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MATTER

Explore the properties of matter, including physical and chemical properties, as well as the different states of matter. Discover how matter can undergo physical and chemical changes. Learn about elements, compounds, and mixtures, and how they can be separated or combined.

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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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