Which of the following molecules has the shortest nitrogen-nitrogen bond?

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11ecba2d_11fe_363f_a3bf_51c0a78a77cf_MD0008_00 Covalent bonds between atoms are formed by sharing electrons, which is made possible through the overlap of the atomic orbitals from each atom. Covalent bonds made by the end-to-end overlap of atomic orbitals are called sigma (σ) bonds whereas covalent bonds made by the side-to-side overlap of p orbitals are called pi (π) bonds. Although some atoms participate only in single covalent bonding (by σ bond), other atoms are capable of participating in multiple bonds (a double or triple bond) by the addition of one or more π bonds. In this way, a double bond consists of one σ bond and one π bond, and a triple bond consists of one σ bond and two π bonds. When comparing single, double, and triple covalent bonds involving the same two types of atoms, the bond length tends to decrease (relative to a single bond) with each added π bond. This occurs because of the shapes of the orbitals and because of the increased electron density between the atoms participating in multiple bonds. Of the given molecules, only N₂ has an N≡N triple bond (one σ bond and two π bonds); therefore, N₂ has the shortest of the nitrogen-nitrogen bonds shown. (Choices B, C, and D) In general, an N-N single bond is longer than an N=N double bond, and an N=N double bond is longer than an N≡N triple bond. Educational objective: Covalent bonds are formed by sharing electrons between atoms through the overlap of atomic orbitals in an end-to-end or side-to-side configuration. Multiple bonds formed by s and p orbitals consist of one σ bond and one or more π bonds, and bond length tends to decrease relative to a single bond with each added π bond.

Which of the Following Molecules Has the Shortest Nitrogen-Nitrogen Bond