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4.Chemical Bonding and Molecular Structure
easy
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
$\sigma {(1s)^2}{\sigma ^ * }{(1s)^2}\sigma {(2s)^2}{\sigma ^ * }{(2s)^2}\sigma {(2p)^2}\pi {(2p)^2}$
Solution
It’s Obvious.
Standard 11
Chemistry
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