Classify each molecule as polar or nonpolar.
(a) \(\mathrm{N}_{2} \mathrm{H}_{2}\)
(b) \(\mathrm{H}_{2} \mathrm{O}_{2}\)
(c) \(\mathrm{CF}_{4}\)
(d) \(\mathrm{NO}_{2}\)
Step 1 of 4
a)
Polar compounds:
The electronegative difference between the species in the range of 0.3 to 1.4 is considered polar compounds.
Example: \(\mathrm{HCl}\) and \(\mathrm{HF}\)
Nonpolar compounds:
The electronegative differences between the species in the range of 0 to 0.2 are considered as non-polar compounds.
The given molecule \(\mathrm{N}_{2} \mathrm{H}_{2}\).
The electronegativity of nitrogen - 3.0
The electronegativity of hydrogen - 2.1
Total difference - 0.9
The shape of molecules with bond dipoles \(\mathrm{N}_{2} \mathrm{H}_{2}\) is as follows.
Shape of the molecule is nonlinear.
In the transform of the molecule, the net dipole moment is zero therefore, the given molecule is non - polar in the transform.
The net dipole moment is non - zero in cis form.
Therefore, the given molecule is polar in the cis form.
