1. Matter chapter 3

2. Matter Anything that has mass and occupies space
Mass is measured in grams or kilograms
Space or volume is 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?
source
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 the appearance and form of matter 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 Mass  volume
depends on amount of matter in sample
Extensive properties depend on quantity of matter

12. Chemical Properties
Describe how matter behaves in presence of other matter
Describe how matter changes into another kind of matter
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 a deep blue solution when in contact with NH3
Forms new substances with HNO3

14. Physical Change
The form or appearance of sample 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 – you just spread it out with water molecules in between
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 chemical change - identity of matter is changed
new substance with unique properties is formed
The chemical formula changes
Ex: 2H2O(l)  2H2(g) + O2(g)

19. Burning Common name for oxidation reaction
Burning means reacting with oxygen
Burning is chemical change, because original substance is changed into new kinds 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 or decomposed into simpler substance
only 1 kind of atom
has definite properties
Formulas have 1 uppercase letter

23. Element Song
Big Bang Version sung by Sheldon

24. Atom smallest particle of element that retains properties of element
smallest particles of element that can undergo a chemical reaction
Atoms can be combined to form molecules

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. Elements can be chemically combined to form compounds, atoms are combined to form molecules
Molecule: A substance that is made up of 2 or more atoms of elements
Examples:
H2, O2, N2
Note: theses are not compounds because each is composed of a single element
H2O, CO2 are molecule, but they are also compounds

27. 2Na + Cl2  2NaCl Na = atom, element Cl2 = molecule, element
NaCl = molecule, compound
Atoms or Molecules?
Element or Compound?

28.         Particle Diagrams Atoms of a monatomic element       
Molecules of a diatomic element        

29.          Particle Diagrams Molecules of a triatomic compound       
Mixture:
monatomic element, diatomic element, triatomic compound             

30. Mixtures Combo of 2 or more pure substances
Physically combined not chemically combined
Each substance retains its own identity and properties

31. Mixtures Variable composition No unique properties
(Think of sugar and salt mixed together)
Separated by physical methods
May be homogeneous or heterogeneous

32. Types of Mixtures
Heterogeneous: definite variation in composition, individual components visible (2 types – colloids and suspensions)
Oil in water
Salad dressing
Granite

33. Colloids (type of heterogeneous mix.)
Particles are suspended- they are too small to see but they are larger than molecules (like Sugar, Salt, etc)

34. Example of Colloids: Aerosols: solid or liquid particles in gas
Ex: Smoke: solid in a gas
Gas in liquid:
Ex: whipped cream
Emulsion: liquid in liquid
Ex: mayonnaise (oil suspended in water – use egg yolk to
Sols: solid particles in a liquid
Ex: Milk of Magnesia (solid magnesium hydroxide in water)
Gels: Liquid in solid
Ex: Quicksand: sand in water

35. 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
Settle out on standing
Can scatter light

36. Homogeneous (aka solutions): constant composition throughout, individual components not visible
Ex: salt water

37. Solution vs Suspension
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

39. CuSO4(aq)
source
source

40. Separating Mixtures Physically combined
Separation based on physical properties
1. Sorting: size & appearance

41. 2. Filtration: size solid in liquid
Can you filter a solution? Like sugar water?
NOTE: Sand and water is SiO2 + H2O or SiO2(aq)

42. 3. Distillation: different bp’s liquids mixed

43. 4. Crystallization: solubility solid in liquid

44. 5. Magnet: magnetization

45. 6. Chromatography: solubility liquids mixed - “Travel” ability

46. Conservation of Mass Mass before = Mass after # of atoms before =
# of atoms after