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Name: __________________________ Date: _____________
1. Choose the response that includes all the items listed below that are pure substances.
i. orange juice
ii. steam
iii. ocean water
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
2. All of the following are properties of sodium. Which one is a physical property of
sodium?
A) It is surface turns black when first exposed to air.
B) It is a solid at 25C and changes to a liquid when heated to 98C.
C) When placed in water it sizzles and a gas is formed.
D) When placed in contact with chlorine it forms a compound that melts at 801C.
E) Sodium is never found as the pure metal in nature.
3. Which one of the following represents a chemical change?
A) boiling water to form steam
B) burning a piece of coal
C) heating lead until it melts
D) mixing iron filings and sand at room temperature
E) breaking glass
4. Lead melts at 601.0C. What temperature is this in F?
A) 302F
B) 365F
C) 1,050F
D) 1,082F
E) 1,114F
5. Express the number 26.7 in scientific notation.
A) 2.67  10–2
B) 2.67  10–1
C) 2.67  101
D) 2.67  102
E) 26.7 is already written in scientific notation
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6. The number 1.050  109 has how many significant figures?
A) 2
B) 3
C) 4
D) 9
E) 13
7. How many significant figures does the result of the following sum contain?
8.5201 + 1.93
A) 1
B) 2
C) 3
D) 4
E) 5
8. Do the indicated arithmetic and give the answer to the correct number of significant
figures.
(1.5  10–4  61.3) + 2.01 =
A) 2.0192
B) 2.0
C) 2.019
D) 2.02
E) 2.019195
9. How many cubic centimeters are there in exactly one cubic meter?
A) 1  10–6 cm3
B) 1  10–3 cm3
C) 1  10–2 cm3
D) 1  104 cm3
E) 1  106 cm3
10. An aluminum beverage can contains 12.0 fluid ounces of liquid. Express this volume
in liters. (1 fl oz = 29.6 mL)
A) 4.07  10-2 L
B) 0.355 L
C) 0.407 L
D) 2.46 L
E) 3.55  102 L
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11. The density of lead is 11.4 g/cm3 at 25C. Calculate the volume occupied by 25.0 g of
lead.
A) 2.19 cm3
B) 0.456 cm3
C) 285 cm3
D) 1.24 cm3
E) 6.05 cm3
12. Bromine is a red liquid at 25C. Its density is 3.12 g/cm3. What is the volume of 28.1
g of liquid bromine?
A) 87.7 cm3
B) 0.111 cm3
C) 9.01 cm3
D) 28.1 cm3
E) None of the above.
13. Define matter.
14. What are the three states of matter?
15. What are the common names for the three states of the compound water?
16. Identify the following as a physical or chemical change: Bacteria convert milk to yogurt.
17. Classify the following as either a physical or a chemical property: Ice melts at 0C.
18. Classify the following as a mixture, a compound, or an element: Sugar to put in a cup of
coffee.
19. An automobile engine has a piston displacement of 1,600 cm3. Express this volume in
liters.
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20. 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.
21. Which of the following elements is most likely to be a good conductor of electricity?
A) N
B) S
C) He
D) Cl
E) Fe
22. An anion is defined as
A) a charged atom or group of atoms with a net negative charge.
B) a stable atom.
C) a group of stable atoms.
D) an atom or group of atoms with a net positive charge.
23. Atoms of the same element with different mass numbers are called
A) ions.
B) neutrons.
C) allotropes.
D) chemical families.
E) isotopes.
24. How many neutrons are there in an atom of uranium whose mass number is 235?
A) 92
B) 143
C) 235
D) 238
E) 327
25. Which one of the following elements is most likely to form a 2+ ion?
A) beryllium
B) carbon
C) fluorine
D) oxygen
E) sodium
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26. An aluminum ion, Al3+, has:
A) 13 protons and 13 electrons
B) 27 protons and 24 electrons
C) 16 protons and 13 electrons
D) 13 protons and 10 electrons
E) 10 protons and 13 electrons
27. An oxide ion, O2–, has:
A) 8 protons and 10 electrons
B) 10 protons and 8 electrons
C) 8 protons and 9 electrons
D) 8 protons and 7 electrons
E) 10 protons and 7 electrons
28. Given that the ion ClO3– is named chlorate, what is the ion ClO4– named?
A) chloride
B) chlorite
C) hypochlorite
D) perchlorite
E) perchlorate
29. Which pair of elements would be most likely to form an ionic compound?
A) P and Br
B) Zn and K
C) F and Al
D) C and S
E) Al and Rb
30. 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
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31. The correct name for KHCO3 is
A) calcium bicarbonate.
B) calcium carbonate.
C) potassium carbonate.
D) calcium hydrogen carbon trioxide.
E) potassium hydrogen carbonate.
32. The correct name for CuSO4·5H2O is
A) copper sulfate acid.
B) copper sulfate pentahydrate.
C) copper(II) sulfate acid.
D) copper(II) sulfate pentahydrate.
E) copper(V) sulfate hydrate.
33. 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.
34. The straight chain hydrocarbon that contains six carbon atoms is
A) propane
B) butane
C) pentane
D) hexane
E) heptane
35. What are the three subatomic particles that are important in chemistry?
36. What are the three types of radiation produced by the decay of substances like uranium?
37. How many electrons, protons, and neutrons does an iron-55 atom have?
38. What are the seven elements that naturally occur as diatomic molecules?
39. Define ion.
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40. Give the formula for potassium oxide.
41. Name the following binary compound: NaH.
42. Name the following binary compound: Fe2O3.
43. Name the following compound: Cl2O7.
44. Write the formula for the acid formed from the fluoride anion, and then name the acid.
45. Write the formula for the acid formed from the nitrite anion, and then name the acid.
46. The elements known as the halogens are useful as disinfectants. Name two halogens.
47. What are isotopes?
48. Write the formula of ammonium chlorate.
49. What is the average mass, in grams, of one potassium atom?
A) 5.14  10–23 g
B) 6.49  10–23 g
C) 6.02  10–18 g
D) 31.0 g
E) 39.1 g
50. The mass of 1.21  1020 atoms of sulfur is
A) 3.88  1021 g.
B) 2.00 mg.
C) 32.06 g.
D) 6.44 mg.
E) 2.00  10–4 g.
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51. How many atoms are in 5.54 g of F2?
A) 6.02  1023 atoms
B) 0.146 atoms
C) 0.292 atoms
D) 8.78  1022 atoms
E) 1.76  1023 atoms
52. How many moles of CF4 are there in 171 g of CF4?
A) 0.51 mol
B) 1.94 mol
C) 4.07 mol
D) 88.0 mol
E) 171 mol
53. Calculate the molecular mass of potassium permanganate, KMnO4.
A) 52 amu
B) 70 amu
C) 110 amu
D) 158 amu
E) 176 amu
54. Formaldehyde has the formula CH2O. How many molecules are there in 0.11 g of
formaldehyde?
A) 6.1  10–27
B) 3.7  10–3
C) 4
D) 2.2  1021
E) 6.6  1022
55. How many fluorine atoms are there in 65 g of CF4?
A) 0.74 atoms
B) 3.0 atoms
C) 4.5  1023 atoms
D) 1.8  1024 atoms
E) 2.4  1023 atoms
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56. What is the mass of 3.00 moles of ethanol, C2H6O?
A) 4.99  10–24 g
B) 138 g
C) 6.52  10–2 g
D) 50 g
E) 1.81  1024 g
57. 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
58. 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
59. 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
60. Aluminum hydroxide reacts with nitric acid to form aluminum nitrate and water. What
mass of water can be formed by the reaction of 15.0 g of aluminum hydroxide with
excess nitric acid?
A) 1.15 g
B) 3.46 g
C) 45.0 g
D) 6.14 g
E) 10.4 g
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61. Calculate the molecular mass, in g/mol, of H2SO4.
62. How many Mg atoms are present in 170 g of Mg?
63. Calculate the volume of 0.15 mole of Br2. The density of Br2 is 3.12 g/mL.
64. Calculate the percent composition by mass of carbon in Na2CO3.
65. Balance the following chemical equation:
C + Fe2O3  Fe + CO
66. What is the theoretical yield of PI3 if 48.0 g of I2 are reacted with an excess of
phosphorus according to the following chemical equation?
2P(s) + 3I2(s)  2PI3(s)
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Answer Key
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B
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Matter is anything that occupies space and has mass.
Solid, liquid, and gas
Ice, water, and steam
Chemical
Physical
Compound
1.6 L
D
E
A
E
B
A
D
A
E
C
B
E
D
C
D
electrons, protons, and neutrons
Alpha, beta, and gamma radiation
26 electrons, 26 protons, and 29 neutrons
Hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, iodine
An ion is an atom or group of atoms that has a net positive or negative charge.
K2O
sodium hydride
iron(III) oxide (or ferric oxide)
dichlorine heptaoxide, or dichlorine heptoxide
HF, hydrofluoric acid
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45. HNO2, nitrous acid
46. (two of these) fluorine, chlorine, bromine, iodine
47. Atoms of the same element that have the same atomic number but different mass
numbers.
48. NH4ClO3
49. B
50. D
51. E
52. B
53. D
54. D
55. D
56. B
57. D
58. E
59. B
60. E
61. 98.09 g/mol
62. 4.2  1024
63. 7.7 mL
64. 11.3%
65. 3C + Fe2O3  2Fe + 3CO
66. 51.9 g
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