Explain the formation of the following molecules using valence bond theory
(a) $N_{2}$ molecules
(b) $O_{2}$ molecules

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Solution

According to valence bond theory, the number of bond formed by and atom is equal to the number of unpaired electron present in it.
Also, only those two atoms make bond which have a unpaired electron with opposite spin.
In $N_{2}$ , both the nitrogen atom have 3 unpaired electron, thus they form triple bond in this molecule.
$: N \equiv N :$
Similarily, the oxygen atom have two unpaired electrons. Thus they form double bond with each other.
$O = O$

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Explain the formation of the following molecules using valence bond theory(a) N2 molecules(b) O2 molecules

Explain the formation of the following molecules using valence bond theory
(a) $N_{2}$ molecules
(b) $O_{2}$ molecules