DESCRIPTION AND SAMPLE QUESTIONS FOR
UT AUSTIN TEST FOR CREDIT IN CHEMISTRY 301

The Chemistry 301 Test Covers the General Topics:

• Atomic structure
• Chemical bonding – ionic, covalent, dot structures
• Molecular shape and structure
• Properties of gases
• Stoichiometry
• Properties of liquids and solids
• Intermolecular forces
• Thermodynamics – work and energy, enthalpy, entropy, free energy

These topics are representative of material covered in the first semester UT Austin course for scientific and technical students. Two hours of working time is allowed. The test is multiple choice.

Textbook for CH301 Test:

Although the test is not based on a specific textbook, the following book contains material that will be covered in the test: Atkins and Jones, Chapters 1-7, Chemical Principles (3rd ed.). New York: W.H. Freeman and Company, 2005. Use of a hand calculator is permitted, but it may not be shared. All programmable calculators are subject to inspection by test administrators.
These same topics are found in varying order in most general chemistry textbooks and almost any of these textbooks could be used to study for this exam.  Some other books students may find helpful:

• Whitten, Davis and Peck, General Chemistry. (6th ed.). Philadelphia: Saunders College Publishing, 2000. 
• Petrucci, Harwood, Herring, and Madura, General Chemistry. (9th ed.). New Jersey: Pearson, 2007.
• Zumdahl, Chemical Principles. (5th ed.). Boston: Houghton Mifflin Company, 2005. 

CH301 Practice Questions

1. A radio station broadcasts at a frequency of 105 MHz.  What is the energy of a photon with this frequency?

2. How many d electrons does I (atomic number 53) possess?

3. The 3d sublevel h as enhanced stability when it contains how many electrons?

4. An electron in a 3d orbital could have which of the following quantum numbers?

1. n = 3; l = 2; ml = 0
2. n = 3; l = 1; ml = -1
3. n = 3; l = 2; ml = -3
4. n = 3; l = 0; ml = 0
5. n = 2; l = 2; ml = 2
6. n = 2; l = 3; ml = 0
7. n = 3; l = 3; ml = 1

5. Vapor obtained by evaporating 0.495 grams  of an unknown liquid is collected in a 127 mL flask.   At 371 K, the pressure of the vapor in the flask is 754 torr. What is the molar mass in g/mol?

6. What is the density of nitrogen gas at STP?

7. Consider two equal-sized containers, one filled with H2 gas and one with O2 gas at the same temperature and pressure. The average velocity of the O2 molecules is (equal to, greater than, less than) that of the H2 molecules.

8. Which of the statements below are true?

1. Real gases act more like ideal gases as the temperature increases.
2. When n and T are constant, a decrease in P results in a decrease in V.
3. At 1 atm and 273 K, every molecule in a sample of a gas has the same speed.
4. At constant T, CO2 molecules at 1 atm and H2 molecules at 5 atm have the same average kinetic energy.

9.  How many sigma and pi bonds are in CH3CH2CHCHCH3?

10.  How many lone pairs are in the structure for IO3-?

11. The molecular geometry of SF5 is ___________.

12. What is the hybridization of the central atom in XeF4?

13. The molecule PBr3 is a (polar/nonpolar) molecule with (polar/nonpolar) bonds.

14. What would be the bond order of C2?

15. Estimate ΔH for the gas-phase reaction
            NCl3 + 3H2O à NH3 + 3 HOCl,
based on the bond energies N-Cl : 190 kJ/mol; O-H : 464 kJ/mol; N-H : 391 kJ/mol; O-Cl : 206 kJ/mol.

16. Calculate the enthalpy change for the reaction
            SO2(g) + ½ O2(g) à SO3(g)

      given the following:                                  ΔH°f (kJ/mol rxn)
            SO2(g) à S(s) + O2(g)                     +296.8
            2SO3(g) à 2 S(s) + 3O2(g)             +791.4

17. Which physical state, solid, liquid, or gas, has the lowest entropy?

18. What is the entropy change of the reaction

            N2(g) + 3H2(g) à 2NH3(g)
            191.5   130.6       192.3

at 298 K and 1 atm pressure? The number below each substance is the absolute entropy of the substance at 298 K, 1 atm, in units of J/mol•K.

19. What is the molarity of a HCl solution if 2.50 L is needed to react with 12.7 g of Al according to the reaction
            2 Al + 6 HCl à2 AlCl3 + 3H2 ?

20. Consider the reaction
            2 SO2(g) + O2(g) à 2 SO3(g)
with a reaction enthalpy of -10.0 kJ/mole rxn. Which response predicts the thermodynamic spontaneity of the reaction?

1. The reaction is spontaneous at all temperatures.
2. The reaction is spontaneous only at low temperatures.
3. The reaction is spontaneous only at high temperatures.
4. The reaction is not spontaneous at any temperature.
5. We cannot predict the spontaneity for this reaction.

21.  Which would you expect to have the largest atomic radius: Ca, K, Rb, or Sr?

22.  What type of intermolecular forces would you expect in a liquid sample of H2S?

23.  Order these molecules in order of increasing melting point: C2H6, H2S, H2O, and NaI.

CH301 Practice Question Answers

1. 6.96 x 1026 J
2. 20
3. 5 or 10
4. A
5. 1.20 g/mol
6. 1.25 g/L
7. less than
8. I and IV
9. 14 sigma, 1 pi
10.  10
11. square pyramidal
12. sp3d2
13. polar; polar
14. 2
15. +171 kJ/mol rxn
16. -98.9 kJ/mol rxn
17. solid
18. -198.7 J/mol•K
19. 0.564
20. B
21. Rb
22. dipole-dipole forces
23. C2H6, H2S, H2O, NaI