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 water 7. aftershave lotion
2. calcium 8. a hamburger
3. vitamin C (ascorbic acid) 9. aluminum foil
4. dry ice (solid CO2) 10. milk
5. copper 11. table salt (NaI or NaCl)
6. grain alcohol 12. iron nail
Part 2: Classify the following as a chemical property or a physical property
1. reacts with H2O 7. is ductile
2. is red 8. is flammable
3. conducts electricity 9. is 1.5 m long
4. resists corrosion 10. is malleable
5. boils at 88 oC 11. is corrosive
6. dissolves in gasoline 12. freezes at – 17 oC
Part 3: Classify each as a physical change or a chemical change
1. alcohol evaporating 5. an explosion
2. a firefly (lightening bug) 6. salt dissolving in water
lighting up 7. digesting food
3. a battery charging 8. hammering hot iron into a sheet
4. ice melting 9. 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, moleculeor 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:
a. hydrogen: ______d. ammonia (NH3) ______
b. sugar: ______e. ocean water: ______
c. 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 / GASCHEMICAL AND PHYSICAL PROPERTIES
1. Properties of Substances A and B.
SAMPLE A / SAMPLE BPhysical 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 the definition 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
2. water and rubbing alcohol
3. salt and pepper (demonstration)
4. C from H and O in sugar (demonstration)
SEPARATION OF MIXTURES VOCABULARY
1. filtration
2. crystallization
3. chromatography
4. 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 à Ash
_____ + _____à ______
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 à NaCl + K
______à ______
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)
3. 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.
4. 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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