Indicate the trend in increasing bond length for molecular...

Indicate the trend in increasing bond length for molecular oxygen, the peroxide ion and superoxide ion. (a) $\mathrm{O}_{2}^{2 \cdot}>\mathrm{O}_{2}>\mathrm{O}^{2-}$ (b) $\mathrm{O}_{2}^{2 \cdot}>\mathrm{O}_{2}^{-}>\mathrm{O}_{2}$ (c) $\mathrm{O}_{2}>\mathrm{O}_{2}^{-}>\mathrm{O}_{2}^{\frac{2}{2}}$ (d) $\mathrm{O}_{2}>\mathrm{O}_{2}^{2}>\mathrm{O}^{2-}$

Indicate the trend in increasing bond length for molecular oxygen, the peroxide ion and superoxide ion.
(a) $\mathrm{O}_{2}^{2 \cdot}>\mathrm{O}_{2}>\mathrm{O}^{2-}$
(b) $\mathrm{O}_{2}^{2 \cdot}>\mathrm{O}_{2}^{-}>\mathrm{O}_{2}$
(c) $\mathrm{O}_{2}>\mathrm{O}_{2}^{-}>\mathrm{O}_{2}^{\frac{2}{2}}$
(d) $\mathrm{O}_{2}>\mathrm{O}_{2}^{2}>\mathrm{O}^{2-}$

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Key Concepts

Molecular Orbital Theory

This theory explains the formation of molecular orbitals by the linear combination of atomic orbitals, allowing for a description of bonding and antibonding interactions. It is crucial for understanding the electronic structure of diatomic molecules and ions, as it helps to determine the bond order by comparing the number of electrons in bonding vs antibonding orbitals.

Bond Order and Bond Length Relationship

Bond order is inversely related to bond length; a higher bond order indicates stronger bonding and typically results in a shorter bond. Conversely, a lower bond order weakens the bond and generally leads to an increase in bond length. This relationship is pivotal in predicting structural trends in molecules and ions.

Effect of Electron Addition on Bonding

Adding extra electrons to a molecule, as in the formation of superoxide and peroxide ions, typically involves placing electrons in antibonding orbitals. This reduces the bond order compared to the neutral molecule, which in turn increases the bond length. Understanding how electron addition modifies the electronic structure is essential for predicting differences in bond lengths among related species.

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