The bond order in $N_2^ + $ ion is
$1$
$2$
$2.5$
$3$
(c) ${\rm{B}}{\rm{.O}}{\rm{.}} = \frac{{{\rm{No}}{\rm{. of }}{N_b} – {\rm{No}}{\rm{. of }}{N_a}}}{2}$$ = \frac{5}{2} = 2.5$.
Bond order of $C_2$ vapour is :
The total number of species from the following in which one unpaired electron is present, is . . . . . . $\mathrm{N}_2, \mathrm{O}_2, \mathrm{C}_2^{-}, \mathrm{O}_2^{-}, \mathrm{O}_2^{2-}, \mathrm{H}_2^{+}, \mathrm{CN}^{-}, \mathrm{He}_2^{+}$
Write the important conditions required for the linear combination of atomic orbitals to form molecular orbitals.
Stability of the species $Li_2, Li_2^-$ and $Li_2^+$ increases in the order of :
During change of $O^2$ to $O_2^-$ ion, the electron adds on which one of the following orbitals?
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