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Subject: SC, Grade: HS
STAAR April 2013 EoC Chemistry
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Student name:
Author: Texas
District: Texas Released Tests
Printed: Tuesday August 27, 2013
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Test Booklet
STAAR April 2013 EoC Chemistry
SC:HS
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STAAR CHEMISTRY REFERENCE MATERIALS
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STAAR April 2013 EoC Chemistry
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STAAR April 2013 EoC Chemistry
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STAAR April 2013 EoC Chemistry
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STAAR April 2013 EoC Chemistry
SC:HS
1 What is the formula of the ion hydrogen sulfite,
which has a charge of -1?
described below.
Some Properties of a Certain Group of Elements
SO3 -1
2 What is the pH of a substance that has a hydrogen
ion concentration of 1.2 × 10−2 M ?
A
B
C
D
2.08
1.92
1.00
0.080
These elements most likely belong to which
group?
A
B
C
D
Alkali metals
Alkaline earth metals
Halogens
Noble gases
to
3 Which of the following includes an example of a
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chemical property of an element?
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reacts with other elements.
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B Sulfur is not shiny and is not malleable.
C Sodium is a solid at room temperature and
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A Aluminum is a solid at room temperature and
is a poor thermal insulator.
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HSO4 -1
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HSO3 -1
• Soft silvery-white color
• Good conductor of thermal energy
• Good conductor of electricity
• Atoms contain a single valence electron
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SO4 -1
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A
B
C
D
4 Elements in a group of the periodic table are
D Silicon is shiny and is a poor conductor of
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electricity.
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5 The diagram below shows what happens when zinc reacts with hydrochloric acid.
Thermal energy → kinetic energy
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Kinetic energy → potential energy
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Potential energy → chemical energy
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Chemical energy → thermal energy
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A
B
C
D
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Which of these best describes the energy transformation that occurs during this reaction?
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6 The diagram below represents a nuclear reaction.
Nuclear fusion is occurring because many smaller nuclei are being fused.
Nuclear fission is occurring because large amounts of energy are being absorbed.
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Nuclear fusion is occurring because many energetic neutrons are being emitted.
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Nuclear fission is occurring because a nucleus is being split into smaller nuclei.
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A
B
C
D
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Which of the following best describes this reaction?
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nd
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7 A detail from a label on a bottle of a water-softening agent is shown below.
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They consist of barium chloride anhydrous.
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B
C
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Which inference about the contents of the bottle can best be drawn?
They consist of barium chloride dihydrate.
They consist of barium chloride hexahydrate.
They consist of barium chloride heptahydrate.
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STAAR April 2013 EoC Chemistry
SC:HS
8 Heart cells require a certain balance of sodium and
molecular mass
specific heat
polarity
density
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A
B
C
D
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potassium ions to function. The blood, which is
approximately 83% water, carries these two types
of ions to the heart. The property of water that
allows it to carry ions to the heart is its -
9 The equation below represents a chemical reaction
that produces a gas.
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2Na(s) + 2H2 O (l) → 2NaOH (aq ) + H2 (g)
5.09 L
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4.88 L
nd
2.44 L
m
0.109 L
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A
B
C
D
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What is the theoretical yield in liters of H2 gas if
5.00 g of Na are completely reacted and the H2 gas
is collected at STP?
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10 Which of these is the electron-dot diagram for Br2 (l)?
C
B
D
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A
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11 The table below lists some properties of a sample of lauric acid.
Mass
m
Boiling point
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Volume
nd
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Number of moles
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A
B
C
D
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Which of these is an intensive property of this sample?
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Answer:
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12 When the equation below is balanced, what is the coefficient for oxygen?
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13 Which mixture can be separated through filtration
because one of the substances is insoluble in
water?
NaClO3 and Pb(ClO3 )2
Na2 SO4 and SrSO4
NaNO3 andPb(NO3 )2
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NaC2 H3 O2 and Pb(C2 H3 O2 )2
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-
A
B
C
D
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STAAR April 2013 EoC Chemistry
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14 Some students used a variety of procedures to investigate four liquid samples. The students recorded the
following information.
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• When Sample W was cooled, solid particles settled out of the liquid.
• The mass and volume of Sample X were measured, and the density of Sample X was calculated to be 1.6
g/mL.
• Sample Y was heated, and the temperature was recorded. All the liquid boiled away at the same
temperature and left no residue in the container.
• When a dilute acid was added to Sample Z, gas bubbles formed and rapidly rose to the surface of the
liquid.
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Sample W
Sample X
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Sample Y
[Ar] 4 s2 4 d10 4 p2
[Kr] 4 s2 3 d10 4 p2
2
10
2
[Kr] 4 s 4 d 4 p
16 Which of the following correctly matches a
compound with its molecular geometry?
A An endothermic reaction occurred.
B A dehydration reaction occurred.
C The water was originally warmer than the
compound.
D The beaker was contaminated by another
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Water (H2 O): linear
Carbon dioxide (CO2 ): tetrahedral
Ammonia (NH3 ): trigonal planar
Methane (CH4 ): tetrahedral
compound.
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A
B
C
D
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[Ar] 4 s2 3 d10 4 p2
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A
B
C
D
water in a clean beaker. A reaction occurs, and
the water temperature drops rapidly. Which of
the following statements is best supported by this
observation?
m
germanium at ground state?
17 A sample of a compound is added to distilled
to
15 What is the electron configuration for an atom of
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Sample Z
nd
A
B
C
D
-
Based on these observations, which sample was clearly identifiable as a pure substance?
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18 Use the equation below to answer the following question.
BaCl2 ( aq ) + Na2 SO4 ( aq ) → 2NaCl( aq ) + BaSO4 ( s )
31.67%
52.03%
75.99%
85.17%
-
A
B
C
D
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The theoretical yield of BaSO4 is 58.35 g. If 44.34 g of BaSO4 are produced from the reaction shown above,
what is the percent yield of BaSO4 ?
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19 When zinc is exposed to air, zinc oxide is
Zinc is oxidized, and oxygen is reduced.
Zinc is reduced, and oxygen is oxidized.
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Both zinc and oxygen are oxidized.
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Both zinc and oxygen are reduced.
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A
B
C
D
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produced. What happens in this reaction?
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20 The equation below represents a nuclear reaction.
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Answer:
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What is the mass number of the missing particle in this reaction?
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21 The graph below shows a solubility curve for ammonia gas and solubility measurements taken at different
temperatures.
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Solubility of Ammonia (NH3) Gas vs.
Water Temperature
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V → W
Y → Z
nd
X → Y
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W → X
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A
B
C
D
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Between which two points did the ammonia solution change from being unsaturated to saturated?
22 How many molecules are in 0.500 mole of N2 O5 ?
1.20 × 1023 molecules
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A
B
C
D
3.01 × 1023 molecules
6.02 × 1023 molecules
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3.01 × 1024 molecules
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23 The following table lists some properties of copper and sulfur.
• Has a density of 5.6 g/cm3
• Has a metallic luster
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• Does not conduct electricity
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Samples of copper metal and sulfur powder are placed in the same test tube and heated over a Bunsen
burner. The resulting substance has the following properties.
• Is a black brittle crystalline solid
a compound
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a homogeneous mixture
nd
an element
.c
a heterogeneous mixture
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A
B
C
D
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This black substance is classified as -
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24 The diagram below shows a gas with an initial pressure of 3060 mm Hg in a cylinder at a constant
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temperature. The gas expands inside the cylinder and pushes the piston up.
784 mm Hg
1830 mm Hg
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544 mm Hg
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25 Which of these statements is an accurate descrip-
26 Which of the following shows a correct Lewis dot
structure?
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tion of the ionization energies of elements in the
periodic table?
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6212 mm Hg
nd
A
B
C
D
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What is the final pressure of the gas after the expansion?
A The ionization energy of lithium is greater than
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that of potassium.
B The ionization energy of iodine is greater than
that of fluorine.
C The ionization energy of magnesium is greater
than that of sulfur.
A
B
C
D
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than that of neon.
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D The ionization energy of krypton is greater
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27 What is the volume of 2.00 moles of chlorine (Cl2 ) at STP, to the nearest tenth of a liter?
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Anser:
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28 In a famous experiment conducted by Ernest
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Rutherford, positively charged alpha particles were
scattered by a thin gold foil. Which of the
following is a conclusion that resulted from this
experiment?
A The nucleus is negatively charged.
B The atom is a dense solid and is indivisible.
C The mass is conserved when atoms react
chemically.
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mostly empty space.
-
D The nucleus is very small and the atom is
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29 The diagram below shows a battery giving off a current producing bubbles in two test tubes.
Which of the following best shows that the investigation results in a chemical change?
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A Liquid condenses on a cold glass rod when gas from the test tube on the left is released.
B A gas probe indicates that the water in the beaker contains dissolved nitrogen and oxygen.
C A burning wood splint placed above the mouth of the test tube on the right glows brighter when some
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D The temperature of the wire connected to the battery increases.
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gas is released from the test tube.
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30 A material safety data sheet (MSDS) for a chemical is shown below.
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Phosphoric acid
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Trihydrogen phosphite
nd
Phosphorous acid
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Phosphorous hydroxide
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A
B
C
D
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Which of these is the IUPAC name for H3 PO4 ( aq )?
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31 The diagram below shows part of Dmitri Mendeleev’s original periodic table, with symbols of known
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elements and their atomic masses.
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Mendeleev’s arrangement of elements is different than that of the modern periodic table. Based on
Mendeleev’s arrangement, which elements should be placed in the shaded boxes labeled X and Z
respectively?
A Indium (In), because it has a slightly higher atomic mass than aluminum (Al), and tin (Sn), because it
to
has a slightly higher atomic mass than silicon (Si)
B Cadmium (Cd), because it has chemical properties similar to those of zinc (Zn), and mercury (Hg),
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because it has chemical properties similar to those of arsenic (As)
it also has a higher atomic mass than zinc (Zn)
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C Antimony (Sb), because it has a slightly higher atomic mass than zinc (Zn), and bismuth (Bi), because
nd
D Gallium (Ga), because it has chemical properties similar to those of aluminum (Al), and germanium
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(Ge), because it has chemical properties similar to those of silicon (Si)
32 Which particle has the lightest mass?
2
4 He
−1
0 e
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A
B
C
D
H
0
1
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1
1
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33 A 5.0 g sample of aluminum with a specific heat of 0.90 J/(g · ◦ C) was heated from 22.1◦ C to 32.1◦ C. How
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much heat, to the nearest joule, did the aluminum gain?
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Answer:
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34 Chemists can identify the composition of some
1 s2 2 s2 2 d6 3 s2 3 d6 4 s1
1 s2 2 s2 2 p6 3 s2 3 p6 4 s1
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1 s2 2 s2 2 p6 3 s2 3 p6 3 d1
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1 s2 2 s2 2 p6 3 s2 3 p6 4 d1
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A
B
C
D
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unknown salts by conducting a flame test. When
potassium salts are heated in a flame, a purple
color is observed. This is due to the movement
of electrons between energy levels. What is the
electron configuration of a potassium atom at
ground state?
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35 Which product balances the chemical equation below?
3AgNO3 ( aq ) + FeCl3 ( aq ) → 3AgCl( s ) + _____
FeCl( aq )
FeCl2 ( aq )
FeNO3 ( aq )
Fe(NO3 )3 ( aq )
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A
B
C
D
36 Sodium, mercury, argon, and neon are used in
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the production of lamps. There are fewer safety
guidelines regarding the handling of neon and
argon than for mercury and sodium. Which of the
following best describes the elements within the
group of the periodic table that contains neon and
argon gas?
reactive with metals
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A Gaseous at room temperature and highly
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B Solid at room temperature and mildly reactive
unreactive with metals
D Solid at room temperature and mostly unreac-
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tive with strong acids
nd
C Gaseous at room temperature and mostly
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with strong acids
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37 The table below shows the standard enthalpy of formation for each of three substances.
.
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CaCO3 decomposes according to the equation
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178.3 kJ
571.8 kJ
-1029 kJ
-2236 kJ
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A
B
C
D
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What is the enthalpy of reaction?
27.4%
16.7%
39 A form of technetium-99 has a half-life of
Tc → ____ + −1
0 e+ γ
43
94
Te
43
99
Es
44
99
Ru
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5.606 × 1023 atoms
6.464 × 1023 atoms
1.078 × 1026 atoms
1.157 × 1026 atoms
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Mo
A
B
C
D
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A
B
C
D
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Which substance correctly completes the equation
above?
42
99
40 How many atoms are present in 179.0 g of
iridium?
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approximately 6 hours.
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99
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37.7%
nd
44.2%
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B
C
D
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38 What is the percentage by mass of sodium (Na) in a formula unit of sodium hydrogen carbonate (NaHCO3 )?
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41 What volume of 1.0 M sodium phosphate, to the nearest tenth of a liter, must be used to make 4.0 L of 0.80
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M sodium phosphate?
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Answer:
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42 X-ray crystallography is a technique that allows
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scientists to determine the ionic and atomic radii
of elements. Which of these statements correctly
describes a trend in ionic or atomic radii in the
periodic table?
A The ionic radius decreases from top to bottom
in a group.
B The atomic radius increases from left to right
across a period.
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left across a period.
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C The ionic radius remains constant from right to
in a group.
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D The atomic radius increases from top to bottom
43 Which of the following substances is a strong
C12 H22 O11
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S2 Cl2
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C2 H5 OH
nd
NaNO3
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A
B
C
D
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electrolyte when dissolved in water?
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44 Which of the following best explains why doubling the temperature of an ideal gas in a closed vessel
doubles the pressure?
A Increasing the temperature increases the size of the gas molecules, which then can put more pressure on
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the vessel walls.
B Increasing the temperature decreases the volume, causing molecules to strike the vessel walls more
frequently.
C Increasing the temperature causes gas molecules to collide more often and with enough force to displace
electrons.
D Increasing the temperature causes gas molecules to move more rapidly, striking the vessel walls more
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frequently and with greater force.
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magnesium and fluorine?
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45 Which of the following diagrams correctly represents the formation of a compound consisting of
.c
nd
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B
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D
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C
A
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46 Which equation represents a neutralization reaction?
H2 CO3 ( aq ) → CO2 ( g ) + H2 O( l )
H2 SO4 ( aq ) + 2NaOH ( ag ) → Na2 SO4 ( aq ) + 2H2 O( l )
p
2H2 ( g) + O2 ( g ) → 2H2 O( l )
2Al(OH)3 ( s ) → Al2 O3 ( s ) + 3H2 O( l )
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A
B
C
D
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47 A scientist filters a sample of river water. The data from this process are listed below.
It is a mixture because dissolved ions in the water pass through the filter paper.
It is a mixture because solid particles are separated from the river water.
A The wavelength becomes longer, and the
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A Molecules of gases have a finite volume.
B Molecules of gases attract and repel one
another.
C Collisions between gas molecules are inelastic.
D The kinetic energy of gas molecules depends
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energy decreases.
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theory?
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light given off by the star has a measurably lower
frequency. What happens to the wavelength and
energy of the photons of light when the frequency
becomes lower?
49 Which of these is a postulate of kinetic molecular
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48 As a distant star moves away from Earth, the
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It is a pure substance because the river water is composed only of free elements.
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It is a pure substance because solid particles cannot pass through the filter paper.
nd
A
B
C
D
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These data support which of the following descriptions of the sample?
B The wavelength becomes shorter, and the
energy decreases.
on temperature.
C The wavelength becomes longer, and the
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energy increases.
D The wavelength becomes shorter, and the
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energy increases.
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50 The solubility of an unknown substance was tested during an experiment.
KNO3
NaNO3
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KCl
nd
NaCl
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A
B
C
D
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Based on the solubility curve information and the results of the experiment, what is most likely the identity
of this unknown solute?
51 Which of the following best explains why CO2 gas
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is easily compressible but solid CO2 (dry ice) is
incompressible?
A The molecules of CO2 gas are much closer
together than the molecules in dry ice.
B The molecules of solid CO2 are much closer
oride?
A
B
C
D
S10 F2
S3 F9
S2 F10
S2 F8
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together than the molecules of CO2 gas.
52 What is the chemical formula for disulfur decaflu-
C The molecules of CO2 gas are much smaller
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than the molecules of solid CO2 .
D The molecules of CO2 gas attract one another,
while the molecules of the solid CO2 repel one
another.
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