XIX. Chemistry, High School

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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.

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S

eSSion

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

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1 An equation for a chemical reaction is

shown below.

2H (g)₂ O₂(g) H O( )₂ l 571.6kJ Which of the following statements indicates that this reaction is exothermic?

A. Energy is released. B. A compound is formed. C. The reactants are two

different gases.

D. There are more reactants than products.

ID:298325 B Common EQ

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2 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?

A. The surface area of the product particles decreased.

B. The collision rate of the reactant particles increased.

C. The concentrations of the reactant particles increased.

D. The concentrations of the product particles decreased.

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ID:281214 D Common EQ

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3 Which of the following statements best

describes the current atomic theory? A. Electrons move in circular orbits

around the nucleus.

B. Electrons are held in an atom by their attraction to each other. C. Electrons are evenly distributed

throughout a mixture of positive and neutral particles.

D. Electrons exist in specific energy levels and have both wave and particle characteristics.

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4 Which of the following molecules has a

nonpolar covalent bond? A. H–Br

B. H–Cl C. H–F D. H–H

ID:244829 244829_ASTDAV69.eps [opt_ A Common EQ

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5 Which of the following equations shows

a fusion reaction? A. 3₁H 2₁H 4₂He 1₀n B. 238₉₂U 234₉₀Th 4₂He C. 24₁₁Na ₁₂24Mg _–10e D. 1₀n 235₉₂U 92₃₆Kr 141_Ba 56 3 1_n 0

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6 Which of the following statements

describes what happens in a buffer solution when a strong acid is added? A. The H ions from the strong acid

combine with basic ions in the buffer. B. The H ions from the strong acid

combine with acidic ions in the buffer. 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.

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7 How many atoms of oxygen (O) are

required to form two molecules of

sulfuric acid (H₂SO₄)?

A. 2 B. 4 C. 6 D. 8

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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.

3Mg(s) Fe SO₂( _{4 3}) (aq) 2Fe (s) 3MgSO aq₄( )

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

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9 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.

X Y Z energy

After the reaction reaches equilibrium, which of the following changes would shift the equilibrium to the left? A. adding more compound X

to the equilibrium

B. adding more compound Y to the equilibrium

C. increasing the temperature of the equilibrium

D. decreasing the temperature of the equilibrium

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10 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.

B. The molecules weigh less as a gas than they do as a liquid.

C. The molecules move faster as a gas than they do as a liquid.

D. The molecules are closer together as a gas than they are as a liquid.

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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

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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

Mass of crucible and iron powder Mass of iron powder

Mass of sulfur added to crucible Mass of crucible and contents after reaction

Mass of iron-sulfur compound

5.23 g 7.46 g x 1.28 g 8.74 g 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.

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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.

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12 Which of the following equations shows a chemical change?

A. H O₂ ( )l heat H O g₂ ( )

B. H O₂ ( )l H O s₂ ( ) heat

C. H O₂ ( )l Na O(s₂ ) 2Na aq( ) 2OH (aq) heat

D. H O₂ ( )l NaCl(s) Na (aq) Cl (aq) H O₂ ( )l

ID:280897 280897_HI_dot.eps [opt_a0 A Common EQ

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13 Which of the following is a Lewis dot

structure for hydrogen iodide (HI)?

A.

H I

B.

H I

C.

H I

D.

H I

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14 Which of the following elements

has both metallic and nonmetallic properties?

A. Ar B. Ge C. Mg D. S

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15 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? A. 1

B. 2 C. 5 D. 10

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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 atm B. 2 atm C. 3 atm D. 4 atm

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ID:226997 3160092_AR1.eps [opt_a01, D Common EQ

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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. Temperature (°C) Pr essur e (atm) 27 0 1.0 2.0 3.0 4.0 250 C. Temperature (°C) Pr essur e (atm) 27 0 1.0 2.0 3.0 4.0 250 B. Temperature (°C) Pr essur e (atm) 27 0 1.0 2.0 3.0 4.0 250 D. Temperature (°C) Pr essur e (atm) 27 0 1.0 2.0 3.0 4.0 250

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18 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.

D. The molecules become arranged in a pattern and maintain fixed positions.

ID:229556 3152531_AR1.eps B Common EQ

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19 The diagram below shows a partial

periodic table.

F O

The electron configuration of oxygen is

1s2_2s2_2p4_{. On the periodic table, fluorine}

is one space to the right of oxygen. Which of the following electron configurations represents fluorine?

A. 1s2_2s2_2p3

B. 1s2_2s2_2p5

C. 1s2_2s2_2p6_3s2_3p3

D. 1s2_2s2_2p6_3s2_3p5

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20 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

C. the number of gas molecules in the sample

D. the distance between gas molecules in the sample

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21 What is the name of the compound with

the chemical formula NH(NH _{4 2}) S?

A. ammonium sulfide B. hydrogen sulfate C. sulfur hydride D. sulfuric acid

ID:287275 ASTDAV252_periodictable.e B Common EQ

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22 The diagram below shows the relative

locations of five unidentified elements in the periodic table: E, X, G, J, and L.

E X

L J

G

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

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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.

ID:272994 BELROB144.eps Common EQ

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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.

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S

eSSion

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.

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24 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? 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. D. Both samples are acids, and

rainwater is more acidic.

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25 The masses of the reactants and the

theoretical yields of the products for a chemical reaction are shown below.

3Sb 3I₂ 2SbI₃ Sb

(1.2 g) (2.4 g) (3.2 g) (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%

B. 67%

C. 75%

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ID:287272 ASTDAV249.eps B Common EQ

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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) Mg (s) MgCl (aq) ₂ H₂( )g

The data for the reaction are shown in the table below.

Mass of Mg

Mass of HCl Solution Total Mass of Substances in Beaker before the Reaction Total Mass of Substances in Beaker after the Reaction

0.24 g 5.49 g 5.73 g 5.71 g 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?

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.

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27 The equation below represents an

equilibrium reaction.

HNO (aq)₃ NH aq₃( ) NO (aq)₃ NH (aq)₄

Which chemical in the forward reaction is a Brønsted-Lowry acid?

A. HNO₃

B. NH₃

C. NO₃

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28 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

What is the molarity of the KOH solution? A. 0.15 M B. 0.30 M C. 0.60 M D. 0.75 M ID:274067 A Common EQ

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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? A. TiC1₄ O₂ TiO₂ 2 1C ₂ B. 2TiC1₄ O₂ TiO₂ 4 1C C. TiC1₄ 2O₂ 2TiO₂ C1₂ D. 2TiC1₄ 2O₂ 2TiO₂ C1₄ ID:261188 B Common EQ

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30 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?

A. The solute melts. B. The solute dissolves. C. The solute remains intact.

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31 Calcium and boron react to form

calcium boride, as represented by the chemical equation below.

Ca 6B CaB₆

Which type of reaction is shown by this equation? A. combination B. decomposition C. double displacement D. single displacement ID:294713 D Common EQ

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32 Methane gas (CH₄) reacts with

oxygen gas (O₂) according to the

equation below.

CH₄ 2O₂ CO₂ 2H O₂ 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;

CO₂ and H O₂ have more chemical

potential energy than CH₄ and O₂.

B. The reaction is endothermic;

CO₂ and H O₂ have less chemical

C. The reaction is exothermic;

CO₂ and H O₂ have more chemical

D. The reaction is exothermic;

CO₂ and H O₂ have less chemical

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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.

ID:260794 ASTDAV148.eps Common EQ

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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.

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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.

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34 One mole of which of the following

substances has the greatest entropy?

A. ethanol (l )

B. iron (s) C. neon (g)

D. water (l )

●

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.

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36 Which of the following is the electron

configuration for sulfur?

A. 1s2_2s2_2p4

B. 1s2_2s2_2p6_3s2

C. 1s2_2s2_2p6_3s2_3p4

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ID:281218 281218_decay.eps B Common EQ

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37 Uranium-238 undergoes radioactive

decay according to the incomplete equation below.

U

238 4

2He X 92

What is the decay product represented

by X? A. 232₉₀Th B. 234₉₀Th C. 242₉₄Pu D. 24494Pu ID:281919 D Common EQ

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applies the law of multiple proportions to the relationship between carbon monoxide

(CO) and carbon dioxide (CO₂)?

A. The mass of a mole of CO is exactly

half that of a mole of CO₂.

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.

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39 Which of the following identifies the

number and location of protons in a lithium atom?

A. 3 protons, located in the nucleus B. 7 protons, located in the nucleus C. 3 protons, located in an atomic orbital D. 7 protons, located in an atomic orbital

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40 Although H O₂ and H S₂ 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 O₂ is

a liquid and H S₂ is a gas under these

conditions?

A. H O₂ is less dense than H S₂ .

B. H O₂ is less chemically reactive

than H S₂ .

C. H O₂ has a smaller molecular mass

than H S₂ .

D. H O₂ has stronger intermolecular

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41 Based on valence electron

configurations, which of the following is a formula for a compound formed from sodium (Na) and oxygen (O)? A. NaO

B. NaO₂

C. Na₂O

D. Na₂O₃

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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.

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43 Particles of which of the following

substances are farthest apart at STP? A. aluminum (s)

B. helium (g)

C. mercury (l )

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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.

ID:274045 Common EQ

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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.

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Write your answer to question 45 in the space provided in your Student Answer Booklet.

ID:294716 Common EQ

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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.

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Common Polyatomic Ions

Ion Ionic Formula

Ammonium NH₄1 Carbonate CO3 2-Hydroxide OH -Nitrate NO3 -Phosphate PO₄ 3-Sulfate SO₄

2-Combined Gas Law: P V

T P V T 1 1 1 2 2 2 5

Ideal Gas Law: PV 5 nRT

Dilution Formula: M₁V₁ 5 M₂V₂

Molar Volume of Ideal Gas at STP: 22.4 L/mol

Ideal Gas Constant: R 5 0.0821 L •atm/mol •K 5 8.31 L •kPa/mol •K

STP: 1 atm (101.3 kPa), 273 K (0°C)

Absolute Temperature Conversion: K 5 °C 1 273

Definition of pH: pH 52log [H₃O1_]₅₂_{log [H}1_]

Avogadro’s Number: 6.02 3 1023_{particles/mol}

Nuclear Symbols

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M

as

sa

ch

u

se

tt

s

C

om

p

re

h

en

si

ve

A

ss

es

sm

en

t

S

ys

te

m

Li 3 Lithium H 1 Hydrogen 9.01 Be 4 Ber yllium 2A 2 3A 13 4A 14 5A 15 6A 16 7A 17 3B 3 4B 4 5B 5 6B 6 7B 7 8B 8 9 10 1B 11 2B 12 Na 11 Sodium 24.31 Mg 12 Magnesium K 19 otassium 40.08 Ca 20 Calcium Rb 37 Rubidium 87.62 Sr 38 Strontium Cs 55 Cesium 137.33 Ba 56 Bar ium Fr 87 Fr ancium (226) Ra 88 Radium 44.96 Sc 21 Scandium 47.88 Ti 22 Titanium 88.91 Y 39 Yttr ium 91.22 Zr 40 Zirconium 138.91 La 57 La nt ha nu m 178.49 Hf 72 Hafnium (227) Ac 89 Actinium (267) Rf 104 Rutherf ordium 50.94 V 23 V anadium 52.00 Cr 24 Chromium 92.91 Nb 41 Niobium 95.94 Mo 42 Molybdenum 180.95 Ta 73 Tantalum 183.85 W 74 Tungsten (268) Db 105 Dubnium (271) Sg 106 Seaborgium 54.94 Mn 25 Manganese 55.85 Fe 26 _Iron (98) Tc 43 Technetium 101.07 Ru 44 Ruthenium 186.21 Re 75 Rhenium 190.23 Os 76 Osmium (272) Bh 107 Bohr ium (277) Hs 108 Hassium 58.93 Co 27 Cobalt 58.69 Ni 28 Nic ke l 102.91 Rh 45 Rhodium 106.42 Pd 46 P alladium 192.22 Ir 77 Ir idium 195.08 Pt 78 Platinum (276) Mt 109 Meitner ium (281) 63.55 Cu 29 Copper 65.39 Zn 30 _Zinc 107.87 Ag 47 Silv er 112.41 Cd 48 Cadmium 196.97 A u ₇₉ Gold 200.59 Hg 80 Mercur y 10.81 B 5 Boron 12.01 C 6 Carbon 26.98 Al 13 Aluminum 28.09 Si 14 Silicon 69.72 Ga 31 Gallium 72.59 Ge 32 Ger manium 114.82 In 49 Indium 118.71 Sn 50 Tin 204.38 Tl 81 Thallium 207.2 Pb 82 _Lead 14.01 N 7 Nitrogen 16.00 O 8 Oxygen 30.97 P 15 Phosphor us 32.06 S 16 Sulfur 74.92 As 33 Arsenic 78.96 Se 34 Selenium 121.75 Sb 51 Antimon y 127.60 Te 52 Tellur ium 208.98 Bi 83 Bismut h (209) Po 84 P olonium 19.00 F 9 Fluor ine 20.18 35.45 Cl 17 Chlor ine 39.95 79.90 Br 35 Bromine 83.80 Kr 126.91 I ₅₃ Iodine 131.29 (210) At 85 Astatine (222) amily) 1A 1 4.00 1 110 140.12 Ce 58 Cer ium 140.91 Pr 59 Praseodymiu m 232.04 Th 90 Thor ium 231.04 P a ₉₁ Protactinium 144.24 Nd 60 Neodymium (145) Pm 61 Promethium 238.03 U 92 Uranium (237) Np 93 Neptunium 150.36 Sm 62 Samar ium 151.96 Eu 63 Europium (244) Pu 94 Plutonium (243) Am 95 Amer icium 157.25 Gd 64 Gadolinium 158.93 Tb 65 Terbium (247) Cm 96 Cur ium (247) Bk 97 Ber kelium 162.50 Dy 66 Dysprosium 164.93 Ho 67 Holmium (251) Cf 98 Calif o rnium (252) Es 99 Einsteinium 167.26 Er 68 Erbium 168.93 Tm 69 Thulium (257) Fm 100 Fe rmium (258) Md 101 Mendele vium 173.04 Yb 70 Ytterbium (259) No 102 Nobelium Lanthanide Ser ies Actinide Ser ies

Mass numbers in parentheses are those of the most stab

le or most common isotope

vised based on IUP

A

C Commission on Atomic

W

eights and Isotopic Ab

undances

, “Atomic

W

eights of the Elements 2007.

”

Ds

Rg 111

(280)

K

ey: _{atomic weight} Symbol _{atomic number}

Name Dar mstadtium Roentgenium

P

er

iodic

Tab

le of the Elements

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Reporting Categories, Standards, and Correct Answers*

Item No. Page No. Reporting Category Standard Correct Answer _(MC)*

1 344 Properties of Matter and Thermochemistry 6.4 A 2 344 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

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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.