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Chapter 10: Problem 73

Sketch the bond moments and resultant dipole moments for the following molecules: \(\mathrm{H}_{2} \mathrm{O}, \mathrm{PCl}_{3},\) \(\mathrm{XeF}_{4}, \mathrm{PCl}_{5}, \mathrm{SF}_{6}\)

Short Answer

Expert verified
The molecules \(H_2O\) and \(PCl_3\) have a net dipole moment making them polar, while the molecules \(XeF_4\), \(PCl_5\), and \(SF_6\) do not have a net dipole moment, hence they are nonpolar.

Step by step solution

01

Structure and Bond Moments of H2O

The molecular structure of water (\(H_2O\)) is bent or V-shaped due to the presence of two lone pairs of electrons on the Oxygen atom. The Oxygen - Hydrogen bonds create dipole moments due to the polarity (yet to opposite directions not on the same line, due to the V shape), which do not cancel each other out. This results in a net dipole moment in the molecule, making it polar.
02

Structure and Bond Moments of PCl3

The molecule phosphorous trichloride (\(PCl_3\)) exhibits a pyramid shaped structure with phosphorous in the center and three chlorine atoms around it. The bond moment between phosphorous and chlorine is directional and they do not cancel out because of the molecular geometry, resulting in a net dipole moment.
03

Structure and Bond Moments of XeF4

The molecular structure of xenon tetrafluoride (\(XeF_4\)) is square planar with xenon in the center and four fluorine atoms in the plane. Two lone pairs of electrons are present above and below the plane at xenon. The bond moments cancel each other because of the symmetry resulting in a nonpolar molecule and hence no dipole moment.
04

Structure and Bond Moments of PCl5

Phosphorous pentachloride (\(PCl_5\)) has a trigonal bipyramidal geometry. With phosphorous in the center and five chlorine atoms surrounding it. Given the symmetry in the molecule structure, the bond moments cancel out, hence resulting in no net molecular dipole moment.
05

Structure and Bond Moments of SF6

The molecular structure of sulfur hexafluoride (\(SF_6\)) is octahedral with sulfur in the center and six fluorine atoms surrounding it. As the structure of the molecule is symmetrical, the bond moments cancel each other out resulting in no molecular dipole moment. The molecule is nonpolar.

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Most popular questions from this chapter

Nitryl fluoride (FNO \(_{2}\) ) is very reactive chemically. The fluorine and oxygen atoms are bonded to the nitrogen atom. (a) Write a Lewis structure for FNO \(_{2}\). (b) Indicate the hybridization of the nitrogen atom. (c) Describe the bonding in terms of molecular orbital theory. Where would you expect delocalized molecular orbitals to form?

Briefly compare the VSEPR and hybridization approaches to the study of molecular geometry.

What is the relationship between the dipole moment and the bond moment? How is it possible for a molecule to have bond moments and yet be nonpolar?

What hybrid orbitals are used by nitrogen atoms in the following species? (a) \(\mathrm{NH}_{3}\), (b) \(\mathrm{H}_{2} \mathrm{~N}-\mathrm{NH}_{2}\) (c) \(\mathrm{NO}_{3}^{-}\)

Give the formula of an anion comprised of iodine and fluorine in which the iodine atom is \(s p^{3}\) \(d^{2}\) -hybridized.
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