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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

Which compound in each of the following pairs has the larger lattice energy? Note: \({\rm{M}}{{\rm{g}}^{{\rm{2 + }}}}\) and \({\rm{L}}{{\rm{i}}^{\rm{ + }}}\) have similar radii; \({{\rm{O}}^{{\rm{2 - }}}}\) and \({{\rm{F}}^{\rm{ - }}}\) have similar radii. Explain your choices.

(a) \({\rm{MgO}}\) or \({\rm{MgSe}}\)

(b) \({\rm{LiF}}\) or \({\rm{MgO}}\)

(c) \({\rm{L}}{{\rm{i}}_{\rm{2}}}{\rm{O}}\) or \({\rm{LiCl}}\)

(d) \({\rm{L}}{{\rm{i}}_{\rm{2}}}{\rm{Se}}\) or \({\rm{MgO}}\)

Which is the most polar bond? (a) \({\rm{C - C}}\) (b) \({\rm{C - H}}\) (c) \({\rm{N - H}}\) (d) \({\rm{O - H}}\) (e) \({\rm{Se - H}}\) .

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

  1. \({\rm{IO}}{{\rm{F}}_{\rm{5}}}\)(I is the central atom)
  2. \({\rm{POC}}{{\rm{l}}_{\rm{3}}}\)(P is the central atom)
  3. \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{SeO}}\)(Se is the central atom)
  4. \({\rm{ClS}}{{\rm{O}}^{\rm{ + }}}\)(S is the central atom)
  5. \({{\rm{F}}_{\rm{2}}}{\rm{SO}}\)(S is the central atom)
  6. \({\rm{N}}{{\rm{O}}_{\rm{2}}}^{\rm{ - }}\)
  7. \({\rm{SiO}}_{\rm{4}}^{{\rm{4 - }}}\)

The lattice energy of \({\rm{LiF}}\) is \({\rm{1023 kJ/mol}}\), and the \({\rm{Li - F}}\) distance is \({\rm{200}}{\rm{.8 pm}}\). \({\rm{NaF}}\) crystallizes in the same structure as \({\rm{LiF}}\) but with a \({\rm{Na - F}}\) distance of \({\rm{231 pm}}\). Which of the following values most closely approximates the lattice energy of \({\rm{NaF}}\): \({\rm{510, 890, 1023, 1175,}}\) or \({\rm{4090 kJ/mol}}\)? Explain your choice.

Use the Molecule Shape simulator (http://openstaxcollege.org/l/16MolecShape) to explore real molecules. On the Real Molecules tab, select “model” mode and S2O. What is the model bond angle? Explain whether the “real” bond angle should be larger or smaller than the ideal model angle.
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