How many of the species are paramagnetic?
$N_{2} O, N O, N O_{2}, O_{2}, N O_{2}^{+}, N O^{+}, C O^{+}$

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Solution

The correct option is D 4
Number of valance electrons in $N_{2} O = 5 + 6 + 5 = 16$
All electrons can be paired up and there is no free electron. $N_{2} O$ molecule is therefore diamagnetic.

Number of valance electrons in $N O = 5 + 6 = 11$
All electrons can not be paired up and there is an odd electron responsible for magnetism. $N O$ molecule is therefore paramagnetic.

Number of valance electrons in $N O_{2} = 5 + 6 + 6 = 17$
All electrons can not be paired up and there is an odd electron responsible for magnetism. $N O_{2}$ molecule is therefore paramagnetic.

Number of valance electrons in $O_{2} = 6 + 6 = 12$
All electrons can be paired up and there is no free electron. $O_{2}$ molecule is exception and is paramagnetic.

Number of valance electrons in $N O_{2}^{+} = 5 + 6 + 6 - 1 = 16$
All electrons can be paired up and there is no free electron. $N O_{2}^{+}$ molecule is therefore diamagnetic.

Number of valance electrons in $N O^{+} = 5 + 6 - 1 = 10$
All electrons can be paired up and there is no free electron. $N O^{+}$ molecule is therefore diamagnetic.

Number of valance electrons in $C O^{+} = 4 + 6 - 1 = 9$
All electrons can not be paired up and there is an odd electron. $C O^{+}$ molecule is therefore paramagnetic.

Overall 4 species are paramagnetic including $N O, N O_{2}, O_{2}$ and $C O^{+}$

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Among the following the total no. of species which are paramagnetic

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