Identify the molecule with the highest dipole moment from the following:

Which is the correct order of dipole moments of $BF_3$,$NF_3$ and $NH_3$?

Each of the following options contains a set of four molecules. Identify the option$(s)$ where all four molecules possess a permanent dipole moment at room temperature.
$(1)$ $BeCl_2, CO_2, BCl_3, CHCl_3$
$(2)$ $SO_2, C_6H_5Cl, H_2Se, BrF_5$
$(3)$ $BF_3, O_3, SF_6, XeF_6$
$(4)$ $NO_2, NH_3, POCl_3, CH_3Cl$

Which of the following bonds will have the highest polarity?

If the bond length and dipole moment of a diatomic molecule are $1.25 \ \mathring{A}$ and $1.0 \ D$ respectively,what is the percent ionic character of the bond?

How many ions are non-polar ions?
$XeF_5^-, SO_3^{2-}, SO_4^{2-}, ClO_4^-, PO_4^{3-}, NO_2^+$