Separation of Matter

1. Separation of Matter

2. MATTER Can it be physically separated? (ex: filtration or evaporation) YES NO Is it made up of only one type of atom on the periodic table? Is the composition uniform throughout? YES NO NO YES Matter is Anything that has mass and takes up space (volume) Pure substance Mixture Heterogeneous Compound Element Homogenous

3. Types of matter • Uniform, unchanging composition. Pure substances exist as either elements or compounds. Pure substances- 1. element ex: silver 2. compound ex: NaHCO3 • Found on the periodic table • cannot be separated into simpler substances by physical or chemical means • It takes a nuclear reaction to break them apart! • two or more elements that are chemically bonded. • A chemical change is required to combine elements into compounds, or to separate compounds back into elements.

4. Mixtures 2 types 1. heterogeneous mixture ex: 2. homogeneous mixture ex: Not uniform throughout. Made of very large molecules. Uniform throughout: also called solutions: made of very small molecules. • Gas / Liquid: Soda (CO2 in H2O) • Gas / Gas: Air (Nitrogen, Oxygen, Argon, Water Vapor) • Liquid / Liquid: Gasoline (mixture of liquid hydrocarbons); Rubbing Alcohol (Isopropyl Alcohol with water); Vinegar (Acetic Acid with water) • Solid / Solid: Alloy (mixture of metals), such as brass, steel, 14-karat gold

5. Example 1 • Soda • Rust • Iced tea • Chicken soup • Dirt • Chlorine • Sugar • Gasoline • water homogenous compound heterogenous heterogenous heterogenous element compound homogenous compound

6. Chemical and Physical Properties

7. Remember, density is tricky! While it’s a number, it’s always the same for a substance, no matter how much of it you have! • ___Chemical____ properties describe the ability of a substance to undergo changes that transform it into different substances. Some sort of chemical reaction must be performed in order to observe these properties. • ___Physical___ properties describe the substance itself. They can be observed or measured without altering the chemical identity of the substance (meaning no chemical reaction is necessary to view these properties)....

8. CHEMICAL AND PHYSICAL PROPERTY EXAMPLES

9. Types of physical properties!!! 1. Extensive physical properties 2. Intensive physical properties DO DEPEND on the amount of matter present DO NOT DEPEND on the amount of matter present **Example 2: Place an I(Intensive) or E(extensive for each of the following properties: Malleability (hammer into sheet) IMass E Melting point IOdor I Ability to react with acid IVolume E Ability to react with base IClarity I Ability to react with water IColor I Ability to rust IConsistency I Ability to tarnish IDensity I Viscosity (resistance to flow) I length E Boiling point IArea E Ability to conduct electricityI Luster (shine) I Dissolves in waterI Hardness I Amount of Energy E Ductility (ability to be molded) I Ability to explode (combust) I Flammability (burning) I

10. Chemical and Physical Changes

11. Changes • Transform one or more substances into new, different substances. They involve some sort of reaction taking place! Physical Changes Chemical Changes • Do not change the identity of a substance. Changes of state are all considered to be physical changes. • Just remember: • 1) nothing new has formed • 2) it is still the same substance How do we know if its chemical? heat • An unexpected change in _______ energy (hotter or colder) • A _________ is produced (bubbling) • An unexpected _________ change • A solid _____________ is produced (cloudiness) • An unexpected apparent _________ • change (means that a gas was involved) • New __________ formed • _________ produced (fire) gas color precipitate mass odor light

12. Example 3: • All of the processes listed below are part of the digestive breakdown of food. For each of the following, classify them as a chemical or physical change, and give a reason why. • A. Chewing food • B. Breakdown of proteins • C. Breakdown of carbohydrates • D. Churning of food • E. Starch breakdown • F. food reacting with HCl Physical Chemical Chemical Physical Chemical Chemical

13. States of Matter and Phase Changes

14. States of Matter far Very container Definite container container Definite Definite Not Somewhat Easily

15. States of Matter Very container Definite Definite Definite Somewhat Not

16. States of Matter far Very shape container Definite volume Definite Definite Easily Not Somewhat

17. Example Problem A student determined that the substance he was working with took the shape of its container, had molecules that moved fast and were very far apart. He also determined that the substance was easily compressed into a smaller container. • GAS

18. PHASE CHANGES • -the process of absorbing or releasing energy to • change from one phase to another phase The types of phase changes include… • ____________: liquid changing to vapor(boiling) liquid + energy  vapor (gas) • ______________: vapor changing to liquid vapor  liquid + energy • ___________: solid changing to liquid solid + energy  liquid • ______________: liquid changing to solid liquid  solid + energy • _______________: solid changing directly to vapor without going through the liquid phase solid + energy  vapor • _______________: vapor changing directly to solid without going through the liquid phase vapor  solid + energy Vaporization Condensation Melting Freezing Sublimation Deposition

19. You will notice that all of the phase changes above either required an input of energy or they released energy. Each phase change is either: Exothermic: or Endothermic: Example 3-7. Which phase changes are exothermic? Example 3-8. Which phase changes are endothermic? A process that releases heat (heat exits the system) A process that takes in heat (heat enters the system) Condensation, Freezing, Deposition Melting, vaporization, sublimation

20. Thank you for entering the magical world of matter!!