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Chapter 7: Q100E (page 405)

Identify the molecules with a dipole moment:

  1. \({\rm{S}}{{\rm{F}}_{\rm{4}}}\)
  2. \({\rm{C}}{{\rm{F}}_{\rm{4}}}\)
  3. \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{CCB}}{{\rm{r}}_{\rm{2}}}\)
  4. \({\rm{C}}{{\rm{H}}_{\rm{3}}}{\rm{Cl}}\)
  5. \({{\rm{H}}_{\rm{2}}}{\rm{CO}}\)

Short Answer

Expert verified

Following are the molecules with net dipole moment:-

\({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{CCB}}{{\rm{r}}_{\rm{2}}}{\rm{,C}}{{\rm{H}}_{\rm{3}}}{\rm{Cl }}\)\({{\rm{H}}_{\rm{2}}}{\rm{CO}}\)

Step by step solution

01

Concept Introduction

Dipole moments arises due to the difference of electronegativity. Higher the difference,higher is the dipole moment.

02

Identify the molecules with a dipole moment

Due to the difference in electronegativity between the bonded atoms\({\rm{(Cl,Br,and O to C) }}\), compounds like \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{CCB}}{{\rm{r}}_{\rm{2}}}{\rm{,C}}{{\rm{H}}_{\rm{3}}}{\rm{Cl }}\)\({{\rm{H}}_{\rm{2}}}{\rm{CO}}\)have a net dipole.

Therefore, although the atoms in \({\rm{S}}{{\rm{F}}_4}\)and \({\rm{C}}{{\rm{F}}_4}\)are electronegative, there is no net dipole since they are symmetrical (equal and opposite dipoles cancels out).

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Most popular questions from this chapter

Which atoms can bond to sulfur so as to produce a positive partial charge on the sulfur atom?

The molecule \({\rm{XC}}{{\rm{l}}_{\rm{2}}}\)has a dipole moment. Is X beryllium or sulfur?

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 \({\rm{MgO}}\)

Does a cation gain protons to form a positive charge or does it lose electrons?

Explain the difference between a nonpolar covalent bond, a polar covalent bond, and an ionic bond.
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