Among the following molecules bond length is short in

C_{2}

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N_{2}

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O_{2}

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F_{2}

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Solution

The correct option is B $N_{2}$
As we know,
Bond length is inversely proportional to Bond order. That means, the higher the bond order, the stronger the force of attraction between the two atoms and the shorter the bond length.
The bond order of $C_{2}$ molecule is 2.
The bond order of $N_{2}$ molecule is 3.
$O_{2}$ has two unpaired electrons in its $π^{*}$ orbitals, and a bond order of 2.
The bond order of $F_{2}$ molecule is 1.

As we see $N_{2}$ has the highest Bond Order. Hence, it has the shortest Bond length. Therefore, option B is correct.

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Similar questions

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