Mississippi Chemistry Summative 2010
2A. CLASSIFYING MATTER
Below is an atomic model.
Table of Densities
Element
g/cm3
Scandium
2.99
Actinium
10.07
Palladium
12.02
Rhenium
21.04
1. Monique is trying to find the density of
an unknown element. She found that
the mass of the element is 24 grams
and the volume is 2cm3. Using the table
above what is the unknown element?
A. Palladium
B. Scandium
C. Actinium
D. Rhenium
2. Which of the following could be
considered as a molecule, but not a
compound?
A. CH3OH
B. I2
C. H2O
D. Kr
3. Which of the following would be
considered as an element?
I. Hydrogen gas
II. Liquid nitrogen
III. Diamonds (made all of carbon)
A.
B.
C.
D.
I, II, and III
I and II
I and III
NONE OF THE ABOVE
4. What matter is displayed in the atomic
model above?
A. Element
B. Compound
C. Heterogeneous mixture
D. Homogeneous mixture
5. Which of the following would be
considered a homogeneous mixture?
A. Salt water
B. Strawberry yogurt with fruit
C. Cooking Oil
D. The metal alloy brass
6. Which of the following statements is
TRUE?
A. Atoms are the closest together in
gases.
B. Atoms have the most amount of
internal energy in gases.
C. Atoms have the least amount of
molecular motion in gases.
D. Atoms do not move in gases.
7. As molecules of a substance goes from
a gas  liquid  solid, what happens
to the molecular motion of the
molecules?
A. Molecules speed up.
B. Molecules remain at constant
speed.
C. Molecules slow down.
D. It is impossible to determine what
happens to the molecules.
The graph below represents the uniform
cooling of a sample of lauric acid starting as
a liquid above freezing point.
8. Using the graph above, what is the
phase change that takes place from
point C and B?
A. Melting
B. Freezing
C. Condensation
D. Sublimation
B. Dalton used the Gold Foil
Experiment to determine protons
are in the center of the atom.
C. Bohr used the Cathode Ray
Experiment to determine protons
are in the center of the atom.
D. Thomson used the Cathode Ray
Experiment to determine protons
are in the center of the atom.
11. Which of the following researchers and
their model is incorrectly paired?
A. Thomson : Plum Pudding Model
B. Rutherford : Nuclear Theory
C. Dalton : Atomic Theory
D. Bohr : Nuclear Theory
12. What element does the Bohr model
below represent?
2B. HISTORY OF THE ATOM
9. Which best describes the current model
of an atom?
A. A solid sphere with electrons and
protons embedded
B. A solid sphere unique for
everything that exists
C. A central nucleus containing
protons with electrons orbiting in
specific paths
D. A central nucleus containing
protons and neutrons with
electrons orbiting in levels of high
probability
10. The most current model of the model is
the wave-mechanical model. Which
scientist discovered that the protons in
the center of the atom and what
experiment did he use to discover these
particles?
A. Rutherford used the Gold Foil
Experiment to determine protons
are in the center of the atom.
A.
B.
C.
D.
Carbon
Beryllium
Boron
Nitrogen
3A. ATOMIC STRUCTURE
13. The atomic number of an atom always
equal to the number of its
A. protons, only
B. protons plus electrons
C. neutrons, only
D. protons plus neutrons
14. Which two particles make up both the
nucleus and the atomic mass?
A. electron and neutron
B. proton and electron
C. proton and neutron
D. electron and positron
15. An atom in the ground state contains a
total of 7 electrons, 7 neutrons, and 7
protons. Which Lewis electron-dot
diagram represents this atom?
19. Which two notations represent
different isotopes of the same element?
32
A. 73 Li and 73 Li
C. 32
15 P and 16 S
B.

14
7
32
15
Be and 146 Be
P and 30
15 P

D.
2D. NUCLEAR CHEMISTRY

 Which nuclear emission has the
20.
16. Which of the following electronic
configurations for Nitrogen is written
correctly?
A. 1p2 2p2 2s6
B. 1s2 2s2 2p6
C. 1s2 2s2 2p1
D. 2p6
17. How many neutrons are in an atom of
Iridium-192 (atomic number 77)?
A. 115
B. 125
C. 92
D. 77
The atomic mass and percent natural
abundance of each naturally occurring
isotope of Neon are given in the data
table below.
18. Using the data table above, which of
the following equations could be used
to find the average atomic mass of
Neon?
A. (.88 x 19.992) + (.12 x 21.991) =
B. (.88 + 19.992) x (.12 + 21.991) =
C. (88 x .19992) + (12 x .21991) =
D. (88 + .19992) x (12 + .21991) =
greatest penetrating power?
A. gamma radiation
B. alpha particle
C. beta particle
D. positron
21. Which nuclear emission has the
greatest mass?
A. 
B. 
C. +
D. 22. In the third step of Uranium decay,
Protactium-234 goes through BETA
DECAY. Which equation represents the
decay?
0
234
A. 234
91Pa1 e + 92 U
B.
234
91
Pa  10 e  23490Th

C.
234
91
Pa42 He +

D.
234
91
Pa  42 He  23490Th
234
92
U
23.
 If 100g of Uranium-239 went through 2
half-lives, then how much is left?
 A. 50g
B. 25g
C. 120g
D. 12.5g
24. The nucleus of a radium-226 atom is
unstable. What does this cause the
nucleus to spontaneously do as a result
of the instability?
A. absorb protons
B. oxidize
C. decay
D. absorb electrons
2E. CHEMICAL BONDS
D. Both B and C
30. Which covalent bond has the greatest
polarity?
A. H-C
B. H-O
C. H-N
D. H-B
25. What type of bond would be predicted
when Oxygen and Sulfur form SO2?
A. isotopic bond
B. ionic bond
C. covalent bond
D. hydrogen bond
31. What electrons are shared during a
covalent bond?
A. Excited electrons
B. Electrons closest to the nucleus
C. Valence electrons
D. All electrons
26. What two types of atoms bond
together in ionic bonding?
A. nonmetal and nonmetal
B. metal and nonmetal
C. metal and metal
D. metal and metalloids
32. Nitrogen, Phosphorus, and Arsenic all
have the same expected charge of its
common ion. What is this charge?
A. 5B. 3+
C. 3D. 5+
27. Which of the following describes what
happens to valence electrons in metallic
bonding?
A. They become delocalized amongst
all atoms.
B. They are shared to fill s-orbitals.
C. They are given from some atoms to
others to fill their valence shells.
D. They remain with their original
atoms but bond
28. How many more electrons does a
Hydrogen atom at ground state need to
complete the octet rule?
A. 7 electrons
B. 1 electrons
C. 2 electrons
D. It already satisfies the octet rule.
2G. THREE-DIMMENSIONAL ATOM
33. What is the correct Lewis dot structure
for arsenic?
A.
C.
B.
D.
34. Which Lewis electron-dot diagram is
correct for S2- ion?
29. Which symbol represents a particle with
a total of 7 electrons?
A. B2+
B. F2+
C. B2-
Below is a student Lewis Dot Diagram of
COH2.
35. Which of the following statements is
FALSE?
A. The two hydrogen atoms are stable.
B. The oxygen atom is stable.
C. The carbon cannot form a double
bond with oxygen.
D. All the valence electrons have been
used in the model.
Below is a student Lewis Dot Diagram
drawing of NH3.
36. What should the student do to finish
the Lewis Dot Diagram above?
E. Add a double bond between an N
and H.
F. Add a lone pair to the nitrogen.
G. Do nothing because everything
satisfies the octet rule.
H. Substitute the nitrogen with boron
and the molecule will be stable
37. In a molecule what is the behavior of
valence electrons?
A. Valence electrons move close to
each other.
B. Valence electrons move away to
each other.
C. Both A and B
D. Valence electrons are neutral, so
they have do not display attractive
or repulsive behavior.
38. What is the name for the molecule
below?
A.
B.
C.
D.
Trigonal Pyramidal
Tetrahedral
Trigonal Planar
Bent
3B. PERIODIC TRENDS
39. When you read the periodic table from
left to right what trend generally DOES
NOT occur?
A. The number of protons increases
B. The number of electrons increases
C. The atomic size increases
D. The number of neutrons increases
40. In a sample of 20 Oxygen atoms, it is
found that 10 are 17O and 10 are 15O.
What is the average atomic mass of
Oxygen?
A. 16.75 g/mol
B. 16 g/mol
C. 16.5 g/mol
D. 15.5 g/mol
41. Fill in the blank.
Elements of the same ___________
share the greatest chemical
characteristics.
A. Period
B. Group
C. Type of Metal
D. Nature
42. What type of element has a low
density, and a low melting point?
A. Metals
B. Nonmetals
C. Metalloids
D. Transition metals
43. From lowest to highest, in what order
do elements best conduct electricity
and heat?
A. nonmetals, metalloids, metals
B. metals, metalloids, nonmetals
C. nonmetals, metals, metalloids
D. metals, non metals, metalloids
44. Which of the following statements is
INCORRECT?
A. Nitrogen is more electronegative
than Carbon.
B. Chlorine is more electronegative
than Iodine.
C. Oxygen is more electronegative
than Sulfur.
D. Boron is more electronegative than
Carbon.
45. Which of the following statements is
INCORRECT?
A. As you move down a group,
ionization energy decreases.
B. As you move down a group,
electron affinity decreases.
C. As you move across a period,
ionization energy decreases.
D. As you move across a period,
electron affinity increases
3C. CHEMICAL REACTIONS
48. Which equation represents a
decomposition reaction?
A. LiOH + HCl  LiCl + H2O
B. 2 Na + 2 H2O  2 NaOH + H2
C. CaCO3  CaO + CO2
D. CH4 + 2 O2  CO2 + 2 H2O
49. What are the coefficients of the
following equations?
_______NaN3 (s)  ____N2 (g) + ____Na (s)
A.
B.
C.
D.
1, 1, 2
2, 3, 2
2, 6, 2
1, 3, 1
50. Which of the following metals cannot
replace Tin?
A. Lithium
B. Zinc
C. Sodium
D. Silver
51. What are the products of the single
replacement reaction below?
Cl2 + KBr  _________
E.
F.
G.
H.
Br + KCl2
KBr + Cl2
Cl2 + KBr2
Br2 + KCl
46. What type of reaction is the following?
2AlCl3 +3H2  6HCl + 2 Al
A.
B.
C.
D.
Combustion
Double displacement
Decomposition
Single displacement
47. What type of reaction is the following?
C3H8 + 5 O2  3 CO2 + 4 H2O
A.
B.
C.
D.
Combustion
Double displacement
Decomposition
Single displacement
3D. THE PERIODIC TABLE
52. What is the relationship between
chemical reactions and chemical
equations?
A. A chemical equation represents a
chemical reaction.
B. A chemical reaction represents a
chemical equation.
C. Chemical equations and chemical
reactions have no similarities.
D. Chemical equations and chemical
reactions are the same thing.
53. For the following balanced equation:
MgCl2 + 2 NaOH  2 NaCl + Mg(OH)2
If 6 moles of NaCl are to be produced, how
many moles of MgCl2 must react?
A. 3
B. 6
C. 1
D. 2
54. What is the approximate molecular
mass of Ca(OH)2?
A. 72 amu
B. 43 amu
C. 74 amu
D. 114 amu
55. What is the percent composition by
mass of aluminum in Al2(SO4)3 (atomic
mass = 342 grams/mole)?
A. 7.89%
B. 15.8 %
C. 20.8%
D. 36.0 %
56. What is the empirical formula for a
compound that is 37.5% C, 12.5% H,
and 50% O? (3D)
A. C3HO4
B. CHO
C. CH4O
D. C6H25O6
57. Which is an empirical formula?
A. C2H4
B. C3H6
C. P2O5
D. P4O6
58. What is the molecular formula of a
compound with the empirical formula
C4H4S and molar mass of 168 grams?
A. C2H2S
B. C8H8S
C. C4H4S
D. C8H8S2
59. How many molecules are inside 3 moles
of Carbon?
A. 12.04 x 1023
B. 6.02 x 1023
C. 18.06 x 1023
D. 24.08 x 1023
60. If you have 6 moles of Boron, then how
many grams do you have?
I. 11g
J. 66g
K. 99g
L. 33g
61. If you 320g of Br2 then how many moles
do you have?
M. 1 moles
N. 3 moles
O. 4 moles
P. 2 moles
4B. IDEAL AND REAL GASES
62. Kenny made an observation of nitrogen
gas. He found that the gas moved at
different speeds and the energy was
conserved in the reactions. What can
he conclude about the gas?
A. The gas is a real gas.
B. The gas is an ideal gas.
C. We cannot conclude anything about
the gas.
D. The gas is in a supersaturated
state.
63. What are the two differences of an
ideal gas and a real gas?
A. Real gases have attractive forces
and have mass.
B. Real gases do not have attractive
forces and do not have mass.
C. Real gases have attractive forces
and do not have mass.
64. Real gases act most like ideal gas under
what conditions?
A. High pressure, high temperature
B. Low pressure, low temperature
C. High pressure, low temperature
D. Low pressure, High temperature
4C. IDEAL GAS EQUATION
65. A tire with a volume of 10L drove from
Convert 560K to Celsius.
A. 833oC
B. 287oC
C. 560oC
D. 14oC
66. Convert 2280mmHg to atm.
A. 1 mol
B. 2 mol
C. 3 mol
D. 4 mol
67. Determine the number of moles of gas
in a 100L container at 800K and 4atm?
A. 6.09 moles
B. 100 moles
C. 200 moles
D. 60.9 moles
68. How many moles of air are there in a
.125L Erlenmeyer flask if the pressure is
760 mmHg and the temperature is 20
°C?
A. .0004 moles
B. 4 moles
C. .005 moles
D. 5 moles
69. If I put 4 moles of Helium gas into a
balloon at STP, then what will the
volume of the balloon be?
A. 92.6L
B. 89.5L
C. 102L
D. 20.4L
70. A bag of chips in a truck travelled from
1atm and moved to a state with a
pressure .5atm. If the volume of the
bag started at 25mL, then what was its
final volume assuming it had constant
temperature and number of moles?
A. 50mL
B. 100mL
C. 5mL
D. 10mL


71. A scuba tank changed from 1 atm to
10atm as it sunk below the water. If
the scuba diver’s tank started at 300K,
then what is the tank’s new
temperature? (Assume there are
constant moles and volume)
A. 4000K
B. 300K
C. 400K
D. 3000K
4D. THERMODYNAMICS
72. A metal rod and brick are both in the
sun. Assuming that both are the same
mass, which property of matter will
make one hotter to the touch than the
other?
A. Density
B. Melting point
C. Specific heat
D. Boiling point
73. A chemical reaction releases 91.85 kJ of
energy. During the reaction, 0.681 kg of
the solution heats up from 93.5°C to
98.1°C. What equation would be used
to solve this problem?
A. PV=nRT
B. Q=mcΔT
C. Q=mΔHf
D. Q=mΔHv
74. When you squeeze an instant hot pack,
it breaks a little baggie inside. After
shaking it, the contents mix and react to
feel warm. Which of the following
accurately describes the situation?
A. vaporization
B. endothermic
C. enthalpic
D. exothermic
75. If table salt (NaCl) is dissolved in water,
which of the following is not necessarily
accurate in describing the mixing
process?
A. Solution
B. Electrolyte
C. Supersaturated
D. Soluble
4E. SOLUTIONS
76. If two liquids do not mix, which of the
following terms applies?
A. Miscible
B. Solute
C. Immiscible
D. Solvent
77. Which of the following will NOT
increase the solubility of a substance in
a solution?
A. Mixing the solute in the
solution
B. Crushing the solute
C. Heating the solution
D. Cooling the solution
78. If I dissolve 10g of SO2 is 100g of H2O at
10oC then what state will the solution
be in?
A. Saturated
B. Supersaturated
C. Unsaturated
D. Equalized
79. What is the molarity of a solution that
contains 0.202 mol KCl in 0.798 L
solution?
A. 3.95 M
B. 0.596 M
C. 1.00 M
D. 0.253M
80. A reaction calls for 20 mL of a 0.8 M
solution of potassium iodide. You only
have 2M and 0.5M solutions in your
stock cabinet. Which could you do to
make your solution?
A. Mix 10mL of each of the 2M and
0.5M solutions
B. Obtain 8mL of the 2M solution and
dilute it to 20mL
C. Obtain 12.5mL of the 0.5M solution
and dilute it to 20mL
D. Add 15mL of 0.5M solution to 5mL
of 2.0M solution
81. If a solution of ethanol (C2H5OH) is 6.5
M. what is the percent mass of ethanol
in the mixture (water’s density is 1g/mL
A. 6.5%
B. 30%
C. 23%
D. 87%
Use the equation below to answer the
following questions.
H2(g) + F2(g) ⇌2HF(g)
82. If the reaction is at equilibrium, and I
add more H2, then what will happen to
the reaction?
A. The reaction will shift right.
B. The reaction will shift left.
C. The reaction will not shift.
D. The reaction will shift left, then
right.
83. If the reaction is at equilibrium, and I
take away 2HF, then what will happen
to the reaction?
A. The reaction will shift right.
B. The reaction will shift left.
C. The reaction will not shift.
D. The reaction will shift left, then
right.
5A. ACIDS AND BASE PROPERTIES
84. Like litmus paper, cabbage juice
changes color based on a substances
pH. Therefore, both cabbage juice and
litmus paper are what?
A. Detectors
B. Notifies
C. Magic
D. Indicators
85. Acids have a _________ taste, whereas
bases have a __________ taste.
A. bitter, sour
B. sour, sour
C. bitter, bitter
D. sour, bitter
86. The pH of a solution was once 7 but
now is 100 times more basic. What is
its new pH?
A. 5
B. 8
C. 9
D. 6
87. The pH of a solution changed from 2 to
3. What happened to the
concentration of H+ ions?
A. decreased by a factor of 10
B. increased by a factor of 100
C. increased by a factor of 10
D. decreased by a factor of 100
88. A reaction calls for 20 mL of a 0.8 M
solution of potassium iodide. You only
have 2M and 0.5M solutions in your
stock cabinet. Which could you do to
make your solution?
A. 8mL of the 2M solution and add
water
B. 10mL of the 0.5M solution and add
water
5C. OXIDATION AND REDUCTION
93. What type of reaction occurs in the
following chemical equation?
C. 8mL of the 0.5M solution and add
water
D. 10mL of the 2M solution and add
water.
5B. BRONSTED-LOWRY AND
ARRHENIUS
89. In the following reaction what does the
role of water play?
H2O + H2S  HS– + H3O+
A.
B.
C.
D.
It is a BrØnsted acid
It is a BrØnsted base
It is both an acid and a base
It neither an acid or a base
90. Which substance is an BrØnsted base in
the following reaction?
HF + NaOH  H2O + NaFCH3Cl
A.
B.
C.
D.
NaOH
H2O
NaFCH3Cl
HF
91. What is the product of the
neutralization reaction below?
H2S + 2KOH 
A.
B.
C.
D.
KS + H2O
H3O+ + SOK
K2S + 2H2O
The products cannot be determined
92. Which volume of 10 M NaOH(aq)
exactly neutralizes 150 milliliters of 2 M
HNO3 (aq)?
A. 1.5 mL
B. 3.0 mL
C. 30 mL
D. 7.5 mL
Ca  Ca 2+  2e A. synthesis
B. combustion
C. oxidation
 D. reduction
Use the following reaction to answer
questions 49 and 50.
2C2H2 + 5O2  4CO2 + 2H2O
94. What is the oxidation state of Carbon in
C2H2?
A. -1
B. +1
C. -2
D. +2
95. What is the element that is reduced?
A. H
B. O
C. C
D. All of the above