A) due to \[{{d}^{10}}\] configuration, metallic bonds are strong.
B) due to \[{{d}^{7}}\] configuration, metallic bonds are weak.
C) due to \[{{d}^{5}}\] configuration, metallic bonds are weak.
D) None of these
Correct Answer: C
Solution :
Due to \[{{d}^{5}}\] configuration, Mn has exactly half filled d-orbitals. As a result the electronic configuration is stable means 3d electrons are more tightly held by the nucleus and this reduces the delocalization of electrons resulting in weaker metallic bonding.
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