Download Honors Chemistry Exam Review Questions

Honors Chemistry Exam Review Questions
Chapter 1
1. Which of the substances listed could be considered inorganic?
A methane, CH4
B rubbing alcohol, C3H7OH
C
D
ammonia, NH3
candle wax, C25H52
2. A hypothesis is:
A
B
C
D
an observation recorded from an experiment
a proposed explanation for what is observed.
a concise statement that summarizes the results of a broad variety of experiments.
a thoroughly tested model.
3. Which of the following is not a part of the scientific method?
A experimenting
B observing
C
D
proving
hypothesizing
4. What does a red 4 mean on a chemical bottle?
A extreme health hazard
B not a health hazard
C
D
extreme fire hazard
not a fire hazard
5. Which piece of laboratory equipment would be best to use if you wanted to measure exactly
8.0 mL of water?
A 100 mL beaker
B 100 mL graduated cylinder
C
D
10 mL graduated cylinder
125 mL Erlenmeyer flask
6. If you spill an acid on the lab counter, what should you do first?
A Clean it up with a paper towel
B Tell your teacher immediately
C
D
Pour water on it
Scream at the top of your lungs
7. Identify the false statement:
A A scientific law fully explains a natural phenomenon.
B The scientific method is a logical, systematic approach to the solution of a problem.
C For the results of an experiment to be accepted, the experiment must produce the same
results no matter how many times it is repeated.
D The scientific process is repeated until a hypothesis either fits all the observed
experimental facts or is discarded.
8. What is the volume of the diagram to the right?
A 25.2 mL
B 25.24 mL
C
D
25.3 mL
25.28 mL
9. Which of these components of scientific research involves stating a relationship but not
proposing an explanation of the relationship?
A observation
B scientific law
C
D
theory
hypothesis
Chapter 2
10. How many of the zeros in the measurement 0.000040200 m are significant?
A 2
B 3
C
D
7
8
C
D
2.5 x 10-4 mg
2.5 x 106 mg
11. How many milligrams are in 2.5 kg?
A 2.5 x 10-6 mg
B 25 mg
12. What is the volume of 60.0 g of ether if the density of ether is 0.70 g/mL?
A 86 mL
B 0.012 mL
C
D
0.025 mL
42 mL
13. The temperature reading of -14oC corresponds to a Kelvin reading of :
A 297.6 K
B -287 K
C
D
287 K
259 K
14. Concentrated hydrochloric acid has a density of 1.19 g/mL. What is the mass, in grams, of
2.00 liters of this acid?
A 2.38 x 103 g
B 2.38 g
C
D
4.20 x 104 g
4.20 x 10-4 g
15. A student measures a volume as 25 mL, whereas the correct volume is 23 mL. What is the
percent error?
A 0.087%
B 8.7%
C
D
0.92%
8.0%
16. Which of the following is the correct scientific notation for 0.00000862?
A 86.2 x 107 km
B 8.62 x 106 km
C
D
86.2 x 10-7 km
8.62 x 10-6 km
17. How many significant figures are in the measurement 603.040?
A 3
B 4
C
D
5
6
18. Which of these equalities is correct?
A 1 g = 1000 kg
B 1 cm = 100 m
C
D
1 L = 1000 mL
1 mm = 10 cm
19. Four kilometers are equal to how many centimeters?
A 4.0 x 10-3 cm
B 4.0 x 105 cm
C
D
4.0 x 10-5 cm
1.0 x 103 cm
20. A conversion factor:
A
B
C
D
is equal to 1
is a ratio of equivalent measurements
does not change the value of a measurement
all of the above
21. Among the measurements given, which is the smallest?
A 470 mm
B 5.1 x 10-4 km
C
D
3.2 m
52 cm
22. The mass of an apple is approximately 125 grams. What conversion factor would you use to
express its mass in kilograms?
A 100 kg/1 g
B 1000 g/1 kg
C
D
1 kg/1000 g
1 g/100 kg
23. How many feet per second are there in 85 miles per hour?
A 120 ft/sec
B 58 ft/sec
C
D
140 ft/sec
7500 ft/sec
24. How many cubic micrometers are there in 3.25 x 10-7 L?
A
B
25. How many cubic centimeters are contained in a volume of 4.25 L?
A 4.25 x 102 cm3
B 4.25 x 10-3 cm3
C
D
4.25 x 103 cm3
4.25 x 10-2 cm3
Chapter 3
26. All of the following are physical properties of a substance in the liquid state except:
A definite volume
B able to flow
C
D
not easily compressed
definite shape
27. Homogeneous mixtures:
A
B
C
D
consist only of liquids
consist of two or more phases
have a varying composition
are known as solutions
28. A compound
A
B
C
D
is a pure substance
has a variable composition
can be physically separated into its elements
has properties similar to those of its elements
29. Physical properties of a substance include:
A color and solubility
B melting and boiling points
C
D
density and odor
all of the above
30. Which term does not fit with the others listed?
A ice
B steam
C
D
salt
water
31. Which of the following is an example of a physical change?
A bread molding
B burning a hamburger
C
D
digesting a banana
melting butter
32. An example of a heterogeneous mixture would be:
A sugar
B salt water
C
D
tap water
vegetable soup
33. A method of separating a mixture based on the difference in particle size is called
A chromatography
B filtration
C
D
distillation
magnetism
C
D
oxygen
water
34. Which of the following is a compound?
A carbon
B hydrogen
35. Which of the following can best distinguish a physical change from a chemical change?
A energy is absorbed or released
B a color change occurs
C
D
a gas is produced
mass is conserved
36. Which of the following changes of state are endothermic?
A gas  liquid
B liquid  gas
C
D
gas  solid
liquid  solid
37. Which of the following is an example of a chemical change?
A rotting meat
B slicing cheese
C
D
dissolving sugar in iced tea
freezing water
38. How much heat is absorbed when 20.0 grams of water is heated from 25.0oC to 39.0oC?
A 380. J
B 1590 J
C
D
1170 J
2090 J
39. What is the specific heat of a 35.0 gram sample of a metal that gives off 825 J of energy
when the cools from 95oC to 25oC.
A 0.589 J/goC
B 0.403 J/goC
C
D
0.672 J/goC
0.337 J/goC
Chapter 4
40. Which of the following is not a part of Dalton’s atomic theory?
A
B
C
D
all elements are composed of atoms
atoms of the same element are alike
atoms are always in motion
atoms that combine do so in simple whole-number ratios
41. The nucleus of an atom is:
A
B
C
D
negatively charged and has a low density
negatively charged and has a high density
positively charged and has a low density
positively charged and has a high density
42. Dalton theorized that atoms are indivisible and that all atoms of an element are identical.
Scientists now know that:
A
B
C
D
Dalton’s theories are completely correct.
atoms of an element can have different numbers of protons.
atoms are all divisible
all atoms of an element are not identical but they all have the same mass
43. The number of neutrons in the nucleus of an atom can be calculated by
A adding together the numbers of electrons and protons.
B subtracting the number of protons from the number of electrons.
C subtracting the number of protons from the mass number
D adding the mass number to the number of protons
44. The sum of the protons and neutrons in an atom equals the:
A atomic number
B number of electrons
C
D
atomic mass
mass number
45. All atoms of the same element have the same:
A number of protons
B number of neutrons
C
D
mass number
mass
46. An atom of an element with atomic number 48 and mass number 120 contains:
A
B
C
D
48 protons, 48 electrons, and 72 neutrons
72 protons, 48 electrons, and 48 neutrons
120 protons, 48 electrons, and 72 neutrons
72 protons, 72 electrons, and 48 neutrons
47. Which of the following statements is not consistent with the results obtained in Rutherford’s
gold foil experiment?
A
B
C
D
the nucleus of an atom is positively charged
the nucleus of an atom contains mostly all the mass of the atom
atoms are composed mainly of empty space
electrons are contained in the nucleus of an atom
48. The identity of an element can be determined on the basis of which of the following?
A
B
C
D
the number of protons in an atom of the element
the number of neutrons in an atom of the element
the mass number of the element
the atomic mass of the element
49. Isotopes of the same element have:
A
B
C
D
the same number of protons but different numbers of neutrons
the same number of protons but different numbers of electrons
the same number of neutrons but different numbers of protons
the same number of neutrons but different numbers of electrons
50. In general, metals are:
A ductile
B malleable
C
D
good electrical conductors
all of these
C
D
oxygen
copper
51. Which of the following is a nonmetal?
A iron
B silver
52. Three isotopes of oxygen occur in nature: oxygen-16, oxygen-17, and oxygen-18. If the
atomic mass of oxygen is 15.994, which of the three isotopes, if any, is the most abundant?
A oxygen-16
B oxygen-17
C
D
oxygen-18
all are equally abundant
Chapter 28
53. Which of the following is not true concerning an alpha particle?
A It has a mass of 4 amu
B It has a +1 charge
C
D
It is a helium nucleus
It contains two neutrons
54. A piece of wood found in an ancient burial mound contains one-fourth as much carbon-14 as
a piece of wood cut from a living tree growing nearby. If the half-life of carbon-14 is 5730
years, what is the approximate age of the ancient wood?
A 1432.5 years
B 2865 years
C
D
5730 years
11460 years
55. If an isotope undergoes beta emission:
A
B
C
D
the mass number changes
the atomic number changes
the atomic number remains the same
the number of neutrons remains the same
56. Which of the following particles is needed to complete this nuclear equation?
54
2
1
25Mn + 1H  _____ + 0n
A
B
56
27Co
57
26Fe
C
D
55
26Fe
58
24Cr
57. In nuclear fission:
A
B
C
D
certain atoms break into fragments when struck by neutrons
a chain reaction cannot occur
energy is absorbed
all of these
58. Nuclear fusion:
A
B
C
D
occurs when large nuclei fuse together
takes place in the sun
generally produces hydrogen nuclei
all of these
59. What particle is needed to complete this equation?
14
14
1
7 N + _____  6C + 1H
1
4
A 0n
C
2He
0
0
C -1e
D
+1e
60. Which of the following is always true about radioisotopes?
A
B
C
D
They have unstable nuclei
Their neutron-to-proton ratio is 1:1.
Their decay products are stable isotopes
all of these
61. Which of the following types of radiation has no mass and no charge?
A alpha
B beta
C
D
gamma
positron
62. When U-238 undergoes radioactive decay by losing an alpha particle, the other product is:
A U-234
B Th-234
C
D
Pu-234
U-242
Chapter 5
63. What is the ionic charge on the chromium ion in the ionic compound that has the formula
Cr2O3?
A +3
B -2
C
D
-5
+5
64. Which element when combined with chlorine would most likely form an ionic compound?
A lithium
B carbon
C
D
phosphorus
bromine
65. Choose the correct formula for calcium hydrogen phosphate?
A CaHPO4
B Ca2HPO4
C
D
Ca(H2PO4)2
Ca(HPO4)2
66. Compounds that are composed of ions:
A
B
C
D
are molecular compounds
are generally crystalline solids at room temperature
are for the most part composed of two or more metallic elements
all of the above
67. The cation Fe+3 is formed when:
A
B
C
D
an atom of iron loses two electrons
an atom of iron gains two electrons
an atom of iron loses three electrons
an atom of iron gains three electrons
68. What is the total number of atoms in one molecule of C6H12O6?
A 3
B 12
C
D
18
24
69. Name the following compound: Fe2(CO3)3
A Iron (III) carbonate
B Diiron (III) tricarbonate
C
D
Iron (II) carbonate
Diron (II) tricarbonate
70. What is the formula for trinitrogen heptachloride?
A N2Cl7
B N4Cl6
C
D
N3Cl6
N3Cl7
71. The name of Copper (II) nitrate
A Cu(NO3)2
B CuNO3
C
D
Cu(NO3)2
CuNO3
72. Among the following, which combination would be most likely to form an ionic compound?
A H and O
C S and Cl
C
D
Na and I
Si and O
73. The nonmetals in Groups 15,16, and 17:
A
B
C
D
lose electrons when they form ions
form positively charged ions
form ions with charges -3, -2, and -1, respectively
form ions with a numerical charge equal to their group number
74. Among the following, which atom is most likely to form an ion with a charge of +2?
A O
B Na
C
D
Al
Ca
75. What is the name of the following compound: (NH4)2S2O3?
A Ammonium sulfate
B Ammonium thiosulfate
C
D
Nitrogen hydrogen thiosulfate
Ammonium disulfate
C
D
H2C2O4
H2CO3
76. What is the formula for Oxalic acid?
A HC2O4
B H2CO3
77. Name the following compound: Fe3(PO4)2
A Iron (III) phosphate tetrahydrate
B Iron (II) phosphite tetrahydrate
C
D
.
4 H2O
Iron (II) phosphate tetrahydrate
Iron (II) phosphate trihydrate
78. Among the following, which is a binary molecular compound?
A CO2
B NaCl
C
D
FeO
MgS
Chapter 8
79. The chemical formula of aspirin is C9H8O4. What is the mass of 0.200 mol of aspirin?
A 22.5 g
B 5.4 g
C
D
80 g
36.0 g
80. How many moles of SO3 are in 2.4 x 1024 molecules of SO3?
A 0.25
B 3.4 x 1022
C
D
4.0
2.9 x 10-23
81. The representative particle for nitrogen gas (N2) is:
A an atom
B a molecule
C
D
a formula unit
none of these
C
D
125.8 g/mol
76.4 g/mol
82. What is the molar mass of MgCl2?
A 59.8 g/mol
B 95.3 g/mol
83. How many atoms of aluminum are present in a 0.275 mole sample of Al2(CO3)3?
A 1.66 x 1023 atoms
B 4.38 x 1024 atoms
C
D
3.31 x 1023 atoms
2.19 x 1024 atoms
84. How many grams of Ba(IO3)2 are there in a 1.25 x 1022 formula unit sample of Ba(IO3)2?
A 14.1 grams
B 101 grams
C
D
6.48 grams
10.1 grams
85. Find the number of moles in 3.30 g of (NH4)2SO4?
A 132.1 mol
B 40.0 mol
C
D
0.0279 mol
0.0250 mol
86. What is the volume (in liters at STP) of 2.50 mol of carbon monoxide?
A 0.112 L
B 3.10 L
C
D
56.0 L
8.96 L
87. Which of the following is not an empirical formula?
A Na2SO4
B C6H5Cl
C
D
N2H4
Sn3(PO4)4
88. A compound has the empirical formula C2H3O and a molar mass of 172.0 g/mol. What is its
molecular formula?
A C6H9O3
B C8H12O4
C
D
C9H16O3
C7H8O5
89. Determine the number of moles in 625 L of H2 gas at STP?
A 3.58 x 10-2 mol
B 27.9 mol
C
D
1.40 x 104 mol
1250 mol
90. What is the percent of aluminum in Al2(SO4)3?
A 28.1%
B 54.0%
C
D
15.8%
56.7%
91. What is the empirical formula of a compound that is 3.05% carbon, 0.26% hydrogen, and
96.96% iodine?
A C2HI7
B CH2I5
C
D
C3H2I11
CHI3
92. The following would be classified as which type of reaction?
CH4 + 2 O2  CO2 + 2 H2O
A
B
C
D
synthesis
combustion
single displacement
double displacement
93. Which of the following describes the products of a double displacement reaction?
A
B
C
D
carbon dioxide and water
a single product
an element and a compound
two ionic compounds
94. When the following equation is balanced, what is the coefficient that goes with water?
_____ Mn(OH)3 + _____ H2SO3  _____ Mn2(SO3)3 + _____ H2O
A
B
C
D
2
3
6
12
Midterm Exam Sample Free Response Questions
For the following problems, SHOW ALL OF YOUR WORK! Include units in all of your
answers, and round each answer off to the correct number of significant figures, where
necessary.
1. Convert 84.3 gallons per square milligram to cubic nanometers per square pounds
2. How many formula units of Mn(NO3)2 are there in 28.9 grams of Mn(NO3)2? Show your set
up for determining molar mass. How many moles of nitrogen are present? How many atoms
of oxygen as present in the sample?
3. Fill in the following table
Atomic #
Mass #
# protons
#neutrons
#electrons
charge AZ
________
_________
___54____
_____
__128__
___52___
4. Name the following compounds
Cr(NO3) 3
___________________________
NaHCO3
___________________________
P4Cl7
___________________________
H2SO4
___________________________
Fe4C3 2 H2O__________________________
Xcharge
__________
Write the formula for the following compounds
Aluminium hydrogen sulfite
____________________________
Trinitrogen hexasulfide
____________________________
Copper (I) thiosulfate
____________________________
Perchloric acid
____________________________
Auric dichromate octahydrate
____________________________
5. The specific heat of a metal is 0.486 J/goC. What is the mass of the metal when a sample of
the metal absorbs 625 J of energy when it is heated from 25.0oC to 96.0oC? Assume that all
of the energy lost by the metal is gained by the water. (Cp of water = 4.18 J/goC).