MATTER – has mass & occupies space

2. MATTER – has mass & occupies space

3. Matter -1:25

4. I. Properties of Matter • Physical properties 1. Definition - any characteristic that can be observed or measured without changing the material; Think!! – What can you physically observe in a material? - What could you measure in a material?

5. 2. Examples - color, mass, volume, length, luster, density (m/v), shape, taste, odor, texture, hardness, conductivity, melting/ boiling points, metal, nonmetal, states of matter

7. Physical Properties – 3:39

8. 3. States of Matter a. Solid – particles close together; low energy; definite shape & volume b. Liquid – particles medium distance & energy; no def. shape & def. volume c. Gas – particles far apart; high energy; no definite shape or volume (Plasma – occurs at high temps.)

10. States of Matter – 4:35

11. d. Phase Diagram – states affected by pressure & temp. Phase diagram of water –melting, freezing, evaporation, condensation – add to diagram

12. Phase diagram of CO2

13. B. Chemical property – 1. Definition - characteristic that allows a substance to change to a newsubstance Think! – How could paper or wood turn to a new substance? - How could copper or a nail turn to a new substance?

14. 2. Examples - flammability (burning) – paper, wood, oxygen rusting (reaction) – iron tarnishing (reaction) – silver, copper reactivity (reacts w/other substances) – vinegar w/baking soda; sodium + water; fireworks

15. Chemical Properties – 1:16

16. II. Changes of Matter A. Physical changes – only changes what the substance looks like; not something new Ex. separating substances – (ex. coins) crushing/grinding – making smaller combining of substances – dye + water change of state – melting/freezing

17. B. Chemical changes – changes to a newsubstance; signs: production of heat, light, smoke, change in color or smell, Ex. Burning rusting – Fe + O2 Fe2O3 tarnishing – Ag2O + H2SAg2S + H2O reactions Photo. CO2 + H2O  C6H12 O6 + O2

18. Chemical Changes – 6:10

19. 1. How could you change an egg physically? 2. How could you change an egg chemically?

20. Kitchen Oil Fire

21. III. Basic Types of Matter – elements, compounds, & mixtures A. Elements – composed of 1 kind of atom; pure - (found on the periodic table) 1. Ex. C, H, N, O, P, S, Au, Ag, Cl, Fe, Ca, Na, He, Ne, Cu 2. Atom – simplest indivisible particle a. proton: + charge; in nucleus b. neutron: neutral charge; in nucleus c. electron: - charge; in shells

22. Atom looks like:

23. 3. Finding # of p+, n, & e- : look at periodic table – different #s give different properties Top # = # of protons, # of electrons (P,E) Bottom # rounded = mass # = (mass of nucleus) # of protons + neutrons # of protons = ______ # of electrons = _____ mass # = __________ # neutrons = _______

24. Ex. Lithium: 3 = 3 p+ / 3 e- Li 6.941 = round to 7 then subtract 3 = 4 neutrons Ex. Sodium (Na) – do on own

25. Structure of Matter – Elements: 2:28

26. B. Compounds – 2 or more elements chemically combined; can’t be physically separated; pure 1. Have formulas – atoms have definite ratios - NaCl; H2O; CO2; MgO, NH3 (ammonia), C6H12O6 (glucose) subscript gives you # of atoms of each element – ex. NaCl : 1 Na & 1 Cl H2O : 2 H & 1 O NH3 : 1 N & 3 H

27. 2. Metal elements (left side) often combine with nonmetal elements (right side) to form compounds

28. 3. Compounds go through chemical rxns: # of atoms & mass of reactants must equal # of atoms & mass of products (law of conservation of matter/mass) reactants  products 2H + 2 O  H2O2 (same # of atoms) 2 g H + 32 g O  34 g H2O2 (same mass)

29. 4. LAW OF CONSERVATION OF MASS/MATTER = mass/matter of the reactants = the mass of the products; mass is neither created nor destroyed

30. Compounds - 3:59

31. C. Mixtures – 2 or more substances physically combined; can be separated into pure substances

32. 1. Homogeneous mixture – same composition throughout called a solution; evenly mixed Ex. saltwater, coffee, koolaid, air, motor oil, tea Water often does the dissolving in a mixture – called the “universal solvent”

33. 2. Heterogeneous mixture – has different composition throughout; unevenly mixed Ex. muddy water, concrete, granite, lemonade w/pulp, watch

34. Physical Changes/Mixtures – 6:43

35. IV. Application A. E,C, M – form all natural resources such as:. Oil, coal, natural gas, metals, stones, sand, air, sun, soil, water, animals, birds, fish and plants. B. Natural resources are used to make: food, alternative fuels and raw materials for the production of goods, such as paper, medicines, electronics, clothes, appliances, & cars

36. Products Made from Natural Resources • Trees Paper, furniture, fuel • Cotton Clothing • Oil/petroleum Plastic, fuel • Natural gas Fuel • Coal Fuel • Iron ore Steel products (cans, bridges) • Bauxite ore Aluminum products (cans, car • parts) • Gold Jewelry, dental material • Copper Wire, coins, electrical equipment • Manganese Steel, cast iron • Cobalt Steel, jet engine parts, cutting • tools • Platinum Air pollution control and telecommunications • equipment, jewelry • Chromium Stainless steel, green glass, • leather treatment • Diamonds Jewelry, mechanical equipment

37. C. Natural resources impact society - can cause environmental problems such as: air, land and water pollution; disruption or destruction of ecosystems; and a decrease in biodiversity. D. Natural resources are: LIMITED – Therefore, we need to reduce, reuse, & recycle

38. THE END!!