1. Draw the Lewis Structure:
* Count valence electrons: N (5 valence electrons) x 2 + O (6 valence electrons) = 16 valence electrons.
* Central atom: Nitrogen is less electronegative than oxygen, so it's the central atom.
* Connect with single bonds: N-N-O
* Complete octets: The structure will look like this:
* N = N = O (with a lone pair on each terminal N and O)
2. Calculate Formal Charges:
* Formal Charge = (Valence Electrons) - (Non-bonding Electrons) - (1/2 Bonding Electrons)
* For the leftmost N: 5 - 2 - (1/2)4 = 0
* For the central N: 5 - 0 - (1/2)8 = +1
* For the O: 6 - 4 - (1/2)4 = 0
3. Resonance Structures:
There are two resonance structures for N₂O:
* Structure 1: N = N = O
* Structure 2: N - N ≡ O
4. Determine Bond Orders:
* Bond order = (Number of bonds between two atoms) / (Number of resonance structures)
* N-N bond:
* Structure 1: Double bond (2)
* Structure 2: Single bond (1)
* Average bond order = (2 + 1) / 2 = 1.5
* N-O bond:
* Structure 1: Double bond (2)
* Structure 2: Triple bond (3)
* Average bond order = (2 + 3) / 2 = 2.5
Therefore, the bond order of the N-N bond in N₂O is 1.5, and the bond order of the N-O bond is 2.5.
