MULTIPLE CHOICE

1. The number of significant figures in 7.360 x 10^-3 is

a.3.

b.4.

c.5.

d.6.

e.7.

2. What is the best answer to the following expression?

(12.125+0.530+71.4)

a.84.055

b.84.06

c.84.1

d.84.0

e.84

3. How many cubic meters equal one cubic millimeter?

a.10⁹

b.10⁶

c.10^-2

d.10^-6

e.10^-9

4. A car averages 35 miles per gallon of gasoline.How many liters of gasoline will be needed for a trip of 450 kilometers?Some conversion factors, which may be helpful are the following:

1 qt = 0.946 L.

1 mile = 1.609 km.

1000 m = 1 km.

4 qt = 1 gallon.

1 ft = 12 inches.

a.2.5 x 10¹ L

b.3.0 x 10¹ L

c.3.5 x 10¹ L

d.4.0 x 10¹ L

e.4.5 x 10¹ L

5. Which of the following is an example of a chemical change?

a.water boiling

b.ice melting

c.natural gas burning

d.alcohol evaporating

e.iodine vaporizing

6.How many protons, neutrons, and electrons are in the tin(II) ion,.‹

Sn²⁺?

a.119p, 50n, 119e

b.50p, 69n, 50e

c.50p, 69n,48e

d.69p, 50n, 69e

e.50p, 119n, 52e

7. The formula of aluminum sulfite is

a.Al₂(SO₃)₃.

b.Al₂(SO₄)₃.

c.Al₃(SO₄)₂.

d.Al₂S₃.

e.Al₃S₂.

8. The formula of chlorous acid is

a.HClO.

b.HClO₂.

c.HClO₃.

d.HClO₄.

e.HCl.

9. Energy from the following reaction provided the lift for the moon lander:

__ (CH₃)₂N₂H₂ + __ N₂O₄ -->__ N₂ + __ H₂O + __ CO₂

When the equation is balanced, the coefficient of nitrogen is

a.1.

b.2.

c.3.

d.4.

e.5.

10. Which of the following equations is (are) balanced?

1.NaCl + Pb(NO₃)_2-->PbCl₂ + NaNO₃

2.(NH₄)₂Cr₂O_7-->N₂ + 4H₂O + Cr₂O₃

3.Fe₃O₄ + 3CO-->3Fe + 3CO₂

a.1 only

b.2 only

c.3 only

d.1 and 2 only

e.1, 2, and 3

12. All of the following are strong acids in aqueous solution except

a.HClO₄.

b.H₃PO₄.

c.H₂SO₄.

d.HNO₃.

e.HCl.

13. What products result from the addition of aqueous solutions of Cu(NO₃)₂ and (NH₄)₂S?

a.CuS(aq) and NH₄NO₃(s)

b.CuS(s) and NH₄NO₃(s)

c.CuS(s) and NH₄NO₃(aq)

d.Cu₂S(s) and NH₄NO₃(aq)

e.CuS(s), NH₃(g), and H₂S(g)

14. All of the following are oxidation-reduction reactions except

a.2Al(s)+Fe₂O₃(s)-->Al₂O₃(s)+2Fe(s).

b.(NH₄)₂Cr₂O₇(s)-->Cr₂O₃(s)+N₂(g)+4H₂O(l).

c.Cu(s)+2H₂SO₄(aq)-->CuSO₄(aq)+SO₂(g)+2H₂O(l).

d.Hg(NO₃)₂+4KI-->K₂HgI₄(aq)+2 KNO₃(aq).

e.2Na(s)+2H₂O(l)-->2NaOH(aq)+H₂(g).

15. All of the following salts are insoluble except

a.lead(II) sulfide.

b.lead(II) sulfate.

c.lead(II) nitrate.

d.lead(II) carbonate.

e.lead(II) phosphate.

16. The net ionic equation for the reaction of the weak acid, carbonic acid, with barium hydroxide to form a precipitate is

a.H₂CO₃(aq) + Ba(OH)₂(aq)-->BaCO₃(s) + 2H₂O(l).

b.2H⁺(aq) + CO₃^2-(aq) + Ba²⁺(aq) + 2OH^-(aq)-->BaCO₃(s) + H₂O(l).

c.H₂CO₃(aq) + Ba²⁺(aq) + 2OH^-(aq)-->Ba²⁺(aq) + CO₃^2-(aq) +

4H⁺(aq) + 2O^2-(aq).

d.H₂CO₃(aq) + Ba²⁺(aq) + 2OH^-(aq)-->BaCO₃(s) + 2H₂O(l).

e.H⁺(aq) + HCO₃^-(aq) + Ba(OH)₂(aq)-->Ba²⁺(aq) + CO₃^2-(aq) +

2H₂O(l).

17. What is the oxidation number of P in H₃PO₃?

a.-3

b.0

c.+1

d.+3

e.+7

18. What is the average oxidation number of S in S₂O₃^2-?

a.2

b.2.5

c.4

d.4.5

e.6

19. In the following oxidation-reduction reaction,

8H⁺(aq) + 6Cl^-(aq) + Sn(s) + 4NO₃^-(aq)-->SnCl₆^2-(aq) + 4NO₂(g) + 4H₂O

the oxidizing agent is

a.H⁺.

b.Cl^-.

c.Sn.

d.NO₃^-.

e.SnCl₆^2-.

20. The following reaction occurs in acid solution.

NO₃^- + I^--->IO₃^- + NO₂

In the balanced equation, the coefficient of NO₃^- is

a.2.

b.3.

c.4.

d.5.

e.6.

21. The following change occurs in acidic solution:

S^2- + Cr₂O₇^2- --> S + Cr³⁺

Complete and balance the foregoing equation.In the balanced equation, for every mole of Cr₂O–^2- that reacts, _____ moles of H⁺ are consumed.

a.5

b.7

c.8

d.10

e.14

22. Sodium cyclamate, C₆H₁₁NHSO₃Na, was used at one time as an artificial sweetener.C₆H₁₁NHSO₃Na has a molecular mass of 201.2 g/mol.How many moles of sodium cyclamate are contained in a 25.6 g sample?

a.0.127

b.0.193

c.0.245

d.7.86

e.5180

23. What is the percentage of nitrogen in ammonium phosphate, (NH₄)₃PO₄?

a.11.6%

b.16.0%

c.28.2%

d.31.9%

e.34.3%

24. A 3.22 g sample of an oxide of chromium contains 2.00 g of chromium. Calculate the simplest formula of the compound.

a.CrO

b.Cr₂O

c.CrO₂

d.Cr₂O₃

e.CrO₃

25.2KHCO₃(s)-->K₂CO₃(s) + CO₂(g) + H₂O(l)

How many moles of carbon dioxide will be produced if 100.0 g of potassium hydrogen carbonate are heated?

a.0.250

b.0.500

c.1.00

d.2.00

e.25.0

26. How much 0.54 M NaCl, (physiological saline) can be prepared via the dilution of 100 mL of a 6.0 M NaCl solution?

a.1.1 L

b.910 mL

c.90 mL

d.540 mL

e.1.9 L

27. What volume of acid must you use to prepare 100 mL of 0.50 M HCl from 2.00 M HCl?

a.25.0 mL

b.50.0 mL

c.100. mL

d.200. mL

e.400. mL

28. The pressure of 4.0 L of nitrogen in a flexible container is decreased to one-third of its original pressure, and its absolute temperature is decreased by one-half.The volume is now

a.1.0 L.

b.4.0 L.

c.6.0 L.

d.8.0 L.

e.24 L.

29. At standard conditions it was found that 1.15 L of a gas weighed 3.96 g.Its molecular mass is

a.3.96 g/mol.

b.11.5 g/mol.

c.39.6 g/mol.

d.47.2 g/mol.

e.77.1 g/mol.

30. It takes 16.6 min for a 10.0-mL sample of an unknown gas to effuse through a pinhole.A 10.0-mL sample of helium, He, required 5.00 min. What is the molecular weight of the unknown gas?

a.13.3 g/mol

b.44.1 g/mol

c.177 g/mol

d.7.3 g/mol

e.53.1 g/mol

31. A 150.0-g sample of metal at 80.0øC is added to 150.0 g of H₂O at 20.0øC.The temperature rises to 23.3øC.Assuming that the calorimeter is a perfect insulator, what is the specific heat of the metal?(Specific heat of H₂O is 4.18 J/gøC.)

a.-0.48 J/gøC

b.0.24 J/gøC

c.0.48 J/gøC

d.0.72 J/gøC

e.0.96 J/gøC

32. Consider the following specific heats of metals.

MetalSpecific Heat

copper0.385 J/(g ú øC)

cobalt0.418 J/(g ú øC)

chromium0.447 J/(g ú øC)

gold0.129 J/(g ú øC)

silver0.237 J/(g ú øC)

If the same amount of heat is added to 100-g samples of each of the metals, which are all at the same temperature, which metal will reach the lowest temperature?

a.copper

b.cobalt

c.chromium

d.gold

e.silver

34. What is the molar heat of combustion of methanol, CH₃OH, if combustion of 1.00 g of methanol causes a temperature rise of 3.68øC in a bomb calorimeter that has a heat capacity of 6.43 kJ/øC?(Formula weight CH₃OH = 32.0)

a.55.9 kJ/mol

b.923 kJ/mol

c.757 kJ/mol

d.18.3 kJ/mol

e.368 kJ/mol

35. From a consideration of the reaction

2NO(g) + O₂(g)-->2NO₂(g)H = -114.1 kJ

if 2.00 x 10² g of NO₂ were produced, then the amount of heat released should be

a.114 kJ.

b.124 kJ.

c.248 kJ.

d.314 kJ.

e.496 kJ.

36. The equation for the standard enthalpy of formation of potassium bromate, KBrO₃, corresponds to which reaction?

a.K(s) + 1/2 Br₂(g) + 3/2 O₂(g)-->KBrO₃(s)

b.K(g) + 1/2 Br₂(g) + 3/2 O₂(g)-->KBrO₃(s)

c.K(s) + 1/2 Br₂(l) + 3/2 O₂(g)-->KBrO₃(s)

d.K(g) + Br(g) + 3O(g)-->KBrO₃(s)

e.K(s) + Br(g) + 3O(g)-->KBrO₃(s)

38. What is the wavelength of light associated with the radiation of 7.26 x 10^-‹ J/photon? (h = 6.63 4 x 10^-„… J ú s)

a.137 nm

b.231 nm

c.274 nm

d.548 nm

e.684 nm

40. The number of orbitals in a d subshell is

a.1.

b.2.

c.3.

d.5.

e.7.

41. Which of the following orbital diagrams represents a diamagnetic atom?

42. Which one of the following elements would be expected to have the largest atomic radius?

a.Li

b.Cs

c.F

d.Br

e.I

43. Which of the following elements has the smallest first ionization energy?

a.P

b.K

c.C

d.Mg

e.Ar

44. What is the electron configuration of Fe³⁺?

a.[Ar] 3d⁶ 4s²

b.[Ar] 3d³ 4s²

c.[Ar] 3d⁴ 4s¹

d.[Ar] 3d⁵

e.[Ar] 3d⁶

45. Which of the following species is isoelectronic with Kr?

a.Xe

b.K⁺

c.In³⁺

d.S^2-

e.Sr²⁺

46. The number of valence electrons in the nitrite ion is

a.16.

b.18.

c.22.

d.23.

e.24.

47. The octet rule is violated by at least one atom in each of the following species except

a.ICl₂^-.

b.CH₃^-.

c.BF₄^-.

d.SF₄.

e.ClF₃.

48. Which of the following covalent molecules does not have the proper Lewis formula?

49. The geometry of the carbonate ion, CO₃^2-, is best described as

a.linear.

b.trigonal planar.

c.tetrahedral.

d.bent.

e.trigonal pyramidal.

50. Of the following, the molecule or ion whose shape is not planar is

a.SeO₃^2-.

b.H₂CO.

c.C₂H₄.

d.BF₃.

e.SO₃.

51. Which one of the following species has a flat triangular structure?

a.NH₃

b.AsF₃

c.HCN

d.SO₃

e.ClO₃^-

52. When a carbon atom has sp³ hybridization, it has

a.four sigma bonds.

b.three sigma bonds and one pi bond.

c.two sigma bonds and two pi bonds.

d.one sigma bond and three pi bonds.

e.four pi bonds.

53. All of the following molecules will be nonpolar except