Question

what is the overall polarity of this molecule? polar nonpolar

Explanation:

• For a molecule to be polar, there must be a significant difference in electronegativity between the atoms and an asymmetrical molecular geometry so that the dipoles do not cancel out.
• In the case of \(N_2\) (\(\colon N\equiv N\colon\)), the two nitrogen atoms are identical. They have the same electronegativity.
• The bond between them is a non - polar covalent bond. Also, the linear geometry of the \(N_2\) molecule (since there are only two atoms) means that there is no overall dipole moment. Any small charge separation (which is actually zero in this case due to identical atoms) is symmetrically distributed.

Answer:

nonpolar