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MATTER

MATTER. Matter – has mass & occupies space – 1:25. I. Properties of Matter. A. Physical prop. – any characteristic that can be observed or measured without changing the material;

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MATTER

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  1. MATTER

  2. Matter – has mass & occupies space – 1:25

  3. I. Properties of Matter A. Physical prop. – any characteristic that can be observed or measured without changing the material; Ex. color, mass, volume, length, density, shape, taste, odor, texture, hardness, conductivity, melting/ boiling points, metal, nonmetal, states of matter

  4. Physical Properties – 3:39

  5. States of Matter 1. Solid – particles close together; low energy; definite shape & volume 2. Liquid – particles medium distance & energy; no def. shape & def. volume 3. Gas – particles far apart; high energy; no definite shape or volume (Plasma – occurs at high temps.)

  6. States of Matter – 4:35

  7. B. Chemical prop. – characteristic that allows a substance to change to a new substance Ex. flammability (burning) – paper, wood, oxygen rusting (reaction) – iron tarnishing (reaction) – silver, copper reactivity (reacts w/other substances) – vinegar w/baking soda; sodium + water;

  8. Chemical Properties – 1:16

  9. 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 change of state – melting/freezing

  10. B. Chemical changes – changes to new substance; 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

  11. Chemical Changes – 6:10

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

  13. Kitchen Oil Fire

  14. III. 3 Basic Kinds 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

  15. Atom looks like: Protons + Neutrons

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

  17. Ex. Lithium: 3 = 3 p+ / 3 e- Li 6.941 = round to 7 then subtract 3 = 4 neutron Ex. Gold = 79 p+/ 79 e- = round to 197 then subtract 79 = 118 neutron

  18. 4. Electrons found in shells – 1st: 2 e- max. - 2nd: 8 e- max. - 3rd: 18 e- max. 6 protons 6 neutrons 6 total electrons – 2 in 1st shell & 4 in 2nd shell

  19. Lithium protons = 3 neutrons = 4 total electrons = 3 2 e- in 1st shell 1 e- in 2nd shell

  20. Practice: Oxygen: Sodium: Aluminum

  21. Structure of Matter – Elements: 2:28

  22. 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

  23. 2. Metal elements (left side) combine with nonmetal elements (right side) to form compounds - metals give up e- to have + charge; - nonmetals take e- to have - charge

  24. - The different charges must balance out to zero: add subscript #s to have a zero charge Na: +1 ; Cl: -1  NaCl Mg: +2 ; Cl: -1  MgCl2 Al: +3 ; F: -1  AlF3 (use cards to make compounds)

  25. 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)

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

  27. (Don’t have to write this down) Law of Conservation of Mass/Matter # of atoms & mass before & after is the same Cl2 + 2NaBr  2NaCl + Br2 71 g 206 g  117 g + 160g Fe 2O 3 + 6HCl  2FeCl3 + 3H2O 160 g + 219 g  325 g + ? g 2H2O2  2 H2O + O2 68 g  36 g + ? g

  28. Compounds - 3:59

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

  30. 1. Homogeneous mixture – same composition throughout called a solution (solute = dissolved substance + solvent = dissolver – water is called the universal solvent) Ex. saltwater (salt is the solute & water is the solvent); air, motor oil, tea

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

  32. Physical Changes/Mixtures – 6:43

  33. THE END!!

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