XIX. Chemistry, High School
High School Chemistry Test
The spring 2013 high school Chemistry test was based on learning standards in the Chemistry content
strand of the Massachusetts Science and Technology/Engineering Curriculum Framework (2006). These
learning standards appear on pages 69–73 of the Framework.
The Science and Technology/Engineering Curriculum Framework is available on the Department website
at www.doe.mass.edu/frameworks/current.html.
Chemistry test results are reported under the following four MCAS reporting categories:
■Atomic Structure and Periodicity
■Bonding and Reactions
■Properties of Matter and Thermochemistry
■Solutions, Equilibrium, and Acid-Base Theory
Test Sessions
The high school Chemistry test included two separate test sessions, which were administered on
consecutive days. Each session included multiple-choice and open-response questions.
Reference Materials and Tools
Each student taking the high school Chemistry test was provided with a Chemistry Formula and Constants
Sheet/Periodic Table of the Elements. Copies of both sides of this formula sheet follow the final question
in this chapter.
Each student also had sole access to a calculator with at least four functions and a square-root key.
The use of bilingual word-to-word dictionaries was allowed for current and former English language learner
students only, during both Chemistry test sessions. No other reference tools or materials were allowed.
Cross-Reference Information
The table at the conclusion of this chapter indicates each item’s reporting category and the framework
learning standard it assesses. The correct answers for multiple-choice questions are also displayed in the
table.
343
Chemistry
Session 1
DIRECTIONS
This session contains twenty-one multiple-choice questions and two open-response questions. Mark
your answers to these questions in the spaces provided in your Student Answer Booklet. You may
work out solutions to multiple-choice questions in the test booklet.
ID:281323 A Common EQ
1
●
ID:298325 B Common EQ
2
●
An equation for a chemical reaction is
shown below.
2H 2 (g)
O 2 (g)
H 2 O( l ) 571.6 kJ
Which of the following statements
indicates that this reaction is
exothermic?
A. The surface area of the product
particles decreased.
A. Energy is released.
B. A compound is formed.
B. The collision rate of the reactant
particles increased.
C. The reactants are two different gases.
C. The concentrations of the reactant
particles increased.
D. There are more reactants
than products.
D. The concentrations of the product
particles decreased.
344
MCAS_2013_Gr10_CHEM_RID
A student observed that the rate of
a chemical reaction increased as the
temperature of the system increased.
Which of the following statements best
explains why thermal energy caused an
increase in the reaction rate?
Chemistry
Session 1
ID:281214 D Common EQ
3
●
ID:244829 244829_ASTDAV69.eps [opt_ A Common EQ
5
●
Which of the following statements best
describes the current atomic theory?
A. Electrons move in circular orbits
around the nucleus.
A.
B. Electrons are held in an atom by
their attraction to each other.
B.
238
U
92
234
Th
90
4
He
2
C. Electrons are evenly distributed
throughout a mixture of positive and neutral particles.
C.
24
Na
11
24
Mg
12
0
e
–1
D. 01n
235
U
92
92
Kr
36
141
Ba
56
D. Electrons exist in specific energy
levels and have both wave and
particle characteristics.
ID:273012 D Common EQ
4
●
Which of the following equations shows
a fusion reaction?
Which of the following molecules has a
nonpolar covalent bond?
A. H–Br
B. H–Cl
C. H–F
D. H–H
345
MCAS_2013_Gr10_CHEM_RID
3
H
1
2
H
1
4
He
2
1
n
0
301n
Chemistry
Session 1
ID:287594 A Common EQ
6
●
ID:229548 D Common EQ
7
●
Which of the following statements
describes what happens in a buffer
solution when a strong acid is added?
How many atoms of oxygen (O) are
required to form two molecules of
sulfuric acid (H2SO4)?
A. The H ions from the strong acid
combine with basic ions in the buffer.
A. 2
B. The H ions from the strong acid
combine with acidic ions in the buffer.
C. 6
B. 4
D. 8
C. The OH ions from the strong acid
combine with acidic ions in the buffer.
D. The OH ions from the strong acid
combine with basic ions in the buffer.
346
MCAS_2013_Gr10_CHEM_RID
Chemistry
Session 1
ID:261464 B Common EQ
8
●
Magnesium metal reacts with iron(III) sulfate to produce iron metal and magnesium sulfate, as
shown in the equation below. The molar mass of iron(III) sulfate is 399.9 g/mol.
3 Mg(s)
Fe 2 ( SO4 )3 ( aq )
2 Fe (s)
3MgSO4 ( aq )
How many grams of iron(III) sulfate are needed to completely react 6.0 g of magnesium?
A. 2.0 g
B. 33 g
C. 99 g
D. 300 g
ID:264320 C Common EQ
9
●
X
ID:252675 C Common EQ
10
●
In an experiment, a student mixes two
compounds, X and Y, which react to
give off energy and form compound Z,
as shown in the equilibrium equation
below.
Y
Z
energy
When a sample of a gas is cooled, it
condenses into a liquid. In which of the
following ways do the molecules of the
original gas sample compare with the
molecules of the liquid?
A. The molecules are larger as a gas
than they are as a liquid.
After the reaction reaches equilibrium,
which of the following changes would
shift the equilibrium to the left?
B. The molecules weigh less as a gas
than they do as a liquid.
A. adding more compound X to the equilibrium
C. The molecules move faster as a gas
than they do as a liquid.
B. adding more compound Y to the equilibrium
D. The molecules are closer together as
a gas than they are as a liquid.
C. increasing the temperature of the equilibrium
D. decreasing the temperature of the equilibrium
347
MCAS_2013_Gr10_CHEM_RID
Chemistry
Session 1
Question 11 is an open-response question.
• BE SURE TO ANSWER AND LABEL ALL PARTS OF THE QUESTION.
• Show all your work (diagrams, tables, or computations) in your Student Answer Booklet.
• If you do the work in your head, explain in writing how you did the work.
Write your answer to question 11 in the space provided in your Student Answer Booklet.
ID:273070 273070_notebookpage.eps Common EQ
11
●
A page from a lab notebook is shown below. The page displays data needed to find the
empirical formula of a compound.
Mass of crucible
5.23 g
Mass of crucible and iron powder
7.46 g
x
Mass of iron powder
Mass of sulfur added to crucible
1.28 g
Mass of crucible and contents
after reaction
8.74 g
Mass of iron-sulfur compound
y
a. Calculate the values for x and y. Show your calculations and include units in your answer.
b. Assume all the iron and sulfur reacted to form an iron-sulfur compound. Calculate the
number of moles of sulfur and the number of moles of iron that reacted to form the
compound. Show your calculations and include units in your answer.
c. Determine the empirical formula for the iron-sulfur compound. Show your calculations or
explain your reasoning.
348
MCAS_2013_Gr10_CHEM_RID
Chemistry
Session 1
Mark your answers to multiple-choice questions 12 through 22 in the spaces provided in your Student
Answer Booklet. Do not write your answers in this test booklet, but you may work out solutions to
multiple-choice questions in the test booklet.
ID:244815 C Common EQ
12
●
Which of the following equations shows a chemical change?
A. H2 O ( l )
B. heat
H2 O ( g )
H2 O ( l )
H2 O ( s )
C. H2 O ( l )
Na 2 O(s )
2 Na ( aq )
D. H2 O ( l )
NaCl(s )
Na (aq )
heat
2OH (aq )
Cl (aq )
ID:280897 280897_HI_dot.eps [opt_a0 A Common EQ
13
●
heat
H2 O ( l )
ID:281317 B Common EQ
14
●
Which of the following is a Lewis dot
structure for hydrogen iodide (HI)?
A. H I
Which of the following elements
has both metallic and nonmetallic
properties?
A. Ar
B. Ge
B. H I
C. Mg
D. S
C. H I
D. H I
349
MCAS_2013_Gr10_CHEM_RID
Chemistry
Session 1
ID:258906 C Common EQ
15
●
ID:274049 A Common EQ
Uranium-234 decays to lead-214 through
a series of alpha decays. Which of the
following is the total number of alpha
particles emitted in this decay series?
16
●
The chemical equation below represents
the reaction of 1 mol of hydrogen gas
(H2) with 1 mol of chlorine gas (Cl2) in
a sealed container at STP. The reaction
produces 2 mol of hydrogen chloride gas
(HCl) in the sealed container.
H2 1 Cl2 → 2HCl
What is the pressure in the container at
standard temperature after the reaction is
complete?
A.   1
B.   2
C.   5
D. 10
A. 1 atm
B. 2 atm
C. 3 atm
D. 4 atm
350
MCAS_2013_Gr10_CHEM_RID
Chemistry
Session 1
ID:226997 3160092_AR1.eps [opt_a01, D Common EQ
17
●
Some manufacturers place rubber plugs in the bottoms of pressurized aerosol cans to prevent
structural failure if the cans are exposed to excessive heat. The normal pressure inside an aerosol
can is 2.0 atm at 27°C. When the temperature of the gas in the can is increased to 250°C, the
pressure reaches 3.5 atm and the plug pops out.
Which of the following graphs best shows the relationship of pressure to the temperature inside the can?
A.
C.
3.0
2.0
1.0
0
B.
27
D.
2.0
1.0
1.0
27
250
Temperature (°C)
27
250
Temperature (°C)
3.0
2.0
1.0
0
250
Temperature (°C)
351
MCAS_2013_Gr10_CHEM_RID
2.0
4.0
Pressure (atm)
Pressure (atm)
3.0
27
3.0
0
250
Temperature (°C)
4.0
0
4.0
Pressure (atm)
Pressure (atm)
4.0
Chemistry
Session 1
ID:281282 C Common EQ
18
●
ID:275910 C Common EQ
20
●
A student puts an ice cube into a beaker
and allows it to melt. Which of the
following statements best describes what
happens to the water molecules during
this investigation?
A. The molecules move apart until the
entire beaker is filled.
B. The molecules move apart until they
are no longer touching each other.
C. The molecules become randomly
arranged and can slide past each other.
The table below provides data about a
gas sample.
Volume
1.0 L
Pressure
303.9 kPa
Temperature
323 K
Which of the following can be
determined using the data?
A. the chemical composition of the gas
B. the condensation temperature of the gas
D. The molecules become arranged in a pattern and maintain fixed
positions.
C. the number of gas molecules in the sample
D. the distance between gas molecules
in the sample
ID:229556 3152531_AR1.eps B Common EQ
19
●
The diagram below shows a partial
periodic table.
O F
The electron configuration of oxygen is
1s22s22p4. On the periodic table, fluorine
is one space to the right of oxygen.
Which of the following electron
configurations represents fluorine?
A. 1s22s22p3
B. 1s22s22p5
C. 1s22s22p63s23p3
D. 1s22s22p63s23p5
352
MCAS_2013_Gr10_CHEM_RID
Chemistry
Session 1
ID:298323 A Common EQ
21
●
ID:287275 ASTDAV252_periodictable.e B Common EQ
22
●
What is the name of the compound with
the chemical formula (NH
NH 4)2 S ?
A. ammonium sulfide
B. hydrogen sulfate
The diagram below shows the relative
locations of five unidentified elements in
the periodic table: E, X, G, J, and L.
E
X
G
C. sulfur hydride
D. sulfuric acid
J
L
Element X has an atomic number of z.
Which unidentified element has an
atomic number of z 1 2 ?
A. element E
B. element G
C. element J
D. element L
353
MCAS_2013_Gr10_CHEM_RID
Chemistry
Session 1
Question 23 is an open-response question.
• BE SURE TO ANSWER AND LABEL ALL PARTS OF THE QUESTION.
• Show all your work (diagrams, tables, or computations) in your Student Answer Booklet.
• If you do the work in your head, explain in writing how you did the work.
Write your answer to question 23 in the space provided in your Student Answer Booklet.
ID:272994 BELROB144.eps Common EQ
23
●
Particle models of four different types of matter are shown in the diagram below.
Model 1
Model 2
Model 3
Model 4
a. Identify which of the four models best represents a pure compound. Explain your answer
and give a specific example of a compound.
b. Identify which of the four models best represents a homogeneous mixture. Explain your
answer and give a specific example of a homogeneous mixture.
c. Describe one method that could be used to separate a homogeneous mixture.
354
MCAS_2013_Gr10_CHEM_RID
Chemistry
Session 2
DIRECTIONS
This session contains nineteen multiple-choice questions and three open-response questions. Mark
your answers to these questions in the spaces provided in your Student Answer Booklet. You may
work out solutions to multiple-choice questions in the test booklet.
ID:273221 B Common EQ
24
●
ID:281263 C Common EQ
25
●
A sample of vinegar has a pH of 5, and
a sample of rainwater has a pH of 6.
Which of the following statements best
describes these two substances?
The masses of the reactants and the
theoretical yields of the products for a chemical reaction are shown below.
3Sb
(1.2 g)
A. Both samples are bases, and vinegar is more basic.
B. Both samples are acids, and vinegar is more acidic.
C. Both samples are bases, and
rainwater is more basic.
B. 67%
C. 75%
D. 100%
355
MCAS_2013_Gr10_CHEM_RID
2SbI3
(3.2 g)
Sb
(0.4 g)
When this reaction was performed in the laboratory, the actual yield for SbI3
was 2.4 g. What was the percent yield
for SbI3?
A. 25%
D. Both samples are acids, and
rainwater is more acidic.
3I2
(2.4 g)
Chemistry
Session 2
ID:287272 ASTDAV249.eps B Common EQ
26
●
A student pours hydrochloric acid (HCl)
into an open beaker that contains a
piece of magnesium (Mg). A chemical
reaction occurs, as shown in the
equation below.
2HCl (aq)
ID:260920 A Common EQ
Mg (s)
27
●
HNO3(aq)
H 2(g)
MgCl 2(aq)
The data for the reaction are shown in
the table below.
Mass of Mg
Mass of HCl Solution
0.24 g
5.49 g
Total Mass of Substances in
Beaker before the Reaction
5.73 g
Total Mass of Substances in
Beaker after the Reaction
5.71 g
NH3(aq)
B. NH3
C. NO3
D. NH 4
A. The HCl and Mg react slowly.
B. The hydrogen produced is a gas.
C. The HCl and Mg react to form a
precipitate.
D. The magnesium chloride produced is soluble.
356
NO3 (aq)
NH 4 (aq)
Which chemical in the forward reaction
is a Brønsted-Lowry acid?
A. HNO3
Which of the following statements
best explains why the total mass of
the substances in the beaker before the
reaction is different from the total mass
after the reaction?
MCAS_2013_Gr10_CHEM_RID
The equation below represents an
equilibrium reaction.
Chemistry
Session 2
ID:261188 B Common EQ
ID:261469 B Common EQ
28
●
30
●
A 20.0 mL sample of 0.15 M
hydrochloric acid (HCl) is needed
to neutralize a 10.0 mL sample of
potassium hydroxide (KOH). A balanced
equation for the reaction is shown
below.
HCl
KOH
KCl
H2O
A. The solute melts.
B. The solute dissolves.
C. The solute remains intact.
What is the molarity of the KOH
solution?
D. The solute reacts to form a precipitate.
A. 0.15 M
B. 0.30 M
C. 0.60 M
D. 0.75 M
ID:274067 A Common EQ
29
●
The white pigment in many paints is
titanium dioxide (TiO2). It is made by
burning titanium(IV) chloride. The other
product in this reaction is chlorine gas.
What is the balanced equation for this
reaction?
TiC14
O2
TiO 2
2 C12
B. 2 TiC14
O2
TiO 2
4 C1
A.
C. TiC14
2 O2
2 TiO 2
C12
D. 2 TiC14
2 O2
2 TiO 2
C14
357
MCAS_2013_Gr10_CHEM_RID
An ionic solid is placed in a beaker of
water. Which of the following occurs
when there is a strong attraction between
the solute and the solvent?
Chemistry
Session 2
ID:252651 A Common EQ
31
●
ID:294713 D Common EQ
32
●
Calcium and boron react to form
calcium boride, as represented by the
chemical equation below.
Ca 6B
CaB6
Methane gas (CH 4) reacts with
oxygen gas (O 2) according to the
equation below.
CH 4
Which type of reaction is shown by this equation?
A. combination
B. decomposition
2O 2
CO 2
2H 2O
energy
This reaction releases 890 kJ of energy
for each mole of methane gas that is
consumed. Which of the following
statements best describes this reaction? A. The reaction is endothermic;
CO 2 and H 2O have more chemical
potential energy than CH 4 and O 2.
C. double displacement
D. single displacement
B. The reaction is endothermic;
CO 2 and H 2O have less chemical
potential energy than CH 4 and O 2.
C. The reaction is exothermic;
CO 2 and H 2O have more chemical
potential energy than CH 4 and O 2.
D. The reaction is exothermic;
CO 2 and H 2O have less chemical
potential energy than CH 4 and O 2.
358
MCAS_2013_Gr10_CHEM_RID
Chemistry
Session 2
Question 33 is an open-response question.
• BE SURE TO ANSWER AND LABEL ALL PARTS OF THE QUESTION.
• Show all your work (diagrams, tables, or computations) in your Student Answer Booklet.
• If you do the work in your head, explain in writing how you did the work.
Write your answer to question 33 in the space provided in your Student Answer Booklet.
ID:260794 ASTDAV148.eps Common EQ
33
●
Formaldehyde (CH2O) occurs in smoke from forest fires and in automobile exhaust.
a. Calculate the total number of valence electrons in one molecule of formaldehyde. Show
your calculations.
Carbon is the central atom in a CH2O molecule.
b. Draw a Lewis dot structure for formaldehyde.
c. Identify the shape of the formaldehyde molecule predicted by valence-shell electron-pair
repulsion (VSEPR) theory. Explain your answer.
359
MCAS_2013_Gr10_CHEM_RID
Chemistry
Session 2
Mark your answers to multiple-choice questions 34 through 43 in the spaces provided in your Student
Answer Booklet. Do not write your answers in this test booklet, but you may work out solutions to
multiple-choice questions in the test booklet.
ID:260916 C Common EQ
34
●
ID:252565 C Common EQ
36
●
One mole of which of the following
substances has the greatest entropy?
A. ethanol (l )
A. 1s 22s 22p 4
B. iron (s)
B. 1s 22s 22p 63s 2
C. neon (g)
C. 1s 22s 22p 63s 23p 4
D. water (l )
D. 1s 22s 22p 63s 23p 64s 2
ID:288269 D Common EQ
35
●
Which of the following is the electron
configuration for sulfur?
Which of the following statements
explains why people spread salt on
icy sidewalks in the winter?
A. The salt causes the ice to undergo
sublimation.
B. The salt lowers the surface tension
of melted ice.
C. The ice-salt mixture has a higher
density than ice has.
D. The ice-salt mixture melts at a lower
temperature than ice does.
360
MCAS_2013_Gr10_CHEM_RID
Chemistry
Session 2
ID:281218 281218_decay.eps B Common EQ
37
●
39
●
Uranium-238 undergoes radioactive
decay according to the incomplete
equation below.
238U
92
ID:273186 A Common EQ
4He
2
X
Which of the following identifies the
number and location of protons in a
lithium atom?
A. 3 protons, located in the nucleus
What is the decay product represented
by X?
B. 7 protons, located in the nucleus
A. 232
90 Th
D. 7 protons, located in an atomic orbital
B.
234
90 Th
C.
242
94 Pu
D.
244
94 Pu
C. 3 protons, located in an atomic orbital
ID:294699 D Common EQ
40
●
ID:281919 D Common EQ
38
●
Which of the following statements
applies the law of multiple proportions to
the relationship between carbon monoxide
(CO) and carbon dioxide (CO2)?
A. H 2O is less dense than H 2S.
B. H 2O is less chemically reactive
than H 2S.
C. H 2O has a smaller molecular mass
than H 2S.
A. The mass of a mole of CO is exactly
half that of a mole of CO2.
D. H 2O has stronger intermolecular
forces than H 2S.
B. There will always be half as much
CO as CO2 in a sample of gas.
C. The proportion of oxygen atoms in
CO molecules is the same as it is in
CO2 molecules.
D. The mass of oxygen in CO
compared to that in CO2 can be
expressed as a whole number ratio.
361
MCAS_2013_Gr10_CHEM_RID
Although H 2O and H 2S have similar
molecular geometries, they exist as
different states of matter at 20°C and
1 atm. Which of the following
statements best explains why H 2O is
a liquid and H 2S is a gas under these
conditions?
Chemistry
Session 2
ID:216954 C Common EQ
41
●
ID:264326 B Common EQ
43
●
Based on valence electron
configurations, which of the following is a formula for a compound formed
from sodium (Na) and oxygen (O)?
A. aluminum (s)
B. helium (g)
A. NaO
C. mercury (l )
B. NaO2
D. sodium (s)
C. Na2O
D. Na2O3
ID:287563 D Common EQ
42
●
Which of the following statements
describes a difference between a
chemical change and a physical change
in a substance?
A. A physical change occurs only in
elements; a chemical change occurs
only in compounds.
B. A chemical change occurs only in
elements; a physical change occurs
only in compounds.
C. The result of a physical change is a different composition; in a
chemical change, the composition
remains the same.
D. The result of a chemical change is a different composition; in a physical change, the composition
remains the same.
362
MCAS_2013_Gr10_CHEM_RID
Particles of which of the following
substances are farthest apart at STP?
Chemistry
Session 2
Questions 44 and 45 are open-response questions.
• BE SURE TO ANSWER AND LABEL ALL PARTS OF EACH QUESTION.
• Show all your work (diagrams, tables, or computations) in your Student Answer Booklet.
• If you do the work in your head, explain in writing how you did the work.
Write your answer to question 44 in the space provided in your Student Answer Booklet.
ID:274045 Common EQ
44
●
Since elements are listed in the periodic table in order of increasing atomic number and
arranged so that elements with similar properties fall into the same group, the periodic table
can be used to predict similarities and differences between elements.
a. Bromine and fluorine are both in group 17 (7A) of the periodic table. Describe two
properties of bromine and fluorine that are the same.
b. Bromine and fluorine are in different periods in the periodic table. Describe two properties
of bromine and fluorine that are different.
c. Based on their positions in the periodic table, bromine and fluorine are most likely to form
ionic compounds with an element from which group: group 1 (1A), group 14 (4A), or
group 18 (8A)? Explain your choice.
363
MCAS_2013_Gr10_CHEM_RID
Chemistry
Session 2
Write your answer to question 45 in the space provided in your Student Answer Booklet.
ID:294716 Common EQ
45
●
A student follows the procedure below to determine how two variables will affect the
dissolution rate of sugar in water.
1. Place a 2.0 g sugar cube into 150 mL of 10°C water.
2. Place an identical 2.0 g sugar cube into 150 mL of 50°C water.
3. Place 2.0 g of granulated sugar into 150 mL of 50°C water.
4. Stir the three sugar-water mixtures equally.
5. Measure the time it takes for all of the sugar in each mixture to dissolve.
a. Identify the two variables being tested in the procedure.
b. Describe the most likely effect each variable in part (a) has on the rate at which the sugar
dissolves in water. Explain your reasoning.
c. Write a procedure to test the effect solvent volume has on the rate at which sugar dissolves
in water.
d. Describe the expected results for the procedure you wrote in part (c). Explain your
reasoning.
364
MCAS_2013_Gr10_CHEM_RID
Massachusetts Comprehensive Assessment System
Chemistry Formula and Constants Sheet
Common Polyatomic Ions
Ion
Ionic Formula
Ammonium
NH41
Carbonate
CO32-
Hydroxide
OH-
Nitrate
NO3-
Phosphate
PO43-
Sulfate
SO42P1 V1
PV
5 2 2
T1
T2
Combined Gas Law:
Ideal Gas Law: PV 5 nRT
Dilution Formula: M1V15M2V2
Molar Volume of Ideal Gas at STP: 22.4L/mol
Ideal Gas Constant: R 50.0821L• atm/mol• K 58.31L• kPa/mol• K
STP: 1atm(101.3kPa),273K(0°C)
Absolute Temperature Conversion: K 5°C1 273
Definition of pH: pH52log[H3O1]52log[H1]
Avogadro’s Number: 6.0231023particles/mol
Nuclear Symbols
Name
Symbol
Alpha particle
or 42 He
Beta particle
bor−01 e
Gamma ray

Neutron
1
0n
365
MCAS_2013_Gr10_CHEM_RID
MCAS_2013_Gr10_CHEM_RID
366
Period
Mg
Ca
40.08
Sc
44.96
3B
3
Ti
47.88
4B
4
V
50.94
5B
5
atomic weight
Symbol
atomic number
Name
Cr
52.00
6B
6
Mn
54.94
7B
7
Sr
87.62
Ra
Zr
91.22
Nb
92.91
Actinide Series
Ta
180.95
Ru
101.07
Os
190.23
Molybdenum
183.85
186.21
Re
44
W
Sg
(271)
89
Actinium
Ac
Pd
106.42
28
Nickel
Ni
58.69
10
Hs
(277)
Mt
(276)
U
238.03
Np
(237)
61
Pm
(145)
P
S
Br
79.90
17
Chlorine
Cl
81
Thallium
Tl
204.38
49
Indium
In
82
Lead
Pb
207.2
50
Tin
Sn
118.71
Te
Po
(209)
At
(210)
53
Iodine
I
126.91
83
84
85
Bismuth Polonium Astatine
Bi
208.98
51
52
Antimony Tellurium
Sb
121.75
127.60
Se
78.96
16
Sulfur
35.45
9
Fluorine
F
19.00
7A
17
114.82
As
74.92
Phosphorus
15
32.06
8
Oxygen
O
16.00
6A
16
34
35
Selenium Bromine
Ge
72.59
14
Silicon
Si
30.97
7
Nitrogen
N
14.01
5A
15
31
33
32
Gallium Germanium Arsenic
Ga
69.72
13
Aluminum
Al
Pu
(244)
62
Sm
150.36
Eu
151.96
Gd
157.25
Tb
158.93
Dy
162.50
Ho
164.93
Am
(243)
96
Curium
Cm
(247)
98
Cf
(251)
99
Es
(252)
Fm
(257)
68
Erbium
Er
167.26
100
Berkelium Californium Einsteinium Fermium
97
Bk
(247)
65
63
67
64
66
Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium
60
Nd
144.24
80
Mercury
Hg
200.59
48
Cadmium
Cd
112.41
30
Zinc
Zn
65.39
2B
12
28.09
6
Carbon
5
Boron
26.98
C
12.01
4A
14
B
10.81
3A
13
86
Radon
Rn
(222)
54
Xenon
Xe
131.29
36
Krypton
Kr
83.80
18
Argon
Ar
39.95
10
Neon
Ne
20.18
2
Helium
He
4.00
8A
18
Yb
173.04
Lu
174.97
Mendelevium
101
Md
(258)
Lr
(262)
102
103
Nobelium Lawrencium
No
(259)
69
70
71
Thulium Ytterbium Lutetium
Tm
168.93
Mass numbers in parentheses are those of the most stable or most common isotope.
111
Roentgenium
Darmstadtium
Rg
(280)
79
Gold
Au
196.97
47
Silver
Ag
107.87
29
Copper
Cu
63.55
1B
11
110
Ds
(281)
78
Platinum
Pt
195.08
92
94
90
93
91
95
Thorium Protactinium Uranium Neptunium Plutonium Americium
Th
Pa
231.04
232.04
59
Pr
140.91
Praseodymium
Ce
140.12
(227)
57
Bh
(272)
77
Iridium
Ir
192.22
105
107
108
109
106
Dubnium Seaborgium Bohrium Hassium Meitnerium
Db
(268)
58
Lanthanum Cerium
La
138.91
Rutherfordium
104
Rf
(267)
Rh
102.91
27
Cobalt
Co
58.93
9
8B
45
46
Technetium Ruthenium Rhodium Palladium
Tc
(98)
43
42
Mo
95.94
26
Iron
Fe
55.85
8
72
73
74
75
76
Hafnium Tantalum Tungsten Rhenium Osmium
Hf
178.49
39
40
41
Yttrium Zirconium Niobium
Y
88.91
Lanthanide Series
87
88
Francium Radium
Fr
(226)
56
Barium
55
Cesium
(223)
Ba
137.33
Cs
132.91
37
38
Rubidium Strontium
Rb
85.47
19
20
21
22
23
24
25
Potassium Calcium Scandium Titanium Vanadium Chromium Manganese
K
39.10
11
12
Sodium Magnesium
Na
24.31
4
Beryllium
3
Lithium
22.99
Be
9.01
2A
2
Li
6.94
1
1
Hydrogen
H
Key:
Periodic Table of the Elements
*Revised based on IUPAC Commission on Atomic Weights and Isotopic Abundances, “Atomic Weights of the Elements 2007.”
7
6
5
4
3
2
1
1.01
Group (Family)
1A
1
Massachusetts Comprehensive Assessment System
High School Chemistry
Spring 2013 Released Items:
Reporting Categories, Standards, and Correct Answers*
Standard
Correct Answer
(MC)*
Properties of Matter and Thermochemistry
6.4
A
344
Solutions, Equilibrium, and Acid-Base Theory
7.5
B
3
345
Atomic Structure and Periodicity
2.1
D
4
345
Bonding and Reactions
4.3
D
5
345
Atomic Structure and Periodicity
2.7
A
6
346
Solutions, Equilibrium, and Acid-Base Theory
8.3
A
7
346
Bonding and Reactions
5.3
D
8
347
Bonding and Reactions
5.5
B
9
347
Solutions, Equilibrium, and Acid-Base Theory
7.6
C
10
347
Properties of Matter and Thermochemistry
6.3
C
11
348
Bonding and Reactions
5.4
12
349
Properties of Matter and Thermochemistry
1.1
C
13
349
Bonding and Reactions
4.2
A
14
349
Atomic Structure and Periodicity
3.2
B
15
350
Atomic Structure and Periodicity
2.5
C
16
350
Properties of Matter and Thermochemistry
6.2
A
17
351
Properties of Matter and Thermochemistry
6.1
D
18
352
Properties of Matter and Thermochemistry
1.3
C
19
352
Atomic Structure and Periodicity
3.3
B
20
352
Properties of Matter and Thermochemistry
6.2
C
21
353
Bonding and Reactions
4.6
A
22
353
Atomic Structure and Periodicity
3.1
B
23
354
Properties of Matter and Thermochemistry
1.2
24
355
Solutions, Equilibrium, and Acid-Base Theory
8.2
B
25
355
Bonding and Reactions
5.6
C
26
356
Atomic Structure and Periodicity
2.3
B
27
356
Solutions, Equilibrium, and Acid-Base Theory
8.1
A
28
357
Solutions, Equilibrium, and Acid-Base Theory
7.2
B
29
357
Bonding and Reactions
5.1
A
30
357
Solutions, Equilibrium, and Acid-Base Theory
7.1
B
31
358
Bonding and Reactions
5.2
A
32
358
Properties of Matter and Thermochemistry
6.4
D
33
359
Bonding and Reactions
4.4
34
360
Properties of Matter and Thermochemistry
6.5
C
35
360
Solutions, Equilibrium, and Acid-Base Theory
7.4
D
36
360
Atomic Structure and Periodicity
2.4
C
37
361
Atomic Structure and Periodicity
2.6
B
38
361
Atomic Structure and Periodicity
2.3
D
39
361
Atomic Structure and Periodicity
2.2
A
40
361
Bonding and Reactions
4.5
D
Item No.
Page No.
1
344
2
Reporting Category
367
MCAS_2013_Gr10_CHEM_RID
Reporting Category
Standard
Correct Answer
(MC)*
Item No.
Page No.
41
362
Bonding and Reactions
4.1
C
42
362
Properties of Matter and Thermochemistry
1.1
D
43
362
Properties of Matter and Thermochemistry
1.3
B
44
363
Atomic Structure and Periodicity
3.4
45
364
Solutions, Equilibrium, and Acid-Base Theory
7.3
* Answers are provided here for multiple-choice items only. Sample responses and scoring guidelines for open-response items,
which are indicated by shaded cells, will be posted to the Department’s website later this year.
368
MCAS_2013_Gr10_CHEM_RID