Put Your Answers on a Separate Sheet of Paper to Allow Enough Room to Work

Put your answers on a separate sheet of paper to allow enough room to work.

1. What are the rules for naming and writing formulas for ionic compounds? (give 2 examples)

2. What are the rules for naming and writing formulas for covalent compounds? (give 2 examples)

3. What are the rules for naming and writing formulas for ionic compounds w/ transition metals? (give 2 examples)

4. Describe important properties for the following types of bonds: (include strength and difference in electronegativity)

Ionic bonds-

Polar covalent-

Non-polar covalent-

5. What type of bonds have unequal sharing of electrons? What type of bonds have equal sharing of electrons?

6. What happens to polarity as difference in electronegativity decreases?

7. What are the oxidation numbers for groups 1, 2, 13, 15, 16, and 17?

8. What does the oxidation number tell you about elements in that group?

9. What type of elements have varying oxidation numbers? Are there any exceptions to varying oxidation numbers with these elements?

10. What are the formulas and charges for the following polyatomic ions?

- Ammonium - Acetate - Chlorate - Cyanide - Nitrate - Hydroxide

- Carbonate - Sulfate - Phosphate

11. Pick 3 of the polyatomic ions from above and draw the correct Lewis dot diagram for each.

12. Explain what a polyatomic like phosphate must have a -3 charge in a compound and how that affects the Lewis Dot Structure.

13. How many electrons are represented by a single bond? Double bond? Triple bond?

14. Describe the trend of electronegativity and how it changes from left to right across the periodic table.

15. Calculate electronegativity difference between the elements in the following compounds and classify each as Ionic, Polar Covalent, or Non-polar covalent.

a. CO b. NaCl c. Fe3P2 d. S4 e. N2O5 f. K2O g.

16. Rank the following in order of strongest to weakest bond and explain why you ranked them that way:

PF3 CaCl2 N2

17. Draw the Lewis dot diagrams for the following covalent compounds:

a. SO2 b. NF3 c. O2 d. NO3-1 e. CHF3

18. Which compound or compounds from number 17 show resonance? Draw the other possible structures.

19. Name and draw the five basic geometric shapes we discussed. How many lone pairs are in each shape? Why do the lone pairs effect molecular geometry?

20. Name the following: identify as ionic or covalent Write formulas for the following:

Cl3I5 ______Lithium sulfide ______

Sn3N2 ______Calcium nitrate ______

Ag2(SO4) ______Lead (II) acetate ______

N2O ______Tetraiodine pentasulfide ______

Ca3(PO4)2 ______ethane ______

(NH4)3P ______propane ______