1. Matter-Properties and Changes I will distinguish between physical and chemical properties I will classify matter by composition: element, compound or mixture I will identify observable characteristics of chemical reactions I will explain the fundamental law of conservation of mass

2. Properties of Matter I will identify the characteristics of a substance I will identify the characteristics of a substance I will distinguish between physical and chemical properties I will distinguish between physical and chemical properties I will differentiate among the physical states of matter I will differentiate among the physical states of matter

3. Substances Matter that has a uniform and unchanging composition Matter that has a uniform and unchanging composition Aka pure substance Aka pure substance Example 1 Example 1 Table Salt Table Salt Always 100% sodium chloride Always 100% sodium chloride Example 2 Example 2 Water Water H 2 O H 2 O NOT AN EXAMPLE NOT AN EXAMPLE Sea water Sea water Samples vary by location Samples vary by location Amount of salts, water, dissolved substances Amount of salts, water, dissolved substances

5. Physical Properties A characteristic that can be observed or measured WITHOUT changing the sample’s composition A characteristic that can be observed or measured WITHOUT changing the sample’s composition Density Density Color Color Odor Odor Taste Taste Hardness Hardness Melting point Melting point Boiling point Boiling point

6. Examples-Physical Properties Salt (sodium chloride) Salt (sodium chloride) Forms solid white crystals at room temperature Forms solid white crystals at room temperature Unique salty taste Unique salty taste Oxygen Oxygen Colorless Colorless Gas at 25 degrees Celsius Gas at 25 degrees Celsius Melting point -218 degrees Celsius Melting point -218 degrees Celsius Boiling point -183 degrees Celsius Boiling point -183 degrees Celsius Density 0.0014 g/cc Density 0.0014 g/cc

7. Extensive Properties Dependent upon the amount of substance present Dependent upon the amount of substance present Examples Examples Mass Mass Volume Volume Length Length Weight Weight

8. Intensive Properties Independent of the amount of the substance present Independent of the amount of the substance present Examples Examples

9. Chemical Properties The ability of a substance to combine with or change into one or more other substances The ability of a substance to combine with or change into one or more other substancesAnd/Or The inability of a substance to change into another substance The inability of a substance to change into another substance Example Example Iron forms rust when combined with air Iron forms rust when combined with air Iron + Nitrogen (at room temperature) = no chemical change Iron + Nitrogen (at room temperature) = no chemical change

10. Observing Properties of Matter Every substance has its own unique set of physical and chemical properties Every substance has its own unique set of physical and chemical properties May vary depending on conditions of immediate environment May vary depending on conditions of immediate environment Room temperature, standard pressure, etc. Room temperature, standard pressure, etc. Example ExampleCopper Physical PropertiesChemical Properties Reddish brown Shiny Malleable (easily shaped) Ductile (drawn into wire) Conducts heat/electricity Density 8.92 g/cc Melting Point 1085 ℃ Boiling Point 2570 ℃ Forms green copper carbonate compound when in contact w/ moist air Forms new substances when combined with nitric and sulfuric acids Forms a deep blue solution when in contact with ammonia

12. States of matter Solid Solid Liquid Liquid Gas Gas Plasma Plasma FUN FACT: (only occurs FUN FACT: (only occurs naturally on Earth in the form of lightening bolts!) PHYSICAL PROPERTY!!!!!

13. Solids A form of matter that has its own definite shape and volume. A form of matter that has its own definite shape and volume. Examples Examples Wood Wood Iron Iron Paper Paper Sugar Sugar Particles are VERY tightly packed Particles are VERY tightly packed Will only expand SLIGHTLY when heated Does NOT conform to shape of container Incompressible Volume stays the same Example Wax (moldable) but volume doesn’t change

14. Liquids A form of matter that flows, has constant volume, and takes the shape of its container A form of matter that flows, has constant volume, and takes the shape of its container Examples Examples Water Water Blood Blood Mercury Mercury Virtually incompressible Tend to expand when heated Liquid Particles NOT rigidly held in place less closely packed than solids Are able to move past each other

15. Gases A form of matter that flows to CONFORM to the shape of its container and fills the ENTIRE volume of its container A form of matter that flows to CONFORM to the shape of its container and fills the ENTIRE volume of its container Examples Examples Neon Neon Lighted signs Lighted signs Methane Methane Cooking Cooking Air Air Mixture of gases Mixture of gases Particles are VERY far apart EASILY compressed A substance NATURALLY in the gaseous state at room temperature RELATED TERMS Vapor The gaseous state of a substance that is a SOLID or LIQUID at room temperature Example steam

16. Quick Think Describe the characteristics that identify a sample of matter as being a substance. Describe the characteristics that identify a sample of matter as being a substance. Classify each of the following as a physical or chemical property Classify each of the following as a physical or chemical property Iron and oxygen form rust Iron and oxygen form rust Iron is more dense than aluminum Iron is more dense than aluminum Magnesium burns brightly when ignited Magnesium burns brightly when ignited Oil and water do not mix Oil and water do not mix Mercury melts at -39 ℃ Mercury melts at -39 ℃ Using what you know about the compressibility of gases, explain why the oxygen in a SCUBA tank is compressed. Create a table that describes the three common states of matter in terms of their shape, volume, and compressibility.

17. Quick Think- Check The sample of matter must have a uniform and unchanging composition to be a substance. The sample of matter must have a uniform and unchanging composition to be a substance. Properties Properties Chemical (rust) Chemical (rust) Physical (density) Physical (density) Chemical (burning) Chemical (burning) Physical (mixing) Physical (mixing) Physical (melting) point) Physical (melting) point) Particles of gas are spaced apart and are easily compressed. Therefore, it is possible to put a significant volume of oxygen in the tank, which allows the diver to remain under water longer! SolidLiquidGas Definite volume Fills volume of container Definite shapeFills container shape Takes shape of container IncompressibleVirtually incompressible Compressible

18. Changes in Matter I will define physical change and list several common physical changes I will define physical change and list several common physical changes I will define chemical change and list several indications that a chemical change has taken place I will define chemical change and list several indications that a chemical change has taken place I will apply the law of conservation of mass to chemical reactions I will apply the law of conservation of mass to chemical reactions

19. Physical CHANGES Alter a substance WITHOUT changing its composition Alter a substance WITHOUT changing its composition Might result in dramatically different appearance (yet leave the composition of the substance unchanged) Might result in dramatically different appearance (yet leave the composition of the substance unchanged) Examples Examples Crunching up a piece of aluminum foil Crunching up a piece of aluminum foil Cutting a sheet of paper Cutting a sheet of paper Breaking a crystal Breaking a crystal Phase changes (solid, liquid, gas) Phase changes (solid, liquid, gas)

20. Key words of Physical Changes Bend Bend Grind Grind Crumple Crumple Split Split Crush Crush

21. Chemical CHANGES A process that involves one or more substances changing into a NEW substance A process that involves one or more substances changing into a NEW substance New substance New substance Formed in reaction Formed in reaction Different compositions — than original substance(s) Different compositions — than original substance(s) Different properties — than original substance(s) Different properties — than original substance(s) Example Example Fermentation of juice, sugars, and other ingredients (making wine) Fermentation of juice, sugars, and other ingredients (making wine) Rusting of iron (a chemical combo of iron and oxygen) Rusting of iron (a chemical combo of iron and oxygen)

22. Chemical CHANGES Commonly referred to as a chemical reaction Commonly referred to as a chemical reaction Reactants Reactants Starting substances Starting substances Products Products New substances New substances Example Example Reactants = Iron, Oxygen Reactants = Iron, Oxygen Product = rust Product = rust

23. Key Words of Chemical Changes Explode Explode Rust Rust Oxidize Oxidize Corrode Corrode Tarnish Tarnish Ferment Ferment Burn Burn Rot Rot

24. The LAW of Conservation of Mass Mass is neither created nor destroyed during a chemical reaction Mass is neither created nor destroyed during a chemical reaction Mass is conserved Mass is conserved Mass of Reactants = Mass of Products Mass of Reactants = Mass of Products

25. Conservation of Mass Problem Known Known Mass mercury (II) oxide = 10.0g Mass mercury (II) oxide = 10.0g Mass liquid mercury = 9.26g Mass liquid mercury = 9.26g Unknown Unknown Mass formed oxygen = ? g Mass formed oxygen = ? g Mass Reactants = Mass Products Mercury (II) oxide = Mercury + Oxygen 10.0g = 9.26g + ? 0.740 g of Oxygen formed

26. Quick Think Describe the results of a physical change and 3 examples. Repeat with chemical change. Describe the results of a physical change and 3 examples. Repeat with chemical change. A friend tells you, “because composition does not change during a physical change, the appearance of a substance does not change.” Is your friend correct? Explain WHY? A friend tells you, “because composition does not change during a physical change, the appearance of a substance does not change.” Is your friend correct? Explain WHY? Solve each of the following In the complete reaction of 22.99 g of sodium with 35.35 g chlorine, what is the mass of the sodium chloride formed? A 12.2 g sample of X reacts with a sample of Y to form 78.9 g XY. What way the mass of Y that reacted?

27. Quick Think-Check During a physical change a substance is altered but its composition does not change. EX melting, freezing, boiling, bending, tearing During a physical change a substance is altered but its composition does not change. EX melting, freezing, boiling, bending, tearing During a chemical change the composition of a substance IS altered. EX color change, odor, temperatures change, formation of gas or solid from a liquid. During a chemical change the composition of a substance IS altered. EX color change, odor, temperatures change, formation of gas or solid from a liquid. The statement is false. Composition doesn’t change but a change in appearance often accompanies a physical change. 58.44g of sodium chloride 66.7 g of Y

28. Mixtures of Matter I will contrast mixtures and substances I will contrast mixtures and substances I will classify mixtures as homogeneous or heterogeneous I will classify mixtures as homogeneous or heterogeneous I will list and describe several techniques used to separate mixtures I will list and describe several techniques used to separate mixtures

29. Mixtures A combination of two or more pure substances A combination of two or more pure substances Each pure substance retains its INDIVIDUAL chemical properties Each pure substance retains its INDIVIDUAL chemical properties Most everyday matter occurs as mixtures Most everyday matter occurs as mixtures Substances naturally tend to mix Substances naturally tend to mix It is very difficult to keep things pure It is very difficult to keep things pure

30. Mixture Examples Water and Sand Water and Sand Water Water Colorless liquid Colorless liquid Sand Sand Grainy solid Grainy solid Doesn’t dissolve in water Doesn’t dissolve in water Easily seen as two substances mixed Easily seen as two substances mixed Water and Table Salt Water Colorless liquid Table Salt White crystal solid Dissolves in water NOT easy to see both substances individually But if you boiled the water a white residue remains (salt!)

31. Types of Mixtures Heterogeneous Heterogeneous Doesn’t blend smoothly throughout Doesn’t blend smoothly throughout Individual substances remain distinct Individual substances remain distinct Examples Examples Water mixed with sand Water mixed with sand Fresh orange juice Fresh orange juice Pulp + Juice Pulp + Juice Pizza Pizza Dough + sauce + cheese + toppings Dough + sauce + cheese + toppings Homogeneous Constant composition throughout Always has a single phase Examples Water mixed with salt Cough syrup lemonade Referred to as SOLUTIONS

32. Solutions Gas-Gas Gas-Gas EX. Air is primarily a mixture of nitrogen, oxygen, and argon gases EX. Air is primarily a mixture of nitrogen, oxygen, and argon gases Gas-Liquid Gas-Liquid EX. Carbonated beverages contain carbon dioxide gas in solution EX. Carbonated beverages contain carbon dioxide gas in solution Liquid-Gas Liquid-Gas Ex. Moist air contains water droplets in air (which is a mixture of gases) Ex. Moist air contains water droplets in air (which is a mixture of gases) Liquid-Liquid Ex. Vinegar contains acetic acid in water Solid-Liquid Ex. Sweetened powder drink contains sugar and other solid ingredients in water Solid-Solid Ex. Steel is an alloy of iron containing carbon

33. Separating Mixtures Filtration Filtration A technique that uses a porous barrier to separate a solid from a liquid A technique that uses a porous barrier to separate a solid from a liquid Ex through filter paper Ex through filter paper Like coffee! Like coffee! Used to filter heterogeneous mixtures composed of solids and liquids Used to filter heterogeneous mixtures composed of solids and liquids Distillation A separation technique that is based on differences in boiling points A mixture is heated until the substance with the lowest boiling point boils to a vapor that can be condensed into a liquid and collected Used to filter homogeneous mixtures

34. Separating Mixtures Crystallization Crystallization Technique results in the formation of pure particles of a substance Technique results in the formation of pure particles of a substance From a solution containing dissolved particles From a solution containing dissolved particles Ex rock candy Ex rock candy From a sugar solution From a sugar solution Often have to add just a little more than what the solution can possibly hold to get the crystals to come out of solution Often have to add just a little more than what the solution can possibly hold to get the crystals to come out of solution Produces HIGHLY PURE solids Produces HIGHLY PURE solids Chromatography Technique that separates the components of a mixture (mobile phase) on the basis of the tendency of each to travel or be drawn across another surface (stationary stage) EX. Soaking up a liquid with paper towel

35. Quick Think How do Mixtures and Substances differ? How do Mixtures and Substances differ? Classify each of the following as either heterogeneous or homogeneous mixtures Classify each of the following as either heterogeneous or homogeneous mixtures Orange juice Orange juice Tap water Tap water Steel (blend of iron/carbon) Steel (blend of iron/carbon) Air Air Raisin muffin Raisin muffin Applying Concepts Describe the separation technique that could be used to separate each of the following mixtures Two colorless liquids A non dissolving solid mixed with a liquid Red and blue marbles of the same size and mass