Download Name_____________________________________ Chemistry

Name_____________________________________
Date ____________________________Period____
Chemistry
Final Exam Review
Properties of Matter
1. Define matter.
2. Classify the following as chemical or physical changes.
a. Burning paper
___________________
d. Boiling water
__________________
b. Chopping wood
___________________
e. Iron rusting
__________________
c. Dissolving sugar
___________________
f. Cooking food
__________________
3. Classify the following as an element, compound.
a. BaCl2 ____________________
d. Ga _______________________
e. FeO _______________________
f. Rn _______________________
4. a. Define Density & write its formula.
b. A solid has a volume of 276.5cm3 & a mass of 405.7g. Will the solid float on
water? Why or why not?
Directions: Identify the letter of the choice that best completes the statement or answers the question.
____ 5.
a. air.
b. light.
Matter includes all of the following EXCEPT
c. smoke.
d. water vapor.
____ 6.
A physical property may be investigated by
a. melting ice.
c. allowing silver to tarnish.
b. letting milk turn sour.
d. burning wood.
____ 7.
Chemical properties
a. include changes of state of a substance.
b. include mass and color.
c. include changes that alter the identity of a substance.
d. can be observed without altering the identity of a substance.
____ 8.
Two features that distinguish matter are
a. mass and velocity.
c. mass and volume.
b. weight and velocity.
d. weight and volume.
____ 9.
One chemical property of matter is
a. boiling point.
c. reactivity.
b. texture.
d. density.
____ 10.
a. volume
b. length
Which of the following is an intensive physical property?
c. color
d. mass
____ 11.
An example of a chemical change is
a. sanding wood.
c. milk going sour.
b. melting ice.
d. vaporizing gasoline.
____ 12.
A physical change occurs when a
a. peach spoils.
c. bracelet turns your wrist green.
b. copper bowl tarnishes.
d. glue gun melts a glue stick.
____ 13.
The state of matter in which a material has neither a definite shape nor a definite volume is the
a. gaseous state.
c. elemental state.
b. liquid state.
d. solid state.
____ 14.
A list of pure substances could include
a. bread dough.
c. vitamin C (ascorbic acid).
b. vinegar (5% acetic acid).
d. sea water.
The Atom
Identifying Properties of Atoms
15. Directions: Complete the following table.
Atom or Ion
# of Protons
# of Electrons
# of Neutrons
Atomic
Number
Na +2
11
12
S-2
18
Ne
Mass Number
32
10
20
____
16.
Who was the schoolmaster who studied chemistry and proposed an atomic theory?
a. John Dalton
c. Robert Brown
b. Jons Berzelius
d. Dmitri Mendeleev
____
17.
a. proton.
b. nucleus.
Experiments with cathode rays led to the discovery of the
c. neutron.
d. electron.
____
18.
Who discovered the nucleus by bombarding gold foil with positively charged particles and noting that some
particles were widely deflected?
a. Rutherford
c. Chadwick
b. Dalton
d. Bohr
____
19.
Rutherford's experiments led to the discovery of the
a. electron.
c. nucleus.
b. cathode ray.
d. neutron.
____
20.
An atom is electrically neutral because
a. neutrons balance the protons and electrons.
b. nuclear forces stabilize the charges.
c. the numbers of protons and electrons are equal.
d. the numbers of protons and neutrons are equal.
____
21.
a. nucleus.
b. nuclides.
Most of the volume of an atom is occupied by the
c. electron cloud.
d. protons.
____
22.
a. electrons.
b. protons.
Isotopes of an element contain different numbers of
c. neutrons.
d. nuclides.
Electron Configurations
23. Electron Configurations
Directions: Using the LONG version, write out the ground state electron configuration for the following species.
a. Mg__________________________________________________________________
b. S __________________________________________________________________
c. Th __________________________________________________________________
24. Directions: Using NOBLE GAS notation, write out the ground state electron configuration for the following species.
a. Ba __________________________________________________________________
b. Ar __________________________________________________________________
c. U __________________________________________________________________
Directions: Answer the following question or complete the following statements.
25. Define valence electrons?
26. The maximum amount of valence electrons an atom can have is __________, this is called an
____________ of electrons.
27. Why do all atoms want to obtain 8 valence electrons?
28. What two atoms do NOT want 8 valence electrons?
29. How many valence electrons do the following atoms have?
a. N ________
b. Br
c. K
________
________
Directions: Identify the letter of the choice that best completes the statement or answers the question.
_____30. For an electron in an atom to change from the ground state to an excited state,
a. energy must be released.
b. energy must be absorbed.
c. radiation must be emitted.
d. the electron must make a transition from a higher to a lower energy level.
____ 31.
If electrons in an atom have the lowest possible energies, the atom is in the
a. ground state.
c. excited state.
b. inert state.
d. radiation-emitting state.
____
32.
The statement that an electron occupies the lowest available energy orbital is
a. Hund's rule.
c. Bohr's law.
b. the Aufbau principle.
d. the Pauli exclusion principle.
____
33.
"Orbitals of equal energy are each occupied by one electron before any is occupied by a second electron, and all
electrons in singly occupied orbitals must have the same spin" is a statement of
a. the Pauli exclusion principle.
c. the quantum effect.
b. the Aufbau principle.
d. Hund's rule.
____
34.
The statement that no two electrons in the same atom can have the same four quantum numbers is
a. the Pauli exclusion principle.
c. Bohr's law.
b. Hund's rule.
d. the Aufbau principle.
____
35.
If the s and p sublevels of the highest main energy level of an atom are filled, how many electrons are in the main
energy level?
a. 2
c. 16
b. 8
d. 32
____
a. 2
b. 8
36.
If an element has an octet of electrons in its highest main energy level, there are ____ electrons in this level.
c. 10
d. 32
____
37.
An element with 8 electrons in its highest main energy level is a(n)
a. octet element.
c. Aufbau element.
b. third period element.
d. noble gas.
The Periodic Table
38. Directions: Label the following on the periodic table:
halogens
transition metals
noble gases
alkaline earth metals
alkali metals
actinides
lanthanides
metalloids
metals
nonmetals
39. ________ According to the modern periodic table, the elements are arranged in periods according to their
A. electron configurations
B. atomic masses
C. atomic numbers
D. valence electrons
40. ________ The most reactive metal is
A. Fr
B. Ca
C. F
41. ________ A group on the periodic table is the same as a(n)
A. period
B. row
D. Li
C. family
D. line
42. ________ Hydrogen is placed separately from the other elements on the periodic table because
A. it is a gas
B. it has 1 electron
C. it has unique properties
D. it is colorless
43. ________ The most reactive nonmetal is
A. Ne
B. O
D. F
C. Fr
Directions: Circle the atom with the LARGEST electronegativity.
44. Li
45. O
K
C
N
46. List the steps for drawing Lewis structures.
Na
_____ 47. What is the shape of a water molecule?
a. Linear
c. Tetrahedral
b. Bent
d. Trigonal Pyramidal
_____ 48. What is the shape of a hydrogen molecule?
a. Linear
c. Tetrahedral
b. Bent
d. Trigonal pyramidal
_____ 49. What is the shape of an ammonia molecule (NH3)?
a. Linear
c. Tetrahedral
b. Bent
d. Trigonal pyramidal
_____ 50. What is the shape of a methane molecule (CH4)?
a. Linear
c. Tetrahedral
b. Bent
d. Trigonal pyramidal
Polarity
_____
51. The chemical bond formed when two atoms share electrons is called a(n)
a. ionic bond.
b. orbital bond.
c. Lewis structure.
d. covalent bond.
____
52.
If two covalently bonded atoms are identical, the bond is
a. nonpolar covalent.
c. nonionic.
b. polar covalent.
d. coordinate covalent.
____
53.
If the atoms that share electrons have an unequal attraction for the electrons, the bond is called
a. nonpolar.
c. ionic.
b. polar.
d. dipolar.
____
54.
In which of these compounds is the bond between the atoms NOT a nonpolar covalent bond?
a. Cl2
c. HCl
b. H2
d. O2
_____ `55. If electrons are transferred between two atoms, the resulting bond is __________
a. nonpolar.
c. ionic.
b. polar.
d. dipolar.
_____
56. If the difference in electronegativity values of two atoms are 0.3, the bond would be _______.
a. nonpolar.
c. ionic.
b. polar.
57. (Polar / Nonpolar) molecules are will dissolve in water.
Naming and Formula Writing
For each of the following, provide either the correct chemical name or chemical formula.
58. cadmium nitrate ______________________________
59. dinitrogen monoxide ______________________________
60. potassium bromide ______________________________
61. nitrous acid ______________________________
62. PCl3 ______________________________
63. V2O5 ______________________________
64. HClO4 ______________________________
65. BaSO4 ______________________________
66. sulfur hexafluoride ______________________________
67. sulfuric acid ______________________________
68. BaO ______________________________
69. SrSO3 ______________________________
70. acetic acid ______________________________
71. CBr4 ______________________________
72. (NH4)2SO4▪6H2O ______________________________
73. calcium hydroxide ______________________________
74. Na2CO3 ______________________________
75. Cu3P ______________________________
76. HI ______________________________
77. lead(II) acetate ______________________________
Types of Chemical Reactions
78. List 4 types of chemical reactions:
a.
b.
c.
d.
79. a. A + B → AB is an example of a(n) ____________________________ reaction.
b. AB → A + B is an example of a(n) ____________________________ reaction.
c. A + BC → AC + B is an example of a(n) ____________________________ reaction.
d. AB + CD → AD + CB is an example of a(n) ____________________________ reaction.
80. Classify the following reactions.
a. ____________________________ 2CuO(s) → 2Cu(s) + O2
b.
_____________________________________________
Ba(s) + 2HCl(aq)
H2(g) + BaCl2(aq)
c. ____________________________ Ca(NO3)2(aq) + 2NaI(aq)
CaI2(s) + Na(NO3)(aq)
81. What do the following symbols represent in a chemical reaction.
(s) = _________________________
(l) = ________________________
(g) = ________________________
(aq)= _______________________
Balancing Equations
82. Balance the following chemical reactions.
a. _____ N2 + ______ H2
b. _____ Na + _____ H2O
______ NH3
______ NaOH + ______ H2
c. ______ Pb(NO3)2(aq) + _____ KI(aq)
______ PbI2(s) + ______ KNO3(aq)
Molar Mass Calculations
83. Directions: Find the molar masses of the following compounds.
Compound
BaCO3
Molar Mass
(NH4)2SO4
Conversions using Molar Mass
Directions: Complete the following molar conversions. Be sure to show your work.
84. How many grams BaCO3 of are in 6.5moles of BaCO3?
85. How moles BaCO3 of are in 76.5g of BaCO3?
86. How many formula units of BaCO3 are in 0.536 mols of BaCO3?
87. How many grams BaCO3 of are in 3.76 X 1022 formula units of BaCO3?
Stoichiometry & Mole Ratios
____
a.
b.
In the reaction Zn + H2SO4
ZnSO4 + H2, what is the mole ratio of zinc to sulfuric acid?
1:6
1:1
____
a.
b.
88.
c.
d.
89.
In the reaction C + 2H2
CH4, what is the mole ratio of hydrogen to methane?
1:1
2:1
____
90.
N2(g) + 3H2(g)
required?
a. 1.0 mol
b. 2.0 mol
1:2
3:1
c.
d.
1:2
2:4
The Haber process for producing ammonia commercially is represented by the equation
2NH3(g). To completely convert 9.0 mol hydrogen gas to ammonia gas, how many moles of nitrogen gas are
c.
d.
____
91.
In the equation 2KClO3
decompose completely?
a. 1.0 mol
b. 2.5 mol
3.0 mol
6.0 mol
2KCl + 3O2, how many moles of oxygen are produced when 3.0 mol of KclO 3
c.
d.
____
92.
a. 2 mol
b. 4 mol
For the reaction C + 2H2
____
93.
water?
a. 40. g
b. 80. g
For the reaction 2Na + 2H2O
____
94.
sulfuric acid?
a. 80.0 g
b. 160. g
For the reaction SO3 + H2O
____
95.
of water?
a. 1.50 mol
b. 4.16 mol
For the reaction HCl + NaOH
3.0 mol
4.5 mol
CH4, how many moles of hydrogen are required to produce 10 mol of methane, CH 4?
c. 10 mol
d. 20 mol
2NaOH + H2, how many grams of sodium hydroxide are produced from 3.0 mol of
c.
d.
120 g
240 g
H2SO4, how many grams of sulfur trioxide are required to produce 4.00 mol of
c.
d.
240. g
320. g
NaCl + H2O, how many moles of hydrochloric acid are required to produce 150. g
c.
d.
8.32 mol
12.2 mol
____
96.
For the reaction SO3 + H2O
trioxide and 100. g of water?
a. 100. g
b. 200. g
____
97.
oxygen?
a. 100. g
b. 124 g
For the reaction 2Zn + O2
H2SO4, how many grams of sulfuric acid can be produced from 200. g of sulfur
c.
d.
245 g
285 g
2ZnO, how many grams of zinc oxide can be produced from 100. g each of zinc and
c.
d.
189 g
200. g
Kinetic Molecular Theory
98. Pressure is the result of the____________________ of gas molecules with walls of a container or surrounding
objects.
99. _________ When gas molecules are at a constant temperature, the speed of the molecules
a. gradually increases
c. gradually decreases
b. remains constant
100. Increasing the volume of a gas causes the pressure to (increase / decrease / remain constant).
101. Decreasing the temperature of a gas causes the volume to (increase / decrease / remain constant).
102. Increasing the pressure of a gas causes the temperature to (increase / decrease/ remain constant).
103. The process by which a gas is able to spread throughout a space is called __________________.
104. The process by which a gas is able to escape through a tiny opening is called _________________.
105. On the graph shown to the right…
a. where is the kinetic energy increasing?
b. where is a change in state occurring?
c. where is the substance a liquid?
Gas Laws
106. __________________________ States that the volume of a gas is directly proportional to its Kelvin temperature
when pressure & amount are held constant.
107. __________________________ States that the pressure of a gas is directly proportional to its Kelvin temperature
when volume & amount are held constant.
108. __________________________ States that pressure of a gas is inversely proportional to its volume when
temperature & amount are held constant.
109. __________________________ States that the volume of a gas is directly proportional to its amount when pressure
& temperature are held constant. This law also states that 1 mole of any gas at STP contains 6.02 x 1023 molecules, and
occupies a volume of 22.4 Liters
110. __________________________ Law that combines, Boyle’s, Charles’, & Gay-Lussac’s laws.
111. For each of the following gas laws, tell whether it is an example of a direct or indirect relationship:
112.
a. Charles’ Law___________________
c. Gay-Lussac’s Law
______________________
b. Boyle’s law ___________________
d. Avogadro’s Law
______________________
Draw the graph of a direct relationship:
|
Draw the graph of an indirect relationship:
|
|
|
|
|
|
|
|
|
|
113. List the standard pressure in atmospheres & standard temperature in Kelvin:
114. The molar volume of a gas is ____________________ at STP.
115. 25oC = __________________K
Gas Law Problems
116. Using Boyle’s Law, calculate the new volume of a gas when its pressure is changed to 530mmHg. The initial
pressure & volume of the gas was 250mmHg and 125.mL.
117. Using the Ideal Gas Law, calculate the volume of a 0.200 mol sample of gas at 10.0ºC and a pressure of 2.30 atm.
118. A 5.0 L propane tank on a camping stove contains propane at a pressure of 2.0 atm when the temperature is 14.0˚C
(in the morning). During the day the tank warms up to a temperature of 34.0˚C. What is the pressure of the propane gas
inside the tank when the temperature is 34.0˚C? Use Gay-Lussac’s law to solve.
119. A balloon contains 500 mL of helium at 20 ˚C. To what temperature should you increase the balloon to give a
volume of 550 mL? Use Charles’ Law to solve.
120. Imagine you blow up a balloon at sea level where there is 1 atm of pressure to a volume of 450 mL. On a scuba
diving trip, you decide to take the balloon with you. If the pressure of the ocean is 2.5 atm, what is the new volume of the
balloon? Use Boyle’s law to solve.
121. If 15 liters of helium are collected at 700 C, what will the volume of this gas be after it cools to 120 C?
122. Argon gas occupies a volume of 300.mL with a pressure of 3.2atm. To what pressure should the gas be
raised to bring the volume to 100.mL?
123. A ball has an internal pressure of 1.25 atm and a volume of 3.0 L. If the temperature of the ball is 170 C, what will
happen to the volume when the ball to taken to an altitude where the pressure is 0.75 atm and the temperature is –100 C?
Solutions
124. Determine the molarity of these solutions:
a.) 0.10 mol of NaCl in 1.0 L of solution
b.) 0.50 mol of NaCl in 500. mL of solution
c.) 25 grams of NaCl in 250 mL of solution
125. Determine the molality of these solutions:
a.) 25 g C6H12O6 in 0.25 L water
b.) 50 g C6H12O6 in 500. mL water