairing them results in loss of energy in the form of ionization.

 

Posted by

Rishi

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