1. Matter, Solutions, and Gas Laws Georgia Performance Standard: SPS2. Students will explore the nature of matter, its classifications, and its system for naming types of matter.

2. Gas Laws 1.Charles Law The direct proportion of the volume of a gas to its temperature (in Kelvin) if the pressure is at STP (standard temperature pressure) V1/T1 = V2/T2 2.Boyle’s Law The inverse variation of the volume of a gas with its pressure if the temperature and the number of particles are constant P1V1=P2V2 Larger volume, less pressure smaller volume, pressure goes up

3. Matter Matter is anything that has mass and takes up space When matter is not the same throughout it is called heterogeneous A mixture is two or more substances that do not combine chemically (they keep their own properties)

4. Properties of Matter Physical Property- a characteristic of a material that you can observe without changing its identity. Ex.- Color, shape, size, magnetic quality, malleability, ability to flow…

5. What are the physical properties of these items?

6. During a Physical Change the internal makeup of a substance does not change. Ex.- Freezing, Melting, Boiling, condensing, cutting into, distillation.

7. Distillation physical change The process of separating a mixture by its boiling point Examples: Making alcohol, separating petroleum, or salt water

8. Petroleum: Fractional Distillation Oil was formed from the remains of animals and plants that lived millions of years ago. Over the years, the remains were covered by layers of mud. Heat and pressure from these layers helped the remains turn into what we today call crude oil. The word "petroleum" means "rock oil" or "oil from the earth." Other products made from petroleum include: ink, crayons, bubble gum, dishwashing liquids, deodorant, eyeglasses, records, tires, ammonia, and heart valves.

9. Other materials made from petroleum Solvents Diesel Motor Oil Bearing Grease Ink Floor Wax Ballpoint Pens Football Cleats Upholstery Sweaters Boats Insecticides Bicycle Tires Sports Car Bodies Nail Polish Fishing lures Dresses Tires Golf Bags Perfumes Cassettes Dishwasher Tool Boxes Shoe Polish Motorcycle Helmet Caulking Petroleum Jelly Transparent Tape CD Player Faucet Washers Antiseptics Clothesline Curtains Food Preservatives Basketballs Soap Vitamin Capsules Antihistamines Purses Shoes Dashboards Cortisone Deodorant Footballs Putty Dyes Panty Hose Refrigerant Percolators Life Jackets Rubbing Alcohol Linings Skis TV Cabinets Shag Rugs Electrician's Tape Tool Racks Car Battery Cases Epoxy Paint Mops Slacks Insect Repellent Oil Filters Umbrellas Yarn Fertilizers Hair Coloring Roofing Toilet Seats Fishing Rods Lipstick Denture Adhesive Linoleum Ice Cube Trays Synthetic Rubber Speakers Plastic Wood Electric Blankets Glycerin Tennis Rackets Rubber Cement Fishing Boots Dice Nylon Rope Candles Trash Bags House Paint Water Pipes Hand Lotion Roller Skates Surf Boards Shampoo Wheels Paint Rollers Shower Curtains Guitar Strings Luggage Aspirin Safety Glasses Antifreeze Football Helmets Awnings Eyeglasses Clothes Toothbrushes Ice Chests Footballs Combs CD's Paint Brushes Detergents Vaporizers Balloons Sun Glasses Tents Heart Valves Crayons Parachutes Telephones Enamel Pillows Dishes Cameras Anesthetics Artificial Turf Artificial limbs Bandages Dentures Model Cars Folding Doors Hair Curlers Cold cream Movie film Soft Contact lenses Drinking Cups Fan Belts Car Enamel Shaving Cream Ammonia Refrigerators Golf Balls Toothpaste Gasoline

10. Properties of Matter Chemical Property-- describes its "potential" to undergo some chemical change or reaction because of its composition. Chemical properties can only be observed by changing a substance's chemical properties. Examples: Flammability, Reactivity, etc Once a chemical change has occurred a NEW SUBSTANCE OR SUBSTANCES is/are produced with totally new physical and chemical characteristics.

11. Examples of Chemical Changes

12. Chemical Changes + = Soft, silver metal Reacts violently with water Green gas toxic Love it on French fries Need it to live

13. Conservation of Mass During a chemical reaction, energy is taken in or given off The Law of Conservation of Mass states mass is neither created or destroyed. The mass of the reactant(s) is equal to the mass of the product(s).

14. Composition of Matter Main Types of Matter: 1.Pure Substances : either elements or compounds. Has the same composition throughout A. Elements – all atoms in the substance are the same 90 elements found in nature 20+ made in laboratories Atom is the smallest particle of an element that still retains the characteristics of that element Examples: copper, gold, hydrogen, carbon

15. 2.Compounds– consisting of two or more different elements bonded together (chemically combined) in a fixed Mass ratio that can be split into simpler substances. Examples: water (H 2 0), carbon dioxide (CO 2 ), sugar (C 6 H 12 0 6 ), hydrochloric acid (H 2 S0 4 ), salt (NaCl)

16. 3. Mixtures: 2 or more materials combined together BUT NOT CHEMICALLY combined, they still retain their own chemical makeup. Unlike compounds, mixtures do not always contain substances in fixed proportions. Heterogeneous

17. Types of Mixtures 1.Heterogeneous Mixtures A type of mixture in which parts of the mixture are noticeably different from one another Usually can pick out the “different” particles Hetero means “different” 2 Main Types: –Suspension –Mixture Examples: salad, hotdog, hamburger, marble…

18. Suspension Heterogeneous mixture between liquids or liquids/solids that will separate out upon standing. Examples: Italian dressing, pond water, oil and vinegar

19. Types of Mixtures 2.Homogeneous Mixture a mixture that contains 2 or more gases, liquids or solids blended consistently throughout. Hard to pick out individual particles (looks the “same” throughout) Homo means “same” Two Main Types: A.Solutions B.Colloids (most of the time)

20. Solutions A homogeneous mixture where one material is indistinguishable in another the dissolved particles are so small you can’t see them Alloy-- a solution of two or more elements, usually metals. brass– zinc and copper stainless steel– copper, nickel and iron Pewter– lead, copper, tin White gold– nickel, palladium and gold Rose gold – copper and gold Bronze– aluminum and copper

21. Colloid A homogenous mixture that contains some particles that are larger in size, but still evenly distributed throughout Does not settle upon standing unless it has gone bad (e.g. milk) Tyndall Effect– dispersion of light due to larger particles… causes milky/cloudy color in colloids…can be used to determine whether something is a solution or colloid Example… milk, fog, peanut butter, butter, mayonnaise, yogurt…

22. Parts of a Solutions 1.Solute– BEING DISSOLVED the particles dissolved in the solution Examples: sugar, Koolaid mix, salt 2. Solvent–DOES DISSOLVING the substance in a solution in which the particles dissolve Usually water

23. Solubility The maximum of amount of solute that normally dissolves in a given amount of solvent at a certain temperature. Solubility chart shows how much of a substance will dissolve at a particular temperature. Soluble--- will dissolve in Salt is soluble in water. Sugar is soluble in water. Insoluble– will NOT dissolve in An oil is insoluble in water. Ink is insoluble in water.

24. Solutions Solutions are concentrated when they contain a lot of solute Solutions are dilute when they contain a small amount of solute Solubility is the ability of a substance to dissolve

25. Rate of Solution Stirring- agitating the solution causes solute particles to come in contact with solvent particles Heating- higher temperature increase the movement of particles to speed dissolving Increasing Surface Area- More solute comes in contact with solvent e.g. granulated sugar versus sugar cubes

26. Solubility Unsaturated- Solution contains less than the maximum amount of solute that can dissolve in the solvent at a given temperature Saturated- Solution that contains the maximum amount of solute that can dissolve at a given temperature Supersaturated- Solution that contains more solute that can dissolve at a given temperature –Only stays supersaturated when condition change e.g. heated then cooled –Otherwise the unusable solute will stay at the bottom

27. Solubility Curves A solubility curve is a graph of a solute usually dissolved in 100 g of water Water is considered the universal solvent Solubility-Ability to dissolve Looking at the solubility curve we see that the type of solute will make a difference in how much is dissolved. Solubility – the amt of solute that can dissolve in a solvent (100 mL of water) SOLUBILITY CURVES ARE ALWAYS ON THE GRAD TEST!!!

30. Solubility chart various materials