UNIT 1: Matter and Energy
Part A: Classification of Matter
Big Picture Ideas:
  1. All matter has identifiable characteristics that can be used for classification purposes.
  2. All changes in matter are accompanied by a change in energy.
Big Picture Questions:
  1. o How can a substance’s properties be used to classify it and separate it from other substances?
  2. How does energy govern the state and properties of matter?

Suggested Resources…
Homework Assignments
Classwork Assignments
Laboratory Activities
Formative Assessments
Textbook pages: Chapter 2
Key Terms:
1. matter
2. solid
3. liquid
4. gas
5. plasma
6. physical property
7. chemical property
8. physical change
9. chemical change
10. law of conservation of matter
11. element
12. compound
13. pure substance
14. mixture
15. heterogeneous mixture
16. homogeneous mixture
17. energy
18. kinetic energy
19. potential energy
20. radiant energy
23 law of conservation of energy
24. Kelvin scale
25. Celsius scale
26. Fahrenheit scale
27. absolute zero
28. distillation
29. crystallization
30. chromatography
31. filtration

Directions: Use this information as a general reference tool to guide you through this unit. Don’t hesitate to ask your teacher for help!
By the conclusion of this unit, you should know the following:
  1. Chemistry is the study of matter and the changes it can undergo.
  2. Lab safety rules must be followed.
  3. Matter can exist in different phases and energy changes occur during phase changes.
  4. Changes in matter can be classified as either physical or chemical changes.
  5. Separation techniques can be employed to determine the components of a mixture.
  6. Energy exists in different forms (kinetic/potential/radiant) and can be converted from one form to another.
  7. Temperature is a measurement of the average kinetic energy of a substance.
  8. Heat is energy which travels from a hot object to a cold object.
/ By the conclusion of this unit, you should be able to do the following:
  1. Define chemistry and matter.
  2. Apply knowledge of proper laboratory safety.
  3. Classify different types of matter using a substance’s physical and chemical properties, states of matter and the physical and chemical changes the substance could undergo.
  4. Describe how different separation techniques can be used to distinguish between substances in a mixture.
  5. Classify examples of different forms of energy.
  6. Differentiate between temperature and heat.

Practice Problems:

Part 1: Indicate which of the following is an element (E), a compound (C), heterogeneous mixture (H), or solution (S).

1. ocean water7. aftershave lotion

2. calcium8. a hamburger

3. vitamin C (ascorbic acid)9. aluminum foil

4. dry ice (solid CO2)10. milk

5. copper11. table salt (NaI or NaCl)

6. grain alcohol12. iron nail

Part 2: Classify the following as a chemical property or a physical property

1. reacts with H2O7. is ductile

2. is red8. is flammable

3. conducts electricity9. is 1.5 m long

4. resists corrosion10. is malleable

5. boils at 88 oC11. is corrosive

6. dissolves in gasoline12. freezes at – 17 oC

Part 3: Classify each as a physical change or a chemical change

1. alcohol evaporating5. an explosion

2. a firefly (lightening bug)6. salt dissolving in water

lighting up7. digesting food

3. a battery charging8. hammering hot iron into a sheet

4. ice melting9. paper burning

INTRODUCTION TO CHEMISTRY

Chemistry-

Matter-

States of Matter:

Group Activity: Classification of Matter

  1. Discuss the terms “element”, “compound” and “mixture” with your group. Write down your group’s definition for each in the space provided below. Include the terms “atom”, “molecule” and “chemical bond” where appropriate.

Element:

GROUP:

CLASS:

Compound:

GROUP:

CLASS:

Mixture:

GROUP:

CLASS:

2. Study petri dishes A-F. Each nut, bolt or washer represents an atom. Determine whether each dish contains atoms or moleclues. Then determine whether each represents an element, a compound or a mixture. If it contains an element or compound, the sample is a substance. If it contains a mixture, it is not a substance.

Petri Dish / Atom, molecule
or both are present / Contents represent a(n) element, mixture or compound / Contents: substance or NOT substance
A
B
C
D
E
F

3. Use your understanding of elements, compounds and mixtures to classify each of the following:

  1. hydrogen: ______d. ammonia (NH3) ______
  1. sugar: ______e. ocean water: ______
  1. orange juice: ______f. silver: ______

4. Mixtures can be homogeneous or heterogeneous. Use the examples given in class to define “homogeneous mixture” and “heterogeneous mixture”.

Homogeneous mixture:

Heterogeneous mixture:

CLASSIFICATION OF MATTER

Determine whether each example or property below is a pure substance. Then label each as an “element” (E), “compound” (C), homogeneous mixture (HO) or Heterogeneous Mixture (HE). Use your own examples to complete the chart.

Substance? / Example / E, C, HO or HE?
1. sand
2. salt
3. pure water
4. tap water
5. aluminum
6. gasoline
7. soda
8. an egg
9. sugar
10. copper
11. steel
12. nitrogen
13. air
14. particles combine in any proportion
15. appears like one substance, but shows two different boiling points
16. only separable by a chemical reaction
17. / homogeneous mixture
18. / element
19. / compound
20. / heterogeneous mixture

MATTER, PHYSICAL /CHEMICAL PROPERTIES & CHANGE

States of Matter:

SOLID / LIQUID / GAS

CHEMICAL AND PHYSICAL PROPERTIES

1. Properties of Substances A and B.

SAMPLE A / SAMPLE B

Physical Property:

Chemical Property:

Identify the following as Physical or Chemical Properties:

the pigment is blue ______

sodium reacts violently with water______

wax melts at 82°C______

iron rusts when left out in the rain______

oil floats on water______

Physical Change:

Chemical Change:

Identify the following as Physical or Chemical Changes:

CO2 is released when alka seltzer is added to water ______

Salt dissolving in water ______

Baking cookies______

Burning coal______

PHYSICAL VS. CHEMICAL

Label each property below as physical (P) or chemical (C):

_____ 1. moth balls vaporize in the closet_____6. Butter melts at 30°C

_____ 2. Hydrofluoric acid attacks glass_____ 7. Sugar dissolves in water

_____ 3. Chlorine gas liquefies at -35°C_____ 8. Paint dissolves in acetone

_____ 4. Hydrogen gas burns in chlorine gas_____ 9. Baking soda fizzes with acid

_____ 5. Hydrogen gas pours “up” because it is lighter than air

Determine whether each change below is physical (P) or chemical (C).

_____ 1. Perfume evaporating on your skin_____ 5. Wood rotting

_____ 2. Autumn leaves changing color_____ 6. Melting copper metal

_____ 3. Burning sugar_____7. Baking a cake

_____ 4. Fogging a mirror with your breath_____ 8. Slicing potatoes for fries

Classify each term below as physical (P) or chemical (C).

_____ 1. Boil_____ 6. Melt

_____ 2. Burn (combustion)_____ 7. Bake

_____ 3. Evaporate _____ 8. Tarnish

_____ 4. Dissolve_____ 9. React

_____ 5. Rust_____10. Freeze

Physical/Chemical Properties/Changes

I. Fill in the Blanks

______properties can be observed without chemically changing matter. ______properties describe how a substance interacts with other

substances. ______have definite shapes and definite volumes.

______have indefinite shapes and definite volumes. ______have indefinite shapes and indefinite volumes.

Phase changes are ______changes. ______point is the

temperature at which a liquid turns to a solid. It is also equal to the

______point which is the temperature at which a ______turns

to a ______. ______point is the temperature at which a liquid

turns to a gas, and ______point is the temperature at which a gas turns

to a liquid. Occasionally, a solid turns directly into a gas without turning into a

liquid first. This is called _sublimation____.

II. Label these properties as chemical (C) or physical (P). Be certain to know thedefinition of each of these properties.

_____ combustibility _____density_____malleability

_____tendency to corrode _____failure to react _____ melting point

_____ ductility _____ odor _____ texture

_____ flammability

III. Label these changes as chemical (C) or physical (P).

_____ digestion of food _____ explosions_____ getting a haircut

_____ lighting a candle _____evaporation _____ tarnishing silver

_____ ice cube melting _____ formation of acid rain

_____ crushing rocks _____ dissolving salt in water
SEPARATION OF COMPOUNDS AND MIXTURES

  1. sand, salt and water
  1. water and rubbing alcohol

3. salt and pepper (demonstration)

4. C from H and O in sugar (demonstration)

SEPARATION OF MIXTURES VOCABULARY

1. filtration

  1. crystallization
  1. chromatography
  1. distillation

MATTER & ENERGY

Energy:

potential energy:

examples:

kinetic energy:

examples:

Units of Energy:

Temperature:

Units:

Celsius:

Kelvin:

Absolute zero:

Law of Conservation of Energy:

Law of Conservation of Matter:

Example: Mg + Oxygen  Ash

_____ + _____ ______

a. If 10.0g of magnesium metal burns in air, and reacts with 6.6g of oxygen, what mass of ash will form?

b. If 25g of magnesium metal burn in air, 41.5g of ash are formed. What mass of oxygen reacted with the magnesium?

Try: Sodium (Na) reacts with potassium chloride (KCl) to produce potassium (K) and sodium chloride (NaCl).

Na + KCl  NaCl + K

______ ______

If 20g of sodium (Na) reacts with 30.g of potassium chloride (KCl) and 15g of potassium (K) are produced, find the mass of sodium chloride (NaCl) also produced.

LAB ASSIGNMENT: SEPARATION OF A MIXTURE

LAB ACTIVITY A: (Maximum Score: 30/30)

  1. Your group will be given a mixture containing sand, salt, rubbing alcohol, iron filings and water. You must collect pure samples of each component by the end of class.
  2. Your group will be given permanent markers, wet-erase markers, water and rubbing alcohol. You must show the separation of ink into its components using chromatography.

LAB ACTIVITY B (Maximum Score: 27/30)

  1. Your group will be given two mixtures. One contains water and rubbing alcohol. The other contains iron filings, sand and salt. You must collect pure samples of each component by the end of class.
  2. Your group will be given permanent markers, wet-erase markers, water and rubbing alcohol. You must show the separation of ink into its components using chromatography.

LAB REPORT:

A. PRE-LAB:

1. Set up a Google Docs account if you do not already have one.

2. Have a group member create a document entitled: Separation of a Mixture and share with the rest of the group members. Share with me at and Ms. Rosenzweig at . (periods 5 & 6 ONLY).

3. Your group will assign you one of the following separation techniques to research: distillation, filtration, crystallization or chromatography.

a. Research the method you are assigned. You can use your textbook, YouTube or any other source.

Watching at least one YouTube of your procedure is strongly recommended.

b. Write a step-by-step procedure that your group can follow in lab tomorrow. Include lab safety tips! It can be typed directly into the Separation of a Mixture document; however, you will need a print copy in lab tomorrow.

4. Discuss the order of the separation with your group. (Discussion can be done in class or on Google Docs).

B. LAB WORK: All group members should participate in each step of the procedure.

C. OBSERVATIONS:

Create a chart for your observations in your Separation of a Mixture document. Use the computer at your lab station. Record your observations as the experiment progresses.

D. LAB EQUIPMENT:

In your Separation of a Mixture document -

1. Name each piece of lab equipment used.

2. Import a picture of each piece of equipment.

E. VERIFY THE RESULTS. ANSWER TEACHER “GROUP” QUESTIONS CORRECTLY:

1. Do not throw out any component of the mixture until the end of lab.

2. Each group member must be prepared to answer questions on ANY part of the lab procedure.

F. ANSWER CONCLUSION QUESTIONS. Questions can be answered directly in the Separation of a Mixture document.

CONCLUSION QUESTIONS:

1. Identify one element, one compound and one homogeneous mixture that was present in your lab.

2. How could you prove that the alcohol you separated from your mixture was pure?

3. Why is dissolving considered a “physical change”?

4. Read the section on hydrocarbons on pages 782-783 in your textbook. Then describe fractional distillation. How does it work? What are the products? Why is cracking necessary?

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