Download Honors Chemistry Exam Review Questions

Honors Chemistry Midterm 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. 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
3. 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
4. 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
5. 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
C
D
2.5 x 10-4 mg
2.5 x 106 mg
Chapter 2
6. How many milligrams are in 2.5 kg?
A 2.5 x 10-6 mg
B 25 mg
7. The temperature reading of -14oC corresponds to a Kelvin reading of :
A 297.6 K
B -287 K
C
D
287 K
259 K
8. 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
9. 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%
10. How many significant figures are in the measurement 603.040?
A 3
B 4
C
D
5
6
11. 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
12. 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
13. 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
14. 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
15. 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
16. Physical properties of a substance include:
A color and solubility
B melting and boiling points
C
D
density and odor
all of the above
17. 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
18. An example of a heterogeneous mixture would be:
A sugar
B salt water
C
D
tap water
vegetable soup
19. A method of separating a mixture based on the difference in particle size is called
A chromatography
B filtration
C
D
distillation
magnetism
20. Which of the following changes of state are endothermic?
A gas  liquid
B liquid  gas
C
D
gas  solid
liquid  solid
21. 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
22. 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
23. 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
24. 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
25. 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
26. 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
27. 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
28. 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
29. 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
30. In general, metals are:
A ductile
B malleable
C
D
good electrical conductors
all of these
C
D
oxygen
copper
31. Which of the following is a nonmetal?
A iron
B silver
32. 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 18
33. 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
34. 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
35. Which of the following particles is needed to complete this nuclear equation?
54
25Mn
A
B
56
27Co
57
26Fe
+ 21H  _____ + 10n
C
D
55
26Fe
58
24Cr
36. 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
37. Nuclear fusion:
A
B
C
D
occurs when large nuclei fuse together
takes place in the sun
generally produces hydrogen nuclei
all of these
38. What particle is needed to complete this equation?
14
7N
A
B
1
0n
0
-1e
+ _____  146C + 11H
C
D
4
2He
0
+1e
39. 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
40. 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
41. Which element when combined with chlorine would most likely form an ionic compound?
A lithium
B carbon
C
D
phosphorus
bromine
42. Choose the correct formula for calcium hydrogen phosphate?
A CaHPO4
B Ca2HPO4
C
D
Ca(H2PO4)2
Ca(HPO4)2
43. 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
44. What is the total number of atoms in one molecule of C6H12O6?
A 3
B 12
C
D
18
24
45. Name the following compound: Fe2(CO3)3
A Iron (III) carbonate
B Diiron (III) tricarbonate
C
D
Iron (II) carbonate
Diron (II) tricarbonate
46. What is the formula for trinitrogen heptachloride?
A N2Cl7
B N4Cl6
C
D
N3Cl6
N3Cl7
47. The formula of Copper (II) nitrate is:
A Cu(NO3)2
B CuNO3
C
D
Cu(NO3)2
CuNO3
48. 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
49. 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
50. 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
51. 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
52. What is the formula for Oxalic acid?
A HC2O4
B H2CO3
53. 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
54. Among the following, which is a binary molecular compound?
A CO2
B NaCl
C
D
FeO
MgS
Chapter 8
55. 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
56. What is the molar mass of MgCl2?
A 59.8 g/mol
B 95.3 g/mol
57. 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
58. 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
59. 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
60. 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
61. Which of the following is not an empirical formula?
A Na2SO4
B C6H5Cl
C
D
N2H4
Sn3(PO4)4
62. 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
63. 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
64. What is the percent of aluminum in Al2(SO4)3?
A 28.1%
B 54.0%
C
D
15.8%
56.7%
65. 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
Chapter 6
66. 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
67. 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
68. 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
Chapter 7
69. The reaction in question 70 is an example of a(n):
A decomposition
B synthesis
C
D
single displacement
combustion
70. In a double displacement reaction:
A
B
C
D
one of the products is always a gas
one of the products must be an element
positive ions are exchanged between two compounds
all of the above
71. Water is always a product in:
A
B
combustion reactions
decomposition reactions
C
D
single-displacement reactions
decomposition reactions
72. The following would be classified as which type of reaction?
CH4 + 2 O2  CO2 + 2 H2O
A
B
synthesis
single displacement
C
D
combustion
double displacement
73. Which of the following describes the products of a synthesis reaction?
A
B
carbon dioxide and water
C
an element and a compound D
a single product
two ionic compounds
74. O2, N2, Cl2, and I2 are examples of—
A
B
diatomic molecules
ionic compounds
C
D
compounds
atoms
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. A metal has a mass of 88.4 grams and an initial temperature of 106.2oC. The heated metal is
then placed into 25.9 grams of water with an initial temperature of 23.4oC. The final temperature of the metal
and the water is 26.7oC. What is the specific heat of the metal, assuming that all of the heat lost by the metal is
gained by the water?
6. Predict the products of the following equations given their reactants along with the type of reaction for each
equation.
___C2H5OH + ___ O2  ___ CO2 + ___ H2O
Type:
___Pb(NO3)2 + ___K3PO4 ___Pb3(PO4)2 + ___KNO3
Type:
___Zn + ___HClO3  ___ H0 + Zn(ClO3)2
Type:
___Na + ___FeBr3  ___ NaBr + Fe
Type:
7. Caffeine, a stimulant found in coffee, contains 49.5% C, 5.15% H, 28.9% N and 16.5% O. The
molecular formula has a molar mass of 194.22 g/mol. Determine the empirical and molecular formulas
for caffeine.
8. Fill in the blanks for the following nuclear decay:
115In 
3protons

2

3 neutrons

3