Place the following molecules and ions in order from smallest to largest bond order: N22+, He2+, Cl2 H2-, O22-.

Verified step by step guidance

1. Bond order is calculated using the formula: Bond Order = (Number of bonding electrons - Number of antibonding electrons) / 2.
2. Determine the molecular orbital configuration for each species.
3. For N2^{2+}, remove two electrons from the highest occupied molecular orbitals of N2.
4. For He2^{+}, remove one electron from the highest occupied molecular orbital of He2.
5. For Cl2 and H2^{-}, use their respective molecular orbital configurations to calculate bond order.

Key Concepts

Bond Order

Bond order is a measure of the number of chemical bonds between a pair of atoms. It is calculated as the difference between the number of bonding electrons and the number of antibonding electrons, divided by two. A higher bond order indicates a stronger bond and typically a shorter bond length. Understanding bond order is essential for comparing the stability and size of different molecules and ions.

Molecular Orbital Theory

Molecular Orbital Theory explains how atomic orbitals combine to form molecular orbitals, which can be occupied by electrons. This theory helps predict the bond order and stability of molecules by considering the distribution of electrons in bonding and antibonding orbitals. It is particularly useful for understanding diatomic molecules and ions, as it provides insight into their electronic structure and reactivity.

Electron Configuration

Electron configuration describes the distribution of electrons in an atom or molecule's orbitals. For diatomic molecules, the arrangement of electrons in molecular orbitals determines their bond order and stability. Understanding the electron configuration of the given species is crucial for determining their bond orders and comparing their sizes, as it directly influences their chemical properties and behavior.