1. Matter chapter 3

2. Matter Anything that has mass & occupies space
Mass: measured in grams or kilograms
Space/volume: measured in liters or cm3

3. Phases
SOLIDS
LIQUIDS
GASES

4. Solid:
definite volume
definite shape

5. Liquid
definite volume
indefinite shape
takes the shape of container

6. Gas indefinite volume indefinite shape
takes the shape and volume of container

7. States of Matter How are the particles packed in each phase?
How do the particles move in each phase?
Why do liquids and gases flow?
Why are gases so easy to compress?

8. 4th Phase of matter Plasma exists in stars
electrons are stripped from atoms

9. Physical Properties Describe appearance & form of matter
Descriptive words:
color, texture, luster, odor
solid, liquid, gas
Measurements:
a number and a unit

10. Intensive properties Physical Constants independent of sample size
Density, freezing point, and melting point
Solubility in water (g/ml)

11. Extensive Properties
Extensive properties (mass  volume) depend on quantity (amount) of matter in sample

12. Chemical Properties Describe how:
matter behaves in presence of other matter
matter changes into another kind of matter
examples:
Flammability
resistance to corrosion
ability to neutralize acids or bases

13. Properties of Copper Physical Prop. reddish brown shiny malleable
Ductile
good conductor
density = 8.92 g/cm3
mp = 1085C
bp = 2570C
Chemical Prop.
reacts to form green copper carbonate
forms deep blue solution when in contact with NH3
forms new substances with HNO3

14. Physical Change
form or appearance of matter may change but identity remains same
cutting, crushing, grinding,tearing
phase changes
dissolving

15. Dissolving Dissolving is physical change think of sugar in water
still have sugar – sugar molecules just spread out between water molecules
C6H12O6(s)  C6H12O6(aq)

17. Phase Changes Phase changes are physical changes
No new substance is created (chemical formula stays the same)
Ex:
ice melting: H2O(s)  H2O(l)
water boiling: H2O (l)  H2O(g)

18. Chemical Change Ex: 2H2O(l)  2H2(g) + O2(g)
chemical change - identity of matter is changed
new substance with own unique properties is formed
chemical formula changes
Ex: 2H2O(l)  2H2(g) + O2(g)

19. Burning common name for oxidation reaction
indicates matter reacting with oxygen
is chemical change - original substance is changed into new kind(s) of matter
Ex:
CH4(g) + 2O2(g)  CO2(g) + 2H2O(g)

20. What kinds of matter are there?

21. Matter Substances Mixtures Mixtures  Separated by physical methods
Elements
Compounds
Heterogeneous
Homogeneous
Mixtures  Separated by physical methods
Compounds  Separated by chemical methods

22. Element substance that: formulas have 1 uppercase letter
cannot be broken down (decomposed) into simpler substance
only 1 kind of atom
has definite properties
formulas have 1 uppercase letter

23. Element Song

24. Atom smallest particle of element that retains properties of element
smallest particles of element that can undergo a chemical reaction

25. Compounds 2 or more elements chemically combined in a definite ratio
properties are different from those of elements formed from
homogeneous
broken into elements by chemical decomposition reaction
formulas have 2 or more uppercase letters

26. Cl(g)
Na(s)
2Na + Cl2  2NaCl
NaCl(s)

27. Mixtures combo of 2 or more pure substances
physically combined not chemically combined
each substance retains its own identity and properties

28. Mixtures variable composition no unique properties
(think of sugar and salt mixed together)
separated by physical methods
may be homogeneous or heterogeneous

29. Types of Mixtures

30. homogeneous: constant composition throughout, single phase
ex: solutions (all 3 phases)
such as air, windex, kool-aid

31. heterogeneous: See a boundary or regions that look different
ex: ice water, granite
suspensions, colloids

32. Suspensions
particles in suspensions are larger than those in solutions
components of suspension can be evenly distributed by mechanical means (shaking the contents) but components will settle out

33. Colloids
particles larger than size of molecule but smaller than particles seen with naked eye
colloidal dispersion
consists of colloids in a dispersing medium
ex: whipped cream,
mayonnaise, milk,
butter, gelatin, jelly,
colored glass

34. Colloid subtypes

35. Aerosols:
solid or liquid particles in gas Ex:
Smoke: solid in a gas
Fog: liquid in a gas

36. Sols:
solid particles in a liquid
ex: Milk of Magnesia (solid magnesium
hydroxide in water)

37. Emulsions:
liquid particles in liquid
ex: mayonnaise: oil in water

38. Gels:
liquids in solid ex:
gelatin: protein in water
quicksand: sand in water

39. Hints for Mixtures solutions in gas & liquid phases transmit light
particles not big enough to scatter light
look translucent
suspensions look cloudy
particles big enough to scatter light
settle on standing

41. CuSO4(aq)
source
source

42.         Particle Diagrams atoms of a monatomic element       
molecules of a diatomic element        

43.          Particle Diagrams molecules of a triatomic compound       
mixture:
monatomic element, diatomic element, triatomic compound             

44. Separating Mixtures physically combined
separation based on physical properties
sorting: size & appearance
filtration: size solid in liquid
distillation: different bp’s liquids mixed
crystallization: solubility solid in liquid
magnet: magnetization
chromatography: solubility liquids mixed
“Travel” ability

47. Distillation

48. Paper Chromatograhy

49. Crystallization

50. Conservation of Mass mass begin with = mass end up with
# of atoms before =
# of atoms after