1. Grudgeball Midterm Review

2. Question 1:  Complete the following chart: Nuclear Symbol # of protons # of neutrons # of Electrons Mass number Charge 30 +3 Al 13

3. Question 1:  Complete the following chart: Nuclear Symbol # of protons # of neutrons # of Electrons Mass number Charge 30 +3 Al 13

4. Question 2:  Calculate the average atomic mass of sulfur if 95.00% of all sulfur atoms have a mass of 31.972 amu, 0.76% has a mass of 32.971amu and 4.22% have a mass of 33.967amu.

5. Question 2:  Calculate the average atomic mass of sulfur if 95.00% of all sulfur atoms have a mass of 31.972 amu, 0.76% has a mass of 32.971amu and 4.22% have a mass of 33.967amu.

6. Question 3: Convert 2.27 mL/min to km 3 /year.

7. Question 3: Convert 2.27 mL/min to km 3 /year.

8. Question 4: A piece of silly putty has a mass of 5.00 g. It is placed in 25.0 mL of water. The volume of water rises to 29.5 mL. Determine the density of the silly putty.

9. Question 4: A piece of silly putty has a mass of 5.00 g. It is placed in 25.0 mL of water. The volume of water rises to 29.5 mL. Determine the density of the silly putty.

10. Question 5: A student dehydrates a sample of CuSO 4 ·5H 2 O and determines the sample contains 35.04% water by mass. What is the student’s percent error in this lab experiment?

11. Question 5: A student dehydrates a sample of CuSO 4 ·5H 2 O and determines the sample contains 35.04% water by mass. What is the student’s percent error in this lab experiment?

12. Question 6: A compound has a molecular weight of 60.06 g/mol. The compound is 39.99% C, 6.73% H, and 53.28% O. What is the empirical & molecular formula for this compound?

13. Question 6: A compound has a molecular weight of 60.06 g/mol. The compound is 39.99% C, 6.73% H, and 53.28% O. What is the empirical & molecular formula for this compound?

14. Question 7: 2 AgNO 3 + Cu  2 Ag + Cu(NO 3 ) 2 If the actual yield of the reaction was 4.44 grams of copper (II) nitrate, what is the percent yield?

15. Question 7: 2 AgNO 3 + Cu  2 Ag + Cu(NO 3 ) 2 If the actual yield of the reaction was 4.44 grams of copper (II) nitrate, what is the percent yield?

16. Question 8: SeCl 6 + O 2  SeO 2 + 3 Cl 2 How many grams of chlorine can be produced from the reaction of 13.7 grams of SeCl 6 and 13.7 grams of oxygen?

17. Question 8: SeCl 6 + O 2  SeO 2 + 3 Cl 2 How many grams of chlorine can be produced from the reaction of 13.7 grams of SeCl 6 and 13.7 grams of oxygen?

18. Question 9: Correctly predict the products (check your solubility chart!) and balance the following reaction: Copper (II) nitrate + barium hydroxide 

19. Question 9: Correctly predict the products (check your solubility chart!) and balance the following reaction: Copper (II) nitrate + barium hydroxide 

20. Question 10: Find the molarity of the fluoride ions when 4.56 g of magnesium fluoride is dissolved in 2.04 L of solution.

21. Question 10: Find the molarity of the fluoride ions when 4.56 g of magnesium fluoride is dissolved in 2.04 L of solution.

22. Question 11: What is the pH of a solution that has a [OH - ] of 4.52 x 10 -9 M? Is the solution acidic, basic or neutral?

23. Question 11: What is the pH of a solution that has a [OH - ] of 4.52 x 10 -9 M? Is the solution acidic, basic or neutral?

24. Question 12: Calculate the oxidation number of carbon in oxalate.

25. Question 12: Calculate the oxidation number of carbon in oxalate.