SEQ CHAPTER \h \r 1AP Exam II Chap 4-6 Name ___________________
A. Multiple Choice: choose the best answer and place it in the space provided.
Choose one of these for questions 1-4:
_____ 1. Which of these is a soluble salt?
_____ 2. This is a weak acid.
_____ 3. This acid is a strong electrolyte
_____ 4. This base ionizes completely.
Choose one of these for questions 5-7:
_____ 5. This is the maximum grams of solute that can dissolve in 100 mL of water at room temperature.
_____ 6. This the moles of solute dissolved in 1 liter of solution.
_____ 7. This is what happens when a weak acid is added to water
_____ 8. What is the molarity of a 200 mL solution which contains 0.1 mol of NaNO3 ?
a. 1.0 M
b. 0.8 M
c. 0.5 M
d. 0.1 M
e. 0.05 M
_____ 9. What volume of 6 M HCl must be used to make 100 mL of 0.50 M HCl solution?
a. 4.2 mL
b. 8.3 mL
c. 12.0 mL
d. 60.0 mL
e. 120 mL
_____10. How many grams of solid Ca(OH)2 is needed to completely neutralize 100.0 mL of a 0.20 M solution of HNO3?
a. 0.74 grams
b. 1.5 grams
c. 3.0 grams
d. 5.4 grams
e. 11 grams
_____ 11. How many milliliters of a 0.20 M NaOH is needed to titrate to endpoint a 10.0 mL of 0.20 M H2SO4 ?
a. 5.0 mL
b. 10.0 mL
c. 15.0 mL
d. 20.0 mL
d. 50.0 mL
_____ 12. What is the heat of formation of diatomic nitrogen ?
a. 0 kJ/mol
b. -25 kJ/mol
c. 25 kJ/mol
d. -250 kJ/mol
e. 250 kJ/mol
_____ 13. What is the heat (q) in joules required to raise the temperature of 10.0 grams of water from 20.0oC to 30.0oC ? The specific heat of water is 4.18 J/goC
a. 30 J
b. 418 J
c. 1254 J
d. 2090 J
e. 3000 J
_____14. In this reaction: CH4 + 2 O2 —> CO2 + 2 H2O + 890kJ
a. two moles of methane is burned.
b. the reaction is endothermic.
c. burning two moles of oxygen produces 890 kJ
d. heat is absorbed in this reaction
e. the change in enthalpy ()H) is positive
_____ 15. What is the oxidation state for phosphorus in phosphoric acid (H3PO4)?
_____ 16. In the reaction below:
Cu (s) + HNO3 (aq) → Cu(NO3)2 (aq) + H2O (l) + NO2 (g)
a. O is oxidized and N is reduced.
b. N is oxidized and Cu is reduced
c. Cu is reduced and O is oxidized
d. O is reduced and Cu is oxidized
e. Cu is oxidized and N is reduced.
Questions 17- 19 refer to the following elements:
_____ 17. This element has a noble gas configuration of [Ar]4s2 3d104p5
_____ 18. This element has a valence configuration of 4s13d5
_____ 19. This element has only one valence electron.
Questions 20-22 refers to the following answers:
A. uncertainty principle
B. exclusion principle
C. Hund’s rule
D. Schrodinger equation
E. photoelectric effect
_____ 20. Demonstrates that light can act as a particle.
_____ 21. Predicts that it is impossible to determine simultaneously the exact position and exact momentum of an electron.
_____22. Treats the electron as a wave and led to the definition of three quantum numbers: n, l, & ml .
_____ 23. Which of the following sets of quantum numbers best describes the valence electron of highest energy in a ground state zinc atom (Z=30).
A. 4, 0, 0, ½
B. 4, 0, 1, ½
C. 3, 1, 1, ½
D. 3, 1, 2, ½
E. 3, 2, 0, ½
_____ 24. If the value for the principle quantum number is n = 3 , what are the possible values for the azimuthal quantum number : l ?
B. 0, 1
C. 0, 1, 2
D. 1, 2
_____25. According to the Bohr equation, the energy of the 4th energy level is equal to
A. –2.18 X 10-18 J
B. –1/4(2.18 X 10-18 J)
C. –1/9(2.18 X 10-18 J)
D. –1/16(2.18 X 10-18 J)
E. –1/25(2.18 X 10-18 J)
B. Short answer:
1. Explain each of the following using the quantum theory and/or orbital filling diagrams.
a.) There are only 14 elements in the actinide series.
b.) The actual electron configuration for Silver is [Kr] 5s1 4d10 whereas the aufbau principle predicts an electron configuration of [Kr] 5s2 4d9 .
2. For each of these reactions:
- write and balance the molecular equation (if a reaction occurs)
- write the complete ionic equation
- write the net ionic equation
a.) KI (aq) + Pb(NO3)2 (aq) →
b.) HC2H3O2(aq) + Sr(OH)2(aq) →
c.) Au(s) + NaNO3 (aq) →
C. Problems : You may use a calculator. Please show your work. Please round your answer, include units and circle your answer
1. Calculate the ΔH for the reaction:
NO(g) + O(g) → NO2(g)
Given the following information:
NO(g) + O3(g) → NO2(g) + O2(g) ΔH = -198.9 kJ
O3 (g) → 3/2 O2(g) ΔH = -142.3 kJ
O2(g) → 2 O (g) )H = 495.0 kJ
2. Determine the heat of formation (in kJ/mol) of liquid water given the following information:
2 H2O2(l) → 2H2O(l) + O2(g) + 196.46 kJ
Substance Hof (kJ/mol)
O2 (g) 0
3. If the reaction in question 2 was carried out in a calorimeter containing 50.0 grams of water at an initial temperature of 25.0oC, and the initial amount of hydrogen peroxide used was 0.500 grams, what would the final temperature of the water be when the reaction was completed?
Assume no heat loss by the calorimeter. The specific heat of water is 4.184 J/goC
4. The hydrogen spectrum has an emission line of 486.1 nm.
a.) What is the energy of a photon of this radiation?
b. What is the energy level of the ground state? Explain your reasoning.
c. Calculate the energy level of the excited state.
Answer Key: 1 b, 2.a, 3.c, 4.e, 5.b, 6.a, 7.c, 8.c, 9.b, 10.a, 11.d, 12.a, 13.b, 14.c, 15.d, 16.e, 17.e, 18.b, 19.a, 20.e, 21,a, 22.d,
23.e, 24.c, 25.d.
B 1. a) There are 7 orbitals - 2 electrons/orbital = 14 electrons (14 boxes)
b) The atom is more stable when the d-sublevel is full.
2. a) Pb2+ + 2I- --> PbI2
b) 2HC2H3O2 + 2OH- --> 2H20 + 2 C2H3O2-
c) No rxn
C 1. -304.1 kJ
2. -285.8 kJ/mol
4. a. -4.09 X 10-19 J