Experiment shows that $H_2O$ has a dipole moment while $CO_2$ does not. Point out the structures which best illustrate these facts.

If $B-Cl$ bond has a dipole moment,explain why $BCl_3$ molecule has zero dipole moment.

Give the correct order of initials $T$ or $F$ for the following statements. Use $T$ if the statement is true and $F$ if it is false.
$I. \, (CH_3)_2P(CF_3)_3$ is non-polar and $(CH_3)_3P(CF_3)_2$ is a polar molecule.
$II. \, CH_3 \widehat{P} CH_3$ bond angles are equal in the $(CH_3)_3P(CF_3)_2$ molecule.
$III. \, PF_3$ will be more soluble in a polar solvent than $SiF_4$.

Which of the following molecules has the maximum dipole moment?

Observe the following list of molecules. The number of polar and non-polar molecules are respectively: $NH_3, BF_3, NF_3, H_2S, CO_2, CH_4, CHCl_3, H_2O$

$A$ diatomic molecule has a dipole moment of $1.2 \ D$. If the bond distance is $1 \ \mathring{A}$,then fractional charge on each atom is.........$\times 10^{-2}$ (Given $1 \ D = 10^{-18} \ esu \ cm$ )