Question

Why is `N_2` a nonpolar covalent bond?

Answer 1

electronegativity

Explanation:

Because the electronegativity difference is zero. When the electronegativity is between 0 - 0.5 the bond would be considered as a covalent bond.

Answer 2

Well, from what does `"polarity"` result?

Explanation:

By definition, `"polarity"` is charge separation...and by way of example we could turn to highly polar molecules such as `H-Cl` and `H_2O`...for which we could represent the dipoles as `stackrel(""^+delta)H-stackrel(delta^-)Cl` or `stackrel(""^+delta)H-stackrel(delta^-)O-stackrel(delta^+)H`...the heteroatom is electronegative with respect to hydrogen, and thus strongly polarizes electron density towards itself to result in the given charge distribution....

On the other hand we gots a homonuclear diatomic molecule in dinitrogen. And since, CLEARLY, the nitrogen atoms are of EQUAL electronegativity there can be no question of unequal charge distribution, of polarity, in this molecule given this scenario...