This is Part 1 of 2.
Source: Langhans and various educators
Here is Part 2 of 2
Source: Langhans and various educators
Part 1: Draw the following Lewis Dot Structures (remember to use the valence electrons)
Part 2: This part is harder. Follow the following rules:
Guidelines for Drawing Lewis Dot Structures for Molecules:
1. The octet rule1 says that atoms “try” to have 8 valence electrons by sharing or transferring
electrons to form compounds. Hydrogen only has 2 electrons in its “octet”.
2. Put the atom which can share the most electrons in the middle.
3. Some atoms can share two or three pairs of electrons (usually it is either C, N, or O)
4. put the hydrogen atoms on last
5. hydrogen NEVER shares two pairs of electrons.
6. fluorine NEVER shares two pairs of electrons.
7. fluorine ALWAYS obeys the octet rule.
8. Any structure which obeys the octet rule (and makes chemical sense) is more 'correct' than any
structure that violates the octet rule.
Part 3: Onto Naming and formula writing:
Write the name of each of the following compounds.
1. HF 1. ______________________
2. H2S 2. ______________________
3. NO 3. ______________________
4. N2O 4. ______________________
5. NO2 5. ______________________
6. N2O5 6. ______________________
7. SO2 7. ______________________
8. CBr4 8. ______________________
9. C2H6 9. ______________________
10. C4H10 10. ______________________
Write the chemical formula for each of the given names.
11. nitrogen triiodide 11. ______________________
12. dinitrogen tetroxide 12. ______________________
13. sulfur trioxide 13. ______________________
14. carbon monoxide 14. ______________________
15. dihydrogen monoxide 15. ______________________
16. hydrogen monobromide 16. ______________________
17. phosphorus trichloride 17. ______________________
18. tricarbon octahydride 18. ______________________
19. carbon tetrahydride 19. ______________________
20. dicarbon tetrahydride 20. ______________________
Source: Langhans and various educators