1. Classification of Matter
Unit 3.3:
Classification of Matter
Vocabulary: matter, mass, volume, substance, chemical change, physical change, state, particle, gas, liquid, solid, attract

2. Vocabulary:
system
phase
atom
molecule
compound
ion
mixture
homogeneous substance
heterogeneous substance
solution
solvent
solute

3. 2.3: Classification of matter
System: the entire “universe” being studied
Phase: any part of the system that is uniform in composition and properties
ex: oil and water
You can see the boundary between the oil and water. This is a 2 phase system

4. 2.3: Classification of matter
Atom: the smallest unit of an element
Cannot be broken down into a simpler type of matter
Ex: Ag (silver), C (carbon)
Molecule: 2 or more atoms held together
Ex: H2O, NaCl, H2

5. 2.3: Classification of matter
Ion: an atom or molecule with a charge
Ex: Na+, Cl-, NO3-, NH4+
Atoms gain or lose
electrons to form an ion

6. DESCRIBING MATTER:

7. Classifying Matter
Matter

8. Classifying Matter
Matter
Pure Substances

9. Classifying Matter
Matter
Pure Substances Mixtures

10. Pure Substance  A substance that is homogeneous and has an unchangeable composition
Examples: sugar, water, copper, iron
Mixture  A system made up of two or more substances, such as the relative amounts can be VARIED (different)
Examples: Salt dissolved in water

11. 2.1 Elements - The Most Simple Kind of Matter
Pure Substance: “Something that with a uniform, fixed
composition at the submicroscopic level”
Recognized by the unchanging nature of their properties
Element: “A pure substance composed of only one kind of atom”
Atom: “The smallest particle of an element”
Atoms of different elements are different and are shown
on the periodic table
Each element has a one or two letter abbreviation
Hydrogen - H
Helium - He
Sodium - Na
Lithium - Li
S 2.0 The Chemical View of Matter

12. Classifying Matter Matter Pure Substances Mixtures
Elements Compounds/molecules

13. 2.3: Classification of matter
Mixture: a group of 2 or more substances that are physically mixed
there are homogeneous and heterogeneous mixtures

14. Examples: Air, water, salt water, a piece of iron
Homogeneous: A substance consisting of only ONE PHASE (gas, liquid, or solid)
Examples: Air, water, salt water, a piece of iron
Heterogeneous: A substance consisting of MORE THAN one phase (gas, liquid, and/or solid)
Examples: A human being, a pencil

15. 2.3 Mixtures and Pure Substances
Homogeneous Sample: “ Matter that has a uniform appearance
and composition throughout “
A mixture of water and alcohol
Sugar dissolved in water
Gold blended with silver (18 karat gold)
The air we breathe - a mixture of oxygen and nitrogen
Solutions: “Homogeneous mixtures, either liquid, solid or gaseous”
continue…..
S 2.0 The Chemical View of Matter

16. Homogeneous Mixtures Homo means “same” Looks like one substance
1 phase
Called solutions  ex: milk tea, water and salt

17. Heterogeneous Mixtures
Hetero means “different”
You can see all the different parts of the mixture
Called mechanical mixtures  ex: m&m’s, sand and water

18. Sand and water do not mix to form a uniform mixture
Copyright 1999, PRENTICE HALL
Chapter 1

19. 3.3 Mixtures:
The substances are mixed together but are not chemically combined
mixtures can be separated into their parts by physical changes

20. Solution: homogeneous mixtures of 2 or more substances
Solvent: dissolves things (usually bigger quantity)
Solute: gets dissolved (usually smaller quantity)
Example: salt and water Solvent = Solute =

22. NaCl(s) + H2O(l)  NaCl(aq)
Aqueous solutions are solutions where the solvent is water.
NaCl(s) + H2O(l)  NaCl(aq)
(aq) = aqueous

23. Types of Solutions Type of Solution Example Gas-in-Gas solution
Air (Nitrogen, Oxygen)
Gas-in-Liquid solution
Soda Pop (Coke Zero…MMMMM!)
Liquid-in-Liquid solution
Water and alcohol
Solid-in-Liquid solution
Salt water
Solid-in-Solid solution
Alloys (Metals melted together)

24. Classifying Matter Matter Pure Substances Mixtures
Elements Compounds/molecules
Classify followings as pure substances and mixtures?
a. Sugar b. dirt c. air

25. Classifying Matter Matter Pure Substances Mixtures
Elements Compounds Homogenous Heterogeneous

26. 2.3: Classification of matter
Compound: pure substance made up of 2 or more different atoms
Ex: H2O, NaCl, C6H12O6
All compounds are also molecules
Not all molecules are compounds (ex: H2, O2) are molecules NOT compounds

27. 2.2 Chemical Compounds (cont)
Compound: “ Any pure substance that can be decomposed by a
chemical change into two or more pure substances
is a compound “ - (another definition)
Compounds are made up of elements
Examples of Compounds:
Water H2O Ethanol C2H6O
Salt NaCl Sugar C6H12O6
Examples of Mixtures of Compounds:
Pepper
Beer, Wine & Soda Pop
Milk
Cheese
continue…..
S 2.0 The Chemical View of Matter

28. 2.2 Chemical Compounds - Atoms in Combination
Chemical Compounds: “ Pure substances made of atoms of different
elements combined in definite ways”
Examples:
H2O Water
NaCl Sodium Chloride
C2H6O Ethanol
C6H12O6 Sugar
S 2.0 The Chemical View of Matter

29. Classification of Matter
Elements
There are 114+ elements known.
Each element is given a unique chemical symbol (one or two letters).
They are building blocks of matter.
The earth’s crust consists of 5 main elements (shown next slide).
The human body consists mostly of 3 main elements (O, C, and H).
Copyright 1999, PRENTICE HALL
Chapter 1

30. The Periodic Table and the Elements
Main Group
Elements
Main Group Elements
Transition Metals
Inner Transition Elements
Copyright 1999, PRENTICE HALL
Chapter 1

31. Classification of Matter
Elements
Copyright 1999, PRENTICE HALL
Chapter 1

32. Classification of Matter
Compounds
Most elements interact to form compounds.
The proportions of elements in compounds are the same irrespective of how the compound was formed.
Law of Constant Composition (or Law of Definite Proportions):
The composition of a pure compound is always the same.
Therefore, if water is decomposed, then there will always be twice as much hydrogen gas formed as oxygen gas.
Copyright 1999, PRENTICE HALL
Chapter 1

33. 2.5 Classification of Matter
Matter - Anything that occupies space and has mass (solid, liquid or gas)
Heterogeneous Mixture: Non-uniform composition
Homogeneous Mixture: Uniform composition
Physically Separable Into
Pure Substances: Fixed composition; cannot be further purified
Solution:
Homogeneous
mixture
Physically Separable Into
Chemically Separable Into
Compounds:
Elements united in
fixed ratios
Elements:
Cannot be subdivided by chemical or physical changes
Combine Chemically to

34. Classifying Matter Matter Pure Substances Mixtures
Elements Compounds Homogenous Heterogeneous
Classify following as Homogeneous and Heterogeneous
Diamond b. Tree c. egg d. Coffee

35. Classifying Matter Matter Pure Substances Mixtures
Elements Compounds Homogenous Heterogeneous
A clear glass bottle contains white sand, some nails, slat water with some dye dissolved in it and a layer of gasoline on top, How many phases are present in the system, excluding the bottle and lid?

36. Classifying Matter Matter Pure Substances Mixtures
Elements Compounds Homogenous Heterogeneous
metals nonmetals

37. Classifying Matter Matter Pure Substances Mixtures
Elements Compounds Homogenous Heterogeneous
metals nonmetals ionic covalent

38. Classifying Matter Matter Pure Substances Mixtures
Elements Compounds Homogenous Heterogeneous
metals nonmetals ionic covalent

39. Classifying Matter Matter Pure Substances Mixtures
Elements Compounds Homogenous Heterogeneous
metals nonmetals ionic covalent
shiney dull

40. Classifying Matter Matter Pure Substances Mixtures
Elements Compounds Homogenous Heterogeneous
metals nonmetals ionic covalent
shiney dull
conduct nonconductors

41. Classifying Matter Matter Pure Substances Mixtures
Elements Compounds Homogenous Heterogeneous
metals nonmetals ionic covalent
shiney dull
conduct nonconductors
ductile brittle

42. Classifying Matter Matter Pure Substances Mixtures
Elements Compounds Homogenous Heterogeneous
metals nonmetals ionic covalent
shiney dull
conduct nonconductors
ductile brittle
maleable

43. Classifying Matter Matter Pure Substances Mixtures
A Elements B Compounds C Homogenous D Heterogeneous
metals nonmetals ionic covalent
shiney dull
conduct nonconductors
ductile brittle
maleable
left right of periodic table Periodic Table

44. Classifying Matter Matter Pure Substances Mixtures
Elements Compounds Homogenous Heterogeneous
metals nonmetals ionic covalent Na

45. Classifying Matter Matter Pure Substances Mixtures
Elements Compounds Homogenous Heterogeneous
metals nonmetals ionic covalent
Na Cl2

46. Classifying Matter Matter Pure Substances Mixtures
Elements Compounds Homogenous Heterogeneous
metals nonmetals ionic covalent
Na Cl NaCl

47. Classifying Matter Matter Pure Substances Mixtures
Elements Compounds Homogenous Heterogeneous
metals nonmetals ionic covalent
Na Cl NaCl NO2

48. Classifying Matter Matter Pure Substances Mixtures
Elements Compounds Homogenous Heterogeneous
metals nonmetals ionic covalent
Na Cl NaCl NO2 NaCl(aq)

49. Classifying Matter Matter Pure Substances Mixtures
Elements Compounds Homogenous Heterogeneous
metals nonmetals ionic covalent
Na Cl NaCl NO2 NaCl(aq) granite

50. Classifying Matter Matter Pure Substances Mixtures
Elements Compounds Homogenous Heterogeneous
metals nonmetals ionic covalent
Na Cl NaCl NO2 NaCl(aq) granite Co

51. Classifying Matter Matter Pure Substances Mixtures
Elements Compounds Homogenous Heterogeneous
metals nonmetals ionic covalent
Na Cl NaCl NO2 NaCl(aq) granite
Co O2

52. Classifying Matter Matter Pure Substances Mixtures
Elements Compounds Homogenous Heterogeneous
metals nonmetals ionic covalent
Na Cl NaCl NO2 NaCl(aq) granite
Co O NH4Cl

53. Classifying Matter Matter Pure Substances Mixtures
Elements Compounds Homogenous Heterogeneous
metals nonmetals ionic covalent
Na Cl NaCl NO2 NaCl(aq) granite
Co O NH4Cl C12H22O11

54. Classifying Matter Matter Pure Substances Mixtures
Elements Compounds Homogenous Heterogeneous
metals nonmetals ionic covalent
Na Cl NaCl NO2 NaCl(aq) granite
Co O NH4Cl C12H22O11 tea

55. Classifying Matter Matter Pure Substances Mixtures
Elements Compounds Homogenous Heterogeneous
metals nonmetals ionic covalent
Na Cl NaCl NO2 NaCl(aq) granite
Co O NH4Cl C12H22O11 tea pineapple juice
Atom Ion

56. Can it be physically separated?
A. Matter Flowchart
MATTER
yes no
Can it be physically separated?
MIXTURE
PURE SUBSTANCE
Is the composition uniform? no
yes
Can it be chemically decomposed? no
yes
Homogeneous Mixture
(solution)
Heterogeneous Mixture
Compound
Element
Mechanical
Suspensions
Atom
Ions

57. A. Matter Flowchart element hetero. mixture compound solution
Examples:
graphite
pepper
sugar (sucrose)
paint
soda
element
hetero. mixture
compound
solution

58. Pure Substances (can NOT be separated by physical change)
Matter
Pure Substances (can NOT be separated by physical change)
Elements
Metal Na
Nonmetal Cl2
Compounds
Ionic NaCl
Covalent H2O
Impure substances (can be separated by physical change)
Mixtures
Homogeneous salt-in-water
Heterogeneous Oil-in-water

59. Learning Check
Classify the following as elements, compounds, or mixtures:
a)   Methane  (CH4)                       
b)   Pizza                                                        
c)   Milkshake                                              
d)   Zinc                                                        
e)   Laughing gas (N2O)                          
f)   Clean air                                                    
g)   A chocolate cookie                                        

60. Learning Check Give an example to show each of the following terms:
a)     Matter -                                                    . 
b)    Solution -                                                    .
c)     Suspension -                                              . 
d)    Mechanical mixture -                     .
e)     Compound -                                            . 
f)     Solution -                                   . 
g)     Element -                                 . 

61. What is the difference between an element and a compound?
Reflection Page
What is the difference between an element and a compound?
Give 3 examples of each.

62. Explain the difference between heterogeneous and homogenous.
Reflection Page
Explain the difference between heterogeneous and homogenous.

63. Reflection Page
What is the difference between a solution, and a suspension? Give an example of each.

64. Workbook page. 52 Question # 33-44
Assignment:
Workbook page. 52 Question # 33-44

65. Assignment:

66. Assignment:

67. Assignment: Make 2 questions about todays Lab Unit 3 Topic 1
Make 1 questions (about vapour and vapour pressure)
Unit 3 Topic 2
Lab due by Monday(one for group)
Tomorrow : Vapour Pressure Lab