Download 47 Which process best demonstrates a chemical change in distilled

47
Which process best demonstrates a chemical change in distilled
water?
A
B
C
D
Freezing the water
Separating the water into its elements
Calculating the water’s density
Dissolving sugar in the water
47
Which process best demonstrates a chemical change in distilled
water?
A
B
C
D
Freezing the water
Separating the water into its elements
Calculating the water’s density
Dissolving sugar in the water
48
Which of these describes a chemical change?
F
G
H
J
Frost disappears from a window in the morning.
A decrease in temperature reduces the volume of a gas.
Soot is formed as a candle burns.
A cup of hot tea cools down.
48
Which of these describes a chemical change?
F
G
H
J
Frost disappears from a window in the morning.
A decrease in temperature reduces the volume of a gas.
Soot is formed as a candle burns.
A cup of hot tea cools down.
49 In photography, which of these is an example of a chemical change?
F
G
H
J
Light being refracted by a camera lens
Adjusting a lens to focus light
Halide granules being activated by light
Allowing a certain wavelength of light into the camera
49 In photography, which of these is an example of a chemical change?
F
G
H
J
Light being refracted by a camera lens
Adjusting a lens to focus light
Halide granules being activated by light
Allowing a certain wavelength of light into the camera
50
A sugar cube in a test tube is heated over a Bunsen burner. The
sugar cube turns black and has less mass than before it was
heated. These changes occur because the sugar has —
A
B
C
D
melted
boiled
reacted chemically
become hydrated
50
A sugar cube in a test tube is heated over a Bunsen burner. The
sugar cube turns black and has less mass than before it was
heated. These changes occur because the sugar has —
A
B
C
D
melted
boiled
reacted chemically
become hydrated
51
When a 1-kilogram log was burned, 0.05 kilogram of ash was
produced. The mass of the ash is less than the mass of the log
because —
A
B
C
D
wind carried away some matter before it burned
some matter was converted to gases that were released
combustion changed some matter into energy
some matter was decomposed by organisms in the soil
51
When a 1-kilogram log was burned, 0.05 kilogram of ash was
produced. The mass of the ash is less than the mass of the log
because —
A
B
C
D
wind carried away some matter before it burned
some matter was converted to gases that were released
combustion changed some matter into energy
some matter was decomposed by organisms in the soil
K + H2O → KOH + H2
52
What is the coefficient for H2O when the above equation is
balanced?
A
B
C
D
1
2
3
4
K + H2O → KOH + H2
52
What is the coefficient for H2O when the above equation is
balanced?
A
B
C
D
1
2
3
4
53
According to the law of conservation of mass, how much zinc was
present in the zinc carbonate?
A
B
C
D
40 g
88 g
104 g
256 g
53
According to the law of conservation of mass, how much zinc was
present in the zinc carbonate?
A
B
C
D
40 g
88 g
104 g
256 g
54
The chemical equation shows CaCO3 being heated. Which of these
statements best describes the mass of the products if 100 g of
CaCO3 is heated?
A
B
C
D
The difference in the products’ masses is equal to the mass of
the CaCO3.
The sum of the products’ masses is less than the mass of the
CaCO3.
The mass of each product is equal to the mass of the CaCO3.
The sum of the products’ masses equals the mass of the
CaCO3.
54
The chemical equation shows CaCO3 being heated. Which of these
statements best describes the mass of the products if 100 g of
CaCO3 is heated?
A
B
C
D
The difference in the products’ masses is equal to the mass of
the CaCO3.
The sum of the products’ masses is less than the mass of the
CaCO3.
The mass of each product is equal to the mass of the CaCO3.
The sum of the products’ masses equals the mass of the
CaCO3.
55
Which chemical equation supports the law of conservation of
mass?
F
2H2O(l) → H2(g) + O2(g)
G
Zn(s) + HCl(aq) → ZnCl2(aq) + H2(g)
H
Al4C3(s) + H2O(l) → CH4(g) + Al(OH)3(s)
J
CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
55
Which chemical equation supports the law of conservation of
mass?
F
2H2O(l) → H2(g) + O2(g)
G
Zn(s) + HCl(aq) → ZnCl2(aq) + H2(g)
H
Al4C3(s) + H2O(l) → CH4(g) + Al(OH)3(s)
J
CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
2Cu + O2 → 2CuO
56
When 127 g of copper reacts with 32 g of oxygen gas to form
copper (II) oxide, no copper or oxygen is left over. How much
copper (II) oxide is produced?
F 32 g
G 95 g
H 127 g
J 159 g
2Cu + O2 → 2CuO
56
When 127 g of copper reacts with 32 g of oxygen gas to form
copper (II) oxide, no copper or oxygen is left over. How much
copper (II) oxide is produced?
F 32 g
G 95 g
H 127 g
J 159 g
Mg + HCl → MgCl2 + H2
57
When the above equation is balanced, the coefficient for
magnesium chloride is —
A
B
C
D
0
1
2
4
Mg + HCl → MgCl2 + H2
57
When the above equation is balanced, the coefficient for
magnesium chloride is —
A
B
C
D
0
1
2
4
58
If all the reactants in a chemical reaction are completely used,
which of the following statements accurately describes the
relationship between the reactants and the products?
F
The products must have a different physical state than the
reactants.
G The total mass of the reactants must equal the total mass of
the products.
H The reactants must contain more complex molecules than the
products do.
J The density of the reactants must equal the density of the
products.
58
If all the reactants in a chemical reaction are completely used,
which of the following statements accurately describes the
relationship between the reactants and the products?
F
The products must have a different physical state than the
reactants.
G The total mass of the reactants must equal the total mass of
the products.
H The reactants must contain more complex molecules than the
products do.
J The density of the reactants must equal the density of the
products.
2C2H2(g) + 5O2(g) → 4CO2(g) + ___
59
Which additional product balances this reaction?
F
G
H
J
4OH(aq)
CH4(g)
H2O2(g)
2H2O(g)
2C2H2(g) + 5O2(g) → 4CO2(g) + ___
59
Which additional product balances this reaction?
F
G
H
J
4OH(aq)
CH4(g)
H2O2(g)
2H2O(g)
60
The mass of a rusty bicycle is found to be slightly greater than the
mass of the same bicycle before it rusted. The change in mass
indicates that the rusting process —
A
B
C
D
is a physical change
involves an energy-to-matter conversion
decreases the density of the metal
involves metal bonding with other atoms
60
The mass of a rusty bicycle is found to be slightly greater than the
mass of the same bicycle before it rusted. The change in mass
indicates that the rusting process —
A
B
C
D
is a physical change
involves an energy-to-matter conversion
decreases the density of the metal
involves metal bonding with other atoms
61
Aluminum metal and oxygen gas combine to produce aluminum
oxide (Al2O3). Which of these is the balanced equation for this
reaction?
F
G
H
J
Al + O2 → Al2O3
2Al + 2O2 → 2Al2O3
2Al + 3O2 → 5Al2O3
4Al + 3O2 → 2Al2O3
61
Aluminum metal and oxygen gas combine to produce aluminum
oxide (Al2O3). Which of these is the balanced equation for this
reaction?
F
G
H
J
Al + O2 → Al2O3
2Al + 2O2 → 2Al2O3
2Al + 3O2 → 5Al2O3
4Al + 3O2 → 2Al2O3
Reaction of
Copper with Sulfur
62
Mass of Cu before reaction:
3.17 g
Mass of S before reaction:
2.93 g
Mass of CuS formed:
4.78 g
Mass of unreacted S:
?G
Copper (Cu) and sulfur (S) were heated in a covered container. After
the reaction was complete, the unreacted sulfur was removed. The
table contains the results of the investigation. How much sulfur, in
grams, failed to react with the copper? Record and bubble in your
answer to the nearest hundredth on the answer document.
Reaction of
Copper with Sulfur
62
Mass of Cu before reaction:
3.17 g
Mass of S before reaction:
2.93 g
Mass of CuS formed:
4.78 g
Mass of unreacted S:
?G
Copper (Cu) and sulfur (S) were heated in a covered container. After
the reaction was complete, the unreacted sulfur was removed. The
table contains the results of the investigation. How much sulfur, in
grams, failed to react with the copper? Record and bubble in your
answer to the nearest hundredth on the answer document.
1.32
63
Which set of coefficients balances the equation?
F
G
H
J
3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6
63
Which set of coefficients balances the equation?
F
G
H
J
3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6
64
Which of these would support the idea that mass is conserved in a
reaction that produces a gas as a product?
A
B
C
D
Heating the reactants to ensure the reaction occurs in a
gaseous state
Subtracting the mass of the gas from the mass of the solid and
liquid products
Mixing the reactants and measuring their total mass
Trapping the gas and measuring its mass
64
Which of these would support the idea that mass is conserved in a
reaction that produces a gas as a product?
A
B
C
D
Heating the reactants to ensure the reaction occurs in a
gaseous state
Subtracting the mass of the gas from the mass of the solid and
liquid products
Mixing the reactants and measuring their total mass
Trapping the gas and measuring its mass
65
When 50 mL of isopropyl alcohol (39.5 g) is added to 50 mL of water
(50 g), the mixture will have a volume of 98 mL. What is the mass
in grams of this mixture? Record and bubble in your answer to the
nearest tenth on the answer document.
65
When 50 mL of isopropyl alcohol (39.5 g) is added to 50 mL of water
(50 g), the mixture will have a volume of 98 mL. What is the mass
in grams of this mixture? Record and bubble in your answer to the
nearest tenth on the answer document.
89.5
66
Liquid 1 and Liquid 2 react to produce a solid and a gas. Which of
the following expressions correctly shows how to determine the
mass of the gas?
F
G
H
J
(mass of Liquid 1 + mass of Liquid 2) − (mass of solid)
(mass of Liquid 1 + mass of Liquid 2) + (mass of solid)
(mass of Liquid 1 × mass of Liquid 2) ÷ (mass of solid)
(mass of Liquid 1 − mass of Liquid 2) ÷ (mass of solid)
66
Liquid 1 and Liquid 2 react to produce a solid and a gas. Which of
the following expressions correctly shows how to determine the
mass of the gas?
F
G
H
J
(mass of Liquid 1 + mass of Liquid 2) − (mass of solid)
(mass of Liquid 1 + mass of Liquid 2) + (mass of solid)
(mass of Liquid 1 × mass of Liquid 2) ÷ (mass of solid)
(mass of Liquid 1 − mass of Liquid 2) ÷ (mass of solid)
67
If the properties of water were to change so that the solid form
was denser than the liquid form, organisms living in a cold pond
environment would be less likely to survive because water would
no longer —
F dissolve enough oxygen from the air
G produce solutions containing vital nutrients
H remain neutral, instead becoming highly acidic
J produce a floating insulating layer of ice
67
If the properties of water were to change so that the solid form
was denser than the liquid form, organisms living in a cold pond
environment would be less likely to survive because water would
no longer —
F dissolve enough oxygen from the air
G produce solutions containing vital nutrients
H remain neutral, instead becoming highly acidic
J produce a floating insulating layer of ice
68
Fish survive through severe winters because of the property of
water that allows water to —
F
form chemical bonds as it freezes, raising the water
temperature below the ice
G increase in density while it freezes, dissolving more oxygen
from the air
H expand when it freezes, creating a floating and insulating
layer of ice
J precipitate vital nutrients when it freezes, increasing the food
supply
68
Fish survive through severe winters because of the property of
water that allows water to —
F
form chemical bonds as it freezes, raising the water
temperature below the ice
G increase in density while it freezes, dissolving more oxygen
from the air
H expand when it freezes, creating a floating and insulating
layer of ice
J precipitate vital nutrients when it freezes, increasing the food
supply
69
Which characteristic of water best explains its ability to dissolve a
great variety of materials?
A
B
C
D
Its transparency in light
Its electrical conductivity
Its physical state of matter
Its molecular arrangement
69
Which characteristic of water best explains its ability to dissolve a
great variety of materials?
A
B
C
D
Its transparency in light
Its electrical conductivity
Its physical state of matter
Its molecular arrangement
70
The diagram on the right shows water molecules and ions from an NaCl
crystal. What is the most likely reason that each water molecule is arranged
so that the oxygen part of the molecule faces a sodium ion?
F
G
H
J
The oxygen in a water molecule contains a partial negative charge.
Gravity rotates the oxygen atoms to face the more-massive sodium ions.
Hydrogen atoms create repulsive forces with chloride ions.
Oxygen atoms form covalent bonds with sodium ions.
70
The diagram on the right shows water molecules and ions from an NaCl
crystal. What is the most likely reason that each water molecule is arranged
so that the oxygen part of the molecule faces a sodium ion?
F
G
H
J
The oxygen in a water molecule contains a partial negative charge.
Gravity rotates the oxygen atoms to face the more-massive sodium ions.
Hydrogen atoms create repulsive forces with chloride ions.
Oxygen atoms form covalent bonds with sodium ions.
71
Water acts as a solvent of ionic compounds because —
F
G
H
J
water is liquid over a wide range of temperatures
water molecules are polar
water is found in three states of matter
water takes the shape of its container
71
Water acts as a solvent of ionic compounds because —
F
G
H
J
water is liquid over a wide range of temperatures
water molecules are polar
water is found in three states of matter
water takes the shape of its container
72
Which of these remains the same while water molecules go through
the water cycle?
F
G
H
J
The ratio of oxygen to hydrogen in the molecules
The rate of vibration of the molecules
The kinds of dissolved substances between the molecules
The amount of energy the molecules can absorb
72
Which of these remains the same while water molecules go through
the water cycle?
F
G
H
J
The ratio of oxygen to hydrogen in the molecules
The rate of vibration of the molecules
The kinds of dissolved substances between the molecules
The amount of energy the molecules can absorb
73
The graph shows the concentration of ions found in the water of the
Dead Sea. Which property of water is responsible for the
dissociation of salts that produces the ion concentrations shown in
the graph?
A
B
C
D
Chemical stability
High polarity
Low melting point
High freezing point
73
The graph shows the concentration of ions found in the water of the
Dead Sea. Which property of water is responsible for the
dissociation of salts that produces the ion concentrations shown in
the graph?
A
B
C
D
Chemical stability
High polarity
Low melting point
High freezing point
74
The structure of pure water makes it a good —
F
G
H
J
solvent
catalyst
conductor
nutrient
74
The structure of pure water makes it a good —
F
G
H
J
solvent
catalyst
conductor
nutrient
75
What is the reason that tap water will conduct electricity but pure
water will not?
A
B
C
D
Pure water has nonpolar bonds.
Tap water has dissolved ions.
Pure water has a neutral pH.
Tap water has a lower density.
75
What is the reason that tap water will conduct electricity but pure
water will not?
A
B
C
D
Pure water has nonpolar bonds.
Tap water has dissolved ions.
Pure water has a neutral pH.
Tap water has a lower density.
76
The solute most likely to create a
solution that produces the current
reading shown on the ammeter is —
A
sucrose, C12H22O11
B
ethyl alcohol, C2H5OH
C
oxygen, O2
D
nitric acid, HNO3
76
The solute most likely to create a
solution that produces the current
reading shown on the ammeter is —
A
sucrose, C12H22O11
B
ethyl alcohol, C2H5OH
C
oxygen, O2
D
nitric acid, HNO3
77
Two clear solutions are placed in separate beakers. The first solution
has a pH of 4, and the pH of the second solution is
unknown. If the
two solutions are mixed and the resulting pH is 5, the second solution must
have —
A
B
C
D
fewer suspended solids
a lower temperature
more dissolved salt (NaCl) particles
a higher concentration of OH– ions
77
Two clear solutions are placed in separate beakers. The first solution
has a pH of 4, and the pH of the second solution is
unknown. If the
two solutions are mixed and the resulting pH is 5, the second solution must
have —
A
B
C
D
fewer suspended solids
a lower temperature
more dissolved salt (NaCl) particles
a higher concentration of OH– ions
78
Bathwater normally has electrolytic behaviors even though distilled
water does not. This is because bathwater —
F contains isotopes of hydrogen
G has been heated
H is separated into H+ and OH– ions
J contains dissolved minerals
78
Bathwater normally has electrolytic behaviors even though distilled
water does not. This is because bathwater —
F contains isotopes of hydrogen
G has been heated
H is separated into H+ and OH– ions
J contains dissolved minerals
79
In this apparatus, the seawater is an example of a —
F strong electrolyte
G weak acid
H nonelectrolyte
J strong base
79
In this apparatus, the seawater is an example of a —
F strong electrolyte
G weak acid
H nonelectrolyte
J strong base
80
Dissolving salt in water increases the conductivity of the solution
because the —
F
G
H
J
alt gives the solution a net negative charge
salt ions bond with the available water molecules
solution has an increase in kinetic energy
concentration of ions in the solution increases
80
Dissolving salt in water increases the conductivity of the solution
because the —
F
G
H
J
alt gives the solution a net negative charge
salt ions bond with the available water molecules
solution has an increase in kinetic energy
concentration of ions in the solution increases
81
Which of these statements is supported by these data?
A
B
C
D
More KNO3 will dissolve than KBr at 0°C.
Temperature has little effect on the water solubility of NaCl.
KBr is insoluble in water at low temperatures.
Temperature increases lower the solubility of NaClO3 in water.
81
Which of these statements is supported by these data?
A
B
C
D
More KNO3 will dissolve than KBr at 0°C.
Temperature has little effect on the water solubility of NaCl.
KBr is insoluble in water at low temperatures.
Temperature increases lower the solubility of NaClO3 in water.
82
When deep-sea divers explore the ocean at great depths,
nitrogen becomes 10 to 100 times more soluble in the blood. A
disorder called the bends occurs when nitrogen bubbles out of the
blood because of a rapid —
A
B
C
D
decrease in pressure
increase in salt concentration
decrease in temperature
increase in blood pH
82
When deep-sea divers explore the ocean at great depths,
nitrogen becomes 10 to 100 times more soluble in the blood. A
disorder called the bends occurs when nitrogen bubbles out of the
blood because of a rapid —
A
B
C
D
decrease in pressure
increase in salt concentration
decrease in temperature
increase in blood pH
83
A 0.2 g crystal of gypsum dissolves very slowly in 100 mL of water
while the water is stirred. Which of these would cause the gypsum to
dissolve faster?
F Decreasing the water temperature
G Stopping the stirring
H Lowering the air pressure
J Crushing the crystal
83
A 0.2 g crystal of gypsum dissolves very slowly in 100 mL of water
while the water is stirred. Which of these would cause the gypsum to
dissolve faster?
F Decreasing the water temperature
G Stopping the stirring
H Lowering the air pressure
J Crushing the crystal
84
All of these can affect the rate at which a solid dissolves in water
except —
A
B
C
D
decreasing air pressure
stirring the water
increasing the temperature of the water
using larger crystals of the solid
84
All of these can affect the rate at which a solid dissolves in water
except —
A
B
C
D
decreasing air pressure
stirring the water
increasing the temperature of the water
using larger crystals of the solid
85
Over time an open soft drink will lose carbonation (dissolved CO2).
Which of these allows the CO2 to remain in solution the longest?
A
B
C
D
Reduced air pressure
Exposure to direct sunlight
Increased air currents
Cooler temperatures
85
Over time an open soft drink will lose carbonation (dissolved CO2).
Which of these allows the CO2 to remain in solution the longest?
A
B
C
D
Reduced air pressure
Exposure to direct sunlight
Increased air currents
Cooler temperatures
Conditions in Four
Containers of Water
86
Container
Temperature
(°C)
Pressure
(kPa)
Q
10
204.5
R
20
204.5
S
30
101.3
T
40
101.3
The table shows temperature and pressure in four containers
holding the same amount of water. According to the table, in which
container can the most sodium chloride be dissolved in the water?
A
B
C
D
Q
R
S
T
Conditions in Four
Containers of Water
86
Container
Temperature
(°C)
Pressure
(kPa)
Q
10
204.5
R
20
204.5
S
30
101.3
T
40
101.3
The table shows temperature and pressure in four containers
holding the same amount of water. According to the table, in which
container can the most sodium chloride be dissolved in the water?
A
B
C
D
Q
R
S
T
87
Power plants that discharge warm water into rivers have a negative
effect on aquatic life. This is because the higher water temperature —
A
B
C
D
increases the pressure of the river water
increases the pH value of the river water
decreases sediment solubility in the river water
decreases the dissolved oxygen in the river water
87
Power plants that discharge warm water into rivers have a negative
effect on aquatic life. This is because the higher water temperature —
A
B
C
D
increases the pressure of the river water
increases the pH value of the river water
decreases sediment solubility in the river water
decreases the dissolved oxygen in the river water
88
Nine groups of students dissolved as much potassium chloride as possible in water.
Each group used 100 mL of water heated to a different temperature. Which graph
shows the relationship between solubility and temperature for potassium chloride?
Group
Temperature
(°C)
Solubility
(g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56
F
H
G
J
88
Nine groups of students dissolved as much potassium chloride as possible in water.
Each group used 100 mL of water heated to a different temperature. Which graph
shows the relationship between solubility and temperature for potassium chloride?
Group
Temperature
(°C)
Solubility
(g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56
F
H
G
J
Properties of Some Solutions
Solution
Electrical Conductivity
of Solution
Original Color of
Litmus Paper
Color of Litmus Paper
After Dipping in Solution
Ph
1
Very high
Red
Blue
10.0
2
Low
Blue
Red
6.5
3
Moderate
Red
Red
5.4
4
Very High
Blue
Red
2.0
89
The table shows data from an investigation designed to find a liquid solution
that is both an acid and a strong electrolyte. Based on the data, a solution that
is both an acid and a strong electrolyte is —
A
B
C
D
Solution 1
Solution 2
Solution 3
Solution 4
Properties of Some Solutions
Solution
Electrical Conductivity
of Solution
Original Color of
Litmus Paper
Color of Litmus Paper
After Dipping in Solution
Ph
1
Very high
Red
Blue
10.0
2
Low
Blue
Red
6.5
3
Moderate
Red
Red
5.4
4
Very High
Blue
Red
2.0
89
The table shows data from an investigation designed to find a liquid solution
that is both an acid and a strong electrolyte. Based on the data, a solution that
is both an acid and a strong electrolyte is —
A
B
C
D
Solution 1
Solution 2
Solution 3
Solution 4
MTBE Solubility
90
Temperature
(°C)
Solubility
(grams per liter)
0
83
9.7
51
19.8
42
29.6
31
39.3
25
48.6
19
MTBE is a gasoline additive that has entered some groundwater
supplies. According to the table above, which of the following water
temperatures would allow 79 grams of MTBE to dissolve in 1 liter of
water?
F
G
H
J
0°C
10°C
30°C
40°C
MTBE Solubility
90
Temperature
(°C)
Solubility
(grams per liter)
0
83
9.7
51
19.8
42
29.6
31
39.3
25
48.6
19
MTBE is a gasoline additive that has entered some groundwater
supplies. According to the table above, which of the following water
temperatures would allow 79 grams of MTBE to dissolve in 1 liter of
water?
F
G
H
J
0°C
10°C
30°C
40°C
Objective 4 Answer Key
Question
Correct Answer
Objective
Measured
Student
Expectation
1
C
4
IPC 7A
2004 Info Booklet - 18
2
A
4
IPC 7A
2004 Info Booklet - 27
3
144.30
4
IPC 7A
2003 TAKS – 20
4
D
4
IPC 7A
2003 TAKS – 25
5
C
4
IPC 7A
Apr 2004 TAKS – 27
6
B
4
IPC 7A
Jul 2004 TAKS – 17
7
D
4
IPC 7A
Jul 2004 TAKS – 35
8
B
4
IPC 7A
Apr 2006 TAKS – 1
9
A
4
IPC 7A
Apr 2006 TAKS – 23
10
G
4
IPC 7A
Oct 2005 TAKS – 18
11
B
4
IPC 7A
Oct 2005 TAKS – 43
12
B
4
IPC 7A
Feb 2006 TAKS – 25
13
B
4
IPC 7A
Jul 2006 TAKS – 43
14
J
4
IPC 7A
Jul 2006 TAKS – 48
15
B
4
IPC 7A
Fall 2005 TAKS – 19
16
D
4
IPC 7A
Fall 2005 TAKS – 25
17
D
4
IPC 7D
2002 Info Booklet – 19
18
B
4
IPC 7D
2004 Info Booklet – 16
19
B
4
IPC 7D
2003 TAKS – 3
20
A
4
IPC 7D
2003 TAKS – 23
21
G
4
IPC 7D
Apr 2004 TAKS – 10
22
B
4
IPC 7D
Apr 2004 TAKS – 23
23
H
4
IPC 7D
Apr 2004 TAKS – 38
24
G
4
IPC 7D
Jul 2004 TAKS – 4
25
J
4
IPC 7D
Jul 2004 TAKS – 28
Source - item number
Objective 4 Answer Key
Question
Correct Answer
Objective
Measured
Student
Expectation
26
D
4
IPC 7D
Jul 2004 TAKS – 37
27
D
4
IPC 7D
Apr 2006 TAKS – 9
28
G
4
IPC 7D
Apr 2006 TAKS – 38
29
J
4
IPC 7D
Apr 2006 TAKS – 42
30
B
4
IPC 7D
Apr 2006 TAKS – 53
31
H
4
IPC 7D
Oct 2005 TAKS – 24
32
H
4
IPC 7D
Feb 2006 TAKS – 8
33
A
4
IPC 7D
Feb 2006 TAKS – 21
34
B
4
IPC 7D
Feb 2006 TAKS – 45
35
D
4
IPC 7D
Jul 2006 TAKS – 17
36
D
4
IPC 7D
Jul 2006 TAKS – 31
37
F
4
IPC 7D
Jul 2006 TAKS – 34
38
D
4
IPC 8A
2003 TAKS – 21
39
B
4
IPC 8A
Apr 2004 TAKS – 7
40
D
4
IPC 8A
Jul 2004 TAKS – 13
41
D
4
IPC 8A
Jul 2004 TAKS – 31
42
D
4
IPC 8A
Apr 2006 TAKS – 11
43
H
4
IPC 8A
Oct 2005 TAKS – 12
44
A
4
IPC 8A
Oct 2005 TAKS – 45
45
C
4
IPC 8A
Feb 2006 TAKS – 9
46
F
4
IPC 8A
Feb 2006 TAKS – 14
47
B
4
IPC 8A
Feb 2006 TAKS – 27
48
H
4
IPC 8A
Feb 2006 TAKS – 40
49
H
4
IPC 8A
Jul 2006 TAKS – 14
50
C
4
IPC 8A
Fall 2005 TAKS – 45
Source - item number
Objective 4 Answer Key
Question
Correct Answer
Objective
Measured
Student
Expectation
51
B
4
IPC 8C
2004 Info Booklet – 17
52
B
4
IPC 8C
2003 TAKS – 19
53
C
4
IPC 8C
2003 TAKS – 39
54
D
4
IPC 8C
Apr 2004 TAKS – 29
55
J
4
IPC 8C
Apr 2004 TAKS – 32
56
J
4
IPC 8C
Apr 2004 TAKS – 40
57
B
4
IPC 8C
Jul 2004 TAKS – 25
58
G
4
IPC 8C
Jul 2004 TAKS – 40
59
J
4
IPC 8C
Apr 2006 TAKS – 16
60
D
4
IPC 8C
Oct 2005 TAKS – 33
61
J
4
IPC 8C
Oct 2005 TAKS – 46
62
1.32
4
IPC 8C
Feb 2006 TAKS – 20
63
H
4
IPC 8C
Jul 2006 TAKS – 12
64
D
4
IPC 8C
Jul 2006 TAKS – 27
65
89.5
4
IPC 8C
Fall 2005 TAKS – 20
66
F
4
IPC 8C
Fall 2005 TAKS – 30
67
J
4
IPC 9A
2003 TAKS – 40
68
H
4
IPC 9A
Apr 2004 TAKS – 26
69
D
4
IPC 9A
Apr 2006 TAKS – 25
70
F
4
IPC 9A
Oct 2005 TAKS – 34
71
G
4
IPC 9A
Oct 2005 TAKS – 38
72
F
4
IPC 9A
Oct 2005 TAKS – 40
73
B
4
IPC 9A
Feb 2006 TAKS – 23
74
F
4
IPC 9A
Fall 2005 TAKS – 36
75
B
4
IPC 9B
2002 Info Booklet – 12
Source - item number
Objective 4 Answer Key
Question
Correct Answer
Objective
Measured
Student
Expectation
76
D
4
IPC 9B
2004 Info Booklet – 19
77
D
4
IPC 9B
2003 TAKS – 33
78
J
4
IPC 9B
Apr 2004 TAKS – 24
79
F
4
IPC 9B
Jul 2004 TAKS – 18
80
J
4
IPC 9B
Fall 2005 TAKS – 22
81
B
4
IPC 9D
2002 Info Booklet – 17
82
A
4
IPC 9D
2004 Info Booklet – 20
83
J
4
IPC 9D
2003 TAKS – 10
84
A
4
IPC 9D
2003 TAKS – 17
85
D
4
IPC 9D
Apr 2004 TAKS – 39
86
D
4
IPC 9D
Jul 2004 TAKS – 23
87
D
4
IPC 9D
Apr 2006 TAKS – 21
88
J
4
IPC 9D
Apr 2006 TAKS – 36
89
D
4
IPC 9D
Oct 2005 TAKS – 37
90
F
4
IPC 9D
Feb 2006 TAKS – 50
Source - item number