Download Chem I Review Part 1

Chem I Review Part 1
Student: ___________________________________________________________________________
1.
Complete the following sentence. A scientific law is:
A. a tentative explanation for a set of observations that can be tested by further experimentation.
B. a statement describing a relationship between phenomena that is always the same under the same conditions.
C. a unifying principle that explains a body of facts and relations.
D. a model used to visualize the invisible.
2.
Choose the response that includes all the items listed below that are pure substances.
i. orange juice ii. steam iii. wine iv. oxygen v. vegetable soup
A. i, iii, v
B. ii, iv
C. i, iii, iv
D. iv only
E. All of them are pure.
3.
Which of these is an example of a physical property?
A. corrosiveness of sulfuric acid
B. toxicity of cyanide
C. flammability of gasoline
D. neutralization of stomach acid with an antacid
E. lead becomes a liquid when heated to 601°C
4.
Which one of these represents a physical change?
A. water, when heated, forms steam
B. bleach turns hair yellow
C. sugar, when heated, becomes brown
D. milk turns sour
E. apples, when exposed to air, turn brown
5.
The diameter of an atom is approximately 1 × 10-8 cm. What is this diameter when expressed in nanometers?
A. 1 × 10-19 nm
B. 1 × 10-15 nm
C. 1 × 101 nm
D. 1 × 10-10 nm
E. 1 × 10-1 nm
6.
Which of these quantities represents the largest mass?
A. 2.0 × 102 mg
B. 0.0010 kg
C. 1.0 × 105 μg
D. 2.0 × 102 cg
E. 10.0 dg
7.
The number 1.050 × 109 has how many significant figures?
A. 2
B. 3
C. 4
D. 9
E. 13
8.
After carrying out the operations below, how many significant figures are appropriate to show in the result?
(13.7 + 0.027) ÷ 8.221
A. 1
B. 2
C. 3
D. 4
E. 5
9.
How many cubic inches are in 1.00 liter?
A. 61.0 in3
B. 155 in3
C. 394 in3
D. 1.64 × 104 in3
E. none of them
10. If a car has an EPA mileage rating of 30 miles per gallon, what is this rating in kilometers per liter? (1 L = 1.06 qt)
A. 200 km/L
B. 180 km/L
C. 70 km/L
D. 13 km/L
E. 11 km/L
11. Table salt (sodium chloride) is 39.1% sodium. How many grams of salt contains 72.0 g of sodium?
A. 28.2 g salt
B. 72.0 g salt
C. 184 g salt
D. 2,820 g salt
E. 1.84 × 105 g salt
12. A piece of metal with a mass of 125 g is placed into a graduated cylinder that contains 25.00 mL of water, raising the water
level to 56.00 mL. What is the density of the metal?
A. 5.00 g/cm3
B. 4.03 g/cm3
C. 2.23 g/cm3
D. 1.51 g/cm3
E. 0.25 g/cm3
13. A block of iron has a mass of 826 g. What is the mass of a block of magnesium that has the same volume as the block of iron?
Given the following densities at 25oC:
magnesium: 1.7 g/cm3 graphite: 1.8 g/cm3 iron: 7.9 g/cm3
A. 1,400 g
B. 3,800 g
C. 830 g
D. 180 g
E. 90 g
14. Calculate the mass of the air contained in a room that measures
2.50 m × 5.50 m × 3.00 m (density of air = 1.29 g/dm3 at 25°C).
A. 3.13 × 10-5 g
B. 32.0 kg
C. 53.2 kg
D. 53.2 g
E. 32.0 g
15. A person walking fast requires 5.0 kcal of energy per minute. How many minutes of such exercise are required to consume 520
kcal, the energy in a large bag of French fries?
A. 0.0096 min
B. 100 min
C. 130 min
D. 520 min
E. 2,600 min
16. Radio waves travel at the speed of light, which is 3.00 × 108 m/s. How many minutes does it take for a radio message to reach
Earth from Saturn if Saturn is 7.9 × 108 km from Earth?
A. 4.4 × 10-2 min
B. 1.6 × 105 min
C. 4.0 × 1015 min
D. 44 min
E. 2.6 min
17. A special flask used in the determination of densities, called a pycnometer, has a mass of 16.3179 g when empty, and it has
a mass of 48.0250 g when filled with water at 20.0°C. When this same pycnometer is filled with ethyl alcohol at 20.0°C, it is
found to have a mass of 41.3934 g. Find the density of ethyl alcohol at 20.0°C.
(Given: at 20.0°C, the density of water is 0.9982 g/mL)
A. 0.7894 g/mL
B. 0.7923 g/mL
C. 0.7908 g/mL
D. 1.303 g/mL
E. 0.7674 g/mL
18. The elements in a column of the periodic table are known as
A. metalloids.
B. a period.
C. noble gases.
D. a group.
E. nonmetals.
19. Which of these materials are usually poor conductors of heat and electricity?
A. metals
B. metalloids
C. nonmetals
D. alkaline earth metals
E. alkali metals
20. The scientist who determined the magnitude of the electric charge of the electron was
A. John Dalton.
B. Robert Millikan.
C. J. J. Thomson.
D. Henry Moseley.
E. R. Chang.
21. When J. J. Thomson discovered the electron, what physical property of the electron did he measure?
A. its charge, e
B. its charge-to-mass ratio, e/m
C. its temperature, T
D. its mass, m
E. its atomic number, Z
22. Which of these scientists developed the nuclear model of the atom?
A. John Dalton
B. Robert Millikan
C. J. J. Thomson
D. Henry Moseley
E. Ernest Rutherford
23. Rutherford's experiment with alpha particle scattering by gold foil established that
A. protons are not evenly distributed throughout an atom.
B. electrons have a negative charge.
C. electrons have a positive charge.
D. atoms are made of protons, neutrons, and electrons.
E. protons are 1840 times heavier than electrons.
24. Atoms of the same element with different mass numbers are called
A. ions.
B. neutrons.
C. allotropes.
D. chemical families.
E. isotopes.
25. How many neutrons are there in an atom of lead whose mass number is 208?
A. 82
B. 126
C. 208
D. 290
E. none of them
26. An atom of the isotope sulfur-31 consists of how many protons, neutrons, and electrons?
(p = proton, n = neutron, e = electron)
A. 15 p, 16 n, 15 e
B. 16 p, 15 n, 16 e
C. 16 p, 31 n, 16 e
D. 32 p, 31 n, 32 e
E. 16 p, 16 n, 15 e
27. Which one of these species is an ion?
A. B3+
B. NaCl
C. He
D. 14C
E. none of these
28. Two isotopes of an element differ only in their
A. symbol.
B. atomic number.
C. atomic mass.
D. number of protons.
E. number of electrons.
29. A magnesium ion, Mg2+, has
A. 12 protons and 13 electrons.
B. 24 protons and 26 electrons.
C. 12 protons and 10 electrons.
D. 24 protons and 22 electrons.
E. 12 protons and 14 electrons.
30. Which of these pairs of elements would be most likely to form an ionic compound?
A. P and Br
B. Cu and K
C. C and O
D. O and Zn
E. Al and Rb
31. What is the formula for the ionic compound formed by magnesium and iodine?
A. MgI
B. Mg2I
C. MgI2
D. MgI3
E. Mg3I
32. What is the formula for the ionic compound formed by calcium ions and nitrate ions?
A. Ca3N2
B. Ca(NO3)2
C. Ca2NO3
D. Ca2NO2
E. CaNO3
33. Which is the correct formula for copper(II) phosphate?
A. Cu2PO4
B. Cu3(PO4)2
C. Cu2PO3
D. Cu(PO4)2
E. Cu(PO3)2
34. The correct name for NH4NO3 is
A. ammonium nitrate.
B. ammonium nitrogen trioxide.
C. ammonia nitrogen oxide.
D. hydrogen nitrogen oxide.
E. hydrogen nitrate.
35. The Stock system name for Mn2O7 is
A. dimanganese heptaoxide.
B. magnesium oxide.
C. manganese(VII) oxide.
D. manganese(II) oxide.
E. manganese(III) oxide.
36. The mineral pyrolusite is a compound of manganese-55 and oxygen-16. If 63% of the mass of pyrolusite is due to manganese,
what is the empirical formula of pyrolusite?
A. MnO
B. Mn2O
C. Mn2O2
D. MnO2
E. none of these
37. The total number of electrons present in a sulfate ion is
A. 2.
B. 26.
C. 32.
D. 48.
E. 50.
38. Which of these elements is chemically similar to magnesium?
A. sulfur
B. calcium
C. iron
D. nickel
E. potassium
39. An atom of bromine has a mass about four times greater than that of an atom of neon. Which choice makes the correct
comparison of the relative numbers of bromine and neon atoms in 1,000 g of each element?
A. The number of bromine and neon atoms is the same.
B. There are one thousand times as many bromine atoms as neon atoms.
C. There are one thousand times as many neon atoms as bromine atoms.
D. There are four times as many neon atoms as bromine atoms.
E. There are four times as many bromine atoms as neon atoms.
40. What is the average mass, in grams, of one atom of iron?
A. 6.02 × 1023 g
B. 1.66 × 10-24 g
C. 9.28 × 10-23 g
D. 55.85 g
E. 55.85 × 10-23 g
41. The mass of 1.63 × 1021 silicon atoms is
A. 2.71 × 10-23 g.
B. 4.58 × 1022 g.
C. 28.08 g.
D. 1.04 × 104 g.
E. 7.60 × 10-2 g.
42. If 0.274 moles of a substance weighs 62.5 g, what is the molar mass of the substance, in units of g/mol?
A. 2.28 × 102 g/mol
B. 1.71 × 101 g/mol
C. 4.38 × 10-3 g/mol
D. 2.17 × 102 g/mol
E. none of these
43. Which of these quantities does not represent 1.00 mol of the indicated substance?
A. 6.02 × 1023 C atoms
B. 26.0 g Fe
C. 12.01 g C
D. 65.4 g Zn
E. 6.02 × 1023 Fe atoms
44. How many silicon atoms are there in 1.00 g of silicon?
A. 1 atom
B. 0.0356 atoms
C. 2.57 × 1023 atoms
D. 2.14 × 1022 atoms
E. 1.75 × 1025 atoms
45. Which of the following samples contains the greatest number of atoms?
A. 100 g of Pb
B. 2.0 mole of Ar
C. 0.1 mole of Fe
D. 5 g of He
E. 20 million O2 molecules
46. What is the molar mass of acetaminophen, C8H9NO2?
A. 43 g/mol
B. 76 g/mol
C. 151 g/mol
D. 162 g/mol
E. 125 g/mol
47. The molecular formula of aspirin is C9H8O4. How many aspirin molecules are present in one 500-milligram tablet?
A. 2.77 molecules
B. 2.77 × 10-3 molecules
C. 1.67 × 1024 molecules
D. 1.67 × 1021 molecules
E. none of these is correct.
48. How many sulfur atoms are there in 21.0 g of Al2S3?
A. 8.42 × 1022 atoms
B. 2.53 × 1023 atoms
C. 2.14 × 1023 atoms
D. 6.02 × 1023 atoms
E. 6.30 × 1026 atoms
49. Boron obtained from borax deposits in Death Valley consists of two isotopes. They are boron-10 and boron-11 with atomic
masses of 10.013 amu and 11.009 amu, respectively. The atomic mass of boron is 10.81 amu (see periodic table). Which
isotope of boron is more abundant, boron-10 or boron-11?
A. This cannot be determined from data given.
B. Neither, their abundances are the same.
C. Boron-10
D. Boron-11
50. The empirical formula of a compound of uranium and fluorine that is composed of 67.6% uranium and 32.4% fluorine is
A. U2F
B. U3F4
C. UF4
D. UF6
E. UF8
51. The percent composition by mass of a compound is 76.0% C, 12.8% H, and 11.2% O. The molar mass of this compound is
284.5 g/mol. What is the molecular formula of the compound?
A. C10H6O
B. C9H18O
C. C16H28O4
D. C20H12O2
E. C18H36O2
52. What is the coefficient of H2O when the following equation is properly balanced with the smallest set of whole numbers?
___ Na + ___ H2O → ___ NaOH + ___ H2
A. 1
B. 2
C. 3
D. 4
E. 5
53. What is the coefficient of H2O when the following equation is properly balanced with the smallest set of whole numbers?
___ Al4C3 + ___ H2O → ___ Al(OH)3 + ___ CH4
A. 3
B. 4
C. 6
D. 12
E. 24
54. Ammonia reacts with diatomic oxygen to form nitric oxide and water vapor:
4NH3 + 5O2 → 4NO + 6H2O
When 40.0 g NH3 and 50.0 g O2 are allowed to react, which is the limiting reagent?
A. NH3
B. O2
C. Neither reagent is limiting.
55. How many grams of Cl2 can be prepared from the reaction of 16.0 g of MnO2 and 30.0 g of HCl according to the following
chemical equation?
MnO2 + 4HCl → MnCl2 + Cl2 + 2H2O
A. 0.82 g
B. 5.8 g
C. 13.0 g
D. 14.6 g
E. 58.4 g
56. What is the theoretical yield of chromium that can be produced by the reaction of 40.0 g of Cr2O3 with 8.00 g of aluminum
according to the chemical equation below?
2Al + Cr2O3 → Al2O3 + 2Cr
A. 7.7 g
B. 15.4 g
C. 27.3 g
D. 30.8 g
E. 49.9 g
57. Calculate the mass of excess reagent remaining at the end of the reaction in which 90.0 g of SO2 are mixed with 100.0 g of O2.
2SO2 + O2 → 2SO3
A. 11.5 g
B. 22.5 g
C. 67.5 g
D. 77.5 g
E. 400 g
58. A 1.375 g sample of mannitol, a sugar found in seaweed, is burned completely in oxygen to give 1.993 g of carbon dioxide and
0.9519 g of water. The empirical formula of mannitol is
A. CHO
B. CH7O3
C. C3H2O
D. C3H7O3
E. CH2O
59. The first step in the Ostwald process for producing nitric acid is
4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g).
If the reaction of 150. g of ammonia with 150. g of oxygen gas yields 87. g of nitric oxide (NO), what is the percent yield of
this reaction?
A. 100%
B. 49%
C. 77%
D. 33%
E. 62%
60. The Hall process for the production of aluminum involves the reaction of aluminum oxide with elemental carbon to give
aluminum metal and carbon monoxide. If the yield of this reaction is 75%, what mass of aluminum metal can be produced
from the reaction of 1.65 × 106 of aluminum oxide with 1.50 × 106 g of carbon?
A. 1.6 × 105 g
B. 3.3 × 105 g
C. 6.6 × 105 g
D. 8.7 × 105 g
E. 1.7 × 106 g
61. A gold wire has a diameter of 1.00 mm. What length of this wire contains exactly 1.00 mol of gold?
[Given: density of Au = 17.0 g/cm3]
A. 2630 m
B. 3.69 m
C. 251 m
D. 14.8 m
E. 62.7 m
Chem I Review Part 1 Key
1. B
2. B
3. E
4. A
5. E
6. D
7. C
8. C
9. A
10. D
11. C
12. B
13. D
14. C
15. B
16. D
17. A
18. D
19. C
20. B
21. B
22. E
23. A
24. E
25. B
26. B
27. A
28. C
29. C
30. D
31. C
32. B
33. B
34. A
35. C
36. D
37. E
38. B
39. D
40. C
41. E
42. A
43. B
44. D
45. B
46. C
47. D
48. B
49. D
50. D
51. E
52. B
53. D
54. B
55. C
56. B
57. D
58. D
59. D
60. C
61. D
Chem I Review Part 1 Summary
Category
Difficulty: Difficult
Difficulty: Easy
Difficulty: Medium
Raymond - 001 Chemistry...
Raymond - 002 Atoms...
Raymond - 003 Mass...
# of Questions
5
19
37
17
21
23