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VER A
Mississippi Chemistry Summative 2010
2A. CLASSIFYING MATTER
Table of Densities
Element
g/cm3
Scandium
2.99
Actinium
10.07
Palladium
12.02
Rhenium
21.04
1. Donovan is trying to find the density of
an unknown element. He found that
the mass of the element is about 6
grams and the volume is 2cm3. Using
the table above what is the unknown
element?
A. Actinium
B. Palladium
C. Scandium
D. Rhenium
4. Which of the following could be
considered as a molecule and an
element?
A. H2O
B. Kr
C. CH3OH
D. I2
The graph below represents the uniform
cooling of a sample of lauric acid starting as
a liquid above freezing point.
Below is an atomic model.
5. Using the graph above, what is the
phase change that takes place from
point C and B?
A. Condensation
B. Sublimation
C. Melting
D. Freezing
2. What matter is displayed in the atomic
model above?
A. Compound
B. Heterogeneous mixture
C. Element
D. Homogeneous mixture
3. 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 slow down.
C. Molecules remain at constant
speed.
D. It is impossible to determine what
happens to the molecules.
2B. HISTORY OF THE ATOM
6. Which best describes the current model
of an atom?
A. A central nucleus containing
protons with electrons orbiting in
specific paths
B. A solid sphere with electrons and
protons embedded
C. A solid sphere unique for
everything that exists
D. A central nucleus containing
protons and neutrons with
electrons orbiting in levels of high
probability
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VER A
7. 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.
B. Thomson used the Cathode Ray
Experiment to determine protons
are in the center of the atom.
C. Dalton used the Gold Foil
Experiment to determine protons
are in the center of the atom.
D. Bohr used the Cathode Ray
Experiment to determine protons
are in the center of the atom.
3A. ATOMIC STRUCTURE
11. Which two particles make up both the
nucleus and the atomic mass?
A. electron and neutron
B. proton and neutron
C. proton and electron
D. electron and positron
12. 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?
8. Which of the following researchers and
their model is incorrectly paired?
A. Thomson : Plum Pudding Model
B. Bohr : Nuclear Theory
C. Rutherford : Nuclear Theory
D. Dalton : Atomic Theory
13. Which of the following electronic
configurations for Nitrogen is written
correctly?
A. 1s2 2s2 2p6
B. 1s2 2s2 2p1
C. 1p2 2p2 2s6
D. 2p6
9. What element does the Bohr model
below represent?
A.
B.
C.
D.
14. How many neutrons are in an atom of
Iridium-192 (atomic number 77)?
A. 115
B. 92
C. 77
D. 125
15. Which two notations represent
different isotopes of the same element?
32
A. 73 Li and 73 Li
C. 32
15 P and 16 S
Carbon
Boron
Nitrogen
Beryllium
10. The atomic number of an atom always
equal to the number of its
A. neutrons, only
B. protons plus neutrons
C. protons, only
D. protons plus electrons
B.

14
7
Be and
14
6
Be
32
D 15 P and
2D. NUCLEAR
CHEMISTRY

 Which nuclear emission

16.
has the
greatest penetrating power?
A. gamma radiation
B. beta particle
C. positron
D. alpha particle
30
15
P
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VER A
17. Which nuclear emission has the
greatest mass?
A. 
B. +
C. D. 
22. 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
18. 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. oxidize
B. absorb protons
C. decay
D. absorb electrons
23. How many more electrons does a
Hydrogen atom at ground state need to
complete the octet rule?
A. 1 electrons
B. 7 electrons
C. 2 electrons
D. It already satisfies the octet rule.
19. 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
20.
 If 100g of Uranium-239 went through 2
half-lives, then how much is left?
 A. 50g
B. 120g
C. 12.5g
D. 25g
2E. CHEMICAL BONDS
21. What type of bond would be predicted
when Oxygen and Sulfur form SO2?
A. covalent bond
B. hydrogen bond
C. isotopic bond
D. ionic bond
24. Which symbol represents a particle with
a total of 7 electrons?
A. B2+
B. F2+
C. B2D. Both B and C
25. Which covalent bond has the greatest
polarity?
A. H-N
B. H-B
C. H-C
D. H-O
2G. THREE-DIMMENSIONAL ATOM
26. Which Lewis electron-dot diagram is
correct for S2- ion?
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Below is a student drawn Lewis Dot
Diagram of COH2.
27. Which of the following statements is
FALSE?
A. Ten valence electrons can be used
to create the bonds in the atom.
B. A lone pair from oxygen needs to
form a double bond with carbon.
C. The two hydrogen atoms satisfy the
octet rule.
D. The oxygen atom has three lone
pairs.
Below is a student drawn Lewis Dot
Diagram drawing of NH3.
28. What should the student do to finish
the Lewis Dot Diagram above?
A. Do nothing because everything
satisfies the octet rule.
B. Substitute the nitrogen with boron
and the molecule will be stable.
C. Add a double bond between an N
and H.
D. Add a lone pair to the nitrogen.
29. In a molecule what is the behavior of
valence electrons?
A. Valence electrons move close to
each other.
B. Valence electrons constantly trade
places with each other.
C. Valence electrons are neutral, so
they do not display attractive or
repulsive behavior.
D. Valence electrons move away to
each other.
VER A
30. What is the name for the molecule
below?
A.
B.
C.
D.
Trigonal Pyramidal
Trigonal Planar
Bent
Tetrahedral
3C. CHEMICAL REACTIONS
31. What type of reaction is the following?
2AlCl3 +3H2  6HCl + 2 Al
A.
B.
C.
D.
Double displacement
Decomposition
Combustion
Single displacement
32. What type of reaction is the following?
C3H8 + 5 O2  3 CO2 + 4 H2O
A.
B.
C.
D.
Combustion
Double displacement
Decomposition
Single displacement
33. What are the coefficients of the
following equations?
_______LiN3 (s)  ____N2 (g) + ____Li (s)
A.
B.
C.
D.
1, 1, 2
2, 6, 2
1, 3, 1
2, 3, 2
34. Which of the following metals cannot
replace Lead?
A. Gold
B. Iodine
C. Lithium
D. Both A and B
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35. What are the products of the single
replacement reaction below?
F2 + KBr  _________
A.
B.
C.
D.
Br + KF2
F2 + KBr2
Br2 + KF
KBr + F2
VER A
40. What is the molecular formula of a
compound with the empirical formula O
and molar mass of 48g/mol?
A. 2O
B. 3O
C. O2
D. O3
CONVERSIONS
3D. THE PERIODIC TABLE
36. What is the relationship between
chemical reactions and chemical
equations?
A. A chemical reaction symbolically
represents a chemical equation.
B. Chemical equations and chemical
reactions have no similarities.
C. A chemical equation symbolically
represents a chemical reaction.
D. Chemical equations and chemical
reactions are the same thing.
37. What is the approximate molecular
mass of Ca(OH)2?
A. 72amu
B. 74amu
C. 114amu
D. 43amu
41. Convert 300K to Celsius.
A. 0oC
B. 573oC
C. 27oC
D. 300oC
42. How do you represent 3,040,000 in
scientific notation?
A. 3.04 x 106
B. 3.040000 x 106
C. 3.040000 x 10-6
D. 3.04 x 10-6
43. How many molecules are inside 3 moles
of H2O?
A. 18.06 x 1023
B. 24.08 x 1023
C. 12.04 x 1023
D. 6.02 x 1023
38. What is the percent composition by
mass of aluminum in Al2(SO4)3 (atomic
mass = 342 grams/mole)?
A. 7.89%
B. 20.8%
C. 36.0 %
D. 15.8 %
44. If you have 4 moles of Lithium, then
how many grams do you have?
A. 7g
B. 14g
C. 21g
D. 28g
39. Which of the following molecules is a
molecular formula?
A. CH3COOH
B. Hg
C. P2O5
D. C2H6O
45. If you 320g of Br2 then how many moles
do you have?
A. 1 moles
B. 4 moles
C. 2 moles
D. 3 moles
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4B. IDEAL GAS
VER A
4C. IDEAL GAS EQUATION
46. Real gases act most like ideal gas under
what conditions?
A. High pressure, high temperature
B. High pressure, low temperature
C. Low pressure, high temperature
D. Low pressure, low temperature
51. What is the pressure of 2 moles of gas
in a 100L container at 500K?
A. 10 atm
B. 100 atm
C. 0.82 atm
D. 8.2 atm
47. Jordan made an observation of nitrogen
gas. She found that the gas moved at
had attractive forces and the energy
was conserved in the reactions. What
can he conclude about the gas?
A. The gas is a real gas.
B. We cannot conclude anything about
the gas.
C. The gas is in a supersaturated
state.
D. The gas is an ideal gas.
52. How many moles of air are there in a
.200L Erlenmeyer flask if the pressure is
760 mmHg and the temperature is 40
°C?
A. .008 moles
B. 8 moles
C. .006 moles
D. 6 moles
48. What are the two differences between
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 gasses do not have attractive
forces and have mass.
D. Real gases have attractive forces
and do not have mass.
49. Convert 1500mL to L.
A. 1.5L
B. .15L
C. 150L
D. 15L
50. Convert 1520mmHg to atm.
A. 1mol
B. 3mol
C. 4mol
D. 2mol
53. If I put 5 moles of Oxygen gas into a
balloon at STP, then what will the
volume of the balloon be?
A. 111.9L
B. 0.002L
C. 4.47L
D. 0.41L
54. A bag of chips in a truck travelled from
1atm and moved to a state with a
pressure of 0.5atm. If the volume of
the bag started at 25mL, then what is its
final volume assuming the truck was at
constant temperature and number of
moles remained constant?
A. 50mL
B. 100mL
C. 5mL
D. 10mL

55. A scuba tank changed from 5atm to
10atm as it sunk below the water. If
the scuba diver’s tank started at 350K,
then what is the tank’s new
temperature? (Assume there are
constant moles and volume)
A. 700K
B. 17,500K
C. 70K
D. 175K
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4E. SOLUTIONS
56. What is another term for to solutions
that cannot mix?
A. Miscible
B. Solute
C. Immiscible
D. Solvent
57. Which of the following will NOT
increase the solubility of a substance in
a solution?
A. Increasing the surface area
B. Crushing the solute
C. Heating the solution
D. Cooling the solution
Use the solubility curve chart on your
reference page for the following
question.
58. If I dissolve 100g of NaNO3 in 100g of
H2O at 50oC then what state will the
solution be in?
A. Saturated
B. Supersaturated
C. Unsaturated
D. Equalized
59. A reaction calls for 20mL of a 2.5 M
solution of potassium iodide. You only
have 4M and 1M solutions in your stock
cabinet. Which could you do to make
your solution?
A. Mix 10mL of each of the 4M and
1M solutions
B. Obtain 12.5mL of the 4M solution
and dilute it to 20mL
C. Obtain 12.5mL of the 1M solution
and dilute it to 20mL
D. Add 15mL of 1M solution to 5mL of
4M solution
VER A
Use the equation below to answer the
following questions.
H2(g) + F2(g) ⇌2HF(g)
60. If the reaction is at equilibrium, and I
add more F2(g), 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
61. Like litmus paper, cabbage juice
changes color based on a substance’s
pH. Therefore, both cabbage juice and
litmus paper are what?
A. Detectors
B. Notifies
C. Magic
D. Indicators
62. Acids have a _________ taste, whereas
bases have a __________ taste.
A. bitter, sour
B. sour, sour
C. bitter, bitter
D. sour, bitter
63. If the pH of a substance is 4, then what
is the pOH?
A. 16
B. 12
C. 10
D. 0
64. The pH of a solution was once 2 but
now is 100 times more basic. What is
its new pH?
A. 4
B. 0
C. 200
D. 6
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65. The pH of a solution changed from 7 to
6. 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
5B. BRØNSTED-LOWRY AND
ARRHENIUS ACID/BASE REACTIONS
66. In the following reaction what does the
role of water play?
H2O + NH3  NH4+ + OHA.
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
67. Which substance is an Arrhenius base in
the following reaction?
HCl + LiOH  H2O + LiCl
A.
B.
C.
D.
LiOH
H2O
LiCl
HCl
68. 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
69. Which volume of 10 M KOH(aq) exactly
neutralizes 200 milliliters of 5 M HNO3
(aq)?
A. 10mL
B. 100mL
C. 10000mL
D. 0.25mL
VER A
Information related to a titration
experiment is given in the balanced
equation and table below.
H2SO4+ NaOH  H2O + NaF
Titration Experiment Results
Volume of H2SO4 (aq) used
5.0 mL
Concentration of H2SO4(aq)
?
Volume of NaOH (aq) used
Concentration of NaOH (aq)
10 mL
2.5 M
70. Based on the equation and the titration
results, what is the concentration of the
H2SO4(aq)?
A. 5M
B. 1 M
C. 4 M
D. 3 M