physical behavior of matter unit regents review -...

adapted from http://www.chemcool.com by DSK 2008

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Name: Date:

Physical Behavior Of Matter Unit Regents Review

Part I:

1. Given:

Which diagram represents a mixture?

2. Which species represents a chemical compound?

(1) N2 (2) NH4+ (3) Na (4) NaHCO3

3. On a field trip, Student X and Student Y collected two rock samples. Analysis revealed that both rocks contained lead and sulfur. One rock contained a certain percentage of lead and sulfur by mass, and the other rock contained a different percentage of lead and sulfur by mass. Student X stated that the rocks contained two different mixtures of lead and sulfur. Student Y stated that the rocks contained two different compounds of lead and sulfur. Their teacher stated that both students could be correct.

Draw particle diagrams in each of the rock diagrams provided to show how Student X’s and Student Y’s explanations could both be correct. Use the symbols in the key provided in your answer booklet to sketch lead and sulfur atoms.


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4. One similarity between all mixtures and compounds is that both

(1) are heterogeneous (2) are homogeneous (3) combine in a definite ratio (4) consist of two or more substances

5. Draw two different compounds using the representations for atoms of element X and element Z given below.

6. Draw a mixture of these two compounds.

7. Which substance can be decomposed by a chemical change?

(1) Co (2) CO (3) Cr (4) Cu

8. Which of these terms refers to matter that could he heterogeneous?

(1) element (2) mixture (3) compound (4) solution

9. Given the reaction between two different elements in the gaseous state:

Box A below represents a mixture of the two reactants before the reaction occurs. The product of this reaction is a gas. In another box draw the system after the reaction has gone to completion, based on the Law of Conservation of Matter.

10. Which substance can not be decomposed by a chemical change?

(1) Ne (2) N2O (3) HF (4) H2O


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11. Which of these contains only one substance?

(1) distilled water (2) sugar water (3) saltwater (4) rainwater

12. Given the diagrams X, Y, and Z below:

Which diagram or diagrams represent a mixture of elements A and B?

(1) X, only (3) X and Y (2) Z, only (4) X and Z

13. Base your answers to questions 65 through 67 on the particle diagrams below, which show atoms and/ or molecules in three different samples of matter at STP.

a. Which sample represents a pure substance?

b. When two atoms of y react with one atom of z, a compound forms. Using the number of atoms shown in sample 2, what is the maximum number of molecules of this compound that can be formed?

c. Explain why XX does not represent a compound.


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14. At STP, the element oxygen can exist as either O2 or O3 gas molecules. These two forms of the element have

(1) the same chemical and physical properties (2) the same chemical properties and different physical properties (3) different chemical properties and the same physical properties (4) different chemical and physical properties

15. Which substance represents a compound? (1) C(s) (2) Co(s) (3) CO(g) (4) O2(g)

Base your answers to questions 54 through 57 on the particle diagrams below. Samples A, B, and C contain molecules at STP.

16. Explain, in terms of the composition, why sample A represents a pure substance.

17. Explain why sample C could represent a mixture of fluorine and hydrogen chloride.

18. Contrast sample A and sample B, in terms of compounds and mixtures. Include both sample A and sample B in your answer.

19. Which particle diagram represents one pure substance, only?

20. Which substance can be decomposed by a chemical change?

(1) calcium (2) potassium (3) copper (4) ammonia


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21. Which terms are used to identify pure substances?

(1) an element and a mixture (2) an element and a compound (3) a solution and a mixture (4) a solution and a compound

22. Given the simple representations for atoms of two elements:

Which particle diagram represents molecules of only one compound in the gaseous phase?

23. Which substance can not be decomposed by ordinary chemical means?

(1) methane (2) mercury (3) ethanol (4) ammonia

24. Given the particle diagram representing four molecules of a substance:

Which particle diagram best represents this same substance after a physical change has taken place?

25. Two substances, A and Z, are to be identified. Substance A can not be broken down by a chemical change. Substance Z can be broken down by a chemical change. What can be concluded about these substances?

(1) Both substances are elements. (2) Both substances are compounds. (3) Substance A is an element and substance Z is a compound. (4) Substance A is a compound and substance Z is an element.


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26. Given the key:

Which particle diagram represents a sample containing the compound CO(g)?

27. Which two substances can not be broken down by chemical change?

(1) C and CuO (2) C and Cu (3) CO2 and CuO (4) CO2 and Cu

28. Which particle diagram represents a mixture of element X and element Z, only?

Base your answers to questions 29 through 32 on the diagram below concerning the classification of matter.

29. What type of mixture is represented by X?

30. What type of substance is represented by Z?

31. Explain, in terms of particle arrangement, why NaCl(aq) is a homogeneous mixture.

32. Given a mixture of sand and water, state one process that can be used to separate water from the sand.


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Part II:

1. Which mixture can be separated by using the equipment shown below? NOTE: (aq) means aqueous solution (“dissolved in water”)

(1) NaCl(aq) and SiO2(s) (2) NaCl(aq) and C6H12O6(aq) (3) CO2(aq) and NaCl(aq) (4) CO2(aq) and C6H12O6(aq)

2. When a mixture of water, sand, and salt is filtered, what passes through the filter paper?

(1) water, only (2) water and sand, only (3) water and salt, only (4) water, sand, and salt

3. Which physical property makes it possible to separate the components of crude oil by means of distillation?

(1) melting point (2) conductivity (3) solubility (4) boiling point

4. At equilibrium, nitrogen, hydrogen, and ammonia gases form a mixture in a sealed container. The data table below gives some characteristics of these substances.

Describe how to separate ammonia from hydrogen and nitrogen.

5. A bottle of rubbing alcohol contains a mixture of 2-propanol and water. These liquids can be separated by the process of distillation because the 2-propanol and water

(1) have combined chemically and retain their different boiling points (2) have combined physically and retain their different boiling points (3) have combined chemically and have the same boiling point (4) have combined physically and have the same boiling point


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Base your answers to question 6 on the information and diagram below and on your knowledge of chemistry.

Crude oil is a mixture of many hydrocarbons that have different numbers of carbon atoms. The use of a fractionating tower allows the separation of this mixture based on the boiling points of the hydrocarbons. To begin the separation process, the crude oil is heated to about 400°C in a furnace, causing many of the hydrocarbons of the crude oil to vaporize. The vaporized mixture is pumped into a fractionating tower that is usually more than 30 meters tall. The temperature of the tower is highest at the bottom. As vaporized samples of hydrocarbons travel up the tower, they cool and condense. The liquid hydrocarbons are collected on trays and removed from the tower. The diagram below illustrates the fractional distillation of the crude oil and the temperature ranges in which the different hydrocarbons condense.

6. State the trend between the boiling point of the hydrocarbons contained in the crude oil and the number of carbon atoms in these molecules.

7. Which property makes it possible to separate the oxygen and the nitrogen from a sample of liquefied air?

(1) boiling point (2) conductivity (3) hardness (4) electronegativity

Part III:

1. Which 5.0-milliliter sample of NH3 will take the shape of and completely fill a closed 100.0-milliliter container?

(1) NH3(s) (2) NH3(l) (3) NH3(g) (4) NH3(aq)


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2. Which statement correctly describes a sample of gas confined in a sealed container?

(1) It always has a definite volume, and it takes the shape of the container.

(2) it takes the shape and the volume of any container in which it is confined.

(3) It has a crystalline structure.

(4) It consists of particles arranged in a regular geometric pattern.

3. In which material are the particles arranged in a regular geometric pattern? (1) CO2 (g) (2) NaCl(aq) (3) H2O(l) (4) C12H22O11(s)

4. Which grouping of the three phases of bromine is listed in order from left to right for increasing distance between bromine molecules?

(1) gas, liquid, solid (2) liquid, solid, gas (3) solid, gas, liquid (4) solid, liquid, gas

5. Given the particle diagram:

At 101.3 kPa and 298 K, which element could this diagram represent? (Note: all elements in group 18 on the periodic table are gasses at 101.3 kPa and 298 K)

(1) Rn (2) Xe (3) Ag (4) Kr

6. Which statement best describes the shape and volume of an aluminum cylinder at STP?

(1) It has a definite shape and a definite volume. (2) It has a definite shape and no definite volume.

(3) It has no definite shape and a definite volume. (4) It has no definite shape and no definite volume.

Part IV:

1. Solid A at 80 C is immersed in liquid B at 60 C. Which statement correctly describes the energy changes between A and B?

1. A releases heat and B absorbs heat. 3. Both A and B absorb heat.

2. A absorbs heat and B releases heat. 4. Both A and B release heat.

2. Which sample of Fe contains particles having the highest average kinetic energy?

(1) 5 g at 10oC (2) 10 g at 25oC (3) 5 g at 400 K (4) 10 g at 300 K

3. Which change in the temperature of a 1-gram sample of water would cause the greatest increase in the average kinetic energy of its molecules?

(1) 1oC to 10oC (2) 10oC to 1oC (3) 50oC to 60oC (4) 60oC to 50oC

4. An increase in the average kinetic energy of a sample of copper atoms occurs with an increase in

(1) concentration (2) temperature (3) pressure (4) volume


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5. The average kinetic energy of water molecules is greatest in which of these samples?

(1) 10 g of water at 35°C (2) 10 g of water at 55°C (3) 100 g of water at 25°C (4) 100 g of water at 45°C

6. Which form of energy is converted to thermal energy when propane burns in air?

(1) electromagnetic (2) nuclear (3) electrical (4) chemical

Part IV:

1. A real gas behaves more like an ideal gas when the gas molecules are

(1) close and have strong attractive forces between them (2) far apart and have strong attractive forces between them (3) close and have weak attractive forces between them (4) far apart and have weak attractive forces between them

2. Under which conditions does a real gas behave most like an ideal gas?

(1) at low temperatures and high pressures (2) at low temperatures and low pressures

(3) at high temperatures and high pressures (4) at high temperatures and low pressures

3. Helium is most likely to behave as an ideal gas when it is under

(1) high pressure and high temperature (2) high pressure and low temperature

(3) low pressure and high temperature (4) low pressure and low temperature

4. The concept of an ideal gas is used to explain

(1) the mass of a gas sample (2) the behavior of a gas sample (3) why some gases are monatomic (4) why some gases are diatomic

5. The kinetic molecular theory assumes that the particles of an ideal gas

(1) are in random, constant, straight-line motion (2) are arranged in a regular geometric pattern (3) have strong attractive forces between them (4) have collisions that result in the system losing energy

Part V:

Base your answers to questions 1 through 3 on the information below:

A rigid cylinder is fitted with a movable piston. The cylinder contains a sample of helium gas, He(g), which has an initial volume of 125.0 milliliters and an initial pressure of 1.0 atmosphere, as shown below. The temperature of the helium gas sample is 20.0°C.

1. Express the initial volume of the helium gas sample, in liters.


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2. The piston is pushed further into the cylinder. Show a correct numerical setup for calculating the volume of the helium gas that is anticipated when the reading on the pressure gauge is 1.5 atmospheres. The temperature of the helium gas remains constant.

3. Helium gas is removed from the cylinder and a sample of nitrogen gas, N2(g), is added to the cylinder. The nitrogen gas has a volume of 125.0 milliliters and a pressure of 1.0 atmosphere at 20.0°C. Compare the number of particles in this nitrogen gas sample to the number of particles in the original helium gas sample.

4. A 1.00-mole sample of neon gas occupies a volume of 24.4 liters at 298 K and 101.3 kilopascals. Calculate the density of this sample. Your response must include both a correct numerical setup and the calculated result.

5. A sample of gas is held at constant pressure. Increasing the Kelvin temperature of this gas sample causes the average kinetic energy of its molecules to

(1) decrease and the volume of the gas sample to decrease (2) decrease and the volume of the gas sample to increase (3) increase and the volume of the gas sample to decrease (4) increase and the volume of the gas sample to increase

6. Which graph shows the pressure-temperature relationship expected for an ideal gas?

7. At the same temperature and pressure, which sample contains the same number of moles of particles as 1 liter of O2(g)?

(1) 1 L Ne(g) (2) 2 L N2(g) (3) 0.5 L SO2(g) (4) 1 L H2O(l)

8. A gas occupies a volume of 40.0 milliliters at 20oC. If the volume is increased to 80.0 milliliters at constant pressure, the resulting temperature will be equal to

(1) 20oC x 80.0 mL / 40.0 mL (2) 20oC x 40.0 mL / 80.0 mL (3) 293 K x 80.0 mL / 40.0 mL (4) 293 K x 40.0 mL / 80.0 mL


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9. Base your answer on the diagram below, which shows a piston confining a gas in a cylinder.

Graph the general relationship between the pressure and the volume of an ideal gas at constant temperature.

10. Refer to the diagram for question 9. The gas volume in the cylinder is 6.2 milliliters and its pressure is 1.4 atmospheres. The piston is then pushed in until the gas volume is 3.1 milliliters while the temperature remains constant.

a) Calculate the pressure, in atmospheres, after the change in volume. Show all work.

b) Record your answer.

11. At the same temperature and pressure, 1.0 liter of CO( g) and 1.0 liter of CO2 (g) have

(1) equal masses and the same number of molecules (2) equal volumes and the same number of molecules (3) different masses and a different number of molecules (4) different volumes and a different number of molecules

12. The volume of a gas is 4.00 liters at 293 K and constant pressure. For the volume of the gas to become 3.00 liters, the Kelvin temperature must be equal to

13. Which graph best represents the pressure-volume relationship for an ideal gas at constant temperature?


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Base your answers to questions 14 through 17 on the following formation. A weather balloon has a volume of 52.5 liters at a temperature of 295 K. The balloon is released and rises to an altitude where the temperature is 252 K.

14. How does this temperature change affect the gas particle motion?

15. The original pressure at 295 K was 100.8 kPa and the pressure at the higher altitude at 252 K is 45.6 kPa. Assume the balloon does not burst. Show a correct numerical setup for calculating the volume of the balloon at the higher altitude.

16. What Celsius temperature is equal to 252 K?

17. What pressure, in atmospheres (atm), is equal to 45.6 kPa?

18. A gas occupies a volume of 444 mL at 273 K and 79.0 kPa. What is the final kelvin temperature when the volume of the gas is changed to 1880 mL and the pressure is changed to 38.7 kPa?

(1) 31.5 K (2) 292 K (3) 566 K (4) 2360 K

19 At STP, 4 liters of O2 contains the same total number of molecules as

(1) 1 L of NH3 (2) 2 L of Cl2 (3) 8 L of He (4) 4 L of CO2

20. A sample of helium gas has a volume of 900. milliliters and a pressure of 2.50 atm at 298 K. What is the new pressure when the temperature is changed to 336 K and the volume is decreased to 450. milliliters?

(1) 0.177 atm (2) 4.43 atm (3) 5.64 atm (4) 14.1 atm

Base your answers to questions 21 through 23 on the information and diagrams below. Cylinder A contains 22.0 grams of CO2(g) and cylinder B contains N2(g). The volumes, pressures, and temperatures of the two gases are indicated under each cylinder.

21. What is the total number of moles of CO2(g) in cylinder A?


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22. Explain why the number of molecules of N2(g) in cylinder B is the same as the number of molecules of CO2(g) in cylinder A.

23. The temperature of the CO2(g) is increased to 450. K and the volume of cylinder A remains constant. In the space below, show a correct numerical setup for calculating the new pressure of the CO2(g) in cylinder A.

Base your answers to questions 24 and 25 on the information below. A lightbulb contains argon gas at a temperature of 295 K and at a pressure of 75 kilopascals. The lightbulb is switched on, and after 30 minutes its temperature is 418 K.

24. In the space below, show a correct numerical setup for calculating the pressure of the gas inside the lightbulb at 418 K. Assume the volume of the lightbulb remains constant.

25. What Celsius temperature is equal to 418 K?

Base your answers to question 26 on the information below. Air bags are an important safety feature in modern automobiles. An air bag is inflated in milliseconds by the explosive decomposition of NaN3(s). The decomposition reaction produces N2(g), as well as Na(s), according to the unbalanced equation below.

NaN3 (s) → Na (s) + N2 (g)

26. When the air bag inflates, the nitrogen gas is at a pressure of 1.30 atmospheres, a temperature of 301 K, and has a volume of 40.0 liters. In the space in your answer booklet, calculate the volume of the nitrogen gas at STP. Your response must include both a correct numerical setup and the calculated volume.

27. A sample of a gas is contained in a closed rigid cylinder. According to kinetic molecular theory, what occurs when the gas inside the cylinder is heated?

(1) The number of gas molecules increases. (2) The number of collisions between gas molecules per unit time decreases. (3) The average velocity of the gas molecules increases. (4) The volume of the gas decreases.


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Part VI:

1. As ice melts at standard pressure, its temperature remains at 0oC until it has completely melted. Its potential energy

(1) decreases (2) increases (3) remains the same

2. The solid and liquid phases of water can exist in a state of equilibrium at 1 atmosphere of pressure and a temperature of

(1) 0oC (2) 100oC (3) 273oC (4) 373oC

3. Given the equation: H2O(s) ↔ H2O(l) At which temperature will equilibrium exits when the atmospheric pressure is 1 atm?

(1) 0 K (2) 100 K (3) 273 K (4) 373 K

4. The table below shows the normal boiling point of four compounds.

Which compound has the strongest intermolecular forces? (1) HF(l) (2) CH3Cl(l) (3) CH3F(l) (4) HCl(l)

5. The vapor pressure of a liquid is 0.92 atm at 60oC. The normal boiling point of the liquid could be (1) 35oC (2) 45oC (3) 55oC (4) 65oC

5 As the temperature of a liquid increases, its vapor pressure


6 As the pressure on the surface of a liquid decreases, the temperature at which the liquid will boil


7 A sample of water is heated from a liquid at 40oC to a gas at 110oC.

a) On the heating curve diagram provided above, label each of the following regions:

Liquid, only ; Gas, only; Phase change


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b) For section QR of the graph, state what is happening to the water molecules as heat is added.

c) For section RS of the graph, state what is happening to the water molecules as heat is added.

8. Base your answers on the graph below, which shows the vapor pressure curves for liquids A and B.

a. What is the vapor pressure of liquid A at 70oC? Your answer must include correct units.

b. At what temperature does liquid B have the same vapor pressure as liquid A at 70oC? Your answer must include correct units.

c. Which liquid will evaporate more rapidly? Explain your answer in terms of intermolecular forces.

9. Which phase change results in the release of energy?

(1) H2O(s) → H2O(l) (2) H2O(s) → H2O(g) (3) H2O(l) → H2O(g) (4) H2O(g) → H2O(l)


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10. The graph below represents the heating curve of a substance that starts as a solid below its freezing point.

What is the melting point of this substance?

(1) 30oC (2) 55oC (3) 90oC (4) 120oC

11. Which change is exothermic? (1) freezing of water (2) melting of iron (3) vaporization of ethanol (4) sublimation of iodine

12. According to Reference Table H, what is the vapor pressure of propanone at 45oC? (

1) 22 kPa (2) 33 kPa (3) 70. kPa (4) 98 kPa

13. The freezing point of bromine is

(1) 539oC (2) -539oC (3) 7oC (4) -7oC

Base your answers to questions 14 through 17 on the information below.

Given the heating curve where substance X starts as a solid below its melting point and is heated uniformly:

14. Identify the process that takes place during line segment DE of the heating curve.

15. Identify a line segment in which the average kinetic energy is increasing.


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16. Using "o" to represent particles of substance X, draw at least five particles as they would appear in the substance at point F.

17. Describe, in terms of particle behavior or energy, what is happening to substance X during line segment BC.

18 According to Reference Table H, what is the boiling point of ethanoic acid at 80 kPa?

(1) 28°C (2) 100°C (3) 111°C (4) 125°C

Base your answers to questions 19 and 20 on the heating curve below, which represents a substance starting as a solid below its melting point and being heated at a constant rate over a period of time:

19. What is happening to the average kinetic energy of the particles during segment BC?

20. How does this heating curve illustrate that the heat of vaporization is greater than the heat of fusion?

21. In which process does a solid change directly into a vapor?

(1) condensation (2) sublimation (3) deposition (4) solidification


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Part VII:

1. Calculate the heat released when 25.0 grams of water freezes at 0oC. Show all work. Record your answer with an appropriate unit.

2. How much heat energy must be absorbed to completely melt 35.0 grams of H2O(s) at 0°C?

(1) 9.54 J (2) 146 J (3) 11,700 J (4) 79,100 J


In a laboratory experiment, 10.00 grams of an unknown solid is added to 100.0 milliliters of water and the temperature of the resulting solution is measured over several minutes, as recorded in the table below.

3. On a graph, plot the data from the data table. Circle and connect the points.

4. Given the statement: The unknown solid is either sodium hydroxide or lithium bromide, and both of these compounds dissolve in water exothermically.

a Explain how the experimental data support the statement.


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b State specific information from Reference Table I to support the statement.


Step 1: In a laboratory investigation, a 50.0-gram sample of copper is at 100.0°C in a boiling water bath.

Step 2: A Styrofoam cup with a lid is used as a calorimeter. The cup contains 100.0 grams of distilled water at 23.2°C.

Step 3: The hot copper is poured into the cup of water, and the cup is quickly covered with the lid.

Step 4: A thermometer is inserted through the lid. The copper and water are gently stirred in the cup. The temperature is checked periodically. The highest temperature noted is 26.3°C.

5. In terms of energy flow, explain why the temperature of the water in the calorimeter increases.

6. Using the information given, complete the data table below.

7. Show a correct numerical setup for calculating the number of joules of heat gained by the water.

8. In this investigation, the change in heat of the copper is greater than the change in heat of the water. What error could account for this apparent violation of the Law of Conservation of Energy? Do not use human error as part of the answer.

Base your answers to questions 9 through 12 on the information below. A substance is a solid at 15°C.

A student heated a sample of the solid substance and recorded the temperature at one-minute intervals in the data table below.

9. On a graph, plot the data from the data table. Circle and connect the points.


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10. Based on the data table, what is the melting point of this substance?

11. What is the evidence that the average kinetic energy of the particles of this substance is increasing during the first three minutes?

12. The heat of fusion for this substance is 122 joules per gram. How many joules of heat are needed to melt 7.50 grams of this substance at its melting point?

Part VIII:

1. Base your answers on the following information below. A hot pack contains chemicals that can be activated to produce heat. A cold pack contains chemicals that feel cold when activated.

a. Based on energy flow, state the type of chemical change that occurs in a hot pack.

b. A cold pack is placed on an injured leg. Indicate the direction of the flow of energy between the leg and the cold pack.

c. What is the Law of Conservation of Energy? Describe how the Law of Conservation of Energy applies to the chemical reaction that occurs in the hot pack.


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2. In which equation does the term "heat" represent heat of fusion?

(1) NaCl(s) + heat → NaCl(l) (2) H2O(l) + heat → H2O(g) (3) NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l) + heat (4) H2O(l) + HCl(g) → H3O+(aq) + Cl-(aq) + heat

3. Which type of change must occur to form a compound?

(1) chemical (2) physical (3) nuclear (4) phase change

4. Based on Reference Table I, which change occurs when pellets of solid NaOH are added to water and stirred?

(1) The water temperature increases as chemical energy is converted to heat energy.

(2) The water temperature increases as heat energy is stored as chemical energy.

(3) The water temperature decreases as chemical energy is converted to heat energy.

(4) The water temperature decreases as heat energy is stored as chemical energy.

5. Which statement describes a chemical property that can be used to distinguish between compound A and compound B?

(1) A is a blue solid, and B is a white solid. (2) A has a high melting point, and B has a low melting point. (3) A dissolves in water, and B does not dissolve in water. (4) A does not burn in air, and B does burn in air.

6. An example of a physical property of an element is the element’s ability to

(1) react with an acid (2) react with oxygen (3) form a compound with chlorine (4) form an aqueous solution

physical behavior of matter unit regents review -...

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