Draw the Lewis Structure for NO2, Predict the Electron Geometry and Molecular Geometry, and State Whether It Is Polar or Nonpolar

To draw the Lewis structure for NO₂, follow these steps:

1. Count the total number of valence electrons: Nitrogen (N) has 5 valence electrons, and each oxygen (O) has 6 valence electrons. Therefore, the total number of valence electrons is 5 + (2 × 6) = 17.
2. Determine the central atom: Nitrogen is the central atom because it is less electronegative than oxygen.
3. Draw the skeletal structure: Place the nitrogen atom in the center and connect it to the two oxygen atoms with single bonds.
4. Distribute the remaining electrons: After forming the single bonds, you have 13 electrons left. Place these electrons around the oxygen atoms to satisfy the octet rule. One oxygen will have a double bond with nitrogen, and the other will have a single bond with a lone pair on nitrogen.
5. Check for formal charges: Ensure that the formal charges are as low as possible. The structure with one double bond and one single bond minimizes formal charges.

Electron Geometry: The electron geometry of NO₂ is trigonal planar. This is because there are three regions of electron density around the central nitrogen atom (two bonding pairs and one lone pair).

Molecular Geometry: The molecular geometry of NO₂ is bent or V-shaped. This is due to the presence of one lone pair on the nitrogen atom, which repels the bonding pairs, causing the molecule to bend.

Polarity: NO₂ is a polar molecule. The bent shape and the difference in electronegativity between nitrogen and oxygen create a dipole moment, making the molecule polar.