CHEMISTRY SCAVENGER HUNT

Pre-AP Chemistry Unit 3 HW Packet

Name _____________________________

WKS 3.1 - Classifying Matter (2 pages)

Complete the blank labels in the diagram below.

Temperature (K)

Pressure (

atm

)

195.42

405.38

0.05997

111.5

1.0

239.8

Temperature (K)

Pressure (

atm

)

195.42

405.38

0.05997

111.5

1.0

239.8

State whether each of the following is a homogeneous mixture, heterogeneous mixture, compound, or an element. Explain how you made your decision in each case.

Element, Compound, Homogeneous Mixture, or Heterogeneous Mixture

Explanation supporting decision

1.

hydrogen

2.

table salt

3.

sugar water

4.

carbon dioxide

5.

ketchup

6.

pure air (tricky!)

7.

water

8.

soil

9.

70% rubbing alcohol

10.

iron

11.

rocky road ice cream

WKS 3.1 - Classifying Matter (continued)

12. How can one tell the difference between a colloid and suspension?

13. How can one tell the difference between a solution and a colloid?

14. What are some examples of physical separation?

15. For each type of mixture draw a picture representing the size and distribution of particles in a liquid.

SOLUTIONCOLLOIDSUSPENSION

16. Lupita states that blood is a heterogeneous mixture while Sven states that blood is a heterogeneous mixture. Who is correct in this argument? Design an experiment that would defend your argument.

17. Compare and contrast a mixture and a compound. How are they alike? How are they different?

18. A chemist heats some white crystals in a test tube. The crystals make a cracking sound, fall apart into smaller pieces, and give off a misty gas. A colorless liquid forms around the cooler top of the test tube. Tell whether you think the crystals are a compound or an element, and why.

WKS 3.2 – Chemical vs. Physical Properties (1 page)

Classify the following properties as either chemical or physical (write out the whole word) and then justify your answer with an explanation.

Physical or Chemical Property

Explanation supporting your decision

1. Blue color

2. Density

3. Flammability

4. Solubility

5. Reacts with acid to form H2

6. Supports combustion

7. Odor

8. Melting point

9. Reacts with water to form a gas

10. Luster

11. Boiling point

12. Can neutralize a base

Physical properties can be further broken down into two types – INTENSIVE & EXTENSIVE. Be sure to write out the whole word. It will be VERY helpful to you in the future to know this because IF a property is INTENSIVE, then we can safely assume any convenient amount we want!

Intensive or Extensive

Explanation supporting your decision

13. Mass

14. Number of atoms

15. Color

16. Odor

17. Melting point

18. Density

19. Malleability

20. Volume

21. Length

22. Electrical Conductivity

WKS 3.3 – Chemical vs. Physical Changes (1 page)

In a physical change, the original substance still exists. It has only changed in form. In a chemical change, a new substance is produced. Classify the following as being a physical or chemical change. If it is chemical, state what evidence(s) of a chemical change would be seen in the example.

1. Sodium hydroxide dissolves in water. ____________________________________________________________

2. Hydrochloric acid reacts with potassium hydroxide to produce a salt, water and heat. ______________________

3. A pellet of sodium is sliced in two. ______________________________________________________________

4. Water is heated and changed to steam. ___________________________________________________________

5. Potassium chlorate decomposes to potassium chloride and oxygen gas. __________________________________

6. Iron rusts. __________________________________________________________________________________

7. When placed in H2O, a sodium pellet catches on fire as hydrogen gas is liberated and sodium hydroxide forms.

__________________________________________________________________________________________

8. Evaporation. ________________________________________________________________________________

9. Ice melting. _________________________________________________________________________________

10. Sugar dissolves in water. ______________________________________________________________________

11. Wood rotting. _______________________________________________________________________________

12. A tire is inflated with air. ______________________________________________________________________

13. Food is digested by hydrochloric acid in the stomach. _______________________________________________

14. Water is absorbed by a paper towel. _____________________________________________________________

15. Breaking a piece of glass with a hammer. ________________________________________________________

16. Milk is left outside of a refrigerator for seven months and spoils. ______________________________________

17. Dew forms on trees leaves from condensation. ____________________________________________________

18. Water is purified by a process of filtration. _______________________________________________________

19. Leaves changing color in the autumn. ___________________________________________________________

20. A student fries an egg for a yummy breakfast. _____________________________________________________

21. Fermenting of cider. __________________________________________________________________________

22. Burning wood. ______________________________________________________________________________

23. Silver tarnishing. ____________________________________________________________________________

WKS 3.4 – States of Matter (2 pages)

1. What are the differences between intramolecular bonding and intermolecular forces?

2. For each of the following, indicate if it represents a solid, liquid, or gas.

SOLID

LIQUID

GAS

Definite volume, definite shape

Molecules organized in set pattern

Molecules far apart

Least dense

Strongest intermolecular interactions

Diffuses an immeasurable amount

Easily compressed

Definite volume, no definite shape

Incompressible

Diffuse easily but slowly

Most dense

Molecules close, but have free motion

No intermolecular interactions

No definite shape, no definite volume

Vibrations only of molecules

Diffuse easily and quickly

3. Match the pictures with the following descriptions.

4. Compare and contrast the motion of particles of solids, liquids, and gases.

5. Gases and liquid are both fluids; they can flow. What is different about the intermolecular forces of attraction between the phases that allows fluids and gases to flow, but prevent solids from flowing?

WKS 3.4 – States of Matter (continued)

6. For each phase transition listed in the center column, draw and arrow from the beginning phase, through the transition, to the ending phase. The first is done for you.

Gas

Sublime

Gas

Freeze

Liquid

Boil

Liquid

Condense

Solid

Deposition

Solid

Melt

7. For each of the six phase changes, which ones are considered endothermic (taking in heat)? Which ones are considered exothermic (releasing heat)?

8. Why do ice cubes shrink if left in the freezer for a long time? Why do moth balls disappear? (Hint: the same thing is happening in both cases.)

9. Your breath contains water vapor. Why does it look like smoke in cold weather? Explain this using phase changes.

10. Energy is added to a solid substance at a constant rate. The temperature of the substance rises for a while, but a point is reached at which the temperature does not rise. At this point, what is happening to the substance? Describe what is happening to the energy being supplied to the solid during this time.

11. Distinguish between evaporation and vaporization.

WKS 3.5 – Heating/Cooling Curves (1 page)

The graph below shows a pure substance which is heated by a constant source of heat supplying 2000.0 joules per minute. Identify the area described in the questions below and complete the necessary calculations.

UV = 0.36 min, VW = 3.6 min, WX = 3.6 min, XY = 19.4 min, YZ = 0.6 min (2000.0 joules applied per minute)

1. Being warmed as a solid __________________

2. Being warmed as a liquid _________________

3. Being warmed as a gas ___________________

4. Changing from a solid to a liquid ___________

5. Changing from a liquid to a gas ____________

6. States present from V to W? ____________________

7. Sates present from X to Y? _____________________

8. What is its boiling temperature? _________________

9. What is its melting temperature? _________________

10. How many joules were needed to change the liquid to a gas? ____________

11. Where on the curve do the molecules have the highest kinetic energy? ________

12. What happened to the temperature during a phase change? WHY?

===============================================================================

Identify the following phase transition and write it on the first line. On the second line, indicate whether energy belongs on the product side or the reactant side of the equation.

Phase transition

Energy side

13. _________________, __________________ CH3CH2OH (l) ( CH3CH2OH (g)

14. _________________, __________________ Al (l) ( Al (s)

15. _________________, __________________ I2 (s) ( I2 (g)

16. _________________, __________________ W (s) ( W (l)

17. _________________, __________________ N2 (g) ( N2 (l)

WKS 3.6 – Phase Diagram (1 page)

Answer the following questions regarding the phase diagram of ammonia.

1. Label the solid, liquid, and gas phases on the above chart.

2. Use arrows to label and indicate the following phase changes:

a. Melting

b. Freezing

c. Vaporization

d. Condensation

e. Sublimation

f. Deposition

3. What is the triple point of ammonia? ____________________________

4. What phase(s) are present at the triple point? ____________________________

5. If ammonia is compressed from 0.005 atm to 0.995 atm at a constant temperature of 230 K, what phase change is observed? ____________________________

6. If ammonia heated from 25 K to 195.42 K at a constant pressure of 0.025 atm, what phase change is observed? ____________________________

7. If a substance’s pressure and temperature are found to fall “on the line”, we would say that substance is in a phase equilibrium. What is the definition of equilibrium?

WKS 3.7 – Review – Part One (1 page)1.Identify each of the following as intensive or extensive.

a.melting point_____________________c.density_____________________

b.mass_____________________d.length_____________________

2."Properties are not affected by changes in temperature and pressure." Is this statement true or false? EXPLAIN!

3.Classify each of the following as either solid, liquid, or gas at room temperature.

a.milk_____________________d.helium_____________________

b.air_____________________e.diamond_____________________

c.candle wax_____________________f.copper_____________________

4.Classify each of the following as a physical property (PP) or a chemical property (CP).

a.aluminum has a silvery color ________ d.water boils at 100°C

________

b.gold has a density of 19.3 g/cm3 ________ e.sodium ignites when dropped in water________

c.silver tarnishes ________ f.mercury is a liquid at room temperature________

5.Classify each of the following as a physical change (PC) or a chemical change (CC)

a.breaking a pencil in two________d.burning wood

________

b.water freezing and forming ice________e.leaves turning color in the fall________

c.frying an egg

________f.water evaporating

________

6.Is a change in phase a physical change or chemical change? EXPLAIN!

7.List four indicators that a chemical change has probably taken place.

a.________________________________c.___________________________________

b.________________________________d.___________________________________

8.Describe the difference between a chemical change and a physical change.

9."A mixture is a chemical bonding of two or more substances in any proportion". Is this statement true or false? EXPLAIN!

WKS 3.8 – Review – Part Two (1 page)

1.Describe how a homogeneous mixture differs from a heterogeneous mixture.

2.Identify each of the following as an example of a physical property (PP) or a chemical property(CP).

a.Silver tarnishes when it comes in contact with hydrogen sulfide in the air

________

b.A sheet of copper can be pounded into a bowl.

________

c.Barium melts at 725°C.

________

d.Helium does not react with any other element.

________

e.A bar of lead is more easily bent than is a bar of aluminum of the same size.

________

f.Potassium metal is kept submerged in oil to prevent contact with oxygen or water._________

g.Diamond dust can be used to cut or grind most other materials.

________

3.Identify each of the following as a property of a solid, liquid, or gas. Some answers will include more than one state of matter.

a.flows and takes the shape of its container________________

b.compressible

________________

c.made of particles held in a specific arrangement________________

d.has a definite volume

________________

e.always occupies the entire space of its container________________

f.has a definite volume but flows

________________

4.Identify each of the following as an example of a element (ELE), a compound (COMP), homogeneous mixture (HOM) or a heterogeneous mixture (HEM).

a.70% isopropyl rubbing alcohol________h.salt water

________

b. aluminum foil

________i.concrete

________

c. gasoline

________j.bread

________

d. sucrose (table sugar) ________ k. a pile of rusty filings ________

e. a diamond ________ l. hydrogen in a balloon ________

f. fruit salad

________ m. air in a balloon ________

g. carbon dioxide ________ n. dirt ________

5.Can two different samples of the same substance have different physical properties? Can they have different chemical properties? Explain your answers to both questions.

Diatomic Gas

Liquid

Solid

Liquid with Diatomic Gas

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