Grade 11

Objective 4

1 What is the density of this magnetic steel alloy?

A 2.67 g/mLB 3.99 g/mLC 6.90 g/mLD 8.01 g/mL

2 Dr. Julian’s foam was most successful in extinguishing oil fires. What are the most likely physical characteristics of this foam?

A Less dense than oil and does not allow oxygen inB Waterproof and contains flammable materialsC More viscous than water and lighter than airD Brightly colored and more porous than plastic

3 A sample of an element has a volume of 78.0 mL and a density of 1.85 g/mL. What is the mass in grams of the sample? Record andbubble in your answer to the nearest tenth on the answer

document.

4 A block of maple wood with a volume of 405 cubic centimeters and a density of 0.67 g/cm3 is sawed in half. The density of the two smaller blocks is now —

A one-fourth the original densityB one-half the original densityC two times the original densityD the same as the original density

5 This pipette is filled with a 20% NaOH solution. The solution is at 20°C and has a density of 1.23 g/mL. According to this information, what is the mass of this NaOH solution?

A 3.88 gB 15.7 gC 23.9 gD 24.6 g

6 Swimmers find that they can float more easily in the ocean than in a freshwater pond. The most likely reason for this phenomenon is that the —

A viscosity of pond water is greater than that of ocean waterB density of ocean water is higher than that of pond waterC temperature of pond water is lower than that of ocean waterD mass of ocean water is greater than that of pond water

7 Compared to 250 g of gaseous nitrogen, 250 g of liquid nitrogen has greater —

A volumeB temperatureC massD density

8 The picture shows the results of pouring a blue liquid into a clear liquid and allowing the mixture to settle for 25 minutes. Compared to the clear liquid, the blue liquid is more —

A massiveB denseC viscousD soluble

9 The table shows properties of four liquids that are insoluble in water. If the four liquids are poured into an Erlenmeyer flask containing water, which liquid will form a layer below the water?

A QB RC SD T

Liquid DescriptionDensity(g/mL)

Boiling Point(°C)

Q Nonflammable colorless compound 1.62 59.5

R Flammable colorless compound 0.71 34.6

S Yellow mixture with strong odor 0.73 160.4

T Viscous pale-yellow oil 0.93 300.0

10 A 500 mL quantity of vanilla ice cream has a mass of 400 grams. The manufacturer then bubbles air into the ice cream so that itsvolume increases by 300 mL. What is the ice cream’s approximate final density?

F 0.30 g/cm3

G 0.50 g/cm3

H 0.80 g/cm3

J 1.30 g/cm

11 A bar of soap produced by this soap-making process normally sinks to the bottom of a container of water. Which of these processescould cause the bar of soap to float in water?

A Making grooves in the surface of the thick pasteB Adding air bubbles to the thick pasteC Letting the thick paste sit for four daysD Chilling the mold filled with the thick paste

12 As the viscosity of a liquid increases, the liquid —

A conducts electricityB pours more slowlyC evaporates more quicklyD forms a precipitate

13 Water normally boils at 100°C at sea level and at 97°C on a North American mountaintop. This difference in boiling points can be explained by the difference between the locations’—

A ultraviolet lightB air pressureC gravitational forceD thermal energy

14 The buoyant force that a fluid exerts on objects is increased when there is an increase in the fluid’s —

F acidityG clarityH solubilityJ density

15 The observation that an air bubble in water rises to the surface is explained by the principle of —

A viscosityB buoyancyC interferenceD polarity

16 Brown sugar consists of crystals of white sugar coated with molasses. If brown sugar hardens, it can be softened by heating. The most likely reason brown sugar softens when heated is that heat —

A increases the moisture of sugarB decreases the volume of molassesC increases the density of sugarD decreases the viscosity of molasses

17

A heat decomposes the compoundB the elements are volatileC pressure increasesD their ionic bond is broken

18 The correct formula for calcium chloride is —

A CaCl

B CaCl2 C Ca2Cl

D Ca2Cl3

19 Which of the following groups contains members with similar chemical reactivity?

A Li, Be, CB Be, Mg, SrC Sc, Y, ZrD C, N, O

20 According to the periodic table, which element most readily accepts electrons?

A FluorineB NitrogenC ArsenicD Aluminum

21 Elements in Group 16 of the periodic table usually —

F form large moleculesG gain electrons when bondingH act like metalsJ solidify at room temperature

Al3+ SO42–

22 According to this information, what is the chemical formula for aluminum sulfate?

A AlSO4

B Al2(SO4)3

C Al3(SO4)2

D Al6SO4

Calcium (Ca2+) + Chloride (Cl–) → Calcium chloride

23 The chemical formula for calcium chloride is —

F Ca2Cl

G CaCl

H CaCl2 J Ca2Cl3

24 An unidentified element has many of the same physical and chemical properties as magnesium and strontium but has a lower atomic mass than either of these elements. What is the most likely identity of this element?

F SodiumG BerylliumH CalciumJ Rubidium

25 The elements from which of the following groups are most likely to react with potassium (K)?

F Group 2G Group 7H Group 13J Group 17

26 The elements of which of these groups on the periodic table are most resistant to forming compounds?

A Group 1B Group 9C Group 14D Group 18

27 The bonding characteristics of oxygen are most similar to the bonding characteristics of —

A hydrogenB siliconC heliumD sulfur

28 Which of these elements is most likely to donate one electron?

F BeG CsH RnJ He

29 Alpha particles are one type of radioactivity. These particles have a nucleus of two protons and two neutrons but have no orbital electrons. Based on this information, it can be inferred that alpha particles are positive ions of the element —

F actiniumG curiumH radiumJ helium

30 A certain atom has a nucleus containing six protons and eight neutrons and has six electrons orbiting the nucleus. This atom is a form of the element —

A siliconB carbonC magnesiumD calcium

31 Calcium ions play an important role in the function of neurons in the brain. Elements that are chemically similar to calcium can interfere with the function of neurons. Which of the following is most likely to imitate calcium’s role in the function of neurons?

F SodiumG PotassiumH StrontiumJ Rubidium

o=x=o

32 The model above shows how an unidentified element, X, forms covalent bonds with oxygen. In which group on the periodic table does Element X most likely belong?

F Group 6G Group 12H Group 14J Group 18

33 In which model of the periodic table does the shaded area show the location of elements that require the least energy to lose one electron?

A C

B D

34 The ionic compounds that result from combining Group 2 and Group 16 elements have a 1:1 ratio because —

A Group 2 elements are electrically neutralB Group 2 elements have two valence electronsC Group 2 elements contain neutrons in the nucleusD Group 2 contains more elements than other groups

35 Silver bromide is a type of halide. Elements from which group in the periodic table are necessary to form halide compounds?

A Group 4B Group 5C Group 10D Group 17

36 Elements found in which shaded area of this periodic table undergo the fewest chemical reactions?

A QB RC SD T

37 According to the periodic table, which of these elements will form an ion with a –2 charge?

F SG MgH FJ Rb

38 The diagram shows physical changes that occur in the water cycle. Which of these shows condensation?

A QB RC SD T

39 Which process in the rock cycle is most likely responsible for moon rocks being converted to lunar soil?

A MetamorphismB WeatheringC SedimentationD Volcanism

40 Which of these changes in rocks is a physical change?

A Acid rain damaging marbleB Iron in rock combining with oxygen to form hematiteC Carbonic acid weathering limestoneD An ice wedge shattering a slab of shale

41 Which of the following processes is an example of a physical change associated with an oak tree?

A Decomposition of bark by bracket fungiB Starches and sugars being broken down during energy productionC Water and carbon dioxide being converted to glucoseD Evaporation of water from the surfaces of leaves

42 Compounds with the same chemical composition may have different densities because they —

A have differences in reactivityB are able to bond with oxygenC vary in solubilityD exist in different phases

43 Limestone is a sedimentary rock consisting mostly of calcium carbonate (CaCO3). Which process is most likely to cause a chemical change to limestone?

F Freezing water cracking limestoneG Flowing water eroding a limestone riverbedH Acid rain forming puddles on limestoneJ Coastal waves dissolving limestone sediments

44 Which of the following is an example of a chemical change?

A Combustion of gasolineB An apple being bittenC An ice cube being swallowedD Absorption of a water molecule

How Portland Cement Is Made

45 Portland cement is used to make concrete, a very common construction material. Which step in the production of portland cement causes a chemical change?A WB XC YD Z

46 Which of the following describes a chemical change that J. B. van Helmont could have observed?

F Limestone combined with an acid produces a gas.G Solid carbon dioxide becomes a gas at room temperature.H Limestone combined with sand results in a mixture.J Diluting an acid with water produces a solution.

47 Which process best demonstrates a chemical change in distilled water?

A Freezing the waterB Separating the water into its elementsC Calculating the water’s densityD Dissolving sugar in the water

48 Which of these describes a chemical change?

F Frost disappears from a window in the morning.G A decrease in temperature reduces the volume of a gas.H Soot is formed as a candle burns.J A cup of hot tea cools down.

49 In photography, which of these is an example of a chemical change?

F Light being refracted by a camera lensG Adjusting a lens to focus lightH Halide granules being activated by lightJ 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 meltedB boiledC reacted chemicallyD 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 wind carried away some matter before it burnedB some matter was converted to gases that were releasedC combustion changed some matter into energyD 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 1B 2C 3D 4

53 According to the law of conservation of mass, how much zinc was present in the zinc carbonate?

A 40 gB 88 gC 104 gD 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 The difference in the products’ masses is equal to the mass of the CaCO3.B The sum of the products’ masses is less than the mass of the CaCO3.C The mass of each product is equal to the mass of the CaCO3.D 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)

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 gG 95 gH 127 gJ 159 g

Mg + HCl → MgCl2 + H2

57 When the above equation is balanced, the coefficient for magnesium chloride is —

A 0B 1C 2D 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.

2C2H2(g) + 5O2(g) → 4CO2(g) + ___

59 Which additional product balances this reaction?

F 4OH(aq)G CH4(g)H H2O2(g)J 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 massindicates that the rusting process —

A is a physical changeB involves an energy-to-matter conversionC decreases the density of the metalD 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 thisreaction?

F Al + O2 → Al2O3

G 2Al + 2O2 → 2Al2O3

H 2Al + 3O2 → 5Al2O3

J 4Al + 3O2 → 2Al2O3

Reaction ofCopper with Sulfur

62 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.

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

63 Which set of coefficients balances the equation?

F 3, 3, 1, 2G 6, 1, 1, 3H 3, 2, 1, 6J 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 Heating the reactants to ensure the reaction occurs in a gaseous state

B Subtracting the mass of the gas from the mass of the solid and liquid products

C Mixing the reactants and measuring their total massD 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 massin grams of this mixture? Record and bubble in your answer to the nearest tenth on the answer document.

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 (mass of Liquid 1 + mass of Liquid 2) − (mass of solid)G (mass of Liquid 1 + mass of Liquid 2) + (mass of solid)H (mass of Liquid 1 × mass of Liquid 2) ÷ (mass of solid)J (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 pondenvironment would be less likely to survive because water would no longer —

F dissolve enough oxygen from the airG produce solutions containing vital nutrientsH remain neutral, instead becoming highly acidicJ 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 iceG increase in density while it freezes, dissolving more oxygen from the airH expand when it freezes, creating a floating and insulating layer of iceJ 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 Its transparency in lightB Its electrical conductivityC Its physical state of matterD 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 The oxygen in a water molecule contains a partial negative charge.G Gravity rotates the oxygen atoms to face the more-massive sodium ions.H Hydrogen atoms create repulsive forces with chloride ions.J Oxygen atoms form covalent bonds with sodium ions.

71 Water acts as a solvent of ionic compounds because —

F water is liquid over a wide range of temperaturesG water molecules are polarH water is found in three states of matterJ water takes the shape of its container

72 Which of these remains the same while water molecules go through the water cycle?

F The ratio of oxygen to hydrogen in the moleculesG The rate of vibration of the moleculesH The kinds of dissolved substances between the moleculesJ 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 Chemical stabilityB High polarityC Low melting pointD High freezing point

74 The structure of pure water makes it a good —

F solventG catalystH conductorJ nutrient

75 What is the reason that tap water will conduct electricity but pure water will not?

A Pure water has nonpolar bonds.B Tap water has dissolved ions.C Pure water has a neutral pH.D 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

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 fewer suspended solidsB a lower temperatureC more dissolved salt (NaCl) particlesD 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 hydrogenG has been heatedH is separated into H+ and OH– ionsJ contains dissolved minerals

79 In this apparatus, the seawater is an example of a —

F strong electrolyteG weak acidH nonelectrolyteJ strong base

80 Dissolving salt in water increases the conductivity of the solution because the —

F alt gives the solution a net negative chargeG salt ions bond with the available water moleculesH solution has an increase in kinetic energyJ concentration of ions in the solution increases

81 Which of these statements is supported by these data?

A More KNO3 will dissolve than KBr at 0°C.B Temperature has little effect on the water solubility of NaCl.C KBr is insoluble in water at low temperatures.D 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 decrease in pressureB increase in salt concentrationC decrease in temperatureD 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 temperatureG Stopping the stirringH Lowering the air pressureJ Crushing the crystal

84 All of these can affect the rate at which a solid dissolves in water except —

A decreasing air pressureB stirring the waterC increasing the temperature of the waterD 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 Reduced air pressureB Exposure to direct sunlightC Increased air currentsD Cooler temperatures

86 The table shows temperature and pressure in four containers holding the same amount of water. According to the table, in whichcontainer can the most sodium chloride be dissolved in the water?

A QB RC SD T

Conditions in Four

Containers of Water

ContainerTemperature

(°C)

Pressure

(kPa)

Q 10 204.5

R 20 204.5

S 30 101.3

T 40 101.3

87 Power plants that discharge warm water into rivers have a negative effect on aquatic life. This is because the higher water temperature —

A increases the pressure of the river waterB increases the pH value of the river waterC decreases sediment solubility in the river waterD decreases the dissolved oxygen in the river water

F H

G J

GroupTemperature

(°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

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?

Properties of Some Solutions

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 Solution 1B Solution 2C Solution 3D Solution 4

SolutionElectrical Conductivity

of Solution

Original Color of

Litmus Paper

Color of Litmus Paper

After Dipping in SolutionPh

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

MTBE Solubility

90 MTBE is a gasoline additive that has entered some groundwater supplies. According to the table above, which of the following watertemperatures would allow 79 grams of MTBE to dissolve in 1 liter of water?

F 0°CG 10°CH 30°CJ 40°C

Temperature

(°C)

Solubility

(grams per liter)

0 83

9.7 51

19.8 42

29.6 31

39.3 25

48.6 19

Grade 11

Objective 4

Answer Key

Grade 11 Objective 4 Answer Key

Question Correct AnswerObjective Measured

Student Expectation Source - item number

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

Grade 11 Objective 4 Answer Key

Question Correct AnswerObjective Measured

Student Expectation Source - item number

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

Grade 11 Objective 4 Answer Key

Question Correct AnswerObjective Measured

Student Expectation Source - item number

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

Grade 11 Objective 4 Answer Key

Question Correct AnswerObjective Measured

Student Expectation Source - item number

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