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Chapter 10: Problem 82

Which of the following molecules would you expect to be polar: (a) \(\mathrm{HCN} ;\) (b) \(\mathrm{SO}_{3} ;\) (c) \(\mathrm{CS}_{2} ;\) (d) OCS; (e) \(\operatorname{SOCl}_{2} ;\) (f) \(\operatorname{SiF}_{4} ;\) (g) \(\operatorname{POF}_{3}\) ? Give reasons for your conclusions.

Short Answer

Expert verified
(a) HCN is Polar (b) SO3 is Nonpolar (c) CS2 is Nonpolar (d) OCS is Polar (e) SOCl2 is Polar (f) SiF4 is Nonpolar (g) POF3 is Polar

Step by step solution

01

Analyze Molecular Structure - HCN

Hydrogen cyanide (HCN) has a linear structure, which means the hydrogen atom, carbon atom, and nitrogen atom are aligned in a straight line. Nitrogen is more electronegative than carbon, resulting in a dipole moment directed towards nitrogen. The carbon and hydrogen atoms, however, do not create a significant dipole due to the hydrogen's low electronegativity. So, HCN is a polar molecule as there is a net dipole.
02

Analyze Molecular Structure - SO3

Sulfur trioxide (SO3) is a planar molecule consisting of a sulfur atom bonded to three oxygen atoms, with no lone pairs of electrons on the sulfur. Here, the symmetry of the molecule cancels out any effects of individual bond dipoles, resulting in a nonpolar molecule.
03

Analyze Molecular Structure - CS2

Carbon disulfide (CS2) is a linear molecule consisting of a carbon atom with two sulfur atoms. The molecule is symmetrical, causing any polar bonds to cancel out; as such, CS2 is nonpolar.
04

Analyze Molecular Structure - OCS

OCS (carbonyl sulfide) has a linear molecular structure. Oxygen is more electronegative than sulfur, so the net dipole is from sulfur to oxygen, making it a polar molecule.
05

Analyze Molecular Structure - SOCl2

Sulfuryl chloride (SOCl2) is a polar compound because its structure is not symmetrical, and the individual bond dipoles do not cancel out. There are two chlorine atoms and an oxygen atom around the sulfur atom, and the oxygen atom has unpaired electrons that contribute to the net dipole moment of the molecule.
06

Analyze Molecular Structure - SiF4

Silicon tetrafluoride (SiF4) is a symmetrical molecule with silicon at the center and fluorine atoms at the corners of a regular tetrahedron. Each Si-F bond is polar, but the dipole moments cancel out due to the symmetry of the molecule. So, SiF4 is nonpolar.
07

Analyze Molecular Structure - POF3

Phosphoryl fluoride (POF3) has a trigonal pyramidal molecular structure. This molecule lacks symmetry, and hence POF3 is a polar molecule.

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Most popular questions from this chapter

Use the VSEPR theory to predict the shapes of the anions (a) \(\mathrm{ClO}_{4}^{-} ;\) (b) \(\mathrm{S}_{2} \mathrm{O}_{3}^{2-}\left(\text { that is, } \mathrm{SSO}_{3}^{2-}\right) ;\) (c) \(\mathrm{PF}_{6}^{-}\); (d) I \(_{3}^{-}\).

Through appropriate Lewis structures, show that the phenomenon of resonance is involved in the nitrite ion.

In your own words, define the following terms: (a) valence electrons; (b) electronegativity; (c) bonddissociation energy; (d) double covalent bond;(e) coordinate covalent bond.

Write plausible Lewis structures for the following molecules that contain only single covalent bonds. (a) \(\mathrm{FCl} ;\) (b) \(\mathrm{I}_{2} ;\) (c) \(\mathrm{SF}_{2} ;\) (d) \(\mathrm{NF}_{3} ;\) (e) \(\mathrm{H}_{2} \mathrm{Te}\).

Derive the correct formulas for the following ionic compounds by writing Lewis structures. (a) lithium sulfide; (b) sodium fluoride; (c) calcium iodide; (d) scandium chloride.
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