1. Figure: 08-T01

2. Figure: 08-03

3. Figure: 08-T02

4. Figure: 08-04

5. Figure: 08-05

6. Lewis Dot Structures (1). Place the nuclei in the proper geometry.
(1). Place the nuclei in the proper geometry.
(2). Determine the total number of valence electrons.
(3). Draw single bonds between the bonded pairs of atoms.
(4). Fill in the remaining electrons as lone pairs without exceeding an octet on each heavy atom or a duet on H or He.
(5). If any atoms do not have a completed octet, then move lone pairs to complete the octets by forming multiple bonds.
(6). If several non-equivalent structures are possible, the lowest energy structure minimizes the formal charges.
(7). Place the largest negative formal charges on the most electronegative atoms.
(8). Use expanded octets on 3rd and 4th period elements only if necessary to accommodate the required total number of electrons.
(9). Show the overall ionic charge in the final structures.

7. Figure: 08-06

8. Figure: 08-07

9. Figure: 08-08

10. Figure: 08-09

11. Figure: 08-10

12. Figure: 08-11

13. Figure: 08-T04

14. Figure: 08-13

15. Figure: 08-T05