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Chapter 10: Problem 136

Which molecule is nonlinear? (a) \(\mathrm{SO}_{2} ;\) (b) \(\mathrm{CO}_{2}\); (c) HCN; (d) NO.

Short Answer

Expert verified
The nonlinear molecules are SO2 and NO.

Step by step solution

01

Draw Lewis structure for SO2

The molecule has one sulfur atom and two oxygen atoms. Sulfur, being electropositive, is in the center. Each oxygen atom is connected to the sulfur by a double bond, making four shared pairs. Sulfur also has one lone pair. The spatial configuration of a molecule with a central atom that possesses one lone pair and two bond pairs is bent or V-shaped.
02

Draw Lewis structure for CO2

This molecule consists of one carbon atom and two oxygen atoms. Carbon, being less electronegative, is located in the center. Both oxygen atoms are connected to the carbon by double bonds, making four shared pairs. There are no lone pairs in the carbon atom, so the molecule is linear.
03

Draw Lewis structure for HCN

In this molecule, carbon forms a triple bond with nitrogen and a single bond with hydrogen. The negative end of the molecule extends towards the nitrogen, not the hydrogen, which implies it is a linear molecule.
04

Draw Lewis structure for NO

In the molecule, nitrogen makes a double bond with an oxygen molecule. Nitrogen has a lone pair of electrons, and oxygen also has two lone pairs of electrons. This arrangement makes the molecule bent or nonlinear.
05

Identify nonlinear molecule

After drawing the Lewis structures and determining the shape of each given molecule, the molecules that are nonlinear are SO2 and NO.

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Most popular questions from this chapter

Which of the following species would you expect to be diamagnetic and which paramagnetic: (a) \(\mathrm{OH}^{-} ;\) (b) \(\mathrm{OH} ;(\mathrm{c}) \mathrm{NO}_{3} ;(\mathrm{d}) \mathrm{SO}_{3} ;(\mathrm{e}) \mathrm{SO}_{3}^{2-} ;(\mathrm{f}) \mathrm{HO}_{2} ?\)

Sketch the propyne molecule, \(\mathrm{CH}_{3} \mathrm{C} \equiv \mathrm{CH}\). Indicate the bond angles in this molecule. What is the maximum number of atoms that can be in the same plane?

Predict the geometric shapes of (a) \(\mathrm{CO} ;\) (b) \(\mathrm{SiCl}_{4}\); (c) \(\mathrm{PH}_{3} ;\) (d) \(\mathrm{ICl}_{3} ;\) (e) \(\mathrm{SbCl}_{5} ;\) (f) \(\mathrm{SO}_{2} ;\) (g) \(\mathrm{AlF}_{6}^{3-}\).

Draw plausible Lewis structures for the following species; use expanded valence shells where necessary. (a) \(\mathrm{Cl}_{2} \mathrm{O} ;\) (b) \(\mathrm{PF}_{3} ;\) (c) \(\mathrm{CO}_{3}^{2-} ;\) (d) \(\mathrm{BrF}_{5}\).

Use the VSEPR theory to predict the shape of (a) the molecule OSF \(_{2} ;\) (b) the molecule \(\mathrm{O}_{2} \mathrm{SF}_{2} ;\) (c) the ion \(\mathrm{SF}_{5}^{-} ;\) (d) the ion \(\mathrm{ClO}_{4}^{-} ;\) (e) the ion \(\mathrm{ClO}_{3}^{-}\).
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