Explain why `BeH_2` molecule has zero diple moment even though the `Be-H` bond are polar.

The dipole moment of BF_3 is zero eventhough the B-F bonds are polar, Justify.

If a molecule MX _(3) has zero dipole moment, the sigma bonding oritals used by Mere

Assertion: CO_2 is non polar, while ROR is polar in nature. Reason: The dipole moments of two CO bonds are equal and opposite to each other in CO_2 , while in R-O-R molecules two dipoles of the R-O bonds are inclined to each other at an angle of 110°.

Which one of the following molecules has the largest dipole moment? (Electro-negativity values of elements concerned are: B=2.0, Cl=3.0, F=4.0, H=2.1, N=3.0, O=3.5, P=2.1, S=2.5)

The net dipole moment of a polyatomic molecule depends on the spatial arrangement of various bonds in the molecule. The dipole moment of BF_3 is zero while that of NF_3 is not zero. Justify

Which of the following molecules has polar bonds but zero dipole moment ?