Group the following molecules/ions according | vedclass

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Question

(A) To group the species by bond order,we calculate the bond order $(B.O.)$ for each using Molecular Orbital Theory: $1$. $O_2^{2-}$ ($18$ electrons):

Vedclass · Accepted Answer

$O_2^{2-}, Li_2, O_2^{2+}, F_2, N_2, He_2^{2+}$

Vedclass · Answer

(A) To group the species by bond order,we calculate the bond order $(B.O.)$ for each using Molecular Orbital Theory: $1$. $O_2^{2-}$ ($18$ electrons): $B.O. = \frac{1}{2}(10-8) = 1$ $2$. $Li_2$ ($6$ electrons): $B.O. = \frac{1}{2}(4-2) = 1$ $3$. $F_2$ ($18$ electrons): $B.O. = \frac{1}{2}(10-8) = 1$ $4$. $He_2^{2+}$ ($2$ electrons): $B.O. = \frac{1}{2}(2-0) = 1$ $5$. $N_2$ ($14$ electrons): $B.O. = \frac{1}{2}(10-4) = 3$ $6$. $O_2^{2+}$ ($14$ electrons): $B.O. = \frac{1}{2}(10-4) = 3$ Thus,the species with $B.O. = 1$ are $(O_2^{2-}, Li_2, F_2, He_2^{2+})$ and the species with $B.O. = 3$ are $(N_2, O_2^{2+})$.

Group the following molecules/ions according to their bond order: $O_2^{2-}, Li_2, O_2^{2+}, F_2, N_2, He_2^{2+}$.

Similar Questions

What is the effect of the following processes on the bond order in $N_{2}$ and $O_{2}$?
$(A)$ $N_{2} \to N_{2}^{+} + e^{-}$
$(B)$ $O_{2} \to O_{2}^{+} + e^{-}$

Why do $N_2$,$NO^+$,$CN^-$,and $CO$ have the same bond order?

The bond order in $O_2^+$ is

Which molecule has the highest bond order?

Arrange the following in the increasing order of their bond order: $O_{2}, O_{2}^{+}, O_{2}^{-}, O_{2}^{2-}$

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