1. ICP Mr. Patel SWHS

2.  Continue to Learn Major Elements and Symbols  Classifying Matter  Physical Properties  Chemical Properties  States of Matter  Phase Changes

3.  Remember matter is anything that has mass and occupies volume.  Matter is described using properties that are extensive or intensive properties.

4.  Extensive Property – a property that depends on the amount of matter in a sample. (Changes with amount) Mass – measure of the amount of matter an object contains Volume – measure of the space taken up Other examples: energy, weight, length, area

5.  Intensive Property – a property that does NOT depend on the amount of matter Density – D = mass/volume matter per unit volume Other examples: hardness, melting/freezing point, concentration, viscosity

6. 1. The Boiling point of water is 100 O C. 2. The mass if 300 kg. 3. The length is 30 m. 4. The density of water is 1.0 g/mL. 1. Intensive 2. Extensive 3. Extensive 4. Intensive

7.  All matter can be divided into substances and mixtures  Substance – always has same composition  Every sample of a substance has identical properties because a substance has a fixed, uniform composition

8. Copper Kettle

9. Matter Anything that has mass and volume Substance Constant Composition; All particles identical Ex: Water, Helium Mixture Variable Composition; 2 or more substances Ex: Sand, Soil Physically Separate

10.  Substances can be classified as elements or compounds  Element – cannot be broken into simpler substances One type of atom only Atom – smallest particle of an element Ex: Gold, Hydrogen, Oxygen (on periodic table) Solids, liquids, gases

11. Make some observation…

12.  Compound – two or more elements chemically combined in fixed ratios Ex: Water, salt, baking soda  Compounds have different properties than parts  Compounds can be chemically separated to elements

13. Make some observation…

14. Matter Anything that has mass and volume Substance Constant Composition; All particles identical Ex: Water, Helium Mixture Variable Composition; 2 or more substances Ex: Sand, Soil Element Made up of identical atoms; on Periodic Table Ex: Zinc, Uranium Compound Made up of 2 or more elements; combined chemically Ex: Carbon dioxide Physically Separate Chemically

15.  Mixture – a physical blend of two or more components (substances)  Heterogeneous Mixture – the composition is not uniform throughout Ex: soil, chicken noodle soup Suspensions (“Shake Well”) or Colloids (Do not settle)  Homogeneous Mixture – (solution) composition is uniform throughout Ex: salt water, alloys (solid in solid)

16. Steel = Iron + Carbon

18. Matter Anything that has mass and volume Substance Constant Composition; All particles identical Ex: Water, Helium Mixture Variable Composition; 2 or more substances Ex: Sand, Soil Element Made up of identical atoms; on Periodic Table Ex: Zinc, Uranium Compound Made up of 2 or more elements; combined chemically Ex: Carbon dioxide Physically Separate Chemically Heterogeneous Uneven Distribution; easy to separate Ex: Vegetable Soup Homogenous Uniform Distribution; called solution Ex: Tap water, Steel

19.  Physical Property – measured properties that do not change the nature of the sample Ex: Boiling Point, Density, Mass  Physical Change – some properties may change but the composition of the material does not change Ex: Boiling, Freezing, Cutting, Splitting Can be Reversible or Irreversible

21. 1. Viscosity – resistance to flow (thickness) 2. Conductivity – ability for heat to flow 3. Malleability – hammered into sheets 4. Hardness 5. Melting/Boiling Point 6. Density

22.  Physical Changes do not involve chemical reactions No Breaking or Forming Chemical Bonds Substance is the same before and after the change

23.  Mixtures can be separated physically  Filtration – solid from liquid  Distillation – liquid from liquid or solid

24.  Chemical Property – the ability of a substance to undergo a chemical reaction Ex: Flammability, Combustibility, decomposition  Chemical Change – the composition of matter will always change Ex: Burning, exploding, reacting, rusting, rotting Also called a chemical reaction

26. 1. Flammability– ability to burn with oxygen 2. Reactivity – ability to chemically combine with other substances

27.  Clues for a chemical reaction: 1. Transfer of Energy – heat, sound, light 2. Color Change 3. Gas Production 4. Formation of Precipitate – solid that settles out of a liquid mixture Don’t confuse for a physical change

29.  Law of Conservation of Mass – mass is neither created nor destroyed; it is only transformed.  The mass before a reaction must always equal the mass after a reaction

31. 1. Burning Gasoline 2. Evaporation of Water 3. Stripping a Copper Wire 4. Mold Growing on Yogurt 5. Alka-Setlzer tablets 1. Chemical 2. Physical 3. Physical 4. Chemical 5. Chemical

32.  There are four states of matter 1. Solid 2. Liquid 3. Gas 4. Plasma  We focus mostly on the first three

33.  Definite Shape  Definite Volume  Incompressible  Particles tightly packed - ordered  Vibrations (Not Fluid)

35.  Indefinite Shape  Definite Volume  Incompressible  Particles in contact but disorderly packed  Particles flow (Fluid)

37.  Indefinite Shape  Indefinite Volume  Highly Compressible  Particles far apart; little contact; collisions  Particles flow (Fluid)

38.  Particles: Have a lot of space between them Are in rapid motion Exert Pressure = Billions of collisions Spontaneously expands

40.  There are 6 state/phase changes  Some change require heat (energy)  Endothermic – requires heat  Exothermic – releases heat

41.  Solid to Liquid  Endothermic  Particles have enough energy to begin to flow  Melting Point – temp when liquid forms

42.  Liquid to Solid  Exothermic  Particles have lose energy and slow down  Freezing Point – temp when Solid forms  Mpt = Fpt

43.  Liquid to Gas  Endothermic  Particles have enough energy to break away  Boiling Point – temp when gas forms

44.  Gas to Liquid  Exothermic  Particles begin to stick  Same as Bpt

45.  Solid to Gas  Endothermic  NO liquid stage  Ex: Dry Ice

46.  Gas to Solid  Exothermic  No Liquid Stage  Ex: Snowing