Place the species below in order of the shortest to the...

Place the species below in order of the shortest to the longest nitrogen-oxygen bond. $\begin{array}{lllll}\mathrm{H}_{2} \mathrm{NOH}, & \mathrm{N}_{2} \mathrm{O}, & \mathrm{NO}^{+}, & \mathrm{NO}_{2}^{-}, & \mathrm{NO}_{3}^{-}\end{array}$ $\left(\mathrm{H}_{2} \mathrm{NOH}\right.$ exists as $\mathrm{H}_{2} \mathrm{~N}-\mathrm{OH} .$.

Place the species below in order of the shortest to the longest nitrogen-oxygen bond.
$\begin{array}{lllll}\mathrm{H}_{2} \mathrm{NOH}, & \mathrm{N}_{2} \mathrm{O}, & \mathrm{NO}^{+}, & \mathrm{NO}_{2}^{-}, & \mathrm{NO}_{3}^{-}\end{array}$
$\left(\mathrm{H}_{2} \mathrm{NOH}\right.$ exists as $\mathrm{H}_{2} \mathrm{~N}-\mathrm{OH} .$.

Key Concepts

Bond Order

Bond order is the number of chemical bonds between a pair of atoms. It is directly related to bond length, where a higher bond order (indicative of multiple bonds such as double or triple bonds) typically results in a shorter bond length because of increased electron density between the nuclei.

Resonance and Electron Delocalization

Resonance involves the depiction of a molecule by two or more valid Lewis structures that differ only in the position of electrons. In molecules with resonance, the actual bond characteristics are an average of the resonance forms, leading to intermediate bond orders and bond lengths as the electrons are delocalized over several atoms.

Formal Charge Distribution

Formal charge distribution affects the electron density around atoms within a molecule. The presence of positive or negative charges can alter bond strength by either drawing electrons closer or pushing them away, which in turn influences the bond order and the resulting bond length.

Molecular Structure and Bonding

The molecular structure, including the types of bonds (single, double, etc.) and the geometric arrangement of atoms, plays a crucial role in determining the bond order. Variations in bond types and arrangements, such as those found in different ions or molecules, lead to differences in bond lengths as the electron density is differently distributed along the bond axes.

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