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Chapter 7: Q97E (page 404)

Which of the following molecules and ions contain polar bonds? Which of these molecules and ions have dipole moments?

  1. \({\rm{Cl}}{{\rm{F}}_{\rm{5}}}\)
  2. \({\rm{Cl}}{{\rm{O}}_{\rm{2}}}{\rm{ - }}\)
  3. \({\rm{TeC}}{{\rm{l}}_{\rm{4}}}^{{\rm{2 - }}}\)
  4. \({\rm{PC}}{{\rm{l}}_{\rm{3}}}\)
  5. \({\rm{Se}}{{\rm{F}}_{\rm{4}}}\)
  6. \({\rm{P}}{{\rm{H}}_{\rm{2}}}^{\rm{ - }}\)
  7. \({\rm{Xe}}{{\rm{F}}_{\rm{2}}}\)

Short Answer

Expert verified

The following molecules and ions contain polar bonds:\({\rm{Cl}}{{\rm{F}}_{\rm{5}}}{\rm{,Cl}}{{\rm{O}}_{\rm{2}}}{\rm{ - ,PC}}{{\rm{l}}_{\rm{3}}}{\rm{,Se}}{{\rm{F}}_{\rm{4}}}{\rm{, and P}}{{\rm{H}}_{\rm{2}}}{\rm{.}}\)

Step by step solution

01

Concept Introduction

A polar bond is one of the types of covalent bond in which the electrons forming the bond are distributed unequally.

02

Molecules and ions that contain polar bonds

Polar bonding can be found in all of these compounds and ions \({\rm{Cl}}{{\rm{F}}_{\rm{5}}}{\rm{,Cl}}{{\rm{O}}_{\rm{2}}}{\rm{ - ,PC}}{{\rm{l}}_{\rm{3}}}{\rm{,Se}}{{\rm{F}}_{\rm{4}}}{\rm{, and P}}{{\rm{H}}_{\rm{2}}}{\rm{ - have dipole moments}}{\rm{.}}\)

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Most popular questions from this chapter

Predict which of the following compounds are ionic and which are covalent, based on the location of their constituent atoms in the periodic table:

(a) \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{CO}}\) (b) \({\rm{MnO}}\) (c) \({\rm{NC}}{{\rm{l}}_{\rm{3}}}\) (d) \({\rm{CoB}}{{\rm{r}}_{\rm{2}}}\) (e) \({{\rm{K}}_{\rm{2}}}{\rm{S}}\) (f) \({\rm{CO}}\) (g) \({\rm{Ca}}{{\rm{F}}_{\rm{2}}}\) (h) \({\rm{HI}}\) (i) \({\rm{CaO}}\) (j) \({\rm{IBr}}\) (k) \({\rm{C}}{{\rm{O}}_{\rm{2}}}\) .

Write the electron configuration for the monatomic ions formed from the following elements (which form the greatest concentration of monatomic ions in seawater): (a) \({\rm{Cl}}\) (b) \({\rm{Na}}\) (c) \({\rm{Mg}}\)(d) \({\rm{Ca}}\) (e) \({\rm{K}}\) (f) \({\rm{Br}}\) (g) \({\rm{Sr}}\) (h) \({\rm{F}}\).

Use the Molecule Shape simulator (http://openstaxcollege.org/l/16MolecShape) to build a molecule. Starting with the central atom, click on the double bond to add one double bond. Then add one single bond and one lone pair. Rotate the molecule to observe the complete geometry. Name the electron group geometry and molecular structure and predict the bond angle. Then click the check boxes at the bottom and right of the simulator to check your answers.

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:

What is the molecular structure of the stable form of \({\rm{FN}}{{\rm{O}}_{\rm{2}}}\) ? (\({\rm{N}}\)is the central atom.)
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