1. What is Chemistry  Chemistry ‑ the study of matter and the changes matter undergoes.  Matter ‑ something that has mass and takes up space (has a volume).

2. States of Matter  Law of Conservation of Mass & Energy- Matter can never be created nor destroyed; neither gained nor lost. It must be conserved.

3. Mass vs. Weight Mass: How much stuff matter) a material contains Weight: A measure of the effect of gravity

4. Characteristics of Matter Chemical Properties  Ability for a substance to undergo a chemical change (new stuff)  Examples. Ability to burn Ability to burn Ability to rust Ability to rust Ability to sour Ability to sour

5. Physical Properties Physical Properties observed or measured without altering makeup of substance (still the same stuff)  Examples mass mass weight weight volume volume color color solubility solubility luster luster melting point melting point boiling point boiling point

6. Intensive vs. Extensive Properties Extensive  depends on amount of matter present  Examples mass mass weight weight volume volumeIntensive:  doesn't depend on amount present  Examples color solubility luster melting point boiling point

7. Classification of Matter Separation

8. Classification of Matter Pure Substances  Elements- 118 on Periodic Table organized according to properties.  Named after famous scientists, countries, states, and planets  Abbreviation (Element symbols) begin with first letter capitalized.  Examples Al - aluminum Al - aluminum O - oxygen O - oxygen Hg - mercury (Latin hydrargyum) Hg - mercury (Latin hydrargyum) Au - gold (Latin Aurum) Au - gold (Latin Aurum) Cl - chlorine Cl - chlorine

9. Classification of Matter Compounds: element combined in a chemical rxn (reaction).  Can not be physically separated.  Many have both common names and scientific names.  Abbreviations (Chemical formulas) use element symbols  Examples NaClsodium chloridesalt NaClsodium chloridesalt NaOHsodium hydroxideDrano NaOHsodium hydroxideDrano NaHCO3sodium bicarbonate Baking Soda NaHCO3sodium bicarbonate Baking Soda H2ODihydrogen monoxideWater H2ODihydrogen monoxideWater

10. Pure SubstancesMixtures Separation Separation by Physical Means 1. Filtration 2. Evaporation 3. Distillation 4. Chromatography Separation

11. Classification of Matter Mixtures: can be physically separated  Methods of separation Filtration – solid/liquid Filtration – solid/liquid Evaporation or crystallization – dissolved substance Evaporation or crystallization – dissolved substance Distillation – purifies a liquid or separates 2 liquids, based on different boiling points Distillation – purifies a liquid or separates 2 liquids, based on different boiling points Chromatography – separates a solution by allowing it to flow along a stationary substance (liquid, gas, paper). Chromatography – separates a solution by allowing it to flow along a stationary substance (liquid, gas, paper).

12. Classification of Matter Types of Mixtures Homogeneous - the same composition throughout  Examples: Pure air or Solutions (Kool-aid) Pure air or Solutions (Kool-aid) Alloys – Brass, Steel, Silverware Alloys – Brass, Steel, Silverware Heterogeneous- varying composition throughout  Examples: Chocolate Chip Cookies Chocolate Chip Cookies River water River water

13. Types of Changes Substances can undergo three types of changes:  Physical  Chemical  Nuclear

14. Physical  Physical- though appearance (color, shape) may change, the mass will still be the same since the molecules remain the same  Examples: Bending Bending Tearing Tearing Melting Melting

15. Separation Cont’d Compounds can only be separated chemically into elements ElementsCompounds Separation

16. Chemical  Chemical- (Rxn) the structure of the substance changes. The new substance possesses different chemical and physical properties  Examples: Burning Burning Molding Molding Souring Souring

17. Parts of Chemical RXN 2 parts to a Chemical Rxn  Reactants  Products  Starting substances yields new substances with new properties. Three Indicators of Chemical Rxn’s  Formation of heat and/or light (energy)  Formation of a new gas (bubbles or fizzes)  Formation of a precipitate (solid formed for two solutions)

18. Nuclear  the structure of the nucleus changes. The energy involved is 6 to 8 times the Magnitude of a chemical or physical change.

19. Bunsen Burner Notes