According to the molecular orbital theory, the bond order in ${C_2}$ molecule is
$0$
$1$
$2$
$3$
(c) $B.O.$ of carbon $ = \frac{{{N_b} – {N_a}}}{2} = \frac{{8 – 4}}{2} = 2$.
The total number of species from the following in which one unpaired electron is present, is . . . . . . $\mathrm{N}_2, \mathrm{O}_2, \mathrm{C}_2^{-}, \mathrm{O}_2^{-}, \mathrm{O}_2^{2-}, \mathrm{H}_2^{+}, \mathrm{CN}^{-}, \mathrm{He}_2^{+}$
According to $MOT$ which of following is correct
The correct molecular orbital diagram for $\mathrm{F}_2$ molecule in the ground state is
Correct order of bond length is
The correct order of the $O-O$ bond length in $O_2, H_2O_2$ and $O_3$ is
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