Lewis structures are diagrams that represent the bonding between atoms of a molecule and the lone pairs of electrons that may exist. Here’s how to write Lewis structures for the following molecules:
a. HNNH
1. Count the total number of valence electrons: H (1) + N (5) + N (5) + H (1) = 12 electrons.
2. Place the atoms in a linear arrangement: H-N-N-H.
3. Connect the atoms with single bonds: H-N-N-H.
4. Distribute the remaining electrons as lone pairs: Each nitrogen has one lone pair.
b. H2CNH
1. Count the total number of valence electrons: H (1) + H (1) + C (4) + N (5) + H (1) = 12 electrons.
2. Place the atoms: H-C-N-H.
3. Connect the atoms with single bonds: H-C-N-H.
4. Distribute the remaining electrons: Carbon has no lone pairs, nitrogen has one lone pair.
c. NO
1. Count the total number of valence electrons: N (5) + O (6) = 11 electrons.
2. Place the atoms: N-O.
3. Connect the atoms with a double bond: N=O.
4. Distribute the remaining electrons: Nitrogen has one lone pair, oxygen has two lone pairs.
d. N2
1. Count the total number of valence electrons: N (5) + N (5) = 10 electrons.
2. Place the atoms: N-N.
3. Connect the atoms with a triple bond: N≡N.
4. Distribute the remaining electrons: Each nitrogen has one lone pair.
e. CO
1. Count the total number of valence electrons: C (4) + O (6) = 10 electrons.
2. Place the atoms: C-O.
3. Connect the atoms with a triple bond: C≡O.
4. Distribute the remaining electrons: Carbon has no lone pairs, oxygen has two lone pairs.
f. CN
1. Count the total number of valence electrons: C (4) + N (5) = 9 electrons.
2. Place the atoms: C-N.
3. Connect the atoms with a triple bond: C≡N.
4. Distribute the remaining electrons: Carbon has no lone pairs, nitrogen has one lone pair.