MATTER – has mass & occupies space

Matter - 1:25

I. Properties of Matter A.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?

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

Physical Properties – 3:39

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.)

States of Matter – 4:35

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

Phase diagram of CO 2

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

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

Chemical Properties – 1:16

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

B. Chemical changes – changes to a new substance; signs: production of heat, light, smoke, change in color or smell, Ex. Burning rusting – Fe + O 2  Fe 2 O 3 tarnishing – Ag 2 O + H 2 S  Ag 2 S + H 2 O reactions Photo. CO 2 + H 2 O  C 6 H 12 O 6 + O 2

Chemical Changes – 6:10

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

Kitchen Oil Fire

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

Atom looks like:

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 = _______

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

Structure of Matter – Elements: 2:28

B. Compounds – 2 or more elements chemically combined; can’t be physically separated; pure 1. Have formulas – atoms have definite ratios - NaCl; H 2 O; CO 2 ; MgO, NH 3 (ammonia), C 6 H 12 O 6 (glucose) subscript gives you # of atoms of each element – ex. NaCl : 1 Na & 1 Cl H 2 O : 2 H & 1 O NH 3 : 1 N & 3 H

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

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  H 2 O 2 (same # of atoms) 2 g H + 32 g O  34 g H 2 O 2 (same mass)

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

Compounds - 3:59

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

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”

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

Physical Changes/Mixtures – 6:43

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

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

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

THE END!!