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Chapter 10: Problem 84

Refer to the Integrative Example. A compound related to nitryl fluoride is nitrosyl fluoride, FNO. For this molecule, indicate (a) a plausible Lewis structure and (b) the geometric shape. (c) Explain why the measured resultant dipole moment for FNO is larger than the value for \(\mathrm{FNO}_{2}\).

Short Answer

Expert verified
The Lewis structure for FNO molecule has N in the middle bonded with F on one side and O on the other, with N-F having a single bond, and N-O having a double bond. It has a bent geomertric shape due to three regions of electron density around the central N atom. The dipole moment for FNO is larger than that of \(\mathrm{FNO_{2}}\) because FNO, being a bent molecule, has a net dipole moment, whereas in \(\mathrm{FNO_{2}}\), the linear structure can lead to dipole cancellation leading to a smaller dipole moment overall.

Step by step solution

01

Finding a Plausible Lewis Structure

In order to draw a plausible Lewis structure for FNO, you need to calculate the total number of valence electrons in the molecule. The molecule is composed of fluorine (F) which has 7 valence electrons, nitrogen (N) with 5 valence electrons, and oxygen (O) also with 6 valence electrons. This gives a total of 18 valence electrons. A plausible Lewis structure would be N in the middle bonded with F on one side and O on the other, with N-F having a single bond, and N-O having a double bond. Remaining electrons are then distributed as lone pairs on F and O, both having three lone pairs.
02

Determining Geometric Shape

The central atom (N) has three regions of electron density (one single bond, one double bond, and one lone pair). Applying the VSEPR theory, the molecule has a bent shape or V-shape with the angle slightly less than 120 degrees due to the presence of the lone pair.
03

Explaining Dipole Moment Comparison

\(\mathrm{FNO}\) being a bent molecule, it has a dipole moment since the pull of electron density is not symmetric around the molecule. On the other hand, for \(\mathrm{FNO_{2}}\), if the molecule is in a linear configuration, it could have a resultant dipole moment of zero as the pull of electron density from each side could cancel each other. Hence, \(\mathrm{FNO}\) is expected to have a larger dipole moment when compared to \(\mathrm{FNO_{2}}\).

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Most popular questions from this chapter

Use VSEPR theory to predict the geometric shapes of the following molecules and ions: (a) \(\mathrm{PCl}_{3} ;\) (b) \(\mathrm{SO}_{4}^{2-}\); (c) \(\mathrm{SOCl}_{2} ;\) (d) \(\mathrm{SO}_{3} ;\) (e) \(\mathrm{BrF}_{4}^{+}\).

One of the isomers of chloromethanol has the formula $\mathrm{ClCH}_{2} \mathrm{OH} .$ Sketch, by using the dash and wedge symbolism, this isomer of chloromethanol, and indicate the various bond angles.

Write Lewis symbols for the following ions. (a) \(\mathrm{H}^{-}\) (b) \(\operatorname{Sn}^{2+} ;\) (c) \(\mathrm{K}^{+} ;\) (d) \(\mathrm{Br}^{-} ;\) (e) \(\mathrm{Se}^{2-} ;\) (f) \(\mathrm{Sc}^{3+}\).

Comment on the similarities and differences in the molecular structure of the following triatomic species: \(\mathrm{CO}_{2}, \mathrm{NO}_{2}^{-}, \mathrm{O}_{3},\) and \(\mathrm{ClO}_{2}^{-}\).

Which of the following species requires a resonance hybrid for its Lewis structure: (a) \(\mathrm{CO}_{2},\) (b) \(\mathrm{OCl}^{-}\) (c) \(\mathrm{CO}_{3}^{2-},\) or \((\mathrm{d}) \mathrm{OH}^{-} ?\) Explain.
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