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Chapter 7: Q98E (page 404)

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

  1. \({{\rm{H}}_{\rm{3}}}{{\rm{O}}^{\rm{ + }}}\)
  2. \({\rm{PC}}{{\rm{l}}_{\rm{4}}}^{\rm{ - }}\)
  3. \({\rm{SnCl}}_{\rm{3}}^{\rm{ - }}\)
  4. \({\rm{BrCl}}_{\rm{4}}^{\rm{ - }}\)
  5. \({\rm{IC}}{{\rm{l}}_{\rm{3}}}\)
  6. \({\rm{Xe}}{{\rm{F}}_{\rm{4}}}\)
  7. \({\rm{S}}{{\rm{F}}_{\rm{2}}}\)

Short Answer

Expert verified

Polar bonding can be found in all of these compounds and ions\({{\rm{H}}_{\rm{3}}}{{\rm{O}}^{\rm{ + }}}{\rm{,PCl}}_{\rm{4}}^{\rm{ - }}{\rm{, and S}}{{\rm{F}}_{\rm{2}}}{\rm { have dipole moments}} {\rm{.}}\)

Step by step solution

01

Concept Introduction

Various substances includes bonds that are intermediate in character i.e; between pure covalent and pure ionic bonds. Here, polar bonds occur when one of the elements attracts the shared electrons much stringly than the other one.

02

Find the molecules and ions contain polar bonds

Polar bonding can be found in all of these compounds and ions\({{\rm{H}}_{\rm{3}}}{{\rm{O}}^{\rm{ + }}}{\rm{,PCl}}_{\rm{4}}^{\rm{ - }}{\rm{, and S}}{{\rm{F}}_{\rm{2}}}{\rm{ have dipole moments}}{\rm{.}}\)

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Most popular questions from this chapter

Question: Using the bond energies in Table \({\rm{7}}{\rm{.2}}\), determine the approximate enthalpy change for each of the following reactions:

(a) \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{(g) + 3}}{{\rm{F}}_{\rm{2}}}{\rm{(g)}} \to {\rm{2Cl}}{{\rm{F}}_{\rm{3}}}{\rm{(g)}}\)

(b) \({{\rm{H}}_{\rm{2}}}{\rm{C = C}}{{\rm{H}}_{\rm{2}}}{\rm{(g) + }}{{\rm{H}}_{\rm{2}}}{\rm{(g)}} \to {{\rm{H}}_{\rm{3}}}{\rm{CC}}{{\rm{H}}_{\rm{3}}}{\rm{(g)}}\)

(c) \({\rm{2}}{{\rm{C}}_{\rm{2}}}{{\rm{H}}_{\rm{6}}}{\rm{(g) + 7}}{{\rm{O}}_{\rm{2}}}{\rm{(g)}} \to {\rm{4C}}{{\rm{O}}_{\rm{2}}}{\rm{(g) + 6}}{{\rm{H}}_{\rm{2}}}{\rm{O(g)}}\)

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.

Write the resonance forms of ozone, \({{\rm{O}}_{\rm{3}}}\), the component of the upper atmosphere that protects the Earth from ultraviolet radiation.

Question: Using the standard enthalpy of formation data in Appendix G, calculate the bond energy of the carbon-sulphur double bond in \({\rm{C}}{{\rm{S}}_{\rm{2}}}\).

Predict the electron pair geometry and the molecular structure of each of the following molecules or ions:

(a)\({\rm{S}}{{\rm{F}}_{\rm{6}}}\)

(b)\({\rm{PC}}{{\rm{l}}_{\rm{5}}}\)

(c)\({\rm{Be}}{{\rm{H}}_{\rm{2}}}\)

(d) \({\rm{CH}}_{\rm{3}}^{\rm{ + }}\)
See all solutions

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