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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

From its position in the periodic table, determine which atom in each pair is more electronegative: (a)\({\rm{Br or Cl}}\)(b)\({\rm{N or O}}\)(c)\({\rm{S or O}}\)(d)\({\rm{P or S}}\)(e)\({\rm{Si or N}}\)(f)\({\rm{Ba or P}}\)(g)\({\rm{N or K}}\).

Methanol,\({{\text{H}}_{\text{3}}}{\text{COH}}\), is used as the fuel in some race cars. Ethanol,\({{\text{C}}_{\text{2}}}{{\text{H}}_{\text{5}}}{\text{OH}}\), is used extensively as motor fuel in Brazil. Both methanol and ethanol produce\({\text{C}}{{\text{O}}_{\text{2}}}\)and\({{\text{H}}_{\text{2}}}{\text{O}}\)when they burn. Write the chemical equations for these combustion reactions using Lewis structures instead of chemical formulas.

Question: Which bond in each of the following pairs of bonds is the strongest?

(a) \({\rm{C - C}}\) or \({\rm{C = C}}\)

(b) \({\rm{C - N}}\) or \({\rm{C}} \equiv {\rm{N}}\)

(c) \({\rm{C}} \equiv {\rm{O}}\) or \({\rm{C = O}}\)

(d) \({\rm{H - F}}\) or \({\rm{H - Cl}}\)

(e) \({\rm{C - H}}\) or \({\rm{O - H}}\)

(f) \({\rm{C - N}}\) or \({\rm{C - O}}\)

Use the simulation (http://openstaxcollege.org/l/16MolecPolarity) to perform the following exercises for a real molecule. You may need to rotate the molecules in three dimensions to see certain dipoles. (a) Sketch the bond dipoles and molecular dipole (if any) for O3. Explain your observations. (b) Look at the bond dipoles for NH3. Use these dipoles to predict whether N or H is more electronegative. (c) Predict whether there should be a molecular dipole for NH3 and, if so, in which direction it will point. Check the molecular dipole box to test your hypothesis.

Write Lewis structures for the following: (a)\({\rm{Se}}{{\rm{F}}_{\rm{6}}}\)(b)\({\rm{Xe}}{{\rm{F}}_{\rm{4}}}\)(c)\({\rm{SeC}}{{\rm{l}}_{\rm{3}}}^{\rm{ + }}\)(d)\({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{BBC}}{{\rm{l}}_{\rm{2}}}\)(contains a\({\rm{B - B}}\)bond).
See all solutions

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