Q100E - Chemistry (OpenStax)

Question

 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. \({{\rm{H}}_{\rm{2}}}{\rm{CO}}\)

Step-by-Step Solution

Answer

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 1: Concept Introduction

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

Step 2: 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).