Part 1, Unit 1: Matter - fabzchem.weebly.comfabzchem.weebly.com/uploads/5/8/3/3/58332297/sg1.1_… · Web viewChanges to Matter. I Define and distinguish between physical change

Part 1, Unit 1: Matter

Unit 1 Performance ObjectivesUnit 1 Performance ObjectivesProperties of Matter

I Define and distinguish between physical property and chemical property.I Recognize and give examples of physical and chemical properties.I Define and distinguish between intensive property and extensive property.I Recognize and give examples of intensive and extensive properties.I I Group given properties as physical or chemical, extensive or intensive.I Define and distinguish between mass and weight.I Define density.I I List the chemical and physical properties of several common pollutants.I I I Relate the properties of matter to the steps in such processes as water treatment, metal ore refining, oil

refining, paper recycling, or aluminum recycling.I I Compare and contrast the properties of easily recycled materials with those of difficult-to-recycle

materials.I I Speculate on the physical and chemical properties of substances that would reduce evaporative water

loss from reservoirs in arid regions.

Changes to MatterI Define and distinguish between physical change and chemical change.I Recognize and give examples of physical and chemical changes.I List clues that a chemical change has occurred.I I Observe and classify changes as either physical or chemical, and justify assertions with observations.I I State the Law of Conservation of Mass and apply it to common physical and chemical processes.

States, Phases, and SystemsI Define and distinguish between system and surroundings.I Define interface, phase, and state.I I For a given system, name or describe all phases and interfaces.I I Distinguish between phase and state.I I Relate phase and interface to the three common states of water.I I Explain why states of matter are not as useful as phases in describing earth’s materialsI I Explain at least one method of separating a mixture using phase differences.I I Design and explain a method of separating parts of a coarse mixture of earth materials.I I Design a method for separating parts of any unknown mixture.

Classification of MatterI Define matter and apply it to the materials in a chemical reaction.I Define and distinguish between substance and mixture.I Recognize, and give examples of pure substances and mixtures.I Define and distinguish between homogeneous and heterogeneous .I Recognize and give example of homogeneous and heterogeneous materials.I Define and distinguish between element, compound, solution, colloid, and crude mixture.I Recognize and give examples of elements, compounds, solutions, colloids, and crude mixtures.I I Reproduce the classification scheme for matter based on homogeneity and purity.I I Group related vocabulary to show mutually exclusive terms when applied to classifying matter.I I Classify common materials as elements, compounds, solutions, colloids, or coarse mixtures, and justify

this classification based on purity and particle size.I I I Differentiate between types of colloidal materials based on phases present and particle size.

Matter and EnergyI Define and distinguish between kinetic energy and potential energy.I Recognize and give examples of chemical energy.I List clues that an energy change has occurred.I I State the Law of Conservation of Energy and apply it to common physical and chemical processes.

Part 1, Unit 1 Study Guide: Page 1

I I Differentiate between ordinary chemical and physical processes and nuclear reactions in terms of the energy involved.

I I Define and distinguish between an exothermic process and an endothermic process.


Unit 1 Vocabulary ListUnit 1 Vocabulary ListProperties of Matter

chemical propertiesdensityextensive physical propertiesintensive physical propertiesmassphysical properties

temperaturevolume

weight

Changes to Matteracts uponchemical changeLaw of Conservation of Massphysical change

States, Phases, and Systemsinterfacephasestate (state of matter)

surroundingssystem

Classification of Mattercolloidcompoundcrude (coarse) mixtureelementheterogeneous materialhomogeneous materialinorganic material

materialmatter

mixtureorganic materialsolutionsubstancesuspension

Matter and Energychemical energyendothermic processexothermic processkinetic energyLaw of Conservation of Energypotential energy



Properties Of MatterProperties Of Matter

In Column A, write M for Measurement or O for Observation for each of the properties below. In Column B, write C if it is a Chemical Property, IP if it is an Intensive Physical Property, and EP if it is an Extensive Physical property.

Data

1. Color

2. Temperature

3. Tendency to oxidize in air

4. Malleability/brittleness

5. Tendency to corrode

6. Hardness

7. Volume

8. Odor

9. Inertia

10. Density

11. Acidity

12. Combustibility

13. Mass

14. Heat Content

15. Streak

16. Conductivity of heat

17. Ease in initiating reaction

18. Melting/Boiling point

19. State

20. ConcentrationColumn A


1. ___________

2. ___________

3. ___________

4. ___________

5. ___________

6. ___________

7. ___________

8. ___________

9. ___________

10.___________

11.___________

12.___________

13.___________

14.___________

15.___________

16.___________

17.___________

18.___________

19.___________

20.___________

Column B

1. ___________

2. ___________

3. ___________

4. ___________

5. ___________


6. ___________

7. ___________

8. ___________

9. ___________

10.___________

11.___________

12.___________

13.___________

14.___________

15.___________

16.___________

17.___________

18.___________

19.___________

20.___________


Part 1, Unit 1: MatterProperties Of Matter, Cont.

In Column A, write QT for Quantitative data or QL for Qualitative data for each of the examples below. In Column B, write C if the data is about a Chemical Property, IP for an Intensive Physical Property, and EP for an Extensive Physical property.

Data

1. 27.6 °C

2. Stinks of rotten eggs

3. Turns black when exposed to air

4. Can be scratched by quartz (SiO2)

5. Burns readily

6. 17.85 grams

7. Freezes at 0.0 °C

8. 3.65 grams per cubic centimeter

9. 45 drops

10. Easily pounded into thin sheets

11. Inert with all common gases

12. Liquifies at 37.2 °C

13. Breaks down when heated

14. Solid

15. Electrical non-conductor

16. Readily reacts with acid

17. pH 8.2

18. Easily vaporized

19. Yellow

20. Formed from H2O & CO2


Column A

1. ___________

2. ___________

3. ___________

4. ___________

5. ___________

6. ___________

7. ___________

8. ___________

9. ___________

10.___________

11.___________

12.___________

13.___________

14.___________

15.___________

16.___________

17.__________

18.___________

19.___________

20.___________

Column B

1. ___________

2. ___________


3. ___________

4. ___________

5. ___________

6. ___________

7. ___________

8. ___________

9. ___________

10.___________

11.___________

12.___________

13.___________

14.___________

15.___________

16.___________

17.__________

18.___________

19.___________

20.___________



Changes to MatterChanges to Matter

Classify each of the changes listed below as physical or chemical.

1. Melting steel

2. Rusting

3. Burning paper

4. Cooling to room temperature

5. Corroding

6. Drying clothes

7. Baking bread

8. CO2 bubbles escaping from soda

9. Crushing ice

10. Using drain cleaner in the sink

11. Evaporating gasoline

12. Dissolving sugar in tea

13. Metabolizing food

14. Lighting a gas stove

15. Shaking up oil/vinegar salad dressing

16. Bleaching stains

17. Mixing water and alcohol

18. Setting concrete

19. Decomposing granite

20. Mixing epoxy glue

1. Physical Change Chemical Change






7. Physical Change Chemical ChangePart 1, Unit 1 Study Guide: Page 9















Part 1, Unit 1: MatterChanges to Matter, Continued

Classify each of the changes below as chemical or physical.

1. Going from 27.6 °C to 31.4 °C

2. Produces an odor of rotten eggs

3. Turns black when exposed to air

4. Scratched easily by quartz (SiO2)

5. Burns readily under water

6. When cut, material loses 17.85 grams

7. Freezes at 0.0 oC

8. Forms a thin wire only with difficulty

9. Add 45 drops more of the liquid

10. Easily pounded into thin sheets

11. Inert with all common gases

12. Liquifies at 37.2oC

13. Breaks down when heated

14. Explodes when touched

15. Electricity passes through easily

16. Readily reacts with acid

17. Bubbles are formed

18. Vaporized easily

19. Turns yellow upon standing

20. Decomposes into H2O and CO2








8. Physical Change Chemical ChangePart 1, Unit 1 Study Guide: Page 11















Properties/Changes Answer KeyProperties/Changes Answer Key

Answers to Page 31. Color O IP2. Temperature M IP3. Tendency to oxidize in air O C4. Malleability/brittleness O IP5. Tendency to corrode O C6. Hardness M IP7. Volume M EP8. Odor O IP9. Inertia M EP10. Density M IP11. Acidity M C12. Combustibility O C13. Mass M EP14. Heat Content M EP15. Streak O IP16. Conductivity of heat M IP17. Ease in initiating reaction O C18. Melting/Boiling point M IP19. State O IP20. Concentration M EP

Answers to Page 41. 27.6 °C QT IP2. Stinks of rotten eggs QL IP3. Turns black when exposed to air QL C4. Can be scratched by quartz (SiO2) QL IP5. Burns readily QL C6. 17.85 grams QT EP7. Freezes at 0.0 °C QT IP8. 3.65 grams per cubic centimeter QT IP9. 45 drops QT EP10. Easily pounded into thin sheets QL IP11. Inert with all common gases QL C12. Liquifies at 37.2 °C QT IP13. Breaks down when heated QL C14. Solid QL IP15. Electrical non-conductor QT IP16. Readily reacts with acid QL C17. pH 8.2 QT IP18. Easily vaporized QL IP19. Yellow QL IP20. Formed from H2O and CO2 QL C

Answers to Page 51. Melting steel Physical2. Rusting Chemical3. Burning paper Chemical4. Cooling to room temperature Physical5. Corroding Chemical6. Drying clothes Physical7. Baking bread Chemical8. CO2 bubbles escaping from soda Physical9. Crushing ice Physical10. Using drain cleaner in the sink Chemical11. Evaporating gasoline Physical12. Dissolving sugar in tea Physical13. Metabolizing food Chemical14. Lighting a gas stove Chemical15. Shaking up oil/vinegar salad dressing Physical16. Bleaching stains Chemical17. Mixing water and alcohol Physical18. Setting concrete Chemical19. Decomposing granite Chemical20. Mixing epoxy glue Chemical

Answers to Page 61. Going from 27.6 °C to 31.4 °C Physical2. Produces an odor of rotten eggs Chemical3. Turns black when exposed to air Chemical4. Scratched easily by quartz (SiO2) Physical5. Burns readily under water Chemical6. When cut, material loses 17.85 grams Physical7. Freezes at 0.0 oC Physical8. Forms a thin wire only with difficulty Physical9. Add 45 drops more of the liquid Physical10. Easily pounded into thin sheets Physical11. Inert with all common gases Chemical12. Liquifies at 37.2oC Physical13. Breaks down when heated Chemical14. Explodes when touched Chemical15. Electricity passes through easily Physical16. Readily reacts with acid Chemical17. Bubbles are formed Either One18. Vaporized easily Physical19. Turns yellow upon standing Chemical20. Decomposes into H2O and CO2 Chemical

Part 1, Unit 1 Study Guide, Page 13


Applying VocabularyApplying Vocabulary

Classifying PropertiesClassifying PropertiesThe passage below might have been taken from a technical encyclopedia or

handbook. Use it to show how well you can apply the vocabulary for the properties of matter. If you need to look up a term that is unfamiliar to you so that you can understand the passage, do so.

Distinguish between chemical properties, extensive physical properties, and intensive physical properties by highlighting each type in a separate color.

Include a key, so that someone else can check your work.

Uranium: U: atomic number 92; atomic mass 238.029 amu; oxidation states +3, +4, +5, and +6. A silver-

white, radioactive, metal that is softer than glass, it is malleable and ductile, and it can be polished. Melting

point is 1132.2oC and boiling point is 3818oC. Density is 19.05 g/cm3. The most common isotope is U-238,

with a half life of 4.51 x 109 years. Specific heat is 0.117 J/g. oC; heat of fusion is 12.1 kJ/mol and heat of

vaporization is 460 kJ/mol.

Uranium burns in air at 150-175 oC to form U3O8. When finely powdered, it reacts quickly with warm water

and more slowly with cold. It burns in fluorine to form the green, volatile material UF4; it reacts similarly in

chlorine and in gaseous bromine and iodine. It replaces hydrogen in acids, forming salts with an oxidation

state of +4. It does not react with alkali bases.

Abundance in the Earth’s crust is 2 x 10-5 percent by mass.


Vocabulary Differentiations IVocabulary Differentiations I

Differentiate between these. Do NOT write definitions. A valid format is “X does this, and Y does not.”

1. Matter vs. Energy

_______________________________________________________________________________

_______________________________________________________________________________

_______________________________________________________________________________

_______________________________________________________________________________2. Mass vs. Weight

_______________________________________________________________________________

_______________________________________________________________________________

_______________________________________________________________________________

_______________________________________________________________________________3. Chemical Properties vs. Physical Properties

_______________________________________________________________________________

_______________________________________________________________________________

_______________________________________________________________________________

_______________________________________________________________________________4. Extensive Properties vs. Intensive Properties

_______________________________________________________________________________

_______________________________________________________________________________

_______________________________________________________________________________

_______________________________________________________________________________5. Qualitative Information vs Quantitative Information

_______________________________________________________________________________

_______________________________________________________________________________

_______________________________________________________________________________

_______________________________________________________________________________


Vocabulary Differentiations IIVocabulary Differentiations II

Differentiate between these. Do NOT write definitions. A valid format is “X does this, and Y does not.”

1. Gases vs. Liquids and Solids

_______________________________________________________________________________

_______________________________________________________________________________

_______________________________________________________________________________

_______________________________________________________________________________2. Solids vs. Liquids and Gases

_______________________________________________________________________________

_______________________________________________________________________________

_______________________________________________________________________________

_______________________________________________________________________________3. State of Matter vs. Phase

_______________________________________________________________________________

_______________________________________________________________________________

_______________________________________________________________________________

_______________________________________________________________________________4. System vs. Surroundings

_______________________________________________________________________________

_______________________________________________________________________________

_______________________________________________________________________________

_______________________________________________________________________________


Recognizing Energy ChangesRecognizing Energy Changes

Classify each of the changes below as exothermic or endothermic.

1. Heating water from 27.6 °C to 31.4 °C

2. Frying eggs.

3. Burning wood.

4. Digesting lunch.

5. Cutting a board.

6. Freezing water.

7. Evaporating sweat during exercise.

8. Setting concrete.

9. Activating a light stick.

10. Nuclear fission.

11. Decomposing water by electrolysis.

12. Photosynthesizing sugar and oxygen.

13. Melting gold.

14. Exploding dynamite.

15. Connecting a battery so a flashlight bulb lights.

16. Creating friction by rubbing two sticks together.

17. Crushing a rock.

18. Colliding two marbles together.

19. Using a chemical cold pack.

20. Aging paper.

1. Exothermic Process Endothermic Process























Vocabulary Differentiations IIVocabulary Differentiations II

Differentiate between these. Do NOT write definitions.

1. Kinetic Energy and Chemical Potential Energy

_______________________________________________________________________________

_______________________________________________________________________________

_______________________________________________________________________________

_______________________________________________________________________________2. Exothermic Processes and Endothermic Processes

_______________________________________________________________________________

_______________________________________________________________________________

_______________________________________________________________________________

_______________________________________________________________________________3. Ordinary Chemical/Physical Processes and Nuclear Reactions

_______________________________________________________________________________

_______________________________________________________________________________

_______________________________________________________________________________

_______________________________________________________________________________


Classification Of MatterClassification Of MatterThe diagram below shows one way to classify matter. A completed version of this diagram can be found in

the text. Use this page as a study guide by filling in a diagram like it on another sheet of paper, filling in the names of each quadrilateral and giving at least three examples. When you have mastered the diagram, it might be useful to make this one complete.

The arrows to the left of the triangle and at its base indicate the classification method from top to bottom and from left to right. The endpoints of these arrows show the thinking that accompanies this classification scheme. Fill in the endpoints in the center of each arrow.

Matter

Part 1, Unit 1: MatterClassification Of Matter, Continued

The diagram below shows another way to classify matter, this one based on purity. Use this page as a study guide by filling in a diagram like it on another sheet of paper. When you have mastered the diagram, it might be useful to make this one complete. When completing the diagram, give the names for each rectangle and at least three examples for the rectangles at the bottom.

Part 1, Unit 1: MatterClassification Of Matter, Cont.

Choose words from the list below to fill in the blanks in the paragraphs at the bottom of the page.

Vocabulary Word List

compoundelementheterogeneous

homogeneousmassmixture

propertysolutionsubstance

Matter may be defined as something that has (1) ________________________ and that also takes up space. It is the stuff Chemistry studies. Matter can be classified in two useful ways, according to its uniformity and according to the types of materials it contains.

Anything that is completely uniform throughout is (2) ________________________ . To be classified as completely uniform, every region within the material must have the same (3) ______________________ as every other region. There are three types of material that may be completely uniform. Two are the pure materials called (4) ______________________ and (5) ______________________ , each of which has a very definite chemical make-up.

Some materials are NOT pure but are still uniform throughout, or (6) _____________________ . Such a material is a special type of (7) ______________________ called a (8) ______________________ , an example being salt water, which is composed of a solute (salt) and a solvent (water).

Some matter has regions with different (9) ________________________ from those in another region, such as the minerals in a rock or the toppings on a pizza. These (10) ________________________ are not uniform throughout and are known as (11) ________________________ matter.

Matter may also be classified by the types of materials it contains. A (12) ___________________ (pure material) cannot be separated into the parts that make it up by physical means. There are two types of such materials (13) __________________________ which may be broken down chemically into other pure materials, and (14) ________________________ , which may not be broken down into any simpler materials by ordinary chemical means.

The simplest of all materials are the 111 chemical (15) ______________________ . Putting two or more of these together in a chemical reaction gives materials known as (16) ______________________ . The size of the particles involved with these materials is the size of individual atoms or molecules. The uniform mixtures known as (17) ______________________ also have particles this same size. Because of this, even though the materials involved may have different properties when by themselves, there are no regions in the (18) -________________________ in which the (19) ________________________ are different from those in any other region.

When the particle size gets larger, the material is no longer (20) ______________________ , and thus there are regions that have different chemical or physical (21) ____________________ . These materials, such as dirt or rocks are called (22) ______________________ .

Part 1, Unit 1: MatterClassification Of Matter, Cont.

Circle the correct classification for the matter listed. There will be three circles per item.Pure water substance mixture homogeneous heterogeneous

element compound solution colloid suspension coarse mixture

Carbon substance mixture homogeneous heterogeneous


Filtered Air substance mixture homogeneous heterogeneous


Table Salt substance mixture homogeneous heterogeneous


Vinegar substance mixture homogeneous heterogeneous


Sandstone substance mixture homogeneous heterogeneous


Helium substance mixture homogeneous heterogeneous


Paint substance mixture homogeneous heterogeneous


A Leaf substance mixture homogeneous heterogeneous


Blood substance mixture homogeneous heterogeneous


Paper substance mixture homogeneous heterogeneous


Hair Gel substance mixture homogeneous heterogeneous


An Apple substance mixture homogeneous heterogeneous


A Copper Penny substance mixture homogeneous heterogeneous




Classifying Common MaterialsClassifying Common MaterialsUnit Vocabulary ApplicationUnit Vocabulary Application

Work ALONE the first time you do this activity. This is important for your learning.

In this applications activity, you will need to use the vocabulary words associated with the classification of matter. You are to apply your understanding of the terms by functionally distinguishing between substances and mixtures , between homogeneous and heterogeneous materials, and between elements, compounds, solutions, colloidal dispersions, suspensions, and coarse mixtures.

For the materials given, circle the one appropriate choice in each of the three sets of answers immediately below it.

1. distilled watera) Subst b) Mix f) Hom g) Het k) Elem l) Comp m) Soln n) Coll o) Suspen p)Cor Mix

2. Batavia tap watera) Subst b) Mix f) Hom g) Het k) Elem l) Comp m) Soln n) Coll o) Suspen p)Cor Mix

3. muddy water from the Fox Rivera) Subst b) Mix f) Hom g) Het k) Elem l) Comp m) Soln n) Coll o) Suspen p)Cor Mix

4. seawatera) Subst b) Mix f) Hom g) Het k) Elem l) Comp m) Soln n) Coll o) Suspen p)Cor Mix

5. oxygen gasa) Subst b) Mix f) Hom g) Het k) Elem l) Comp m) Soln n) Coll o) Suspen p)Cor Mix

6. the breath you exhalea) Subst b) Mix f) Hom g) Het k) Elem l) Comp m) Soln n) Coll o) Suspen p)Cor Mix

7. the air you breathe a) Subst b) Mix f) Hom g) Het k) Elem l) Comp m) Soln n) Coll o) Suspen p)Cor Mix

8. nickel steel alloya) Subst b) Mix f) Hom g) Het k) Elem l) Comp m) Soln n) Coll o) Suspen p)Cor Mix

9. shaving creama) Subst b) Mix f) Hom g) Het k) Elem l) Comp m) Soln n) Coll o) Suspen p)Cor Mix

10. celerya) Subst b) Mix f) Hom g) Het k) Elem l) Comp m) Soln n) Coll o) Suspen p)Cor Mix

11. quartz sanda) Subst b) Mix f) Hom g) Het k) Elem l) Comp m) Soln n) Coll o) Suspen p)Cor Mix


Part 1, Unit 1: MatterClassifying Common Materials, Cont.

12. diamonda) Subst b) Mix f) Hom g) Het k) Elem l) Comp m) Soln n) Coll o) Suspen p)Cor Mix

13. rock candy (crystallized sucrose)a) Subst b) Mix f) Hom g) Het k) Elem l) Comp m) Soln n) Coll o) Suspen p)Cor Mix

14. 2allbeefpatiespecialsauseletuscheezpicklesonionsonasesameseedbuna) Subst b) Mix f) Hom g) Het k) Elem l) Comp m) Soln n) Coll o) Suspen p)Cor Mix

15. mayonnaise (salad oil, eggs, vinegar, whipped together with some air)a) Subst b) Mix f) Hom g) Het k) Elem l) Comp m) Soln n) Coll o) Suspen p)Cor Mix

16. the sodapop inside a closed bottle before the cap has been opened (not the can)a) Subst b) Mix f) Hom g) Het k) Elem l) Comp m) Soln n) Coll o) Suspen p)Cor Mix

17. 2% milka) Subst b) Mix f) Hom g) Het k) Elem l) Comp m) Soln n) Coll o) Suspen p)Cor Mix

18. plain lime jelloa) Subst b) Mix f) Hom g) Het k) Elem l) Comp m) Soln n) Coll o) Suspen p)Cor Mix

19. 14K gold ring (no stone)a) Subst b) Mix f) Hom g) Het k) Elem l) Comp m) Soln n) Coll o) Suspen p)Cor Mix

20. graphite (the major ingredient in pencil lead)a) Subst b) Mix f) Hom g) Het k) Elem l) Comp m) Soln n) Coll o) Suspen p)Cor Mix

21. high-octane gasolinea) Subst b) Mix f) Hom g) Het k) Elem l) Comp m) Soln n) Coll o) Suspen p)Cor Mix

22. granitea) Subst b) Mix f) Hom g) Het k) Elem l) Comp m) Soln n) Coll o) Suspen p)Cor Mix

23. rust (iron oxide) a) Subst b) Mix f) Hom g) Het k) Elem l) Comp m) Soln n) Coll o) Suspen p)Cor Mix

24. motor oila) Subst b) Mix f) Hom g) Het k) Elem l) Comp m) Soln n) Coll o) Suspen p)Cor Mix

25. topsoila) Subst b) Mix f) Hom g) Het k) Elem l) Comp m) Soln n) Coll o) Suspen p)Cor Mix



Vocabulary Differentiations IIIVocabulary Differentiations III

Differentiate between these. Do NOT write definitions.

1. Matter and Energy

_______________________________________________________________________________

_______________________________________________________________________________2. Substances and Mixtures

_______________________________________________________________________________

_______________________________________________________________________________3. Heterogeneous Materials and Homogeneous Materials

_______________________________________________________________________________

_______________________________________________________________________________4. Elements and Compounds

_______________________________________________________________________________

_______________________________________________________________________________5. Solutions and Other Mixtures

_______________________________________________________________________________

_______________________________________________________________________________6. Colloids and Suspensions

_______________________________________________________________________________

_______________________________________________________________________________

_______________________________________________________________________________

_______________________________________________________________________________



This page is left blank for future expansion.



Content OutlineContent Outline

I.I. Characteristics of MatterCharacteristics of MatterA. Def.: Matter:

B. Characteristics all matter has:1. Def.: Mass:

2. Def.: Volume:

3. Def.: Inertia:

4. States of Matter

a. Def.: State of Matter:

b. List: States of Matter:

c. Ex. : States of Matter:

5. Phases

a. Def.: Phase:

b. Types of Phases:i. Def.: Continuous Phase:

ii. Def.: Dispersed Phase:

c. Examples of Phases:i. Same Phase, 2 different substances:

ii. Different Phases, the same substance:

d. Distinguish between phases and states of matter

6. Interfaces

a. Def.: Interface:

b. Chemical reactions take place at the interfaces between materials.

c. Ex.: Interfaces:


Part 1, Unit 1: MatterContent Outline, Cont.

II.II. Properties of MatterProperties of MatterA. Properties of matter are closely related to its structureB. Physical Properties

1. Def.: Physical Properties:

2. Types of Physical Properties

a. Extensive Propertiesi. Def.: Extensive Property:

ii. Ex.: Extensive Properties:

b. Intensive Propertiesi. Def.: Intensive Property:

ii. Ex.: Intensive Properties:

D. Chemical Properties1. Def.: Chemical Property:

2. Chemical properties include the chemical makeup of a material at the atomic/molecular level.

3. Chemical properties also describe the tendency toward reactions or LACK OF reactions with other substances or within itself.

4. Chemical properties are essentially invisible.

5. Ex.: Chemical Properties:



III.III. Changes to MatterChanges to MatterA. Physical Changes

1. Def.: Physical Change:

2. Ex.: Physical Changes:

B. Chemical Changes1. Def.: Chemical Change (Reaction):

2. For a chemical change to occur, bonds must be broken and new ones may be reformed.

3. Energy changes ALWAYS accompany chemical changes.

a. Chemical changes that release energy to the surroundings are exothermic, and those that take up energy from the surroundings are endothermic.

b. Energy must ALWAYS be used up to break chemical bonds

4. Ex.: Chemical Changes:

5. List.: Clues that a chemical change has occurred:

C. Distinguishing Between Chemical and Physical Changes

D. Law of Conservation of Mass (Matter)1. In ordinary chemical and physical processes in closed systems,

;

it is only changed in form.

2. After an ordinary chemical reaction, the products will have

as the reactants had before the reaction took place.

3. Mass is never converted to energy in ordinary chemical or physical processes, but only in

.



IV.IV. Classification of MatterClassification of MatterA. Classification of matter based on Uniformity

1. Homogeneous Materials

a. Def.: Homogeneous:

b. Ex.: Homogeneous materials:

2. Heterogeneous Materials

c. Def.: Heterogeneous:

d. Ex.: Heterogeneous materials:

3. Distinguish between homogeneous and heterogeneous materials

B. Classification Of Matter Based on Purity1. Substances:

a. Def.: Substance:

b. Types of Substances:i. Def.: Element:

ii. Ex.: Elements:

iii. Def.: Compound:

iv. Ex.: Compounds:

2. Mixtures:

a. Def.: Mixture:

b. List Mixture Types:

c. Different Mixture types are distinguished from one another by

3. Distinguish between substances and mixtures



4. Properties of Mixtures

a. Properties of Solutionsi. Homogeneous; any sample of the same solution will have uniform properties

ii. Different solutions of the same substances may be quite different in their compositions

iii. Only one phase because no separate regions exist

iv. Particles are < 1 nm in size, the size of atoms, molecules, or ions; invisible to opticalmicroscopes, but visible to electron tunnelling microscopes

b. Properties of Colloidsi. Heterogeneous

ii. Different colloidal dispersions of the same substances may be quite different in their compositions

iii. Must have at least two phases, the continuous phase and the dispersed phase

iv. Particles are > 1 nm but < 100 nm in size; invisible to optical microscopes, but visible toultramicroscopes

v. Not effected greatly by gravity and so the particles of the dispersed phase remainsuspended in the continuous phase

c. Properties of Suspensionsi. Heterogeneous, and they may be composed of mixtures themselves

ii. Different suspensions of the same materials may have different compositions and differentparticle sizes

iii. Must have at least two phases, the continuous phase and the dispersed phase

iv. Particles are > 100 nm in size; visible to optical microscopes and frequently the unaided eye

v. Effected by gravity and so the particles of the dispersed phase will settle or rise on standing,depending on their density compared to the that of the continuous phase, as long as thecontinuous phase is fluid enough.

d. Properties of Crude Mixturesi. Heterogeneous, and they may be composed of mixtures themselves

ii. Different crude mixtures of the same materials will probably have different compositions anddifferent particle sizes

iii. Must have at least two phases; the continuous phase is not necessarily fluid

iv. Particle size may be quite large.



V.V. Matter and EnergyMatter and EnergyA. Processes in nature tend toward lower energy states.B. Law of Conservation of Energy.

1. In ordinary chemical and physical processes in closed systems,

;

it is only changed in form.

2. After a chemical reaction, the products may have more or less potential energy (usually called heat content) than the reactants had before the reaction took place. Some energy must have been added or released to account for this difference, because the total amount of energy present has not changed.

3. Mass is never converted to energy in ordinary chemical or physical processes, but only in

.

C. Energy Changes Accompany Physical and Chemical Changes1. Changes that release energy to the surroundings are exothermic.

a. Any energy that is released is potential energy that was present before the change.

b. In a chemical reaction, the energy released as heat, light, sound, or mechanical energy was present in the reactants. The products have less heat content than the reactants, and the difference is the energy that was released.

c. Examples of exothermic processes.i. All combustion reactions, for example are exothermic. When burning wood, the energy released that creates

the warmth of the fire was present all the time in the wood. No energy was created.

ii. .

2. Changes that absorb energy from the surroundings are endothermic.

a. Energy must be supplied by the surroundings or the change will not take place.

b. Any energy that is added becomes potential energy after the change.

c. In a chemical reaction, the energy added as heat, light, sound, electrical, or mechanical energy will be added to the heat content of the products. The products will have more heat content than the reactants, and the difference is the energy that was added.

d. Examples of endothermic processes.i. Photosynthesis requires that light energy be present for the cholorphil in plants to convert the carbon dioxide

and water into oxygen and glucose. This provides the energy in glucose that the cells can use to do their work.

ii. .


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Part 1, Unit 1: Matter - fabzchem.weebly.comfabzchem.weebly.com/uploads/5/8/3/3/58332297/sg1.1_… · Web viewChanges to Matter. I Define and distinguish between physical change