How do you draw the lewis structure for NO₂?

To draw the Lewis structure for nitrogen dioxide (NO₂), follow these steps:

Step 1: Count the 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 (from N) + 6 (from O) + 6 (from O) = 17 valence electrons

Step 2: Determine the Central Atom

The nitrogen atom is less electronegative than oxygen, so it will be the central atom in the structure.

Step 3: Connect Atoms with Bonds

Place the nitrogen atom in the center and connect each oxygen atom to it with a single bond:

• Each bond uses 2 electrons, so 2 bonds use 4 electrons.

Step 4: Distribute Remaining Electrons

After forming the bonds, you have:

• 17 total electrons - 4 used in bonds = 13 electrons remaining.

Distribute these remaining electrons to the oxygen atoms to satisfy their octets. Start by giving each oxygen atom 6 electrons (3 lone pairs) to complete their octets.

Step 5: Check for Octet Rule

At this point, the oxygen atoms have complete octets, but nitrogen only has 4 electrons. To satisfy nitrogen's octet, you can form a double bond with one of the oxygen atoms:

• Change one lone pair from that oxygen into a bonding pair with nitrogen.

Final Structure

The final Lewis structure for NO₂ shows nitrogen in the center, bonded to one oxygen with a double bond and to the other oxygen with a single bond. The structure looks like this:

• N with a double bond to O and a single bond to O, with the single-bonded oxygen having three lone pairs.

This arrangement satisfies the octet rule for all atoms involved. Remember to check that the total number of electrons used matches the total valence electrons counted initially!