Two different compounds exist having the formula $\mathrm{N}_{2} \mathrm{F}_{2}$ . One compound is polar whereas the other is nonpolar. Draw Lewis structures for \(\mathrm{N}_{2} \mathrm{F}_{2}\) consistent with these observations.

Polarity occurs in a molecule when there is an unequal distribution of electron density, resulting in a molecular dipole moment, caused by atoms with different electronegativities bonded together or a non-symmetrical arrangement of atoms. A polar molecule will have a partial positive charge on one side and a partial negative charge on the other side. On the other hand, a nonpolar molecule has no net molecular dipole moment, and its electron distribution is symmetrical.

To draw a Lewis structure for the polar \(\mathrm{N}_{2}\mathrm{F}_{2}\) compound, we need to create a structure where there is an unequal distribution of electron density. The most likely structure that satisfies this condition is a bent geometry. Here's how to draw the polar Lewis structure: 1. Place an N atom at the central position and connect it with the other N atom. 2. Attach one F atom to each N atom. 3. Complete octets for all atoms by adding lone pairs of electrons. N atoms will have one lone pair and F atoms will have three lone pairs each. The resulting structure is: ``` F F \ / N - N / \ F F ``` In this structure, the electron density is not distributed symmetrically, and there is a net molecular dipole moment, making it a polar molecule.

To draw a Lewis structure for the nonpolar \(\mathrm{N}_{2}\mathrm{F}_{2}\) compound, we need an arrangement of atoms that leads to a symmetrical electron distribution and no net molecular dipole moment. Here's how to draw the nonpolar Lewis structure: 1. Place an N atom at the central position and connect it with the other N atom via a double bond. 2. Attach one F atom to each N atom. 3. Complete octets for all atoms by adding lone pairs of electrons. N atoms will have one lone pair and F atoms will have three lone pairs each. The resulting structure is: ``` F F \ / N = N / \ F F ``` In this structure, the electron density is distributed symmetrically, and there is no net molecular dipole moment, making it a nonpolar molecule. In summary, we have drawn two different Lewis structures for \(\mathrm{N}_{2}\mathrm{F}_{2}\): one with a bent geometry being polar and the other with a linear geometry being nonpolar.