1. Which is a list of elements in order of increasing metallic character?
A. Si, P, S
B. As, P. N
C. Sr, Ca, Mg
D. Br, Se, As
E. Na, Ne, F

2. The electron configuration of the oxide ion is most similar to the electron configuration of the
A. Sulfide ion
B. Nitride ion
C. Oxygen atom
D. Nitrogen atom
E. Fluorine atom

3. The value of Plank’s constant is 6.63X10-34 J * s. The velocity of light is 3.0X108 m * s-1. Which value is closest to the wave length in nanometers of a quantum of light with frequency of 8X1015 sec-1?
A. 3X107
B. 4X101
C. 5X10-18
D. 2X10-25
E. 1X10-25

4. What is the number of half-filled orbitals in an atom of chromium?
A. 0
B. 2
C. 4
D. 6
E. 12

5. What is the number of electrons in an atom of scandium that have an l quantum number of 1?
A. 1
B. 3
C. 4
D. 6
E. 12

6. The electron configuration of atoms of element X is shown below

[Ar] 4s23d10

Which is the most likely formula for the compound of this element and oxygen?
A. XO
B. X2O
C. XO2
D. X2O3
E. X2O5

7. Which lists species with the same electron configuration?
A. Mg, Ca, Sr
B. Mg2+, Ca2+, Sr2+
C. S2-, Cl-, K+
D. Fe, Co, Ni
E. F-, S2-, As3-

8.One atomic mass unit (amu) is closest to the mass of
A. One proton
B. One electron
C. The oxygen-16 nucleus
D. The carbon-12 nucleus
E. 6.02X1023 atoms of hydrogen

9. All of these molecular shapes can be explained by dsp3 hybridization of electrons on the central atom EXCEPT
A. Linear
B. T-shape
C. See-saw
D. Octahedral
E. Trigonal bipyramidal

10. Which species has a Lewis dot diagram that does not illustrate the octet rule?

A. NO3-
B. NH3

C. NH4+
D. N2
E. NO2

11. Which substance has the greatest ionic character?
A. Cl2O
B. NCl3
C. PbCl2
D. BaCl2
E. Ch2Cl2

12. The shape of the IO3- ion is best described asA. see-saw
B. T-shaped
C. Tetrahedral
D. Trigonal planer
E. Trigonal pyramidal

13. Pi bonding is found in all of the following EXCEPT:
A. N2
B. SCN-
C. CO32-
D. AsH3
E. C(graphite)

14. What is the number of sp3 hybrid orbitals associated with the hydronium ion, H3O+?
A. none
B. two
C. three
D. four
E. six

15. Which change increases the mean free path of molecules in a sample of gas?
A. increase in pressure at constant temperature
B. increase in density at constant temperature
C. increase in temperature at constant pressure
D. increase in temperature at constant volume
E. increase in pressure at constant volume

16. Which occurs when a substance is converted from liquid to gas at the normal boiling point? I. Potential energy of the system increases.
II. The distance between molecules increases.
III. The average kinetic energy of the molecules increases.

A. I only

B. II only
C. I and II only
D. II and III only
E. I, II, and III

17. The lattice points of a crystal of hydrogen iodide, HI, are occupied by
A. HI molecules
B. H atoms and I atoms
C. H+ cations and I- anions
D. H2I+ cations and I- anions
E. H2 molecules and I2 molecules

18. Which element forms an oxide that is a molecular solid?
A. sodium
B. argon
C. carbon
D. silver
E. iron

19. What is the final concentration of Cl- ion when 250 mL of 0.20 M CaCl2 solution is mixed with 250 mL of 0.40 M KCl solution? (Assume additive volumes.)
A. 0.10 M
B. 0.20 M
C. 0.30 M
D. 0.40 M
E. 0.60 M

20. What volume of water should be added to 0.40 L of 6.0 M H2SO4 solution to produce a solution that is 2.0 M H2SO4?
A. 0.40 L
B. 0.80 L
C. 1.2 L
D. 1.6 L
E. 2.4 L

21. What is the percent methanol by mass in a solution that contains 20 grams of methanol, CH3OH, in 30 grams of water?
A. 20%
B. 33%
C. 40%
D. 60%
E. 67%

22. Compared to water, a 0.20 M solution of NaCl will have all of the following properties EXCEPT:
A. greater density
B. lower vapor pressure
C. lower boiling point
D. lower freezing point
E. greater osmotic pressure

23. In a spontaneous, exothermic dissolving process, which of these values has a negative sign?

I. /\Gsoln

II. /\Hsoln
III. T

A. I only
B. III only
C. I and II only
D. II and III only
E. I, II, and III

24. Which of these Group 2 oxides has the greatest percent by mass oxygen?
A. barium oxide
B. beryllium oxide
C. calcium oxide
D. magnesium oxide
E. strontium oxide

25. Which oxides of manganese, Mn, have percent by mass of manganese that is greater than 50%.

I. MnO II. MnO2 III. Mn2O2

A. II only
B. III only
C. I and III only
D. II and III only
E. I, II, and III

26. Which sample contains the greatest number of nitrogen atoms? (All measurements taken at STP.)
A. 0.20 mol N2O4(g)
B. 0.40 mol N2(g)
C. 40. L NO2(g)
D. 40. g NH3(g)
E. 80. g N2O4(g)

27. Al3+ + 3e- -----> Al0

In the half-reaction shown above, the 3e- represents

A. 3X96, 500 electrons
B. 3X(6.02 * 1023) electrons

C. 3X(6.02 * 1023) coulombs

D. 3/27X96, 500 electrons
E. 3/27X(6.02 * 1023) electrons

28. All of the following apply to the reaction A(g) + B(g) -----> C(g) as it is carried out at constant temperature in a rigid container EXCEPT:
A. The total pressure decreases
B. The rate of reaction decreases
C. The entropy of the system decreases
D. The number of molecules of C decreases
E. The frequency of collisions between molecule A and B decreases

29. At the beginning of one trial of this reaction, [A] = 4.0 and [B] = 1.0. The observed rate was 0.048 mol CL-1sec-1
Rate = k[A]2[B]

The value of the rate constant for this reaction is closest to
A. 3X102
B. 4X100
C. 8X10-1
D. 1X10-2
E. 3X10-3

30. Which is the label for the rate constant?
A. mol2L-2sec-1
B. Lmol-2sec-1
C. L2mol-2sec-1
D. L2sec(mol-1)
E. L2sec(mol-2 )

31. All of the following decrease the rate of a gas phase reaction EXCEPT
A. adding inert gas
B. removing the catalyst
C. increasing the volume
D. lowering the temperature
E. decreasing the concentration of one of the reactants

Rate = k[Br-][BrO3-][H+]2

32. The overall order for this reaction is
A. 2
B. 3
C. 4
D. 6
E. 12

33. The pH of a 0.010 M solution of a weak acid is 4.0. What is the value for the ionization constant, Ka, for this acid? A. 10-2
B. 10-4
C. 10-6
D. 10-8
E. 10-10

34. The Ksp for PbCl2 is 1.6 * 10–5. Which maximum amount of NaCl(s) may be added to 1.0 L of 0.010 Pb(NO3)2 solution without causing precipitate to occur?
A. 1.6 * 10-5 mol
B. 3.2 * 10-5 mol
C. 1.6 * 10-3 mol
D. 3.2 * 10-3 mol
E. 1.6 * 10-2 mol

35. 2O3(g) <===> 3O2(g) Kp = 2.5 * 1012

Consider a system at equilibrium based on the reaction above. In such a system, the concentration of O2(g) is

A. constant and equal to the concentration of O3(g)
B. constant and less than the concentration of O3(g)
C. constant and greater than the concentration of O3(g)
D. increasing and the concentration of O3(g) is increasing
E. increasing and the concentration of O3(g) is decreasing

36. The molar heat of fusion, /\Hfus, for water is 6.01 kJ / mol. Which expression gives the molar entropy of fusion, /\Sfus, in kJ / K * mol for ice at its normal melting point?
A. 6.01 / 273
B. 6.01 / 298
C. 6.01X4.18
D. 6.01X273
E. 6.01X298

37. All of the following reactions illustrate an increase in entropy EXCEPT:
A. N2O4(g) -----> 2NO2(g)
B. C6H6(l) -----> C6H6(g)
C. 2KClO3(s) -----> 3O2(g) + 2KCl(s)
D. 3Fe(s) + 2O2(g) -----> Fe3O4(s)
E. C2H5OH(l) + 3O2(g) -----> 2CO2(g) + 3H2O(g)

38. For the burning of propane

C3H8(g) + 5O2(g) -----> 3CO2(g)+4H2O(g) which of the following is true at any temperature?

I. /\G < 0
II. /\S > 0
III. /\H < 0

A. I only
B. III only
C. I and II only
D. II and III only
E. I, II, and III

39. Which is a polyprotic acid in water?

I. Ca(NO3)2
II. Na2HPO4
III. H3AsO4

A. I only
B. III only
C. II and III only
D. I and II only
E. I, II, and III

40. When solid potassium hydride is dissolved in water, which of the following is the strongest base in the resulting solution?
A. H+
B. K+
C. O2-
D. KH
E. OH-

41. Which range includes the pH that results when 0.10 mole NaOH is added to 100 mL of 1.0 M HCl solution?
A. between 1 and 4
B. between 4 and 6.5
C. between 6.5 and 7.5
D. between 7.5 and 10
E. between 10 and 14

42. Which range includes the pH that results when 0.10 mole of NaOH is added to 100 mL of 1.0 M H2SO4 solution?
A. between 1 and 4
B. between 4 and 6.5
C. between 6.5 and 7.5
D. between 7.5 and 10
E. between 10 and 14

43. AlCl3 + Cl- -----> AlCl4-

Which description applies to the reaction above?

A. amphoterism
B. anion hydrolysis
C. Arrhenius neutralization
D. Lewis acid-base reaction
E. Bronsted-Lowery proton transfer

Questions 44-45: Balance the following equation using the electron transfer method. You may wish to assign oxidation numbers and write the electronic equations for oxidation and reduction to help balance the overall reaction.

__ HNO3 + __ P + __ H2O ----> __ H3PO4 + __ NO

44. What is the sum of the coefficients in this balanced equation?
A. 5
B. 8
C. 10
D. 12
E. 18

45. What is the oxidizing agent in this equation?
A. P
B. H+
C. H2O
D. OH-
E. HNO3

46. Which is the best description of one faraday?
A. 8.31 joules
B. 96,500 amperes
C. one coulomb / volt
D. one joule / coulomb
E. 6.02 * 1023 electrons

47. H2O + Br2 -----> HOBr + HBr

Which is the best description of the behavior of bromine in the reaction above?
A. oxidized, only
B. proton donor
C. proton acceptor
D. both oxidized and reduced
E. neither oxidized nor reduced

48. Which organic compound is an electrolyte?
A. C2H6
B. CH3Cl
C. HCOOH
D. CH3OH
E. C6H12O6

49. In the complete combustion of butane, the products are
A. water and carbon
B. butanone and water
C. butanoic acid and water
D. carbon dioxide and water
E. carbon dioxide and hydrogen

50. The compound, 2-methyl-2-propanol, is an isomer of
A. butane
B. propane
C. butanol
D. propanoi
E. methanol

51. What is the number of isomers possible for C2H2Cl2?
A. 1
B. 2
C. 3
D. 4
E. 5

52. Which is most likely to be formed in the chemical reaction that occurs when a gas phase mixture of C4H10 and Cl2 is subjected to ultraviolet light?
A. H2
B. HCl
C. CCl4
D. C4H11Cl
E. C4H10Cl2

53. What is the total number of shared electron pairs between adjacent carbon atoms in a propyne molecule?
A. 1
B. 2
C. 3
D. 4
E. 5

54. Which general formula applies to hydrocarbons with one double covalent between adjacent atoms?
A. CnH2n+2
B. CnH2n
C. CnH2n-2
D. CnH2n-4
E. CnH2n-6