To draw the Lewis structure for the following molecules, follow these steps:
1. Count the total number of valence electrons for the molecule.
2. Arrange the atoms with the least electronegative atom in the center.
3. Distribute the electrons among the atoms, first by placing pairs between bonded atoms, then completing the octets for outer atoms.
4. If there are not enough electrons to complete the octets, form double or triple bonds as needed.
For example, let's consider molecule A: CO2.
1. Total valence electrons: C (4) + 2 * O (6) = 4 + 12 = 16 electrons
2. Place the least electronegative atom (C) in the center: O-C-O
3. Distribute electrons:
O-C-O (4 used)
O:C:O (8 used)
4. Form double bonds to complete octets:
O::C::O (16 used)
Lewis structure for CO2: O::C::O
Repeat this process for each molecule. Once you have the Lewis structures, you can match them with their structural characteristics, such as molecular geometry, bond angles, and polarity. For example, the CO2 molecule has a linear geometry, bond angles of 180°, and is nonpolar.
Please provide the specific molecules you would like to have the Lewis structures drawn for, and I will gladly help you match them with their structural characteristics.