CH111 Final
Fall 1999

_____________________
Name

You must show all work for credit!!!!!

Grading:

1. ___________ 2. ____________

3. ___________ 4. ____________

5. ___________ 6. ____________

7. ___________ 8. ____________

9. ____________ 10. ___________

11. ___________ 12. ___________

13. ____________ 14. ____________

15. ____________ 16. ___________
1. Write electronic configurations for: (12 pts)

(a) Cr

(b) Pd+2

2. Name the following: (10 pts)

(a) KClO4

(b) CuBr2

(d) P4O10

(e) HBr in water

3. For the molecule O2SF2, write all the possible Lewis dot structure(s). Use formal charge to choose the best structure(s).(12 pts)

4. Predict the electron pair structures and the molecular structures for the following: (15 pts)

(a) TeCl4 (b) ICl4-1 (c) PF4+1

5. Balance the following by the half-reaction method: (12 pts)

CN-1(aq) + MnO4-1 (aq) -------> CNO-1(aq) + MnO2(s) (basic solution)

Identify the oxidizing agent and the reducing agent for the above. (4 pts)

6 .Balance the following reaction by the oxidation number method. You must assign oxidation numbers and show your work. (12 pts)

PbS(s) + O2(g) -------> PbO(s) + SO2(g)

7. Predict the following and give the reason for your choice: (28 pts)

(a) The lowest first ionization energy of Be, B, or C?

(b) The largest size of Mg, Ca or Sr?

(d) The highest ionization energy of P, S or Se?

(e) The most exothermic electron affinity of O-1, N or F?

(f) The most polar bond, NF, SiF, SnF?

(g) The lattice energy in NaF or NaCl?

8. Glucose is a carbohydrate that contains only C, H and O. Complete combustion of 0.360 mg of glucose produced 0.528 mg of carbon dioxide and 0.216 mg of water. Find the empirical formula of glucose. (15 pts)

9. How many atoms of all types are present in 10.0 g of NH3? (10 pts)

10. Write balanced net ionic equations for the following reactions. If no reaction occurs, write NR. (12 pts)

(a) CuSO4(aq) and Na2S(aq)

(b) Na2SO4(aq) and KOH(aq)

11. What is the theoretical mass of phosphoric acid (H3PO4) that could be obtained by the following reaction:

Ca3(PO4)2(s) + 3H2SO4(aq) -----> 3CaSO4(s) + 2H3PO4(aq)

if 100.0 g of Ca3(PO4)2 is reacted with 200.0 g of H2SO4? (12 pts)

12. Uranium hexafluoride is a solid at room temperature but it boils at 56oC. Determine the density of uranium heafluoride at 60.0 oC and 745 torr. ( 12 pts)

13. What mass of solid AgBr is produced when 100.0 mL of 0.150 M AgNO3 is mixed with 20.0 mL of 1.00M NaBr? (12 pts)

14. A coffee-cup calorimeter contains 50 mL of a 1.0 M solution of H2SO4 at 25oC. To this solution in the calorimeter, 100 mL of a 1.0 M NaOH solution (also at 25oC) is added. The temperature of the solution in the calorimeter increased to 33.9oC. Assuming no heat is lost to the calorimeter or the surroundings and that the specific heat of the solution is 4.18 J/g oC, calculate the heat of reaction in kJ/mol. (12 pts)

15. Consider the reaction

2ClF3(g) + 2NH3(g) ------> N2(g) + 6HF(g) + Cl2(g) Ho = - 1196 kJ

Calculate the standard heat of formation for ClF3(g). (The standard heat of formation of NH3(g) = -80 kJ/mol and of and HF(g) =-271 kJ/mol) (12 pts)

16. A 2.00 L of O2(g) was collected over H2O at a total pressure of 785 torr and at 25oC. When the O2(g) was dried (water vapor removed), the gas had a volume of 1.94 L at 25oC and 785 torr. Calculate the vapor pressure of water at 25oC.(12 pts)