1. Chapter 2 Matter Mixtures Elements and Compounds Chemical Reactions

2. What states of matter are represented?

3. Properties of Matter Matter – anything that has mass and takes up space Mass – amount of matter an object contains

4. Properties of Matter Substance – matter that has a uniform and definite composition Example: Sugar Pure Substance – only contains one kind of matter

5. Properties of Matter Physical Property – a quality of condition of a substance that can be observed or measured without changing the substances composition Example: Color, solubility, odor, hardness, density, melting point

6. States of Matter PropertySolidLiquidGas or Vapor Shape Volume Expansion on Heating Compressibility

7. States of Matter PropertySolidLiquidGas or Vapor ShapeDefiniteIndefinite VolumeDefinite Indefinite Expansion on Heating Very SlightModerateGreat Compressibility Almost Incompressible Readily Compressible

8. Physical Changes Cutting Grinding Bending Melting Freezing Boil Dissolve Split

9. Chapter 2.2 Mixtures What is a mixture? How can it be separated?

10. Classifying Mixtures Mixture – physical blend of two or more substances

11. Classifying Mixtures Heterogeneous – a mixture that is not uniform in composition, its components are readily distinguished Example: Salad

12. Classifying Mixtures Homogeneous - a mixture that is completely uniform in composition, its components are not readily distinguished Example: salt water

13. Classifying Mixtures Solution – homogenous mixture Example: Sterling Silver (Copper in silver)

14. Classifying Mixtures Phase – any part of a system with uniform composition and particles

15. Phase Homogeneous mixture – Single Phase Heterogeneous mixture – two or more phases

16. Separating Mixtures Separate physically by shape, size, color, etc… Separate with a magnet, filter Separate by distillation

17. Distillation A liquid is boiled to produce a vapor that is condensed back into a liquid Used to separate impurities in liquids

18. Matter MixturesPure Substance Homogenous Mixtures Heterogeneous Mixtures CompoundElements Solution

19. Ch 2.3 Elements and Compounds

21. Distinguishing Elements and Compounds Element – simplest form of matter that can exist, cannot be separated into simpler substances by chemical means

22. Top Ten Elements in the Human Body – Oxygen65% – Carbon18% – Hydrogen10% – Nitrogen3% – Calcium1.5% – Phosphorus1.2% – Potassium0.2% – Chlorine0.2% – Sulfur0.2% – Sodium0.1%

23. Distinguishing Elements and Compounds Compound – 2 or more elements that combine chemically, can be separated into simpler substances by chemical means

24. Sugar Sugar compound Carbon Element Water Compound + Water compound Hydrogen element Oxygen element + HEAT ELECTRICITY

25. Symbols and Formulas Chemical Symbols – One or two letters – First letter always capitalized – Second letter lower case

26. NameSymbolLatin Name SodiumNanatrium PotassiumKkalium AntimonySbstibium CopperCucuprum GoldAuaurum SilverAgargentum IronFeferrum LeadPbplumbum MercuryHghydrargyrum TinSnstannum TungstenWwolfram

27. Ch 2.4 Chemical Reactions

28. Chemical Reaction – the changing of substances to other substances by the breaking of bonds in reactants and the formation of bonds in products

29. Parts of a Reaction Reactants  Products Reactants – starting substances Products – substances formed

30. Chemical Property Ability of a substance to undergo a chemical reaction and form new substances

31. Examples of Chemical Reactions Burn Rot Rust Decompose Ferment Explode Corrode

32. Clues that a chemical reaction has occurred Heat given off Heat absorbed Odor given off Irreversibility

33. Law of Conservation of Mass Total mass of reactants = Total mass of products In any physical or chemical reaction, mass is neither created or destroyed