`BF_(1) and NF_(3)` both molecules, are covalent, but `BF_(3)` is non - polar and `NF_(3)` pole. Its reason is

NF_(3) is

Both BF_(3) and NF_(3) are covalent compounds. But BF_(3) is non - polar while NF_(3) is polar. This is because :

The molecules BF_3 and NF_3 are covalent compounds. But BF_3 is non-polar and NF_3 is polar. The reason is

A polar covalent bond with positive and negative charge centres at its ends is called a dipole. The polarity of a dipole is measured by its dipole moment. Mathematically it is expressed as dipole moment, mu=q xx d where q and d are the net charge and the distance between the two charges respectively. Dipole moment is a vector quantity. The net dipole moment of a polyatomic molecule is the resultant of the various bond moments present in the molecule. The values of dipole moment are expressed in Debye (D) or in SI units in terms of coulomb- metre (Cm). One of the most important applications of dipole moment is in the determination of geometry and shape of molecules besides prediction of a number of properties of the molecules. The molecules BF_3 and NH_3 both are covalent compounds but BF_3 is non-polar while NF_3 is polar . The reason is that

BF_(3) and NF_(3) both are covalent compounds but NF_(3) is polar whereas BF_(3) is non-polar. This is because :

BF_(3) and NF_(3) both are covalent compounds but NF_(3) is polar whereas BF_(3) is non-polar. This is because :