$\sigma {(1s)^2}{\sigma ^ * }{(1s)^2}\sigma {(2s)^2}{\sigma ^ * }{(2s)^2}\pi {(2p)^4}\sigma {(2p)^1}$

4.Chemical Bonding and Molecular StructureEasy

From elementary molecular orbital theory we can give the electronic configuration of the singly positive nitrogen molecular ion $N_2^ + $ as

A
$\sigma {(1s)^2}{\sigma ^ * }{(1s)^2}\sigma {(2s)^2}{\sigma ^ * }{(2s)^2}\pi {(2p)^4}\sigma {(2p)^1}$
B
$\sigma {(1s)^2}{\sigma ^ * }{(1s)^2}\sigma {(2s)^2}{\sigma ^ * }{(2s)^2}\sigma {(2p)^1}\pi {(2p)^3}$
C
$\sigma {(1s)^2}{\sigma ^ * }{(1s)^2}\sigma {(2s)^2}{\sigma ^ * }{(2p)^2}\pi {(2p)^4}$
D
$\sigma {(1s)^2}{\sigma ^ * }{(1s)^2}\sigma {(2s)^2}{\sigma ^ * }{(2s)^2}\sigma {(2p)^2}\pi {(2p)^2}$

The linear combination of atomic orbitals to form molecular orbitals takes place only when the combining atomic orbitals

$A$. have the same energy

$B$. have the minimum overlap

$C$. have same symmetry about the molecular axis

$D$. have different symmetry about the molecular axis

Choose the most appropriate from the options given below:

Difficult

Medium

Easy

Medium

Difficult