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Period________
Date_________________________
2013-2014 – Year Final - Review
1. Which measurement contains a total of three significant figures?
A) 0.010 g
B) 0.01 g
C) 0.01000 g
D) 0.0100 g
2. The following weighings were made during a laboratory exercise:
Mass of evaporating dish.... 59.260 g
Mass of sugar sample.......... 1.61 g
What is the total mass of the evaporating dish plus the sample, expressed to the proper number of significant figures?
A) 60.9 g
B) 60.870 g
C) 60.87 g
D) 61 g
3. What is the number 2.1 x 103 expressed in conventional form with the proper number of significant digits?
A) 2,100
B) 21,000.
C) 0.0021
D) 2,100.
4. What is the number 0.00034 expressed in proper scientific notation with the correct number of significant digits?
A) 3.40 x 104
B) 3.40 x 10-4
C) 3.4 x 104
D) 3.4 x 10-4
5. Which figure represents an Graduated cylinder?
6. The diagram below shows the upper part of a laboratory burner.
What letter represents the hottest part of the burner flame?
A) A
B) B
C) C
D) D
7. A student has to measure the diameter of a test tube in order to calculate the tube's volume. Based on the diagram
below, the tube's diameter is closest to
A) 12.5 cm
B) 2.32 cm
C) 3.25 cm
D) 1.25 cm
8. The diagram below represents a portion of a triple-beam balance.
If the beams are in balance with the riders in the positions shown, what is the total mass of the object?
A) 545.20 g
B) 545.52 g
C) 540.20 g
D) 540.52 g
9. Which of the following is the correct reading of the meniscus as shown in the portion of the buret below?
A) 42.65 mL
B) 41.30 mL
C) 41.35 mL
D) 42.60 mL
C) 0.37 g/cm3
D) 54 g/cm3
10. The solid block shown below has a mass of 146 grams.
What is the block's density?
A) 2.7 g/cm3
B) 8.1 g/cm3
11. How many neutrons would 34
16𝑆
A) 16
−2
have?
B) 18
C) 20
D) 32
12. What is the mass number of a carbon isotope that consists of 6 protons, 6 electrons, and 8 neutrons?
A) 2
B) 12
C) 14
D) 20
13. Why is an atom considered electrically neutral?
A) neutrons equal the number of protons
B) proton forces pull on the neutrons
C) electrons equal the number of protons
D) electrons equal the number of Neutrons
14. An isotope of mercury has 80 protons and 120 neutrons. What is the mass number of this isotope?
A) 80
B) 120
C) 200
D) 201
C) 48
D) 45
15. How many electrons are in a Cd3+ ion?
A) 112
B) 51
16. Matter is defined as anything that occupies space and has
A) odor
B) mass
C) color
D) a definite shape
17. Which pair is classified as pure substances?
A) elements and mixtures
C) elements and compounds
B) compounds and mixtures
D) elements and solutions
18. Mixtures are defined as
A) combinations of compounds and/or elements
C) always in definite proportions
B) combinations of elements, only
D) always homogeneous
19. An example of a mixture is
A) pure water
B) silver
C) salt water
D) gold
C) oil and water
D) air
20. An example of a homogeneous mixture is
A) concrete
B) salt and pepper
21. An example of a heterogeneous mixture is
A) carbon monoxide
B) carbon dioxide
C) sugar
D) dirt
22. Compounds are usually broken down into their component elements by
A) physical changes
B) evaporation
C) chemical changes
D) filtration
23. What is the frequency of light with a wavelength of 1.87 x 10-14 m?
A. 5.61 x 10-6 Hz
m/s
B. 1.60 x 1022 Hz
C. 6.23 x 10-23 Hz
D. 1.60 x 1022
24. What is the wavelength of light with a frequency of 5.60 x 1014 Hz?
F. 5.35 x 10-7 m
G. 1.87 x 106 m
H. 1.68 x 1023 m
J. 1.87 x 106 Hz
25. What condition is an atom in, when all electrons are in their normal energy levels?
A.
Excited State
B. Photon
C. Ground State
D. Bohr
H. Trough
J. Amplitude
26. What is the distance between the crests of a wave?
F. Frequency
G. Wavelength
27. Which of the following is arranged from highest frequency to lowest frequency?
A.
B.
C.
D.
Radio waves, microwaves, visible light, x-rays
Microwaves, X-rays, Visible light, Radio waves
Gamma rays, X-rays, Ultraviolet light, Violet light
Red light, Green light, Blue light, Violet light
28. Complete the following: If the Frequency increases the wavelength _____________________.
F. Increases
G. Decreases
H. Stays the same
J. Is zero
B. 3.00 x 108 ft/s
C. 6.36 x 10-34 J-s
D. 3.00 x 108
29. The Speed of Light (c) is…
A. 3.00 x 102 m/s
m/s
30. According to the Dual Nature of Light, light acts as a __________________ and a _________________.
F. Particle, Plank
G. Particle, Wave
31. What is the correct electron configuration for 24
12𝑀𝑔 ?
H. Wave, Crest
J. Crest, Particle
PAP 1
F. 1s2 2s2 2p6 3s23p6 4s23d4
G. 1s2 2s2 2p6
H. 1s3 2s2 2p5 3s2
J. 1s2 2s2 2p6 3s2
32. Which of the following represents the electron configuration of Fluorine and the ion that it forms?
F. 1s2 2s2 2p5
1s2 2s2 2p6
G. 1s2 2s2 2p3
1s2 2s1 2p3
H. 1s2 2s2 2p3
1s2 2s2 2p33s2
J. 1s2 2s2 2p3
4s2 2s2 2p2
33. Which type of elements are found on the left side of the Periodic Table?
F. Non-metals
G. Liquids
H. Metalloids
J. Metals
C. Metals
D. Noble gases
H. Mendeleev
J. Moseley
34. What do you call the family in column 18?
A. Alkali metals
B. Halogens
35. Who developed the first periodic table in 1869?
F. Dalton
G. Bohr
36. Which of the following are the only two liquids, at room temperature, found on the periodic table?
B. Ag, F
B. He, Hg
C. H, O
D. Br, Hg
H. Ne, Ar
J. F, Cl
C) 3
D) 6
C) Bi(NO3)3
D) NaClO3
C) Hg2Cl4
D) Hg2Cl2
C) Fe3O2
D) Fe3O
C) Sodium dioxide
D) Nadium
37. Which of the following are examples of Alkali Metals?
F. Mg, Ca
G. Li, Na
38. In the compound Co(NO2)3, how many nitrites are present?
A) 1
B) 2
39. Which of the following is the formula of a binary compound?
A) Al2S3
B) KOH
40. What is the chemical formula for mercury (I) chloride?
A) Hg2Cl
B) HgCl2
41. What is the correct chemical formula for iron (III) oxide?
A) FeO3
B) Fe2O3
42. What is the correct name for Na2O?
A) Disodium monoxide
oxide
B) Sodium oxide
43. What is the anion in the compound Ca(OH)2?
PAP 2
A) Calcium
B) Oxygen
C) Hydrogen
D) Hydroxide
44. Which formula is correctly paired with its name?
A) CuCl2 Copper (II) chloride
C) K2O Phosphorus dioxide
B) FeO  Iron (III) oxide
D) MgCl2  Magnesium chlorine
45. The correct name of the compound with the formula PbO2 is
A) Lead (III) oxide
oxide
B) Lead (I) oxide
C) Lead (IV) oxide
D) Lead (II)
46. What is the oxidation number/ charge of Copper in the compound, CuS?
A) -2
B) +2
C) +3
D) +4
47. In the compound chromium (III) sulfate, what is chromium’s oxidation number/charge?
A) +1
B) +2
C) +3
D) +4
48. Which formula correctly represents the compound calcium hydroxide?
A) Ca(OH)2
B) Ca2OH
C) CaOH
D) CaOH2
B) NH4CO3
C) (NH4)2(CO3)2
D) (NH4)2CO3
B) Sodium chlorate
C) Sodium chlorite
D) Sodium
C) Dinitrogen trioxide
D)
C) Hydrosulfurous acid
D) Sulfuric acid
49. What is the formula for ammonium carbonate?
A) NH4(CO3)2
50. What is the name of NaClO2?
A) Sodium perchlorate
chloride
51. Which of the following is not allowed?
A) Nitrogen dioxide
Mononitrogen oxide
B) Nitrogen monoxide
52. What is the name of the compound whose formula is H2SO3?
A) Sulfurous acid
B) Hydrosulfuric acid
53. What is the name for Al(MnO4)3?
A) Aluminum manganite
C) Aluminum magneside
B) Aluminum (III) permanganate
D) Aluminum permanganate
54. What are the chemical on the left side of the yield sign in a chemical equation called?
a. subscripts
b. products
c. coefficients
d. reactants
55. In a chemical equation, the symbol that takes the place of the word yields is a(n)
PAP 3
a. equal sign
b. coefficient
c. plus sign
d. arrow
56. In a chemical reaction, what is the relationship between the total mass of the reactants and the total mass of
the products?
a. They must be equal.
c. The mass of the reactants must be greater.
b. The mass of the products must be greater.
d. There is no general relationship between the two.
57. In a chemical equation, the number of molecules of a given substance is indicated by a
a. subscript.
b. coefficient.
c. superscript.
d. reaction number.
58. How many atoms of oxygen are represented in 2 Ca(NO3)2?
a. 4
b. 6
c. 10
d. 12
59. In balancing a chemical equation, which of the following are you allowed to do?
a. change subscripts
b. write coefficients
c. change superscripts
d. add new substances
60. What is the general form for a single-replacement reaction?
a. AX + BY  AY + BX
b. AB  A + B
c. A + B  AB
d. A + BX  AX + B
61. What is the general form for a double-replacement reaction?
a. AX + BY  AY + BX
b. AB  A + B
c. A + B  AB
d. A + BX  AX + B
62. What kind of reaction is represented by the equation C2Cl4 + Cl2  C2Cl6?
a. synthesis
b. double replacement c. single replacement
d. combustion
63. Which observation DOES NOT indicate that a chemical reaction has occurred?
a. formation of a precipitate
c. evolution of heat and light
b. production of a gas
d. change in total mass of substances
64. To balance a chemical equation, it may be necessary to adjust the
a. coefficients.
b. subscripts.
c. formulas of the products.
d. number of products.
65. According to the law of conservation of mass, the total mass of the reacting substances is
a. always more than the total mass of the products.
b. always less than the total mass of the products.
c. sometimes more and sometimes less than the total mass of the products.
d. always equal to the total mass of the products.
66. After the first steps in writing an equation, the equation is balanced by
a. adjusting subscripts to the formula(s).
b. adjusting coefficients to the smallest whole-number ratio.
c. changing the products formed.
PAP 4
d. making the number of reactants equal to the number of products.
67. The reaction Pb(NO3)2(aq) + 2KI(aq)  PbI2(s) + 2KNO3(aq) is a
a. double-replacement reaction.
c. decomposition reaction.
b. synthesis reaction.
d. combustion reaction.
68. The reaction 2KClO3(s)  2KCl(s) + 3O2(g) is a(n)
a. synthesis reaction.
c. combustion reaction.
b. decomposition reaction.
d. ionic reaction.
69. Using the following chemical reaction, perform the stoichiometric calculations requested:
_____Mg
+
_____H3PO4
→
_____Mg3(PO4)2
+
____H2
a. If 12.25 moles of Phosphoric Acid reacts to completion, how many moles of Magnesium phosphate are produced in
the reaction?
Assume an excess of magnesium.
b. If 25.0 grams of Magnesium reacts to completion, how many moles of Hydrogen gas will be produced? Assume the
Phosphoric Acid is in excess.
70. Use the following equation to answer the questions below:
_____Na2S2O3 + _____Cl2
+
_____H2O

_____NaHSO4
+
_____HCl
a. How many grams of Na2S2O3 are needed to react with 100.125 grams of Cl2?
b. How many moles of H2O are required for the reaction of 0.127 mol of Cl2?
71. An ideal gas is made up of gas particles that
PAP 5
a.
have no energy
b. attract each other
c. are in random motion
d. that do not flow
72. At which temperature would the molecules of a gas have the lowest average kinetic energy?
b. -100.0 oC
a. 5.00 K
c. 100.0 K
d. 5.00 oC
73. At constant temperature, the volume on 8.00 liters of a gas is increased from 1.00 atmosphere to 4.00
atmospheres. What will be the new volume of the gas? (SHOW WORK)
a. 1.00 L
b. 2.00 L
c. 32.0 L
d. 4.00 L
74. This scientific law is a mathematical expression of the direct relationship between temperature, and pressure as
volume remains constant.
a. Dalton’s Law
b. Boyle’s Law
c. Charles’s Law
d. Gay-Lussac’s Law
75. This scientific law is a mathematical expression of the indirect relationship between volume, and pressure as
temperature remains constant.
a. Combined Gas Law
b. Boyle’s Law
c. Charles’s Law
d. Gay-Lussac’s Law
76. This scientific law is a mathematical expression of the direct relationship between temperatures and volume as
pressure remains constant.
a. Combined Gas Law
b. Boyle’s Law
77. Convert 1.500 psi into kPa. (SHOW WORK)
a. 151.95 kPa
b. 0.01480 kPa
c. Charles’s Law
d. Dalton’s Law
c. 152.0 kPa
d. 10.3 kPa
c. 118 oK
d. 118 K
78. Convert -155.0 °C into Kelvin. (SHOW WORK)
a. -428 K
b. 118 °C
79. At standard temperature, a gas has a volume of 125.0 mL. The temperature is then increased to 348.0 K, and
the pressure is held constant. What is the new volume? (SHOW WORK)
a. 98.06 mL
b. 34.34 mL
c. 159 mL
d. 9375 mL
80. A rigid plastic container holds 1.00 L methane gas at 0.700 atm pressure when the temperature is 250.0 °C.
What is the new pressure that the gas will exert, if the temperature is raised to 300.0 °C? (Assume volume is
constant) (SHOW WORK)
PAP 6
a. 0.639 atm
b. 0.767 atm
c. 0.583 atm
d. 0.84 atm
81. What pressure, in mm Hg, is exerted by 0.750 mol of a gas at a temperature of 0.00 oC and a volume of 25.00 L?
82. A sample of gas at 52.0 oC has a volume of 5.20 L and exerts a pressure of 7.550 kPa. How many moles of gas are in the
sample?
83. What is the temperature of 0.250 mol of hydrogen gas occupying an 8.65 L vessel at a pressure of 0.255 atm?
84. What is the volume that is occupied by 32.80 g of Chlorine gas at 645.0 mm Hg and 125.0 K?
85. What is the molarity of a 0.30 liter solution containing 0.50 moles of NaCl?
86. Calculate the molarity of 0.289 moles of FeCl3 dissolved in 120 ml of solution?
87. How many moles of NaCl are present in 600.0 ml a 1.55 M NaCl solution?
88. How many moles of H2SO4 are present in 1.63 liters of a 0.954 M solution?
89. How many liters of solution are needed to make a 1.66 M solution containing 2.11 moles of KMnO4?
PAP 7
90. What volume of a 0.25 M solution can be made using 0.55 moles of Ca(OH)2?
91. What is the molarity in 650.0 ml of solution containing 63.0 grams of NaCl?
PAP 8
Information
Standard Air Pressure
Standard Temperature
Temperature Conversion
14.7
1.00
101.325
760.0
760.0
29.93
273 K
0.00 oC
Kelvin =
o
C
=
psi
atm
kPa
torr
mm Hg
in Hg
o
C + 273
K - 273
Boyle’s Law
Charles’s Law
Gay-Lussac’s Law
Combined Gas Law
__Dalton’s Law___
T is Constant
P is Constant
V is Constant
Nothing Constant
Pressure Only
P1V1 = P2V2
V1 / T1 = V2 / T2
P1 / T1 = P2 / T2
P1V1 / T1 = P2V2/ T2
PT = P1 + P2 + P 3 + …
P1 = P2 V2
V1
V1 = V2 T1
T2
P 1 = P 2 T1
T2
P1 = P2 V2 T1
V1 T2
V1 = P2 V2
P1
T1 = V 1 T2
V2
T1 = P 1 T2
P2
V1 = P2 V2 T1
P 1 T2
P2= P1 V1
V2
V2 = V1 T2
T1
P 2 = P 1 T2
T1
T1 = P 1 V 1 T2
P2 V2
V2 = P1 V1
P2
T2= V2 T1
V1
T2 = P 2 T1
P1
P2= P1 V1 T2
V2 T1
V2= P1 V1 T2
P 2 T1
T2 = P 2 V 2 T1
P1 V1
PAP 9