A pair of isoelectronic species having bond o | vedclass

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(C) To determine the bond order,we calculate the number of electrons and use the molecular orbital theory formula: $B.O. = \frac{N_b - N_a}{2}$.For $O

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$O_2^{2-}, F_2$

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(C) To determine the bond order,we calculate the number of electrons and use the molecular orbital theory formula: $B.O. = \frac{N_b - N_a}{2}$.For $O_2^{2-}$,the total number of electrons is $8 + 8 + 2 = 18 \ e^{-}$. The bond order is $\frac{10 - 8}{2} = 1$.For $F_2$,the total number of electrons is $9 + 9 = 18 \ e^{-}$. The bond order is $\frac{10 - 8}{2} = 1$.Both species are isoelectronic $(18 \ e^{-})$ and have a bond order of $1$.

$A$ pair of isoelectronic species having bond order of $1$ is

Similar Questions

In which of the following processes does the value of bond order and magnetic nature not change?

Answer the following questions:
$(i)$ Give the molecular orbitals and their types formed by $LCAO$ from $2s, 2p_{x}, 2p_{y}$ and $2p_{z}$ atomic orbitals.
$(ii)$ Provide the energy order of molecular orbitals for $Li_{2}, Be_{2}, C_{2}, N_{2}, O_{2}$ and $F_{2}$.

The correct statement regarding $SO_2$ molecule is

If the sum of bond orders of $O_2^{-}$ and $O_2^{2-}$ is $x$,then bond order of $O_2^{2+}$ will be (in $x$)

During the change of $O_2$ to $O_2^-$ ion,the electron adds to which one of the following orbitals?

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