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Chapter 20: Problem 54

The \(\mathrm{N}_{2} \mathrm{O}\) molecule is linear and polar. a. On the basis of this experimental evidence, which arrangement, NNO or NON, is correct? Explain your answer. b. On the basis of your answer to part a, write the Lewis structure of \(\mathrm{N}_{2} \mathrm{O}\) (including resonance forms). Give the formal charge on each atom and the hybridization of the central atom. c. How would the multiple bonding in $$: \mathrm{N} \equiv \mathrm{N}-\mathrm{O}$$ be described in terms of orbitals?

Short Answer

Expert verified
The correct arrangement for the $\mathrm{N}_{2} \mathrm{O}$ molecule is NNO, as it results in a stable molecule with zero formal charges. The Lewis structure is N≡N-O with no resonance forms, and formal charges of N (0), N (0), and O (0). The central nitrogen atom has sp2 hybridization. The triple bond between the nitrogen atoms consists of one sigma (σ) bond formed by the overlap of sp2 hybrid orbitals and two pi (π) bonds formed by the side-by-side overlap of unhybridized p orbitals.

Step by step solution

01

Determine the correct arrangement of the N2O molecule

To decide whether the arrangement is NNO or NON, we must check which arrangement results in a polar molecule, since the problem tells us that the molecule is linear and polar.
02

Check polarity of the arrangements

For the NNO arrangement: Since N has a higher electronegativity than O (3.44 for N and 3.44 for O), the N-O bond will be polar with the electron density being pulled towards the N atom. Overall, this arrangement results in a polar molecule. For the NON arrangement: The molecule has a central N atom, so the N-O bond would be polar in the opposite direction compared to the N-N bond (nonpolar). This results in a net polarity in the molecule. Since both arrangements result in a polar molecule, we need to check other factors to determine the correct arrangement.
03

Check formal charges and stability of the molecule

For the NNO arrangement: There would be a triple bond between N atoms and a single bond between N and O atoms. Formal charge on each atom: N (0), N (0), O (0). This arrangement results in a stable molecule with zero formal charges. For the NON arrangement: There would be a single bond between N and O atoms and a single bond between N and N atoms. Formal charge on each atom: N (1-), N (1+), O (0). This arrangement results in an unstable molecule with nonzero formal charges. Since the NNO arrangement leads to a stable molecule with zero formal charges, it is the correct arrangement.
04

Draw the Lewis structure and provide the formal charges

The correct Lewis structure for \(\mathrm{N}_{2} \mathrm{O}\) is N≡N-O, and there are no resonance forms. Formal charges for each atom are N (0), N (0), and O (0).
05

Determine the hybridization of the central atom

In the N≡N-O structure, the central nitrogen atom is connected to two other atoms (N and O) and has one lone pair of electrons, making a total of 3 hybrid orbitals. This corresponds to sp2 hybridization for the central nitrogen atom.
06

Describe the multiple bonding in terms of orbitals

The triple bond between the two nitrogen atoms consists of one sigma (σ) bond and two pi (π) bonds. The σ bond is formed by the overlap of sp2 hybrid orbitals from both nitrogen atoms, while the two π bonds are formed by the side-by-side overlap of unhybridized p orbitals from each nitrogen atom.

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