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Chapter 7: Q89E (page 402)

Explain how a molecule that contains polar bonds can be nonpolar.

Short Answer

Expert verified

Since, the polar bonds lie at opposite directions hence they cancel out each other and a molecule that contains polar bonds becomes nonpolar.

Step by step solution

01

Concept Introduction

A molecule is a group of atoms joined together by chemical bonds; the term might include ions that meet this condition depending on the context.

02

Non-polarity of polar bonds

This case can arise in the situation when two identical atoms are found across the central atom from one another. So, in this case although each bond with central atom is polar but overallmolecule is non-polar as polarity of both bonds are in opposite direction and it cancels each other out.

Therefore, due to bonds being on opposite side the whole molecule becomes non-polar.

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Most popular questions from this chapter

Correct the following statement: 鈥淭he bonds in solid\({\text{PbC}}{{\text{I}}_{\text{2}}}\)are ionic; the bond in a\({\text{HCl}}\)molecule is covalent. Thus, all of the valence electrons in\({\text{PbC}}{{\text{I}}_{\text{2}}}\)are located on the\({\text{C}}{{\text{I}}^{\text{ - }}}\)ions, and all of the valence electrons in a\({\text{HCl}}\)molecule are shared between the\({\text{H}}\)and\({\text{CI}}\)atoms.鈥�

Write the Lewis structures for the following, and include resonance structures where appropriate. Indicate which has the strongest carbon-oxygen bond.

(a) \(C{O_2}\)

(b) \(CO\)

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.

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. \({\rm{Xe}}{{\rm{F}}_{\rm{2}}}\)

The molecule XF3 has a dipole moment. Is X boron or phosphorus?
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