Draw the Lewis Dot Structure for NO2 and Provide the Following Information

To draw the Lewis dot 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. Since there are two oxygen atoms, the total number of valence electrons is 5 + (6 × 2) = 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 lone pairs around the oxygen atoms to satisfy the octet rule. Each oxygen atom will have 3 lone pairs, and the nitrogen atom will have 1 lone pair.
5. Check for octet rule: Ensure that all atoms (except hydrogen) have 8 electrons around them. If not, form double bonds by converting lone pairs into bonding pairs.

Now, let’s answer the specific questions:

1. Number of atoms bonded to the central atom: There are 2 atoms (both oxygen) bonded to the central nitrogen atom.
2. Number of lone electron pairs on the central atom: The central nitrogen atom has 1 lone electron pair.
3. Hybridization of the central atom: The nitrogen atom is sp² hybridized.
4. Molecular shape: The molecular shape of NO₂ is bent or V-shaped.
5. Polarity: NO₂ is a polar molecule due to the presence of lone pairs on the nitrogen atom and the bent shape, which creates a dipole moment.