In which of the following diatomic molecules would the bond...

In which of the following diatomic molecules would the bond strength be expected to weaken as an electron is removed?
a. $\mathrm{H}_{2}$
c. $\mathrm{C}_{2}^{2-}$
b. $\mathrm{B}_{2}$
d. $\mathrm{OF}$

Key Concepts

Molecular Orbital Theory

Molecular Orbital Theory explains how atomic orbitals combine to form molecular orbitals that extend over the entire molecule. These molecular orbitals can be classified as bonding or antibonding, and electrons fill them according to their energies, which in turn determines the stability and characteristics of the bond between atoms.

Bond Order

Bond order is a quantitative measure of bond strength and stability, defined as half the difference between the number of electrons in bonding orbitals and the number in antibonding orbitals. A higher bond order indicates a stronger, more stable bond, while a lower bond order means a weaker bond.

Effect of Electron Removal on Bonding

The removal of an electron from a molecule affects bond strength depending on whether the electron is removed from a bonding or antibonding orbital. Removing an electron from a bonding orbital decreases the bond order and weakens the bond, whereas removing an electron from an antibonding orbital increases the bond order and can potentially strengthen the bond.

Ionization and Orbital Energy Considerations

When an electron is removed (ionization), its removal depends on the relative energies of the molecular orbitals. The change in electron configuration, particularly in regards to which orbital the electron is taken from, directly affects the overall stability and bond strength of the molecule. Understanding these orbital energy levels is crucial for predicting changes in bond strength upon ionization.

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