bonding pairs and one lone pair in the Lewis structure.

It seems like you've missed to provide the full question. However, I can explain what bonding pairs and lone pairs are in a Lewis structure.

1. Identify the central atom in the molecule. This is usually the atom that can form the most bonds.

2. Draw a skeletal structure for the molecule. Connect the atoms with single bonds.

3. Count the total number of valence electrons in the molecule. This includes all the electrons in the outermost energy level of each atom.

4. Distribute the electrons among the atoms, giving octets (or duets for hydrogen) to as many atoms as possible. Each bond counts as two electrons.

5. Bonding pairs are the pairs of electrons that form a bond between two atoms. They are represented by a line in the Lewis structure.

6. Lone pairs are pairs of electrons that do not participate in bonding. They belong to a single atom. They are represented by a pair of dots next to the symbol of the atom in the Lewis structure.

7. If there are not enough electrons to give every atom an octet, try multiple bonds (double and triple).

Please provide more specific details or a specific molecule for a more detailed explanation.