Chemistry in Focus A Molecular View of Our World 5th Edition by Nivaldo J. Tro – Test Bank

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Chemistry in Focus A Molecular View of Our World 5th Edition by Nivaldo J. Tro – Test Bank

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Chapter 2—The Chemist’s Toolbox

 

MULTIPLE CHOICE

 

1. Significant figures represent the ___________ of a measurement.

a.	accuracy
b.	precision
c.	both precision and accuracy
d.	neither precision nor accuracy

 

 

ANS:  B                    PTS:   1

 

2. When adding and subtracting the number of significant figures in the answer is determined by __________.

a.	the most precise number
b.	the least precise number
c.	the number with the most significant figures in the calculation
d.	the number with the fewest significant figures in the calculation

 

 

ANS:  B                    PTS:   1

 

3. When multiplying and dividing, the number of significant figures in the answer is determined by ________________.

a.	the most precise number
b.	the least precise number
c.	the number with the most significant figures in the calculation
d.	the number with the fewest significant figures in the calculation

 

 

ANS:  D                    PTS:   1

 

4. How many significant figures are there in the number 10.00?

a.	1
b.	2
c.	3
d.	4

 

 

ANS:  D                    PTS:   1

 

5. How many significant figures are there in the number 10,100?

a.	1
b.	3
c.	4
d.	5

 

 

ANS:  B                    PTS:   1

 

6. Calculate the density with the correct number of significant figures of a 50.0 g sample of mercury with a volume of 3.66 mL.

a.	13.66 g/mL
b.	13.7 mL
c.	183 g/mL
d.	0.0732 g/mL
e.	0.073 g/mL

 

 

ANS:  B                    PTS:   1

 

7. Calculate the density to the correct number of significant figures of a 100.0 g sample of mercury which occupies a volume of 7.36 cm³.

a.	13.7 g/mL
b.	13.66 g/mL
c.	183 g/mL
d.	0.0732 g/mL
e.	0.073 g/mL

 

 

ANS:  A                    PTS:   1

 

8. Determine the mass in grams of a gold sample which occupies a volume of 16.39 mL? Gold has a density of 19.3 g/mL.

a.	0.118 g
b.	0.316 g
c.	0.849 g
d.	1.18 g
e.	316 g

 

 

ANS:  E                    PTS:   1

 

9. Determine the volume occupied by 1.5 g of ethyl alcohol. The density of ethyl alcohol is 0.789 g/mL.

a.	1.9 mL
b.	1.3 mL
c.	0.53 mL
d.	0.526 mL
e.	1.331 mL

 

 

ANS:  A                    PTS:   1

 

10. Chloroform is a commonly used anesthetic with a density of 1.483 g/mL. Determine the volume of chloroform needed to deliver a 9.37 g sample of the anesthetic.

a.	0.158 g
b.	6.32 g
c.	13.9 g
d.	13.89 g
e.	0.0632 g

 

 

ANS:  B                    PTS:   1

 

11. If 15.0 mL of a metal has a mass of 103.0 g, what is the density of the metal?

a.	6.87 g/mL
b.	1550 g/ mL
c.	0.146 g/mL
d.	1.46 g/mL
e.	None of these.

 

 

ANS:  A                    PTS:   1

 

 

12. The density of gold is 19.3 g/mL. If the current price of gold is $56.75 per gram, what is the volume of a nugget of gold worth $150.00?

a.	1.15 mL
b.	0.868 mL
c.	1.72 mL
d.	1.27 mL
e.	0.137 mL

 

 

ANS:  E                    PTS:   1

 

13. Which is the standard SI unit for mass?

a.	gram
b.	pound
c.	ounce
d.	kilogram
e.	ton

 

 

ANS:  D                    PTS:   1

 

14. Which is the standard SI unit for length?

a.	meter
b.	feet
c.	mile
d.	kilometer
e.	centimeter

 

 

ANS:  A                    PTS:   1

 

15. Which is the correct SI unit for time?

a.	meter
b.	hour
c.	second
d.	minute
e.	gram

 

 

ANS:  C                    PTS:   1

 

16. Which of these represents the SI prefix for micro (m)?

a.	10–6
b.	10–3
c.	10–9
d.	10–2
e.	106

 

 

ANS:  A                    PTS:   1

 

17. Which of these represents the SI prefix for centi (c)?

a.	10–6
b.	10–3
c.	10–1
d.	10–2
e.	106

 

 

ANS:  D                    PTS:   1

 

 

18. Which of these represents the SI prefix for mega (M)?

a.	109
b.	106
c.	103
d.	10–2
e.	10–6

 

 

ANS:  B                    PTS:   1

 

19. The diameter of the nucleus of an atom is approximately 1 ´ 10^–13 meters. If 1 nm is equal to 10 Angstroms, what is the diameter of the nucleus in Angstroms? (1 nm = 1 x 10^–9 meter)

a.	1 ´ 10–21 A
b.	1 ´ 10–6 A
c.	1 ´ 10–5 A
d.	1 ´ 10–4 A
e.	1 ´ 10–3 A

 

 

ANS:  E                    PTS:   1

 

20. Convert 89.5 meters to millimeters.

a.	8.95 ´ 104 mm
b.	8.95 ´ 10–4 mm
c.	8.95 ´ 102 mm
d.	8.95 ´ 10–2 mm
e.	None of these.

 

 

ANS:  A                    PTS:   1

 

21. Which of the following is not true.

a.	1 cm = .01 m
b.	100 cm = 1 m
c.	1 cm = 100m
d.	.01 cm = .0001m
e.	10000 cm = 100 m

 

 

ANS:  C                    PTS:   1

 

22. Given that 1 in = 2.54 cm, which of the following is true?

a.	1 in2 = 2.54 cm2
b.	1 in2 = 5.08 cm2
c.	1 in2 = 6.45 cm2
d.	1 in2 = 1.27 cm2
e.	None of these.

 

 

ANS:  C                    PTS:   1

 

23. One m³ equals ____________.

a.	1000 mm3
b.	1,000,000 mm3
c.	1,000,000,000 mm3
d.	1,000,000,000,000 mm3

 

 

ANS:  C                    PTS:   1

 

 

24. One milliliter is equal to ___________.

a.	2.54 cubic inches
b.	1000 liters
c.	1 cubic centimeter
d.	16.39 cubic inches

 

 

ANS:  C                    PTS:   1

 

25. 1.00 in³ equals ________.

a.	2.54 cm3
b.	7.62 cm3
c.	16.4 cm3
d.	.394 cm3

 

 

ANS:  C                    PTS:   1

 

26. The long jump record is 8.90 m. What is the length in inches? (1 m = 39.37 inches)

a.	9.73 inches
b.	293 inches
c.	350 inches
d.	4204 inches
e.	5000 inches

 

 

ANS:  C                    PTS:   1

 

27. The long jump record is 8.90 m. What is the length in yards? (1 yd = 0.9144 m)

a.	9.73 inches
b.	293 inches
c.	350 inches
d.	4204 inches
e.	5000 inches

 

 

ANS:  A                    PTS:   1

 

28. A football field is 100.0 yards long. What is its length in meters? (1 yd = 0.9144 m)

a.	0.09144 m
b.	91.44 m
c.	274.32 m
d.	334 m
e.	9.144 ´ 103 m

 

 

ANS:  B                    PTS:   1

 

29. A football field is 100 yards long. What is its length in centimeters? (1 yd = 0.9144 m)

a.	0.09144 cm
b.	91.44 cm
c.	274.32 cm
d.	334 cm
e.	9.144 ´ 103 cm

 

 

ANS:  E                    PTS:   1

 

 

30. How many kilograms of calcium are there in a 173 pounds of calcium?(1 pound = 454 grams)

a.	1.1 kg
b.	78.54 kg
c.	1.1 ´ 102 kg
d.	3.8 ´ 104 kg
e.	7.85 ´ 104 kg

 

 

ANS:  E                    PTS:   1

 

31. Most races are now measured in kilometers. What is the distance in miles a runner must complete in a 10 kilometer run. (1 km = 0.62137 mile)

a.	3.1 miles
b.	6.2 miles
c.	16.1 miles
d.	32.2 miles
e.	62.137

 

 

ANS:  B                    PTS:   1

 

32. Convert 2.50 ´ 10⁴. meters to miles ( 1 mile = 5280 feet).

a.	76.2 miles
b.	6.35 miles
c.	15.5 miles
d.	155 miles
e.	186 miles

 

 

ANS:  C                    PTS:   1

 

33. Convert 10.5 mm/s to ft/hr.

a.	124 ft/hr
b.	9.57 ´ 10–6 ft/hr
c.	.0344 ft/hr
d.	37800 ft/hr
e.	None of these.

 

 

ANS:  A                    PTS:   1

 

34. Which of these numbers has the most significant figures?

a.	0.5071
b.	0.201
c.	6.02 ´ 1023
d.	51
e.	103

 

 

ANS:  A                    PTS:   1

 

35. Solve the problem.

 

3.728 + 6.272

a.	10
b.	10.0
c.	10.00
d.	10.000
e.	10.0000

 

 

ANS:  D                    PTS:   1

 

36. Solve the problem.

 

3.72 ´ 10⁸ ´ 9.26 ´ 10^–3

a.	3.44 ´ 106
b.	4.02 ´ 1010
c.	3.45 ´ 105
d.	3.44 ´ 10–4
e.	4.02 ´ 10–10

 

 

ANS:  A                    PTS:   1

 

37. Solve the problem.

 

1.5 ´ 10³ + 3.14 ´ 10⁴  – 1.21 ´ 10² = ?

a.	3.28 ´ 104
b.	3.30 ´ 103
c.	3.3 ´ 10–4
d.	3.30 ´ 105
e.	3.43 ´ 109

 

 

ANS:  A                    PTS:   1

 

38. Solve the problem.

 

(5.46 ´ 10⁷ + 3.13 ´ 10⁶) ´ (7.65 ´ 10⁵)

a.	65.7 ´ 1018
b.	130.7 ´ 1018
c.	4.42 ´ 1013
d.	2.39 ´ 1012
e.	65.7 ´ 108

 

 

ANS:  C                    PTS:   1

 

39. Solve the problem.

 

(3.21 ´ 10¹⁰ – 3.13 ´ 10¹²) ¸ (7.65 ´ 10⁵)

a.	4.13 ´ 106
b.	2.37 ´ 1018
c.	65.7 ´ 1018
d.	-23.7 ´ 1017
e.	-4.04 ´ 106

 

 

ANS:  E                    PTS:   1

 

 

40. Solve the problem.

 

(12.67 ´ 4.23) ¸ 23.42

a.	2.3
b.	2.29
c.	2.228
d.	2.88
e.	2.2884

 

 

ANS:  B                    PTS:   1

 

41. 0.01% is equivalent to which of the following?

a.	100 ppm
b.	100 ppb
c.	0.000001 ppm
d.	0.000001 ppb
e.	None of these.

 

 

ANS:  A                    PTS:   1

 

42. Which of these is the correct scientific notation for 6,000,220?

a.	6.022 ´ 105
b.	6.00022 ´ 105
c.	6.00022 ´ 106
d.	6.00022 ´ 10–5
e.	6.00022 ´ 10–6

 

 

ANS:  C                    PTS:   1

 

43. Which of the following is correctly written in scientific notation?

a.	50.0 ´ 106
b.	4.02 ´ 10216
c.	1 ´ 10–6.8
d.	1.005 ´ 10–9.05
e.	10–5

 

 

ANS:  B                    PTS:   1

 

44. Which of these is incorrectly matched?

a.	centi     c     10–2
b.	mega     M     106
c.	milli     m     10–3
d.	nano     n     109
e.	micro     m     10–6

 

 

ANS:  D                    PTS:   1

 

 

Figure 2-1

 

 

45. Refer to Figure 2-1. What is the pH of the solution after 8 mL of base have been added.

a.	3
b.	4
c.	6
d.	7
e.	8

 

 

ANS:  B                    PTS:   1

 

46. Refer to Figure 2-1. What affect was there on the pH of the solution when the volume of base added was increased from 8 mL to 13 mL?

a.	The pH dropped by a value of 4.
b.	The pH increased by a value of 4.
c.	The pH remained relatively unchanged.
d.	The pH increased by a value of 10.
e.	The pH increased by a value of 20.

 

 

ANS:  B                    PTS:   1

 

47. Refer to Figure 2-1. Which of these statements is true based on the data provided by the graph.

a.	The pH of the solution is must be determined algebraically.
b.	The pH of the solution is relatively unaffected by the addition of base.
c.	The pH of the solution is 7 when approximately 12 mL of base have been added.
d.	The pH of the solution is relatively constant with addition of the first 14 mL of base.
e.	The pH of the solution rises significantly when the volume is increased from 14 mL to 18 mL.

 

 

ANS:  C                    PTS:   1

 

48. Which of these numbers has the four significant figures?

a.	0.3211
b.	0.201
c.	6.02 ´ 1023
d.	5100
e.	0.0103

 

 

ANS:  A                    PTS:   1

 

 

49. Solve the problem.

 

131.7 ´ 1.05

a.	1.38 ´ 103
b.	1.38 ´ 102
c.	1.3 ´ 103
d.	1.3 ´ 103
e.	1.3 ´ 10–3

 

 

ANS:  B                    PTS:   1

 

50. Solve the problem.

 

33.5 ¸ 3.011

a.	1.11 ´ 101
b.	1.11 ´ 103
c.	1.113 ´ 101
d.	1.11 ´ 102
e.	1.112587 ´ 101

 

 

ANS:  A                    PTS:   1

 

51. Which of these is the correct normal decimal notation for 5.23 ´ 10^–4?

a.	0.0523
b.	0.00523
c.	0.0000523
d.	0.000523
e.	52,300

 

 

ANS:  D                    PTS:   1

 

52. Which of these is the correct normal notation for 7.77 ´ 10⁷?

a.	0.000000777
b.	0.0777
c.	7,770
d.	7,770,000
e.	77,700,000

 

 

ANS:  E                    PTS:   1

 

53. Which of these is the correct normal notation for 8.14 ´ 10⁵?

a.	0.0000814
b.	0.000814
c.	81.400
d.	814,000
e.	81,400,000

 

 

ANS:  D                    PTS:   1

 

 

54. Which of these series correctly orders the values given from smallest to largest?

 

I.	100 cm
II.	1 km
III.	10 m
IV.	100,000 mm

 

a.	I < II < III < IV
b.	II < I < IV < III
c.	I < II = III < IV
d.	I < IV < III < II
e.	I < III < IV < II

 

 

ANS:  E                    PTS:   1

 

55. Which of these series correctly orders the values given from smallest to largest?

 

I.	0.001 Mg
II.	2,000,000 ng
III.	1 Gg
IV.	100,000 cg

 

a.	III < II < II < IV
b.	II < I < IV < III
c.	II < I = IV < III
d.	I < IV = III < II
e.	I < III < IV < II

 

 

ANS:  C                    PTS:   1

 

56. Because of the high heat and humidity in the summer in Death Valley, California, a hiker requires about 1 quart of water for every two miles traveled on foot. If the density of water is 0.999 g/mL at 45(C, how many kilograms of water are required for a person to walk 30 kilometers in Death Valley? (1 L = 1.0567 qt; 1 km = 0.62317 mi)

a.	8.8 kg
b.	70 kg
c.	350 kg
d.	700 kg
e.	8.8 ´ 103 kg

 

 

ANS:  A                    PTS:   1

 

57. A sample of molten iron occupies of a volume of 7.11 ´ 10^–3 L. If the density of iron is 7.86 g/cm³, what is the mass of iron in grams in the sample?

a.	0.000904 g
b.	0.0559 g
c.	0.904 g
d.	1.105 g
e.	55.85 g

 

 

ANS:  E                    PTS:   1

 

 

58. An irregular shaped piece of metal with a mass of 220 g was placed in a graduated cylinder that contained 35.00 mL of water. This raised the water level to 52.50 mL. What is the density of the metal?

a.	0.285 g/mL
b.	4.19 g/mL
c.	17.5 g/mL
d.	12.6 g/mL
e.	38.5 g/mL

 

 

ANS:  D                    PTS:   1

 

59. An irregular shaped piece of metal with a mass of 105 g was placed in a graduated cylinder that contained 25.00 mL of water. This raised the water level to 45.35 mL. What is the density of the metal?

a.	0.238 g/mL
b.	2.3 g/mL
c.	4.2 g/mL
d.	5.16 g/mL
e.	20.35 g/mL

 

 

ANS:  D                    PTS:   1

 

60. Convert 4.5 inches to meters. (2.54 cm = 1 inch)

a.	0.1143 m
b.	1.77 m
c.	11.43 m
d.	0.0177 m
e.	1143 m

 

 

ANS:  A                    PTS:   1

 

61. Determine the volume in liters of a 1.00 ounce bottle.(1.06 qt = 1 L; 32 ounces = 1 qt)

a.	0.0295 L
b.	0.03125 L
c.	0.03313 L
d.	30.2 L
e.	33.9 L

 

 

ANS:  A                    PTS:   1

 

62. A regulation soccer field is 110.0 yards in length. Calculate the length in millimeters. (1.094 yards = 1 m)

a.	0.101 mm
b.	1.01 mm
c.	100.5 mm
d.	1.01 ´ 104 mm
e.	1.01 ´ 105 mm

 

 

ANS:  E                    PTS:   1

 

 

63. A 5 foot 7 inch track athlete weighs 110 pounds. What his her height in cm and her weight in kilograms? (2.54 cm = 1 inch; 454 g = 1 pound)

a.	14.5 cm     242 kg
b.	152 cm     49.9 kg
c.	170 cm     49.9 kg
d.	154 cm     242 kg
e.	152 cm     4.99 ´ 104 kg

 

 

ANS:  C                    PTS:   1

 

64. Chemical waste is often shipped in 55-gallon drums. What is the weight in pounds of a 55-gallon drum if the density of the waste is 1.5942 g/cm³? (454 g = 1 pound; 0.9463 L = 1 quart; 4 quarts = 1 gallon)

a.	130 lbs
b.	730 lbs
c.	810 lbs
d.	4.5 ´ 104 lbs
e.	5.9 ´ 104 lbs

 

 

ANS:  B                    PTS:   1

 

65. Solve the problem.

 

5.6 ´ 10² ´ 7.41 ´ 10³ = ?

a.	232 ´ 101
b.	7.55 ´ 105
c.	2.32 ´ 105
d.	4.1 ´ 106
e.	232 ´ 105

 

 

ANS:  D                    PTS:   1

 

66. What is the mass in kilograms of a 25.00 pound dumbbell? (454 g = 1 pound)

a.	1.377 ´ 10–3 kg
b.	1.377 kg
c.	11.35 kg
d.	1.377 ´ 103 kg
e.	1.135 ´ 107 kg

 

 

ANS:  C                    PTS:   1

 

67. An international group of zookeepers with successful breeding programs made the following animal exchanges last year. Using the same bartering system, how many monkeys can a zoo obtain in exchange for 15 flamingos?

 

3 oryxes = 1 tiger	2 flamingos = 1 anteater
1 camel = 6 anteaters	5 lemurs = 1 rhino
1 rhino = 4 monkeys	3 lemurs = 1 camel
3 monkeys = 1 tiger	1 rhino = 4 oryxes

 

a.	3 monkeys
b.	5 monkeys
c.	8 monkeys
d.	12 monkeys
e.	15 monkeys

 

 

ANS:  A                    PTS:   1

 

68. Which of these samples of aluminum will occupy the greatest volume?(Density of aluminum = 2.70 g/cm³; 454 g = 1 pound)

a.	10,000 g
b.	25 pounds
c.	1 kg
d.	5 ´ 10–2 L
e.	2,000 mL

 

 

ANS:  B                    PTS:   1

 

69. Which of these samples of water will have the greatest mass?(Density of water = 1.00 g/cm³; 454 g = 1 pound)

a.	10,000 g
b.	25 pounds
c.	1 kg
d.	5 ´ 10–2 L
e.	2,000 mL

 

 

ANS:  B                    PTS:   1

 

70. Solve the following equation for y.

 

3y + 24 = 6y – 3

a.	3
b.	6
c.	7
d.	8
e.	12

 

 

ANS:  C                    PTS:   1

 

71. Solve the following equation for y.

 

3y = 24

a.	3
b.	6
c.	7
d.	8
e.	12

 

 

ANS:  D                    PTS:   1

 

72. Solve the following equation for z.

 

2(z + 6) – 10 = 42

a.	6
b.	10
c.	12
d.	20
e.	40

 

 

ANS:  D                    PTS:   1

 

 

73. Solve the following equation for z.

 

4z ¸ 2z + 3 = 30

a.	2
b.	6.25
c.	10
d.	11
e.	13.5

 

 

ANS:  E                    PTS:   1

 

74. Solve the following equation for x: 13x = x + 156

a.	13
b.	20
c.	1
d.	7
e.	12

 

 

ANS:  A                    PTS:   1

 

Chapter 4—Molecules, Compounds, and Chemical Reactions

 

MULTIPLE CHOICE

 

1. Which of these substances is a compound?

a.	Na
b.	Cl2
c.	Pb
d.	NO
e.	H2

 

 

ANS:  D                    PTS:   1

 

2. Which of these substances is a compound?

a.	air
b.	salt water
c.	gasoline
d.	salt
e.	lemonade

 

 

ANS:  D                    PTS:   1

 

3. A tiny crystal of sodium chloride contains 5,000,000 sodium ions and 5,000,000 chloride ions. The correct formula for sodium chloride is:

a.	NaCl
b.	Na5Cl5
c.	Na50Cl50
d.	It could be any of the above.
e.	None of the above

 

 

ANS:  A                    PTS:   1

 

4. A tiny amount of magnesium chloride contains 150 magnesium ions and 300 chloride ions.  The correct formula for magnesium chloride is:

a.	MgCl
b.	Mg2Cl
c.	MgCl2
d.	Mg150Cl300

 

 

ANS:  C                    PTS:   1

 

5. Methane can be decomposed into two simpler substances, hydrogen and carbon. Therefore, methane

a.	is a gas.
b.	is an element.
c.	is a mixture.
d.	is a compound.
e.	must have the formula CH.

 

 

ANS:  D                    PTS:   1

 

 

6. Which is of these is the correct ratio of sulfur to oxygen in SO₂?

a.	1 sulfur: 2 oxygen
b.	2 sulfur: 1 oxygen
c.	2 sulfur: 2 oxygen
d.	2 sulfur: 3 oxygen
e.	1 sulfur: 3 oxygen

 

 

ANS:  A                    PTS:   1

 

7. Which is of these is the correct chemical formula for carbon tetrachloride?

a.	CCl3
b.	CCl4
c.	CCl5
d.	C4Cl
e.	None of the above

 

 

ANS:  B                    PTS:   1

 

8. Metals tend to ____ electrons and form ions with a ____ charge?

a.	lose, positive
b.	lose, negative
c.	gain, positive
d.	gain, negative
e.	lose , zero

 

 

ANS:  A                    PTS:   1

 

9. Nonmetals tend to ____ electrons and form ions with a ____ charge?

a.	lose, positive
b.	lose, negative
c.	gain, positive
d.	gain, negative
e.	lose , zero

 

 

ANS:  D                    PTS:   1

 

10. Which statement about ionic compounds is incorrect?

a.	Ionic compounds contain nondirectional bonds.
b.	Ionic solids dissolved in water will conduct electricity.
c.	Ionic bonds are formed between metals and nonmetals.
d.	Ionic bonds involve the sharing of electrons by metals and nonmetals.
e.	Ionic compounds are held together by attraction between positive and negative ions.

 

 

ANS:  D                    PTS:   1

 

11. Which of these will not form a positive ion in an ionic compound?

a.	Ba
b.	Rb
c.	P
d.	Sn
e.	Mg

 

 

ANS:  C                    PTS:   1

 

 

12. Which of these will not form a negative ion in an ionic compound?

a.	Br
b.	N
c.	Se
d.	I
e.	Al

 

 

ANS:  E                    PTS:   1

 

13. Barium fluoride is often used in glass manufacturing. Which of these is the correct formula and bonding type for barium fluoride?

a.	BaF, ionic
b.	BaF, covalent
c.	BaF2, ionic
d.	BaF2, covalent
e.	Ba2F, ionic

 

 

ANS:  C                    PTS:   1

 

14. Which of these is an ionic compound?

a.	NCl3
b.	Li2O
c.	PF5
d.	CH4
e.	I2

 

 

ANS:  B                    PTS:   1

 

15. Which of these is an ionic compound?

a.	AlCl3
b.	H2O
c.	SiO2
d.	IBr
e.	S8

 

 

ANS:  A                    PTS:   1

 

16. Which of these statements about covalent compounds is incorrect?

a.	Covalent bonds involve the combination of two nonmetals.
b.	Covalent compounds dissolve in water to form electrolyte solutions.
c.	Covalent compounds contain atoms which share electrons to gain stability.
d.	The bonds in covalent compound are often oriented in a particular direction.
e.	Electrons in covalent compounds are not always equally shared between atoms.

 

 

ANS:  B                    PTS:   1

 

17. For an ionic compound, X₂Y₅, if the charge on each Y ion is -2, the charge on each X ion is:

a.	-2
b.	-5
c.	-10
d.	+10
e.	+5

 

 

ANS:  E                    PTS:   1

 

 

18. Which of these is not a covalent compound?

a.	H2O
b.	TeCl4
c.	XeF4
d.	C2H2
e.	AlCl3

 

 

ANS:  E                    PTS:   1

 

19. Which of these is not a covalent compound?

a.	SiO2
b.	CH4
c.	N2O
d.	CaO
e.	ICl3

 

 

ANS:  D                    PTS:   1

 

20. The correct formula for the sulfate ion is:

a.	SO3–
b.	SO32-
c.	SO4–
d.	SO42-
e.	none of the above

 

 

ANS:  D                    PTS:   1

 

21. The correct formula for the nitrate ion is:

a.	NO–
b.	NO3-
c.	NO3–
d.	NO32-
e.	none of the above

 

 

ANS:  C                    PTS:   1

 

22. Nicotine has the chemical formula C₁₀H₁₄N₂. What is the molecular weight of nicotine?

a.	26 amu
b.	81 amu
c.	138 amu
d.	162 amu
e.	366 amu

 

 

ANS:  D                    PTS:   1

 

23. What is the molecular weight of PCl₃?

a.	66.5 amu
b.	106.5 amu
c.	137.5 amu
d.	180 amu
e.	360 amu

 

 

ANS:  C                    PTS:   1

 

 

24. What is the molecular weight of cholesterol, C₂₇H₄₆O?

a.	194 amu
b.	208 amu
c.	224 amu
d.	180 amu
e.	386 amu

 

 

ANS:  E                    PTS:   1

 

25. What is the molecular weight of boric acid, B(OH)₃?

a.	51 amu
b.	61.83 amu
c.	101.3 amu
d.	153 amu
e.	306 amu

 

 

ANS:  B                    PTS:   1

 

26. Which of the following is not true for 3 moles of CaCO₃?

a.	It contains 3 moles of O.
b.	It contains 3 moles of Ca.
c.	It contains 3 moles of C.
d.	It contains 9 moles of O.
e.	None of the above.

 

 

ANS:  A                    PTS:   1

 

27. Which of the following does not contain the same number of chlorine atoms as 60 CCl₄ molecules?

a.	240 HCl molecules
b.	120 chlorine molecules
c.	40 SCl6 molecules
d.	80 CFCl3 molecules
e.	60 CHCl3 molecules

 

 

ANS:  E                    PTS:   1

 

28. How many hydrogen atoms are in 25.6 grams of sucrose, (C₁₂H₂₂O₁₁)?

a.	1.647 atoms
b.	2.6 ´ 1023 atoms
c.	4.51 ´ 1022 atoms
d.	6.02 ´ 1023 atoms
e.	9.92 ´ 1023 atoms

 

 

ANS:  E                    PTS:   1

 

29. How many chromium atoms are in 78.8 g or K₂Cr₂O₇?

a.	2.24 ´ 1024 atoms
b.	1.12 ´ 1024 atoms
c.	3.23 ´ 1023 atoms
d.	1.61 ´ 1023 atoms
e.	2.25 ´ 1022 atoms

 

 

ANS:  C                    PTS:   1

 

 

30. Determine the number of moles in a 1.95 ´ 10^–2 gram sample of the amino acid glycine, CH₂(NH₂)CO₂H.

a.	2.6 ´ 10–4 moles
b.	2.6 ´ 10–2 moles
c.	1.46 moles
d.	2.0 ´ 10–2 moles
e.	3.85 ´ 10–1 moles

 

 

ANS:  A                    PTS:   1

 

31. How many moles of potassium cyanide are in a 113.5 gram sample of KCN?

a.	3.487 moles
b.	2.903 moles
c.	1.743 moles
d.	0.872 moles
e.	0.0173 moles

 

 

ANS:  C                    PTS:   1

 

32. How many moles of oxygen atoms are in a 0.6163 grams of niacin, C₆H₅NO₂?

a.	5.14 ´ 10–2 moles
b.	3.00 ´ 10–2 moles
c.	1.00 ´ 10–2 moles
d.	5.01 ´ 10–3 moles
e.	8.56 ´ 10–3 moles

 

 

ANS:  C                    PTS:   1

 

33. How many moles of carbon are atoms are in 1.574 g of novocain, C₁₃H₂₁N₂O₂Cl?

a.	0.01008 moles
b.	0.005776 moles
c.	0.07510 moles
d.	0.12096 moles
e.	0.006148 moles

 

 

ANS:  B                    PTS:   1

 

34. How many moles of caffeine are in 1.250 kg sample, C₈H₁₀N₄O₂?

a.	6.4 ´ 10–6 moles
b.	0.006 moles
c.	0.008 moles
d.	6.44 moles
e.	8.56 moles

 

 

ANS:  D                    PTS:   1

 

35. Calculate the number of oxygen atoms in 45.0 g of Co₂(SO₄)₃ (molar mass =405.8 g/mole).

a.	8.01 ´ 1023 atoms
b.	2.67 ´ 1023 atoms
c.	12.0 atoms
d.	6.68 ´ 1022 atoms
e.	1.07 ´ 1024 atoms

 

 

ANS:  A                    PTS:   1

 

 

36. Calculate the mass in grams of a 1.070 moles of acetylene, C₂H₂.

a.	0.02434 grams
b.	0.04415 grams
c.	14.98 grams
d.	25.68 grams
e.	27.82 grams

 

 

ANS:  E                    PTS:   1

 

37. How many grams are in 2.35 moles of calcium carbonate, CaCO₃?

a.	0.01175 grams
b.	0.0235 grams
c.	0.0588 grams
d.	107 grams
e.	235 grams

 

 

ANS:  E                    PTS:   1

 

38. An international group of zookeepers with successful breeding programs made the following animal exchanges last year. Using the same bartering system, how many monkeys can a zoo obtain in exchange for 10 camels?

 

3 oryxes = 1 tiger
2 flamingos = 1 anteater
1 camel = 6 anteaters	5 lemurs = 1 rhino
1 rhino = 4 monkeys	3 lemurs = 1 camel
3 monkeys = 1 tiger	1 rhino = 4 oryxes

 

a.	6 monkeys
b.	12 monkeys
c.	15 monkeys
d.	24 monkeys
e.	30 monkeys

 

 

ANS:  D                    PTS:   1

 

39. An international group of zookeepers with successful breeding programs made the following animal exchanges last year. Using the same bartering system, how many anteaters can a zoo obtain in exchange for 4 oryxes?

 

3 oryxes = 1 tiger	2 flamingos = 1 anteater
1 camel = 6 anteaters	5 lemurs = 1 rhino
1 rhino = 4 monkeys	3 lemurs = 1 camel
3 monkeys = 1 tiger	1 rhino = 4 oryxes

 

a.	6 anteaters
b.	10 anteaters
c.	15 anteaters
d.	20 anteaters
e.	30 anteaters

 

 

ANS:  B                    PTS:   1

 

 

40. An international group of zookeepers with successful breeding programs made the following animal exchanges last year. Using the same bartering system, how many flamingos can a zoo obtain in exchange for 6 rhinos?

 

3 oryxes = 1 tiger	2 flamingos = 1 anteater
1 camel = 6 anteaters	5 lemurs = 1 rhino
1 rhino = 4 monkeys	3 lemurs = 1 camel
3 monkeys = 1 tiger	1 rhino = 4 oryxes

 

a.	10 anteaters
b.	30 anteaters
c.	50 anteaters
d.	120 anteaters
e.	160 anteaters

 

 

ANS:  D                    PTS:   1

 

41. Using the old English measurements of volume listed, determine the number of noggins in one butt.

 

1 gill = 1 noggin	1 butt = 2 hogsheads
1 kilderkin = 2 firkins	1 firkin = 9 gallons
1 hogshead = 52.458 gallons	1 peck = 64 noggins
1 peck = 2 gallons

 

a.	104.92 noggins
b.	128.00 noggins
c.	209.83 noggins
d.	1678.7 noggins
e.	3357.3 noggins

 

 

ANS:  E                    PTS:   1

 

42. Using the old English measurements of volume listed, determine the number of gallons in two gills.

 

1 gill = 1 noggin	1 butt = 2 hogsheads
1 kilderkin = 2 firkins	1 firkin = 9 gallons
1 hogshead = 52.458 gallons	1 peck = 64 noggins
1 peck = 2 gallons

 

a.	0.0039 gallons
b.	64 gallons
c.	256 gallons
d.	512 gallons
e.	2304 gallons

 

 

ANS:  C                    PTS:   1

 

43. Using the old English measurements of volume listed, determine the number of hogsheads in five kilderkins.

 

1 gill = 1 noggin	1 butt = 2 hogsheads
1 kilderkin = 2 firkins	1 firkin = 9 gallons
1 hogshead = 52.458 gallons	1 peck = 64 noggins
1 peck = 2 gallons

 

a.	1.72 hogsheads
b.	2.91 hogsheads
c.	90 hogsheads
d.	4,721 hogsheads
e.	42,489 hogsheads

 

 

ANS:  A                    PTS:   1

 

44. How many moles of calcium atoms are 2.5 moles of calcium carbonate, CaCO₃?

a.	1 mole
b.	1.25 moles
c.	2.5 moles
d.	5.0 moles
e.	100 moles

 

 

ANS:  C                    PTS:   1

 

45. How many moles hydrogen atoms are in 3 moles of codeine, C₁₈H₂₁NO₃?

a.	3 mole
b.	21 moles
c.	36 moles
d.	54 moles
e.	63 moles

 

 

ANS:  E                    PTS:   1

 

46. How many moles carbon atoms are in 5 moles of ethanol, CH₃CH₂OH?

a.	2.5 mole
b.	5 moles
c.	10 moles
d.	30 moles
e.	120 moles

 

 

ANS:  C                    PTS:   1

 

47. How many atoms of aluminum are contained in 36.0 ounce aluminum bat? 1 ounce = 28.35 grams

a.	2.28 ´ 1025
b.	6.28 ´ 10–23
c.	6.15 ´ 1026
d.	6.33 ´ 1023
e.	Can’t tell from the given information

 

 

ANS:  A                    PTS:   1

 

48. How many moles nitrogen atoms are in 12 moles of NH₄NO₃?

a.	6 mole
b.	12 moles
c.	14 moles
d.	24 moles
e.	28 moles

 

 

ANS:  D                    PTS:   1

 

 

49. Which of these is the correct formula for aluminum oxide?

a.	Al2O2
b.	Al2O3
c.	AlO
d.	Al3O2
e.	AlO2

 

 

ANS:  B                    PTS:   1

 

50. What is the correct name of K₂O?

a.	Dipotassium monoxide
b.	Dipotassium oxide
c.	Potassium monoxide
d.	Potassium oxygen
e.	Potassium oxide

 

 

ANS:  E                    PTS:   1

 

51. Which of these is the correct name for MgCl₂?

a.	magnesium chloride
b.	magnesium chlorine
c.	magnesium dichloride
d.	magnesium monochloride
e.	monomagnesium dichloride

 

 

ANS:  A                    PTS:   1

 

52. Which of these is the correct name for N₂O₃?

a.	nitrogen trioxide
b.	trinitrogen dioxide
c.	dinitrogen trioxide
d.	nitrogen dioxygenide
e.	dinitrogenide dioxygenide

 

 

ANS:  C                    PTS:   1

 

53. Which of these is the correct formula for potassium phosphate?

a.	KPO4
b.	K3PO4
c.	K(PO4)3
d.	K2(PO4)3
e.	K3P

 

 

ANS:  B                    PTS:   1

 

54. Which of these is the correct name for Li₂SO₄?

a.	lithium sulfide
b.	dilithium sulfide
c.	dilithium sulfate
d.	lithium sulfate
e.	dilithium tetrasulfide

 

 

ANS:  D                    PTS:   1

 

 

55. Which of these is the correct name for NaHCO₃?

a.	sodium carbonate
b.	sodium trioxide
c.	sodium monocarbide
d.	sodium bicarbonate
e.	sodium carbide oxide

 

 

ANS:  D                    PTS:   1

 

56. Which of these is the correct name for Ca(OH)₂?

a.	calcium carbonate
b.	calcium oxide
c.	calcium dihydride
d.	calcium oxygen hydride
e.	calcium hydroxide

 

 

ANS:  E                    PTS:   1

 

57. Which of these is the correct name for Rb₃N?

a.	rubidium nitride
b.	radon nitride
c.	trirubdium nitride
d.	triradon nitride
e.	rubidium trinitride

 

 

ANS:  A                    PTS:   1

 

58. When properly balanced, what are the correct coefficients for the reaction : H₂ + O₂ ® H₂0 ?

a.	1,1,1
b.	1,1/2,1
c.	1,2,1
d.	2,1,2
e.	10,5,10

 

 

ANS:  D                    PTS:   1

 

59. What is the coefficient in front of sodium nitride when the equation is balanced?

 

__ Na₃N ® __ Na(s) + __ N₂(g)

a.	0
b.	1
c.	2
d.	3
e.	4

 

 

ANS:  C                    PTS:   1

 

60. What is the coefficient in front of HF when the equation is balanced?

 

__ B₂O₃ + __ HF ® __ BF₃ + __ H₂O

a.	1
b.	2
c.	3
d.	5
e.	6

 

 

ANS:  E                    PTS:   1

 

61. What is the coefficient in front of oxygen (O₂) when the equation is balanced?

 

__ C₃H₈ + __ O₂ ® __ CO₂ + __ H₂O

a.	2
b.	3
c.	4
d.	5
e.	10

 

 

ANS:  D                    PTS:   1

 

62. Which of these is the correct SUM of the coefficients when the equation is balanced?

 

__ CaCl₂(aq) + __ K₂CO₃(aq) ® __ KCl(aq) + __ CaCO₃(s)

a.	2
b.	4
c.	5
d.	8
e.	10

 

 

ANS:  C                    PTS:   1

 

63. When properly balanced, what will the coefficients be in the equation, respectively?

 

__Mg + __N₂ ® __Mg₃N₂

a.	1,1,1
b.	3,2,1
c.	3,1,1
d.	3,1,2
e.	None of the above.

 

 

ANS:  C                    PTS:   1

 

64. How many moles of oxygen gas will react with 6.2 moles of aluminum?

 

4Al(s) + 3O₂(g) ® 2Al₂O₃(s)

a.	0.12 moles
b.	1.55 moles
c.	2.4 moles
d.	4.65 moles
e.	8.27 moles

 

 

ANS:  D                    PTS:   1

 

65. How many moles of tetraphosphorous decaoxide will form when 3.30 moles of P₄  react with oxygen gas?

 

P₄ + 5O₂ ® P₄O₁₀

a.	0.825 moles
b.	3.3 moles
c.	13.2 moles
d.	16.5 moles
e.	20 moles

 

 

ANS:  B                    PTS:   1

 

66. How many moles of oxygen gas are needed to react with 9 moles of acetylene,C₂H₂?

 

2C₂H₂ + 5O₂(g) ® 4CO₂ + 2H₂O

a.	0.4 moles
b.	4.5 moles
c.	9 moles
d.	18 moles
e.	22.5 moles

 

 

ANS:  E                    PTS:   1

 

67. How many grams of carbon dioxide are produced when 18.5 moles of oxygen react with excess acetylene, according to the following equation.

 

2C₂H₂ + 5O₂(g) ® 4CO₂ + 2H₂O

a.	2,030 grams
b.	814 grams
c.	651 grams
d.	88.0 grams
e.	37.0 grams

 

 

ANS:  C                    PTS:   1

 

68. How many grams of water are produced when 10.0 grams of O₂ react with excess H₂?

 

2H₂ + O₂(g) ® 2H₂O

a.	11.25 grams
b.	20 grams
c.	46 grams
d.	180 grams
e.	360 grams

 

 

ANS:  A                    PTS:   1

 

69. How many grams of nitrogen dioxide are required to produce 260 grams of nitrogen monoxide?

 

3NO₂ + H₂O ® 2HNO₃ + NO

a.	8.67 grams
b.	56.52 grams
c.	132 grams
d.	399 grams
e.	1196 grams

 

 

ANS:  E                    PTS:   1

 

 

70. Automotive air bags inflate when a sample of NaN₃ (molar mass = 65 g/mol) is rapidly decomposed. What mass of NaN₃ is required to produce 368 L of nitrogen gas (molar mass = 28 g/mol) with a density of 1.25 g/L?

 

2NaN₃(s) ® 2Na(s) + 3N₂(g)

a.	228 g
b.	712 g
c.	1709 g
d.	2136 g
e.	3203 g

 

 

ANS:  B                    PTS:   1

 

71. How many grams of methanol (CH₃OH) are produced when 5.00 kg of H₂ reacts with excess carbon monoxide?

 

CO + 2H₂ ® CH₃OH

a.	40 g
b.	80 g
c.	320 g
d.	640 g
e.	40,000 g

 

 

ANS:  E                    PTS:   1

 

72. Which of the following has the largest mass of oxygen?

a.	16.0 g of O2
b.	0.500 mol of O2
c.	2 moles of O atoms
d.	10 grams of carbon dioxide CO2
e.	All of these have the same mass of oxygen.

 

 

ANS:  C                    PTS:   1

 

73. For the reaction:    4 NH₃  +  5 O₂  ±  6 H₂O  +  4 NO

If 2.5 moles of NH₃ is reacted with 3.0 moles of O₂ , what is the limiting reagent?

a.	NH3
b.	O2
c.	H2O
d.	NO

 

 

ANS:  B                    PTS:   1

 

74. For the reaction:    4 NH₃  +  5 O₂  ±  6 H₂O  +  4 NO

If 125.0 g of NH₃ is reacted with 225.0 g of O₂ , what is the limiting reagent?

a.	NH3
b.	O2
c.	H2O
d.	NO
e.	None of the above.

 

 

ANS:  B                    PTS:   1

 

 

75. For the reaction:    4 NH₃  +  5 O₂  ±  6 H₂O  +  4 NO

If 125.0 g of NH₃ is reacted with 225.0 g of O₂ , how many grams of H₂O will be present after a complete reaction?

a.	0 grams
b.	151.9 grams
c.	198.5 grams
d.	350.0 grams

 

 

ANS:  B                    PTS:   1

 

76. For the reaction:    4 NH₃  +  5 O₂  ±  6 H₂O  +  4 NO

If 125.0 g of NH₃ is reacted with 225.0 g of O₂ , how many grams of NO will be present after a complete reaction?

a.	0 grams
b.	168.8 grams
c.	220.6 grams
d.	350.0 grams

 

 

ANS:  B                    PTS:   1

 

77. For the reaction:    4 NH₃  +  5 O₂  ±  6 H₂O  +  4 NO

If 125.0 g of NH₃ is reacted with 225.0 g of O₂ , how many grams of NH₃ will be present after a complete reaction?

a.	0 grams
b.	29.4 grams
c.	95.6 grams
d.	125.0 grams

 

 

ANS:  B                    PTS:   1

 

78. For the reaction:    4 NH₃  +  5 O₂  ±  6 H₂O  +  4 NO

If 125.0 g of NH₃ is reacted with 225.0 g of O₂ , how many grams of O₂ will be present after a complete reaction?

a.	0 grams
b.	125.0 grams
c.	225.0 grams
d.	350.0 grams

 

 

ANS:  A                    PTS:   1