1. Matter and Change 2.1 Properties of Matter 2.2 Mixtures
2.3 Elements and Compounds
2.4 Chemical Reactions

2. Objectives: 2.1 Properties of Matter
Identify properties of matter as extensive and intensive
Define physical and chemical properties
Differentiate between the 3 states of matter

3. KEY TERMS Mass Volume Extensive Property Intensive Property Substance
Physical Property
Solid
Liquid
Gas
Vapor
Physical Change

4. Definitions
Mass (m) – the amount of matter an object contains (a numerical value
of its inertia)
Volume(V) – the amount of space an object occupies
Extensive
property - a property that depends on the amount of matter an object
contains
Intensive
property – a property that depends on type of matter an object contains
Substance – matter with uniform properties
Physical
property - a quality or condition of a substance that can be observed without
changing the composition of the substance
Chemical
property – a quality or condition of a substance that can be observed with
change - a change that do not affect the composition of a substance
change – a change that does affect the composition of a substance

5. Some Criteria for the Classification of Matter
Properties
State (solid, liquid, gas)
Composition

6. Intensive and Extensive Properties
Sulfur

7. Examples of Physical Properties
Color, odor, hardness, density, melting point, boiling point, state, solubility.

8. Example: Physical Properties
Substance
State
Color
Melting
Point (C°)
Boiling Point (C°)
Density (g/cm3)
Oxygen O2
Gas
Colorless
-218
-183
0.0014
Mercury Hg
Liquid
Silvery-white
-39
357
13.5
Bromine
Br2
Red-brown -7 59
3.12
Water
H2O
100
1.00
Sodium Chloride
NaCl
Solid
White
801
1413
2.17

9. fixed shape and volume, incompressible Liquid
States of Matter
Solid
fixed shape and volume, incompressible
Liquid
fixed volume, takes the shape of its container
Gas
takes the volume and shape of its container

11. Solid Liquid Gas

12. Bromine
Gas (Vapor)
Liquid

13. Change of Phase Melting solid  liquid Condensation gas  liquid
Freezing liquid  solid
Evaporation liquid  gas
Sublimation solid  gas
Boiling: Evaporation occurring beneath the liquid’s surface.

14. Is changing phase a physical or chemical change?

15. Classification of Matter (by composition)

16. Matter that has a uniform and definite composition.
(Pure) Substance
Matter that has a uniform and definite composition.
Elements
Compounds

17. 2.2 MIXTURES
Objectives:
Categorize samples of matter into substance or mixture
Differentiate between homogeneous and heterogeneous
Describe two ways that components of mixtures can be separated

18. KEY TERMS Mixture - physical blend of 2 or more substances
Heterogeneous – mixture in which the composition is not uniform
throughout
Homogeneous – mixture with a uniform composition throughout
Phase – a part of a mixture with uniform composition
Solution – another name for homogeneous mixture
Filtration a process that separates a solid from a liquid
Distillation a process that separates a solid dissolved in a liquid/
separation of 2 miscible liquids with different boiling
temperatures
Miscible or more liquids that can form a homogeneous mixture

19. A physical blend of two or more substances.
Mixture
A physical blend of two or more substances.

20. Copper II Sulfate and its solution in water.

21. Example: Stainless Steel
A homogeneous mixture of:
-Iron (Fe)
-Chromium (Cr)
-Nickel (Ni)

22. Example: Gaseous Mixture
Elements argon and nitrogen and a compound (water vapor).

23. Heterogeneous Mixtures
Example:
Oil and vinegar
Non-uniform composition throughout the mixture
Two or more phases.

24. Mixtures can be physically separated.
Note:
Mixtures can be physically separated.
Mixtures exhibit physical properties similar to the components of the mixture.

25. Separation Methods
Use differences in the physical properties of the components of the mixture.

26. Example: Separate iron filings from sulfur using a magnet.

27. Filtration: separates a solid from a liquid in a heterogeneous mixture

28. Distillation: -separate dissolved solids from a liquid -uses boiling and condensation.

29. Distillation of Crude Oil (Refining)
Crude Oil is a mixture of Hydrocarbons

30. Distillation of Crude Oil

31. c) Elements and Compounds

32. The simplest substances. Can not be separated into simpler substances.
Elements
The simplest substances.
Can not be separated into simpler substances.
Building blocks of all matter.
More than 100 known elements.
Represented by chemical symbols.

33. Chemical Symbols of Elements
System started by Jons Berzelius (Sweden, )
One or two first letters of name of the element.
Many elements names have roots from: Latin, Greek, mythology, geography, names of scientists.

34. Examples: Americium, Am Einsteinium, Es Bromine, Br Helium, He
Lead(Plumbum), Pb
Niobium, Nb
Iron (Ferrum), Fe
Mendelevium, Md

35. Compound
A substance that contains two or more elements chemically combined.
Compounds have different properties from the individual substances.
(Ex: H2O)

36. Example: H2O

37. If composition is fixed and may not changesubstance
Substance or mixture?
If composition is fixed and may not changesubstance

39. d) Chemical Properties and Chemical Changes

40. H2O composition is fixed- compound
Gaseous Phase
Liquid Phase

41. Chemical Properties
The ability of a substance to transform into a new substance (to undergo a chemical change).
Example: Magnesium reacts with oxygen to form magnesium oxide.

42. Magnesium Mg

43. Burning of Magnesium 2Mg+ O2 2MgO

44. Physical Changes
Physical change: a change in the physical properties of a substance.
Composition does not change.
May be reversible or irreversible.
Examples:
Reversible:
Irreversible:

45. Chemical Change
A change that produces matter with a different composition than the original matter.
Atoms rearrange themselves into new combinations.

46. Burning of Methane CH4 +2O2 CO2 + 2H2O

47. Burning of Methane CH4 + 2O2 CO2 + 2H2O

48. Recognizing a Chemical Change
energy exchange
production of a gas
color change
formation of a precipitate

49. Formation of a Precipitate
Cu(OH)2
Precipitate

50. The Law of Conservation of Mass (Antoine Lavoisier)
In any chemical or physical change, mass is neither created or destroyed
Mass is CONSTANT