Matter, Solutions, Acids & Bases

Georgia Performance Standards SPS2. Students will explore the nature of matter, its classifications, and its system for naming types of matter.

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

What are the physical properties of these items?

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

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

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.

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

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. Flammability, Reactivity, etc Once a chemical change has occurred a NEW SUBSTANCE OR SUBSTANCES is/are produced with totally new physical and chemical characteristics.

Examples of Chemical Changes

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

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 product(s) is equal to the mass of the reactant(s).

Composition of Matter 2 Main Types of Matter: 1.Pure Substances : either ____________ or compounds. Has the same composition throughout A. Elements – all atoms in the substance are alike 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

Pure Substances continued 2.Compounds– consisting of two or more different elements bonded together (chemicallly 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 ), hydrochloric acid (H 2 S0 4 ), salt (NaCl)

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

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” Examples: salad, hotdog, hamburger, marble…

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

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

Solutions A homogeneous mixture where on material dissolves in another the dissolved particles are so small you can see them Alloy-- a solution of two or more elements, usually metal and metal 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

Parts of a Solutions 1.Solutes– the particles dissolved in the solution Examples: sugar, Koolaid mix, salt 2. Solvent– the substance in a solution in which the particles dissolve Usually water

Colloid A homogeneous mixture that contains some particles that are larger in size, but still evenly distributed throughout Does not settle upon standing Tyndall Effect– scattering of light due to larger particles… causes milky/cloudy color in colloids Example… milk, fog, peanut butter, butter, mayonnaise, yogurt…

Gas Laws 1.Charles Law The direct proportion of the volume of a gas to its temperature (in Kelvins) if the pressure and the number of particles of the gas are constant As temperature goes up, volume goes up (if pressure stays same)

Gas Laws 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 If the volume goes down, then the pressure will go up (if the temperature stays constant)