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$The superoxide ion, $ \mathrm{O}_{2}^{-} $, is a reactive species that may play a role in the chemistry of aging. Use a molecular orbital diagram to determine$

The superoxide ion, $ \mathrm{O}_{2}^{-} $, is a reactive species that may play a role in the chemistry of aging. Use a molecular orbital diagram to determine the bond order of the superoxide ion. Enter the number (no units).

Ask by Pope Hardy.

Nov 22,2024 19:58

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The bond order of the superoxide ion $ \mathrm{O}_{2}^{-} $ is 2.

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To determine the bond order of the superoxide ion $(\mathrm{O}_{2}^{-})$, we can use the molecular orbital theory. The molecular orbital configuration for $\mathrm{O}_{2}$ (neutral oxygen molecule) is $(\sigma_{1s})^2(\sigma_{1s}^*)^2(\sigma_{2s})^2(\sigma_{2s}^*)^2(\sigma_{2p_z})^2(\pi_{2p_x})^2(\pi_{2p_y})^2(\pi_{2p_x}^*)^1$, where $\sigma$ and $\pi$ refer to the types of bonds formed by the overlap of atomic orbitals, and the asterisk indicates an antibonding orbital. In $\mathrm{O}_{2}^{-}$, an additional electron is added to one of the $\pi^*$ antibonding orbitals, resulting in the configuration $(\pi_{2p_x}^*)^2$. The bond order can be calculated using the formula: \[ \text{Bond Order} = \frac{(\text{Number of bonding electrons}) - (\text{Number of antibonding electrons})}{2} \] For $\mathrm{O}_{2}$, there are 10 bonding electrons and 2 antibonding electrons. In $\mathrm{O}_{2}^{-}$, it becomes 10 bonding electrons and 3 antibonding electrons: \[ \text{Bond Order} = \frac{10 - 3}{2} = \frac{7}{2} = 3.5 \] Thus, the bond order of the superoxide ion $(\mathrm{O}_{2}^{-})$ is $1.5$.