Which of the following have identical bond order:

Question

TestHub · Accepted Answer

To determine bond order, calculate the total number of valence electrons for each species and apply the molecular orbital theory formula: Bond Order = $0.5 \times (n u mb ero f e l ec t ro n s inb o n d in g or bi t a l s - n u mb ero f e l ec t ro n s inan t ib o n d in g or bi t a l s)$ .

For isoelectronic species (same total number of electrons), the bond order is often identical.

1. $O_{2}^{2 +}$ : 10 valence electrons (12 from 2O - 2 for charge) $\to$ B.O. = 3

2. $NO^{+}$ : 10 valence electrons (5 from N + 6 from O - 1 for charge) $\to$ B.O. = 3

3. $CN^{-}$ : 10 valence electrons (4 from C + 5 from N + 1 for charge) $\to$ B.O. = 3

4. $CN^{+}$ : 8 valence electrons (4 from C + 5 from N - 1 for charge) $\to$ B.O. = 2.5

Thus, $O_{2}^{2 +}$ , $NO^{+}$ , and $CN^{-}$ all have a bond order of 3.

Chemistry - CHEMICAL BONDING Question with Solution | TestHub

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