Name: _______________________________________________ Date: _______________ Period: _____
LEWIS DOT PRACTICE
Drawing Lewis Structures:
1. Draw skeletal structure of compound showing what atoms are bonded to each other. Put least
electronegative element in the center.
2. Count total number of valence e-. Add 1 for each negative charge. Subtract 1 for each positive
charge.
3. Complete an octet for all atoms except hydrogen
4. If structure contains too many electrons, form double and triple bonds on central atom as needed.
Draw Lewis Structures for the following compounds.
1. F2
6. CO
2. H2O
7. CO32-
3. SCl2
8. SO42-
4. AsF3
9. N2F2
5. SiH4
10. C3H6O
Extra Tips:
 When drawing the initial skeleton, try to make the most symmetrical arrangement possible.
 Carbon loves to be in the center.
 Hydrogen and Halogens love to be on the ends and don’t partake in double or triple bonds.
 Bonds always form between pairs of electrons (you should never see unpaired electrons).
 Always check the final electron count after you are done drawing!
 Remember for polyatomic ions to put brackets around the entire structure with the charge
written on the outside