Name: Answer KeyStandard 1 Students will understand the nature of CHANGES IN MATTER. Objective 1 A. Describe the chemical and physical properties of various substances.

Properties of Water Why Water is so Great…Name:________________________________Property Meaning Importance of Property

1. Transparency Light passes thru water.

Light reaches chloroplasts in cells & aquatic plants.

2. Universal Solvent

Many compounds dissolve in water.

Dissolved compounds can be transported in environment and life.

3. CohesionWater molecules stick together due to H bonds.

Small animals may walk on water.

4. Adhesion Water molecules stick to other molecules.

Capillary action. Water pulled to top of trees.

5. Heat CapacityLarge amounts of energy are needed to raise temp of water.

Water bodies have stable temperatures. Body temps can be maintained. Transfer of heat from warm to cool body parts.

6. High boiling point.

Much energy needed to pull water molecules apart.

In nature, water rarely boils so life is spared.

7. Density of IceIce is less dense than water so it floats because of rigid H- Bonds.

Ice insulates organisms living beneath.

8. Evaporation Evaporation (boiling) requires much energy.

Evaporation can cool warm cells.

Penny Experiment:How many drops of water could you put on your penny? Draw a picture of what your

penny looks like from the side.Example: 30

Balloon Experiment:What do you think will happen to the balloon with water in it if a match is put under it? It will explode

What happened when the match was put under it? Why?Nothing happened. The reason is because water has a high heat capacity. As a result, the water absorbed the heat from the match and did not allow it to pop.

St. 1 Obj. 1Differentiate between chemical and physical properties. Physical and Chemical Changes

For the notes to this page, please go through the Chem Phys Change ppt.Matter:- --The difference between Physical Property and Physical Change:-

-

Physical Change vs. Property-

-

What are some examples of physical change?

Chemical ChangeChemical changes –

- To identify a chemical change…

- A chemical change occurs when…

What is another example of chemical change?

Chemistry & MatterWe can explore-

What is an example of a chemical symbol?

Matter consists of –

The In-Betweenies: Physical or Chemical?Some properties (abilities) can be either physical or chemical.Examples:

Take the Quiz: Is it Chemical or Physical?1._________________________ 2. _________________________ 3. _________________________

4._________________________ 5. _________________________ 6. _________________________

7._________________________ 8. _________________________ 9. _________________________

St 1 Obj 1 b. Classify substances based on their chemical and physical properties (e.g., reacts with water, does not react with water, flammable or nonflammable, hard or soft, flexible or nonflexible, evaporates or melts at room temperature).

Density Block LabFor each station determine the block’s MASS and VOLUME, then figure out the block’s DENSITY by dividing the mass by the volume.

MASS = DENSITY After determining the DENSITY answer if it will float in water. Water’sVOLUME density is 1.00 g/cm3.

**** Then determine any properties that the block might have. For example, answer each of the following questions:

1. Does it burn in the presence of oxygen? (If yes, then it is FLAMMABLE. If no, then it is NONFLAMMABLE.)

2. Does it shine? (If yes, then it has a LUSTER. If no, then it has NO LUSTER.)

3. Could it melt easily? (If yes, then it has a LOW MELTING POINT. If no, it has a HIGH MELTING POINT.)

4. Is it see through? (If yes, then it is TRANSPARENT. If no, then it is OPAQUE.)*If there are other properties you can think of, please list them.

* All of the blocks in this lab have the same volume but different masses. What is the volume of each block? ________Volume= length x width x height

Station DENSITY Does it float in water?

Physical Properties? Chemical Properties?

Station 1: Acrylic Mass: _________ = Volume

g cm3

Station 2: Oak & PineOak Mass: _________ = Volume

Pine Mass: _________ = Volume

g cm3

g cm3

Station 3: Poplar Mass: _________ = Volume

g cm3

Station 4: Steel & AluminumSteel Mass: _________ = Volume

Aluminum Mass: _________ = Volume

g cm3

g cm3

Station 5: Copper Mass: _________ = Volume

g cm3

Station 6: Brass Mass: _________ = Volume

g cm3

Station 7: Nylon Mass: _________ = Volume

g cm3

Station 8: PVC Mass: _________ = Volume

g cm3

1. Viscosity : the ability to resist flowingEx: syrup flows more slowly than water

2. Hardness: the ability to scratch or be scratched by other materialsEx: diamonds is hardest mineral and can easily scratch other substancesEx: If something is scratched by a penny it is considered quite soft.

3. Flammability: the ability to burn in the presence of OxygenEx: some materials can more easily burn

in oxygen than others

4. Reactivity: the ability to combine with another substance in a chemical bondEx: Magnesium will easily react with water to form Magnesium Oxide (MgO) and hydrogen Gas (H2)

5. Density: how heavy a substance is; g/mLEx: gold is extremely heavy, 19.32 g/cm3

6. Melting point: the point at which a solid becomes a liquidEx: Ice (water) becomes a liquid at 0 C

7. Freezing Point: the point at which a liquid becomes a solid.Ex: water freezes into Ice below 0 C.

8. Boiling point: the point at which a liquid becomes a gasEx: water becomes a gas at 100 C

9. Condensation Pt. : the point at which a gas becomes a liquid.Ex: water vapor in the air will condense into a liquid below 100 C.

10. Conductivity: the ability to allow heat/electrons to flow through itEx: a pan can move heat up to the handle

11. Maleability: the ability to be flatten the solid without it shattering

Ex: metals can be hammered into thin sheets under when heated or pressure.

12. Luster: the ability to reflect light/shineEx: many metals such as gold, copper, aluminum will shine because it’s surface reflects light.

13. Solubility: the ability to be dissolved in a liquidEx: sugar will easily dissolve in water, however oil will not dissolve in water.

14. Magnetic: the ability for a substance to be attracted to magnets.Ex: Iron filing will be attracted to a magnet.

15. Flexible: The ability to change shapes and then go back to the original shape easily.Ex: putty is quite flexible.

16. Evaporation: The ability to release gases under conditions before the boiling pointEx: water can evaporate even at room temperature. If water is in warmer temperature (ex: 100 F) then it will evaporate more quickly.

17. Physical the materials ability to change shapes but notProperties: change what it is.

Ex: malleability, solubility, M.P., B.P., viscosity.

18. Physical Change: When the materials actually change in someway but do not change what it is.Ex: change in: textures, shape, size, color, odor, volume, mass, weight & density.

19. Chemical the ability of being able to change what it isProperties: is under some process

Ex: flammability, reactivity

20. Chemical Change: When the materials actually change into a new substance. Atoms are rearranged into new molecules.

Ex: wood is burned and becomes ash (carbon) and carbon dioxide gas. Any Reaction is a chemical change.

5 Signs there is a Chemical Change (** can occur in Physical Change)

1. Produce an Odor: A smell is given off. Ex: something rotting.

2. Change in Temperature: A chemical reaction gets cold or warm. Ex: heat from a fire.

3. Change in Color**: Ex: fruit changes color when ripens(but color dye or kool aid dissolving is a physical change)

4. Formation of Gas: When bubble are given off or smoke.Ex: smoke in a fire is CO2 gas, which is an indicator of that new substance being made.

5. Formation of a Solid: The solid is called a precipitate. Example: crabs and mussels use chemicals in their body to react with water creating a solid shell. Their shell is the precipitate!

_______________________________________________________________________________Chemical and Physical Properties…..

B I N G OFormation of a Solid:

Density: Reactivity: Formation of Gas:

Freezing Point:

Hardness: Change in Temperature:

Condensation Pt. :

Luster: Change in Color**:

Boiling point: Chemical Change:

FREE Physical Change:

Conductivity:

Flexible: Produce an Odor:

Evaporation: Solubility: Melting point:

Viscosity: Flammability: Magnetic: Maleability: PhysicalProperties:

Objective 2 Observe and evaluate evidence of chemical and physical change.a. Identify observable evidence of a physical change (e.g., change in shape, size, phase). b. Identify observable evidence of a chemical change (e.g., color change, heat or light given off, change in odor, gas given off).

Name That CHANGEFor the following activity, please list the change that occurs and then what type of change it is and why.Description of Change Physical or Chemical Change WHY?

Notes under NAME THAT CHANGE

St. 1 Obj. 1.c. Investigate and report on the chemical and physical properties of a particular substance.

Investigate Chemical and Physical Properties:1. Choose a substance from home and analyze which chemical and physical properties it may have.

2. DO NOT PERFORM ANY TESTS AT HOME THAT COULD BE HAZARDOUS!!!3. Make observations about that substance and research any properties it may have.

4. Write a page report on that property using the vocabulary terms mentioned above.

5. Be sure to include a reference of books, websites you used in your investigation and research.

6. Be sure that the writing is yours and is not directly copied from any website. This would be a form of cheating and you can get a zero if it is suspected.

This assignment is due:__________________________ Go to www.myaccess.com for more directions. Or under websites there is a word document with information.

St. 1 Obj. 3 B. Relate the amount of energy added or taken away from a substance to the motion of molecules in the substance Watching the Phases of MatterPlease go to these websites and go through each module.Go to the following website: http://www.bbc.co.uk/schools/scienceclips/ages/9_10/changing_state.shtmlFollow the directions and answer the following questions:

1. What happens to the ice when the temperature reaches 0 C?

2. Can you change your water back into ice again? Does ice take up a bigger or smaller amount of volume than water?

3. What happens to the water when the temperature reaches 100 C?

4. Can you turn your steam back into water again? How?

5. What happens if you heat the steam over a 100 C?

Go to the next website: http://mutuslab.cs.uwindsor.ca/schurko/animations/waterphases/status_water.htmAnswer the following questions after watching the simulation and pressing the square button with the two lines: (You may need to perform this experiment more than once.)

1. What temperatures is the water a solid at (ice block)? (remember if there is any amount of ice present it is in its solid phase)

2. What temperatures is the water a liquid at? (remember if there is any amount of liquid water present then it is in its solid phase)

3. When do particles begin to escape?

4. What temperatures is the water a gas at (water vapor)?

5. Draw a picture of the molecules and describe their speed at conditions in:#1 Solid #2 Liquid #3 Gas

Go to the following website: http://vital.cs.ohiou.edu/physical_chemical_change.html Number your paper below and describe what is happening at each question, what type of change it is, and why.

What’s Happening: Chem/Phys Change? Why

title: Boiling pointpurpose: To see what temperature water boils at in our location.

prediction: I think water boils at _____ ̊C in Brigham City UT.materials: heat plate burner, goggles, beaker, thermometer,

procedure: 1. Fill beaker with ice water to 100 mL.2. Record the temperature in ̊C & fill in Data table at 0 seconds.3. Plug in heat plate burner & begin watching the clock for 25 seconds to pass.4. Put in the thermometer for 5 seconds & record temperature after 5 seconds or the 30 second mark. 5. Begin watching for another 25 seconds to pass and repeat step #4 every 30 seconds. 6. Stop recording after 5 temperature recordings have been at a rolling boil.

data:time temperature time temperature time temperature

0 9.5 4:30 30.6 9:00 80.830 9.5 5:00 39.0 9:30 84.5

1:00 10.4 5:30 45.7 10:00 90.01:30 10.8 6:00 48.5 10:30 93.22:00 10.0 6:30 51.6 11:00 94.42:30 11.7 7:00 53.3 11:30 95.03:00 15.4 7:30 60.6 12:00 95.33:30 17.6 8:00 67.1 12:30 95.54:00 25.5 8:30 75.6 13:00 95.5

analysis

1. What temperature was your boiling point? What is the class average for boiling point?95.5 ̊C; we didn’t record a class average.2. In Celsius, boiling point is supposed to be 100 degrees. In San Diego it is 100 degrees. Why not here?Elevation affects boiling pt. because air pressure is greater at lower elevations so a higher boiling pt. Here, elevation is higher which is less air pressure which means a lower boiling pt. 3. Is boiling a chemical or Be sure to graph the boiling water based on the table from the last page

physical change? WHY?Boiling is a physical change because it changes from water (as a liquid) & water (as a gas).

4. What is boiling? 5. What are the bubbles in boiling water made of?When a substance (like water) goes from Watera liquid to a gas.6. What is happening to the molecules of water as they are heated?The molecules are getting faster as more heat is added.

Conclusion: What are two things you learned? Be specific and write in complete sentences.1. Boiling water does not change into a new substance but is still the same substance,

water.2. Elevation or Altitude changes the boiling point because if air pressure is greater,

than it requires more energy for water to switch from a liquid to a solid. Therefore greater air pressure will create a higher boiling point.

Objective 4 Identify the observable features of chemical reactions.a. Identify the reactants and products in a given chemical change and describe the presence of the same atoms in both the

reactants and products. Distinguishing between Molecules and Atoms:* As you may have already realized, the periodic table of elements describe the different types of atoms that occur in the universe.

Our planet has some very common elements such as:H – Hydrogen O- Oxygen C- Carbon

N- Nitrogen Si – Silicon Na – Sodium

(note Si- 1element Silicon SI- 2 elements Sulfur Iodide; starts where capitalized )

* When these molecules combine they make molecules or compounds:NaCl- Salt H2O – Water CO2- Carbon Dioxide

C6H12O6- Glucose (C6H12O6)2 – Sucrose (Sugar)

O2- Oxygen (gas, we breathe)

* It’s also important to remember that these molecules bind in certain ways (based on what properties each element has) and when you see a number, that tells you how many atoms that are present per element.

Ex: H2O – 2 Hydrogen atoms, 1 Oxygen atom CO2- 1 Carbon atom, 2 Oxygen atom

C6H12O6- 6 Carbon atoms, 12 Hydrogen Atoms, 6 Oxygen Atoms

* If there is a number INFRONT of the molecule/compound, it tells you the number of molecules present.

Ex: 2 H2O – 2 Water molecules 6 CO2- 6 Carbon dioxide molecules NaCl- 1 salt molecule

Before and After: Chemical Reactions:

* Chemical Reactions: occur when there has been a chemical change and atoms are rearranged to make new bonds and new molecules or compounds.

* Substances that are going to be changed are called Reactants

* Substances that are changed after the reaction has taken place are called Products.

* An Arrow separates reactants and products. The reactants are always what you start with(comes before the arrow) and products are always at the end.

See if you can pick out which is the reactant & which is the product and what molecules are present.Reactants Products

1. 4 H2 (g) + O2 (g) → 2 H2O ( l ) H2 Hydrogen Gas (4)(reactants) (products) O2 Oxygen Gas (1)

H2O Water(liquid) (2)

2. 2 Na (s) + Cl2 (g) → 2 NaCl (s) Na Sodium (solid) (2)(reactants) (products) Cl2 Chlorine gas (1)

NaCl Sodium Chloride (2)

3. Ca + 2 H2O → Ca (OH)2 + H2 Ca Calcium (1)(reactants) (products) H2O Water (2)

Ca (OH)2 Calcium Hydroxide (1)H2 Hydrogen gas (1)

If you were to count the number of atoms on the reactant side and the number of atoms on the product side they would be Equal!

This is law is called The Conservation of Mass; it occurs when no atoms are gained or destroyed in a chemical reaction.

Please determine if this equation shows the conservation of mass by counting the number of atoms for each type of element on both sides. If they are equal then this reaction is correct.

CH3COOH + NaHCO3 → CH3COONa + H2O + CO2

Reactants: Products:C= 3 Na = 1 C= 3 Na = 1

H= 5 O = 5 H= 5 O = 5

This experiment is actually very common. Label each of the molecules/compounds by their common name:CH3COOH + NaHCO3 → CH3COONa + H2O + CO2

Vinegar Baking Soda Sodium Acetate Water Carbon dioxide

Conservation of mass can also be seen on a balance.Observe mass 110.5 g Observe Mass 110. 5 gBefore Reaction: After Reaction:

What happens if the mass if the CO2 gas is released? 110 g

The mass decreases because that’s the amount of CO2 gas that escape. The gas was .5 grams.

Complete all of the reactions below by counting if they obey the law of conservation of mass. Write Yes or No if it is balanced correctly. Reactants: Products: Does it follow the

Conservation of Mass?

1. 2 HgO → 2 Hg + 1 O2

____YES_____Hg = 2 O = 2 Hg = 2 O = 2

2. 3 Hf + 2 N2 → 1Hf N4

NO: not a real equationHf = 3 N = 4 Hf = 1 N = 4

3. 1 Fe + 3 H2O → Fe2O3 + 3 H2

NO: not a real equation Fe = 1 H = 6 O = 3 Fe = 2 H = 6 O = 3

4. 1 Te + 1 H2O → 1 TeO + 1 H2

____YES_____Te = 1 H = 2 O = 1 Te = 1 H = 2 O =1

5. Combustion of pentane gas in Oxygen:C5H12 + 8 O2 → 5 CO2 + H2O NO: not a real equation

C = 5 H = 12 O = 16 C = 5 H = 2 O = 11

6. Photosynthesis:6CO2 + 6 H2O → C6H12O6 + 6 O2

_____YES_____ C = 5 H = 12 O = 18 C = 6 H = 12 O = 18

St. 1 Obj. 4. B. Cite examples of common significant chemical reactions (e.g., photosynthesis, respiration, combustion, rusting) in daily life. C. Demonstrate that mass is conserved in a chemical reaction (e.g., mix two solutions that result in a color change or formation of a precipitate and weigh the solutions before and after mixing). Demonstrate the CONSERVATION OF MASS:Baking Soda and Vinegar1. Describe the reactants and products of the chemical reaction of Baking Soda and Vinegar:2. Count the atoms on each side to be sure they balance.

Reactants: Products:

Baking Soda & Vinegar Sodium Acetate, Water, & Carbon Dioxide

Notebook Activity: On a separate piece of paper draw the atoms in the molecules of both photosynthesis and respiration.Photosynthesis and Respiration:1. Describe the reactants and products of photosynthesis: (Which organisms perform photosynthesis?)Count the number of atoms on each side to be sure they balance. PLANTSReactants: Products:

Carbon Dioxide & Water Glucose & Oxygen

2. Describe the reactants and products of respiration: (Which organisms perform respiration?)Count the number of atoms on each side to be sure they balance. ANIMALSReactants: Products:

Glucose & Oxygen Carbon Dioxide & Water

St 1. Obj. 2 Observe and evaluate evidence of chemical and physical change.c. Identify observable evidence of a physical change (e.g., change in shape, size, phase). d. Identify observable evidence of a chemical change (e.g., color change, heat or light given off, change in odor, gas given off).

St. 1. Obj. 3. A. Identify the kinds of energy (e.g., heat, light, sound) given off or taken in when a substance undergoes a chemical or physical change

Chemistry WEBQUEST: Go to www.usborne-quicklinks.com Click on USA. Type in Science Encyclopedia. Click on Find Book. Scroll down and click on Usborne Science encyclopedia. Type in 76. Click on Find Links

Recently they changed the website so that the animation no longer works. We will be doing this in class instead.

1. “Energy changes: Breaking and forming bondsWhen methane, CH4 burns in oxygen gas, O2, bonds must first be BROKENin both molecules before new bonds forming the products can be made.”

1 CH4 2 O2 1 CO2 2H2O

2. In the above equation write down which are the reactants and which are the products.

Reactants: 1 CH4 & 2 O2 Products: 1 CO2 & 2H2O

3. Now count how many atoms are on the reactant side and the product side. Compare the two.Reactants: C = 1 H = 4 O = 4 Products: C = 1 H = 4 O = 4

4. Now push Play to allow the reaction to take place. How could you describe what happened to the atoms?They’re the same atoms. The atoms rearranged from reactants to products.

5. Read the web page and Fill in the guided notes below:

“Energy is measured in kilojoules or_____________. When bonds break, energy must be absorbed from their surroundings. Taking in energy reduces the temperature of the surroundings - this is called an ____Endothermic__ ___Reaction______. This value is always given a __Positive ___ sign, for example, +345kJ.

When bonds are made, energy is released to the surroundings. Energy that is released to the surroundings is called an

____Exothermic Reaction_______. This value is always given a _____negative_______value, for example, -345kJ.

Remember, when a reaction takes place bonds ____Break___________ (____Endothermic_____) then bonds are ____Formed__________ (_______Exothermic____________).

Overall, the reaction will be exothermic if more energy is released into the surroundings than was absorbed.

An endothermic reaction will occur overall if, more energy is absorbed from the surroundings than is released.

_____Bond______ ______Energy______: This is the energy required to break one mole of bonds. The bond energy is also the energy given out when a mole of bonds is formed.

____Activation________ _______Energy_________: This is the minimum amount of energy required to break bonds to start the reaction off.”

Go back to Usborne Quicklinks. Click on Website #2. Watch each of the different chemical reactions. & fill out the table below.

Chemical Equation *write down what each molecule looks like (color & state of matter)___________________________________________________________________________________1. Sodium Iodide + Mercury ChlorideReactants: Products Evidence of Chem Change?

HgCl2(aq) + 2 NaI(aq) HgI2(s) + 2 NaCl(aq)Color: Clear Pale Yellow Orange Clear Color Change

State: Liquid Liquid Solid Liquid Formed a Solid

___________________________________________________________________________________2. Cadmium Nitrate + Sodium SulfideReactants: Products Evidence of Chem Change?Na2S + Cd(NO3) 2 2 NaNO3 + CdSColor:Clear Clear Clear Yellow-orange Color Change State:liquid liquid liquid solid Formed a Solid_________________________________________________________________________________3. Copper(II) Nitrate + AmmoniaReactants: Products Evidence of Chem Change?NH3 + Cu(NO3)2 Cu(OH)2(s) + Cu(NH3)4

2+

Color: Color ChangeClear Light Blue Light Blue Dark Blue

State:Liquid liquid solid liquid Formed a Solid___________________________________________________________________________________Please Go to www.usborne-quicklinks.com Evidence of Chemical Change? Follow directions above And fill in the blanks4. Oxidation of Glycerin by Potassium Permanganate___________________________________________________________________________________5. Nitrogen Triiodide Detonation2 NI3 N2 + 3 I2

___________________________________________________________________________________6. Sodium + AcidNa + HCl NaCl + H2 (g)___________________________________________________________________________________

7. Denaturation of Protein

Other Physical Changes: Please describe the physical property showed and why. 8. Ferrofluid

___________________________________________________________________________________9. Ice Bomb___________________________________________________________________________________

10. Like Dissolves Like

Title: Natural vs. SyntheticIntroduction: One of the first things everyone does in the morning is to select clothes to wear. How do we choose clothes? Style, fit? How about what fabric they are made of? Do you wear polar fleece in the winter and cotton t-shirts in the summer? Do you know what fabric you are wearing today? We can divide fabrics into two categories, natural and synthetic. Natural fabrics come from nature, like wool from sheep and flax from plants to make linen. Chemists have also developed fibers from petroleum that are synthetic or man-made. Nylon, polyester, and spandex are synthetics. In this activity you will see similarities and differences between natural and synthetic fabrics.

Materials- 2 pieces of 8 fabrics, alcohol burner, probe or tweezers, bleach, beaker, test tubesProcedures:1. Describe the fabrics in the data table-color, feel, stretchiness, and thickness. 2. Test water absorption rate by placing a drop of water on each. Time how long it takes to sink in.3. Take an extra piece of the fabric your teacher assigns you and place it in a test tube. Add some bleach to the fabric. Label it and let sit overnight.4. Hold a piece of fabric over the burner until it starts to burn. Have a beaker of water ready and take it out of flame and hold it over the water. Time how long it takes and what it looks like as it burns.

Prediction: Which fabric will burn quickest?Data:Natural

or Synthetic

Fabric Name Description Absorption of water (# of

drops)

Burn Time (sec)

Reaction to Bleach

N Cotton Thin No (3) 25 Unsure

S C.P. Flanel Thick, soft No (7) 34 Unsure

S C.S. Spandex Stretchy, like Jeans Yes (2) 1:36 No

N Wool Thick, itchy No (9) 1:27 Yes

S Acetate Silky No (1) Melt, 23 Yes

S Nylon Very stretchy, light, No (5) Melt, 42 Yes

S C.P. Fleece Stretchy, soft No (7) 30 A little

S Polyester Thick, grainy No (12) 2:10 Yes

N T-shirt Stretchy, soft Yes (2) 1:15 Unsure

Analysis:1. Which fabrics would be safe to bleach? unsafe?Cotton polyester flannel & cotton polyster spandex….. the other ones

2. Which fabrics were the most stretchy?(natural or synthetic)synthetic

3. Which absorbed water better, natural or synthetic? Synthetic: acetate absorbed in one drop.

4. What type fabric burned fastest?Acetate & Cotton

5. What was the main difference between how natural and synthetic fabrics burn? Most natural fabrics burned normal.. the synthetics however either melted or sparkled as they burned

6. What are advantages of synthetic fabrics?The synthetic fabrics can have the correct texture: such as stretch, extra soft, light/transparent, or silky

7. What are disadvantages of synthetic fabrics?They melt when they burn, which can mean they melt to skin in a fire.

8. What are advantages of natural fabrics?They do not melt when they burn and most of them take a longer time to burn, which gives a person in a fire more time to put out the fire that might be on the fabric.

9. What are disadvantages of natural fabrics?You can’t always have the fun desire texture: stretch, extra soft, etc.

Conclusion-2 things you learned written in complete sentences.That acetate will melt very quickly and absorb water very quickly.That a lot of the fabrics we are familiar with today are synthetics.

Student Taught Chemical Reactions:St1. Obj 2. C. Observe and describe chemical reactions involving atmospheric oxygen (e.g., rust, fire, respiration, photosynthesis). St. 1 Obj.2 D. Investigate the effects of chemical change on physical properties of substances (e.g., cooking a raw egg, iron rusting, polymerization of a resin).St. 1. Obj 3. A. Identify the kinds of energy (e.g., heat, light, sound) given off or taken in when a substance undergoes a chemical or physical change.

1. Name of Rxn:_ Photosynthesis 6CO2 + 6 H2O → C6H12O6 + 6 O2Reactants by Products by Signs of aCommon Name: Common Name: Chemical Reaction: Endothermic or

Exothermic?Carbon dioxide + water food + oxygen gives off gas Endothermic

-takes in heat

2. Name of Rxn:___ Respiration C6H12O6 + 6 O2 → 6CO2 + 6 H2OReactants by Products by Signs of aCommon Name: Common Name: Chemical Reaction: Endothermic or

Exothermic?Food + oxygen Carbon dioxide + water - gives off a gas Exothermic

-gives off heat

3. Name of Rxn:__ Combustion of octane gas in Oxygen2 C8H18 + 25 O2 → 16 CO2 + 18 H2OReactants by Products by Signs of aCommon Name: Common Name: Chemical Reaction: Endothermic or

Exothermic?

Octane gas + oxygen carbon dioxide + water - gives off a gas Exothermic-gives off heat

4. Name of Rxn:____ Metal Rusting 2 Fe + O2 → 2 FeOReactants by Products by Signs of aCommon Name: Common Name: Chemical Reaction: Endothermic or

Exothermic?Iron + oxygen rust -color change Endothermic

5. Name of Rxn:___ Baking with Baking Soda 2NaHCO3 → Na2CO3 + H2O + CO2Reactants by Products by Signs of aCommon Name: Common Name: Chemical Reaction: Endothermic or

Exothermic?Baking Soda SodiumBicarbonate gives off a gas Exothermic

+ Water +Carbon -gives off heat

6. Name of Rxn:____ Wood Burning CxHyOz + O2 ------> CO2 + H20Reactants by Products by Signs of aCommon Name: Common Name: Chemical Reaction: Endothermic or

Exothermic?Wood + oxygen carbon dioxide + water -gives off heat and light

-color change -gas given off Exothermic