A) \[O_{2}^{-}\]is less stable.
B) Both \[O_{2}^{+}\]and \[O_{2}^{-}\] are paramagnetic.
C) \[O_{2}^{+}\] have higher bond order than\[O_{2}^{-}\] .
D) \[O_{2}^{+}\] is diamagnetic while \[O_{2}^{-}\] is paramagnetic.
Correct Answer: D
Solution :
: Molecular orbital configuration of \[O_{2}^{+}\]: \[\sigma 1{{s}^{2}}\sigma *1{{s}^{2}}\sigma 2{{s}^{2}}\sigma *2{{s}^{2}}\sigma 2p_{z}^{2}\pi 2p_{x}^{2}=\pi 2p_{y}^{2}\pi *2p_{x}^{1}\] Bond order \[=\frac{1}{2}(10-5)=2.5\] Number of unpaired electrons =1, hence paramagnetic. Molecular orbital configuration of\[O_{2}^{-}\]: \[\sigma 1{{s}^{2}}\sigma *1{{s}^{2}}\sigma 2{{s}^{2}}\sigma *2{{s}^{2}}\sigma 2p_{z}^{2}\pi 2p_{x}^{2}=\pi 2p_{y}^{2}\pi *2p_{x}^{2}\]\[=\pi *2p_{y}^{1}\] Bond order \[=\frac{1}{2}(10-7)=1.5\] Number of unpaired electron = 1, hence paramagnetic. Both \[O_{2}^{+}\] and \[O_{2}^{-}\] are paramagnetic. \[O_{2}^{+}\] have higher bond order than 02. \[O_{2}^{-}\]is less stable.
You need to login to perform this action.
You will be redirected in
3 sec
