Quiz (117 points) MULTIPLE CHOICES. Write the letter of the correct answer. (3 points each) 1. What is the oxidation number of P in H3PO4?

A. 4 B. 5 C. 6 D. 7

2. Choose the INCORRECT statement.

A. The heat capacity is the quantity of heat required to change the temperature of the system by one degree.

B. The specific heat is the heat capacity for one mole of substance. C. Specific heat is an intensive property. D. Most metals have low specific heats, as metals can be heated quickly.

3. How much heat is required to raise the temperature of 175 g of aluminum from 21.0C to 145C? The

specific heat of aluminum is 0.903 J g-1 C-1. A. 19.6 kJ B. 24.0 kJ C. 1.27 J D. 22.9 kJ

4. 100.0 g of nickel at 150 C was placed in 1.00 L of water at 25.0C. The final temperature of the nickel-

water mixture was 26.3C. What is the specific heat of the nickel? The specific heat of water is 4.184 J/g C. A. 0.14 J/g C B. 0.13 J/g C C. 0.55 J/g C D. 0.44 J/g C

5. 14.0 g of metal at 24.0C has 250 joules of heat added to it. The metal's specific heat is 0.105 J/g C.

What is its final temperature? A. 25.9 C B. 146. C C. 194 C D. NONE of the above

6. A system absorbs 623 J of heat while doing 457 J of work. What is the value of U?

A. +1080 J B. -166 J C. +166 J D. -1080 J

7. What is the work done in joules by the system when H2 expands against a constant pressure of

75 atm at 45.3C? The change in volume is 24.0 L. A. 1.8 103 J

B. -8.2 104 J

C. 8.2 104 J

D. -1.8 105 J

8. Calculate the work needed to make room for products in the combustion of sulfur, S8(s), to SO2(g) at 25

and 1 atm. A. 0 kJ B. -2.27 kJ C. -4.54 kJ D. -18.2 kJ

9. Calculate the standard enthalpy of formation of Cl-(aq), given the following thermochemical data at 1 atm,

and knowing that the standard enthalpies of formation of H2(g) and H+(aq) are both zero.

HCl(g) H+(aq) + Cl-(aq) -75.15 kJ H2(g) + Cl2(g) 2HCl(g) -184.62 kJ

A. -167.46 kJ/mol B. +109.47 kJ/mol C. -17.16 kJ/mol D. +34.32 kJ/mol

10. Which of the following statements are true? I) Liquids have more entropy than their solids. II) Solutions have more entropy than the solids dissolved. III) Gases and their liquids have equal entropy. IV) Gases have less entropy than their solids. V) Entropy of a substance increases as its temperature increases.

A. II), III), and V) B. I), III), and V) C. I), IV), and V) D. I), II), and V)

11. Which of the following processes would result in a decrease in system entropy?

A. melting of an ice cube B. sublimation of a moth ball C. evaporation of a puddle of gasoline D. condensation of water vapor on a cold windshield

12. Predict whether S is positive or negative for the following process: 2 Cl2O7(g) 2 Cl2(g) + 7 O2(g)

A. negative B. positive C. There is not enough information to determine. D. S doesn't change.

13. A reaction is spontaneous if: I) G is a negative value II) both enthalpy and entropy increase III) H is negative and S is positive IV) both enthalpy and entropy decrease V) H is positive and S is negative

A. I and III B. I and II C. II and V D. III and IV

Use the following information to answer 14 and 15. 3 N2(g) + 2 O3(g) 6 NO(g)

Hf 0.00 142.2690.37 kJ/mol

S 191.5 237.7210.6 J/mol K 14. What is Grxn for this reaction in kJ at 500 K?

A. 93 kJ B. 151 kJ C. 365 kJ

D. -1.00 105 kJ 15. At what temperature range will the reaction be spontaneous?

A. 1204 K B. < 1204 K C. 829.9 K D. < 829.9 K

16. Which of the following orbital designations is impossible?

A. n=2, l = 0, ml = 0 B. n=3, l = 0, ml = 0 C. n=3, l = 1, ml = 1 D. n=3, l = 3, ml = -3

17. Which of the following sets of quantum numbers is not matched with the orbital designation.

A. n=1, l = 0: a 1s orbital B. n=2, l = 0: a 2p orbital C. n=3, l = 0: a 3s orbital D. n=3, l = 2: a 3d orbital

18. Identify the element with the lowest atomic number for which: The outermost electron of a particular element has magnetic quantum number, m l, of -1; and The element has two other electrons that are energy degenerate to the one described by m l = -1.

A. C B. N C. P D. Be

19. Which of the following is the condensed electron configuration for bismuth?

A. [Xe]6s24f

145d

106p

3

B. [Xe]6s26f

146d

106p

3

C. [Xe]5s24f

144d

105p

3

D. [Xe]6s24f

124d

106p

5

20. Which group has the elements listed in order of increasing atomic radius? Al, P, Cl, Ar Rb, Sr, Ca, Mg N, P, S, Se Ne, Ar, Cl, Br

21. Which of the following has the smallest radius? A. Li B. Li

+

C. O2-

D. Be

2+

22. Which of the following species is most likely to accept another electron? A. Ar B. O C. C D. N

23. Which of the following has the highest second ionization energy?

A. Na B. Mg C. Al D. K

24. Consider the chlorine difluoride molecule, ClF3. Which of the following statements are correct: I) The molecule is polar. II) All bonds in this molecule are polar. III) The central atom has five groups surrounding it. IV) Molecular geometry is trigonal pyramidal.

A. I, III, and IV B. II, III, IV C. II and III D. I, II, and III

25. The electron group geometry for SF4 is?

A. Trigonal planar B. Tetrahedral

C. Trigonal bipyramidal D. Octahedral

26. Describe the hybridization of the middle carbon in acetone, (CH3)2CO.

A. sp B. sp

2

C. sp3

D. sp3d

27. Which of the following statements is incorrect according to MO theory?

A. O2 is paramagnetic B. O2

2- is diamagnetic

C. O22-

has a greater bond strength than O2 D. O2

2+ has a greater bond strength than O2

PROBLEM SOLVING. Show complete solution and BOX your final answer. 1. Balance the following reactions. (5 points each)

a. S2-

+ NO3- NO + 3S (acidic)

b. Cu(OH)2 + Zn Cu + Zn2+

(basic) 2. In a coffee-cup calorimeter, 10.00 mL 1.00 M HCl was mixed with 5.00 mL 1.00 M NaOH. The temperature of the calorimeter increased by 4.00 K. In the same calorimeter, 10.00 mL 1.00 M HA was mixed with 5.00 mL 1.00 M NaOH and the recorded change in temperature was 4.5 C. Calculate the: a. heat capacity of the calorimeter (3 points) b. H for the reaction between NaOH and HA. (3 points) 3. Kenshin immediately performed an experiment after receiving a mixture of two solutions from Kaoru. The mixture contains 3 ions. Identify the ions (X, Y, Z) present in the unknown solution. The results of his experiment are listed below. (6 points) Unknown solution + few drops of 1.0 M NaOH brown precipitate + several drops of 1.0 M NaOH precipitate did not dissolve Unknown solution + few drops of 1.0 M NH3 brown precipitate + several drops of 1.0 M NH3 precipitate did not dissolve; blue supernate Unknown solution + few drops of 1.0 M Ba(NO3)2 no visible reaction Unknown solution + 5 drops 1.0 M HNO3, +1 drop 0.1 M KMnO4, + 10 drops toluene pink toluene layer,

orange aqueous layer 4. State the color displayed by each ion in flame test. (1 point each) a. Cu

2+

b. Ba2+

c. K+

d. Na+

e. Ca2+

5. Draw the Lewis structures and the resonance structures (if any) of the following compounds. For b indicate the formal charge of all atoms. a. Ca(CN)2 (3 points) b. Cl2SO (6 points)