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Chapter 7: Q99E (page 404)

Which of the following molecules have dipole moments?

  1. \({\rm{C}}{{\rm{S}}_{\rm{2}}}\)
  2. \({\rm{Se}}{{\rm{S}}_{\rm{2}}}\)
  3. \({\rm{CC}}{{\rm{l}}_{\rm{2}}}{\rm{\;}}{{\rm{F}}_{\rm{2}}}\)
  4. \({\rm{PC}}{{\rm{l}}_{\rm{3}}}{\rm{(P is the central atom)}}\)
  5. \({\rm{ClNO (N is the central atom)}}\)

Short Answer

Expert verified

The \({\rm{Se}}{{\rm{S}}_{\rm{2}}}{\rm{,CC}}{{\rm{l}}_{\rm{2}}}{\rm{\;}}{{\rm{F}}_{\rm{2}}}{\rm{,PC}}{{\rm{l}}_{\rm{3}}}{\rm{ and CINO}}\) have moments of dipole.

Step by step solution

01

Concept Introduction

A dipole moment occurs in any system which have separation of charges. Therefore it can arise in ionic bonds as well as in covalent bonds.

02

Find molecules have dipole moments of \({\rm{C}}{{\rm{S}}_{\rm{2}}}\)

a.

There is no dipole moment in \({\rm{C}}{{\rm{S}}_{\rm{2}}}\)because it is linear.

03

Find molecules have dipole moments of \({\rm{Se}}{{\rm{S}}_{\rm{2}}}\)

b. \({\rm{Se}}{{\rm{S}}_{\rm{2}}}\)is bent. As a result, there is an overall dipole moment.

04

Find molecules have dipole moments of \({\rm{CC}}{{\rm{l}}_{\rm{2}}}{\rm{\;}}{{\rm{F}}_{\rm{2}}}\)

c. The dipoles of the CCl and CF bonds are not totally cancelled, hence they are not balanced. It possesses a dipole moment as a result.

05

Find molecules have dipole moments of \({\rm{PC}}{{\rm{l}}_{\rm{3}}}\)

d.

\({\rm{PC}}{{\rm{l}}_{\rm{3}}}\)Is a trigonal pyramidal structure. The dipoles of the bonds do not cancel due to this form, thus there is an overall dipole moment

06

Find molecules have dipole moments of \({\rm{ClNO}}\)

e. A dipole moment is created when the CINO molecule is bent.

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Most popular questions from this chapter

Identify the molecules with a dipole moment:

  1. \({\rm{S}}{{\rm{F}}_{\rm{4}}}\)
  2. \({\rm{C}}{{\rm{F}}_{\rm{4}}}\)
  3. \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{CCB}}{{\rm{r}}_{\rm{2}}}\)
  4. \({\rm{C}}{{\rm{H}}_{\rm{3}}}{\rm{Cl}}\)
  5. \({{\rm{H}}_{\rm{2}}}{\rm{CO}}\)

Describe the molecular structure around the indicated atom or atoms:

  1. The sulfur atom in sulfuric acid, H2SO4 [ (HO)2 SO2]

  2. The chlorine atom in chloric acid, HClO3 [HOClO2]

  3. The oxygen atom in Hydrogen peroxide, HOOH

  4. The nitrogen atom in nitric acid, HNO3 [HONO2]

  5. The oxygen atom in OH group in nitric acid, HNO3 [HONO2]

  6. The central oxygen atom in the ozone molecule, O3

  7. Each of the carbon atoms in the propyne, CH3 CCH

  8. The carbon atom in Freon, CCl2 F2

  9. each of the carbon atoms in allene H2CCCH2

In terms of the bonds present, explain why acetic acid, \(C{H_3}C{O_2}H\), contains two distinct types of carbon-oxygen bonds, whereas the acetate ion, formed by loss of a hydrogen ion from acetic acid, only contains one type of carbon-oxygen bond. The skeleton structures of these species are shown:

Write Lewis structures for: (a) \({\rm{P}}{{\rm{O}}_{\rm{4}}}^{{\rm{3 - }}}\) (b) \({\rm{IC}}{{\rm{I}}_{\rm{4}}}^{\rm{ - }}\) (c) \({\rm{S}}{{\rm{O}}_{\rm{3}}}^{{\rm{2 - }}}\) (d) \({\rm{HONO}}\) .

A compound with a molar mass of about\({\rm{42 g/mol}}\)contains\({\rm{85}}{\rm{.7 \% }}\)carbon and\({\rm{14}}{\rm{.3 \% }}\)hydrogen by mass. Write the Lewis structure for a molecule of the compound.
See all solutions

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