h = 6.63 x 10-34 J-s
c = 3.0 x 108 rn/s
R = 0.08206 L-atrn/mol-K
STP = 1 atm, 0°C
1 atm =760 torr

1 Which of the following statements concerning VSEPR is NOT true?

a) If there are no lone pairs on the central atom, the electronic and molecular geometries are the same.
b) "See-saw" is a molecular geometry, but not an electronic geometry.
c) "Tetrahedral" is both a molecular and an electronic geometry.
d) The electronic geometry with six "Regions of High Electron Density" is octahedral.
e) A double bond counts as two regions of high electron density.

2. Which of the following is the molecular geometry of AsF3?

a) trigonal bipyramidal
b) trigonal planar
c) trigonal pyramidal
d) tetrahedral
e) T-shaped

3. A molecule is trigonal planar and has only single bonds to the central atom. What can be said about the central atom?

a) it obeys the octet rule
b) it has fewer than 8 electrons
c) it has more than 8 electrons
d) none of these are definitely true

4. Which of the following molecules is polar, i.e. possesses a dipole moment?

a) CO2
b) PF3
c) PF5
d) N2
e) CF4

5. Which of the following does NOT have a linear molecular geometry?

a) CO2
b) CS2
c) H2O
d) N2
e) HCl

6. What is the molecular geometry of BrF5?

a) trigonal bipyramidal
b) square planar
c) square pyramidal
d) see-saw
e) trigonal pyramidal

7. A compound has the electron dot structure:

What is the molecular geometry?

a) T-shaped
b) trigonal bipyramidal
c) trigonal planar
d) tetrahedral
e) see-saw

8. Which of the following has a tetrahedral molecular geometry?

a) CF4
b) SF4
c) XeF4
d) CO2
e) PF5

9. The pressure of air inside a certain cold tire (15°C) is 1.50 atm. After the tire warms up on the highway to 30.°C, the volume inside the tire changes slightly, from 2.7 L to 2.8 L. What is the highway pressure inside the tire?

a) 1.52 atm
b) 2.89 atm
c) 1.64 atm
d) 3.00 atm
e) 1.57 atm

10. The following reaction produced 2.24 L of O2 collected at STP. How many grams of KClO3 were originally present? 2 KClO3(s) ---> 2 KCl(s) + 3 O2(g)

a) 8.16 g
b) 12.2 g
c) 183 g
d) 18.36 g
e) 6.66 x 10-2

11. At STP which of the following species would have the highest average molecular speed?

a) O2
b) NO2
c) N2
d) HCI
e) all would be the same

12. A 750. mL sample of a pure gaseous compound, measured at 0.00°C and 1.00 atm is found to weigh 2.86 grams. What is the molecular weight (molar mass) of the compound?

a) 0.080 g/mol
b) 144 g/mol
c) 44.0 g/mol
d) 85.5 g/mol
e) 28.6 g/mol

13. How many moles of argon gas are contained in 11.2 L at 25°C at 0.500 atm?

a) 0.458 mol
b) 1.00 mol
c) 0.229 mol
d) 2.73 mol
e) 0.500 mol

14. Identify the INCORRECT statement below:

a) The average speed of molecules of different gases depend on their molecular weight (molar mass).
b) The average kinetic energy of gas molecules is directly proportional to the temperature of the sample.
c) The average kinetic energies of molecules of different gaseous species are equal at a given temperature.
d) All the molecules of a gaseous sample at a fixed temperature are travelling at the same speed at any given instance.

15. According to Avagadro's hypothesis, which gas has the largest number of molecules per liter, given that all are at STP?

a) N2
b) O2
c) Ar
d) He
e) all would be the same

16. Which has the lowest boiling point?

a) Ne
b) Kr
c) Xe
d) Ar

17. A sample of gas having a volume of 1.0 L at 25°C and 1.0 atm pressure is subjected to an increase in volume and a decrease in temperature. The pressure of the gas:

a) decreases
b) increases
c) remains the same
d) either increases or decreases, depending on the size of the pressure and temperature changes.

18. A 5.0 liter sample of O2 gas is initially at STP. The volume is doubled, while holding the temperature fixed. What is the final pressure in torr units?

a) 2.5 torr
b) 380 torr
c) 1520 torr
d) 5.0 torr
e) 760 torr

19. On the following typical phase diagram, which statement is INCORRECT?

a) Point A corresponds to sublimation/deposition.
b) Point B corresponds to the critical point, where all three phases coexist.
c) Point C corresponds to the liquid phase of the substance.
d) At a higher temperature and pressure than point D, the substance exists as a supercritical fluid.
e) Raising the pressure from point E to point C causes the substance to condense.

20. Arrange these substances in order of INCREASING boiling point: Xe, H2, H2O, LiCl, H2S.

a) Xe < H2 < H2O < LiCl < H2S
b) Xe < H2 < H2S < H2O < LiCl
c) H 2 < Xe < H2S < H2O < LiCl
d) H2 < Xe < H2O < H2S < LiCl

21. Which of the following is NOT a molecular solid?

a) solid CO2
b) solid water
c) white phosphorus (solid P4)
d) S8
e) diamond

22. Which is the weakest intermolecular force among a group of molecules of comparable molecular weight (molar mass)?

a) dipole-dipole
b) London
c) ionic bonding
d) hydrogen bonding

23. Which of the following best describes the properties of a metallic solid?

a) soft, very low melting point, poor electrical conductor
b) an amorphous solid with no unit cell, conducts electricity, doesn't conduct heat well
c) very hard, very high melting point, poor electrical conductor
d) variable hardness, variable melting point, excellent thermal conductor

24. Which of the following pure substances exhibits hydrogen bonding?

a) NH3
b) H2S
c) HCl
d) CH4
e) all of these do

25. Which compound/formula name combination is INCORRECT?

a) CaSO4 is calcium sulfate
b) NaCO3 is sodium carbonate
c) K2S is potassium sulfide
d) Mg(OH)2 is magnesium hydroxide
e) BaCl2 is barium chloride

26. A compound has the following percent (by mass) composition: 87.2% Ti (thallium, atomic number = 81), 2.6% C and 10.2% oxygen. What is the empirical formula of this compound?

a) TlCO
b) TICO3
c) T12CO2
d) T12CO3
e) TICO2

27. HCI(g) is bubbled into water. It is found that the concentration of HCl in the solution is 0.20 M, and that the volume of the solution is 250.0 mL. What mass of HCl is dissolved in the solution?

a) 7.29 g
b) 1.82 g
c) 9.11 g
d) 7.02 g
e) 2.45 g

28. A solution is 8.00% acetic acid by mass, and has a specific gravity of 1.13. What mass of glucose is present in 40.0 mL of this solution?

a) 7.08 g
b) 2.83 g
c) 3.20 g
d) 3.62 g
e) 8.00 g

29. Consider the reaction 2 Al203(s) + 3 C(s) + 6 Cl2(g) ---> 4 AlCl3(s) + 3 CO2. What mass of AlCl3 can be made from 150.0 g Al2O3, given excess C and C12?

a) 98 g
b) 150.0 g
c) 472 g
d) 392 g
e) 196 g

30. Calculate the percent carbon by mass in ferrocene, FeC10H10.

a) 64.6%
b) 30.1%
c) 92.3%
d) 47.6%
e) 15.3%

31. How many moles of Na+ are present in 41.0 grams of Na3PO4?

a) 0.25 mol
b) 0.50 mol
c) 0.75 mol
d) 0.083 mol
e) 1.78 mol

32. Which of the following would NOT be classified as a strong electrolyte?

a) K2SO4
b) H2SO4
c) NaBr
d) NH4NO3
e) CH3OH

33. Consider the reaction 2 ZnS(s) + 3O2(g) ---> 2 ZnO(s) + 2 SO2(g). If 100.0 g of ZnS is reacted with 75.0 grams of O2, what mass of ZnO(s) is produced, assuming 100% yield?

a) 175 g
b) 83.6 g
c) 127 g
d) 100. g
e) 50.0 g

34. Exactly 1 ft3 of tungsten (W) has a mass of 1202 pounds. What is the density of tungsten in g/cm3? (1 kilogram = 2.2 lb, 1 in = 2.54 cm, 1 ft = 12 in).

a) 17.9 g/cm3
b) 19.2 g/cm3
c) 8.73 g/cm3
d) 12.0 g/cm3
e) 42.2 g/cm3

35. Calculate the mass of a SINGLE MOLECULE of CH4?

a) 2.66 x 10-23 g
b) 16 g
c) 1.66 x 1024 g
d) 32 g
e) 4.3 x 10-16 g

36. Identify the INCORRECT statement below:

a) All atoms of a given element have the same mass.
b) Avogadro's number is the number of atoms in exactly 12 grams of Carbon- 12.
c) The electron and the proton have charges equal in magnitude and opposite in sign.
d) The mass number is the total number of protons and neutrons in the nucleus.

37. The valence electrons of an atom, "E", are ns2np1. What is the most likely formula for the chloride of this compound?

a) ECl2
b) ECl3
c) ECl4
d) EC6
e) ECl8

38. Rank the elements Al, P, and Ga in order of LARGEST first ionization energy to SMALLEST first ionization energy.

a) Al > Ga > P
b) Ga > Al > P
c) Ga > P > Al
d) P > Al > Ga
e) P > Ga > Al

39. Which of the following is the NET IONIC equation for the reaction between AgNO3(aq) and Na3PO4(aq)?

a) Ag3+(aq) + PO43-(aq) ---> AgPO4(s)
b) Ag+(aq) + NO3- (aq) + Na+(aq) + PO43-(aq) ---> AgPO4(s) + Na+(aq) + NO3-(aq)
c) 3 Ag+(aq) + 3 NO3-(aq) + 3 Na+(aq) + PO43-(aq) ---> Ag3PO4(s) + 3 Na+(aq) + 3 NO3-(aq)
d) 3 Ag+(aq) + PO43-(aq) ---> Ag3PO4(s)
e) There is no reaction between AgNO3(aq) and Na3PO4(aq)

40. An atom de-excites by emitting a photon whose wavelength is 285 run. What is the energy loss by the atom (in joules)?

a) 4.03 x 10-18 J
b) 3.51 x 106 J
c) 1.05 x 1015 J
d) 6.97 x 10-28 J
e) 6.97 x 10-19 J

41. Rank the elements, O, S, and Si in order from SMALLEST to LARGEST.

a) O < Si < S
b) O < S < Si
c) Si < S < O
d) S < Si < O
e) Si < O < S

42. Given that the following reactions occur:

CuSO4(aq) + Cd(s) ---> Cu(s) + CdSO4(aq)
CuSO4(aq) + V(s) ---> Cu(s) + VSO4(aq)
CdSO4(aq) + V(s) ---> Cd(s) + VSO4(aq)

Which of the following lists Cu, V, and Cd from MOST active to LEAST active?

a) V, Cd, Cu
b) V, Cu, Cd
c) Cu, Cd, V
d) Cu, V, Cd
e) Cd, V, Cu

43. In which of the following is the oxidation number of chlorine +1?

a) Cl2O
b) Cl2O7
c) ClF3
d) ClF5
e) HCl

44. Which of the following atoms or ions has 2 UNPAIRED electrons?

a) O2-
b) C
c) F
d) Cu
e) Mn

45. In which of the following electron dot structures are there two or more equivalent resonance structures?

a) PCl3
b) SO2
c) SO42-
d) H2O
e) O2

46. In which of the following are there NO lone pairs on the central atom?

a) SO2
b) PCl3
c) ICl3
d) SO42-
e) H2O

47. What is the wavelength (in nanometers) of a photon whose frequency is 7.00 x 1013 s-1?

a) 720 nm
b) 4286 nm
c) 1.28 x 10-5nm
d) 7.08 nm
e) 582 nm

48. From the following list of observations, choose the one that most clearly supports the following conclusion: photons have particle nature.

a) Emission spectrum of hydrogen
b) The photoelectric effect
c) Diffraction
d) Scattering of alpha particles by metal foil
e) Cathode "rays"

49. Which of the following combinations of quantum numbers (n, l, ml, ms) would not be possible for an electron in an atom?

a) (2, 0, 0, -1/2)
b) (3, 1,-1, 1/2)
c) (4, 2, -2, -1/2)
d) (3, 2, -3, 1/2)
e) (6, 1, 0, 1/2)

50. Which of the following electron dot structures has ONLY single bonds and lone pairs?

a) CO2
b) O2
c) SO42-
d) SO2
e) NO3

KEY

1)e 2)c 3)b 4)b 5)c 6)c 7)a 8)a 9)a 10)a 11)c 12)d 13)c 14)d 15)e 16)a 17)a 18)b 19)b 20)c 21)e 22)b 23)d 24)a 25)b 26)d 27)b 28)d 29)d 30)a 31)c 32)e 33)b 34)b 35)a 36)a 37)b 38)d 39)d 40)e 41)b 42)a 43)a 44)b 45)b 46)d 47)b 48)b 49)d 50)c