1. Unit 1 Chapter 2-pg38 Matter and Change
Chemistry 334

2. Essential Question:
How do chemists classify matter?

3. Section 2.1
Properties of Matter

4. Describing Matter KC: How can Properties be used to describe matter?
A: Properties used to describe matter can be classified as ether extensive or intensive.

5. Extensive Properties
A property that depends on the amount of matter in a sample.

6. Examples of extensive properties:
Mass—the amount of matter an object contains.
Volume—the measure of the space occupied by an object.

7. Intensive Properties:
A property that depends on the type of matter in a sample, not the amount.
Examples
Hardness
Odor
Conductivity
State of matter
*******What it is made of******

8. Identifying Substances
KC: Why do all samples of a substance have the same intensive properties?
Every sample of a given substance has identical intensive properties because every sample has the same composition.

9. Substance Matter that has definite and uniform composition.
AKA: Pure substance
Examples: Au Ag
NaCl
CH4

10. NaCl vs. NaCl Water (H2O) Q: Is salt water a pure substance????
INDEX CARD CHALLENGE!!!!

11. INDEX CARD CHALLENGE
Without talking, find someone who has a different answer that you
IDK—does not count as an answer!!!
Explain why you chose this answer.

12. The Answer NaCl is a pure substance Salt water is not
It can have variable composition

13. Physical Properties
Physical property—any quality or condition of a substance that can be observed without changing the substance’s composition.
Examples:
State Mp Bp
Color

14. States of matter: KC: What are 3 states of matter?
A: Three states of matter are solid, liquid, gas.

15. Solid
Definite shape
Definite volume
Not easily compressed

16. Liquid
Indefinite shape
Definite volume
Not easily compressed

17. Gas
Indefinite shape
Indefinite volume
Easily compressed

18. Three States of Matter

19. Vapor
Describes the gaseous state of a substance that is generally a liquid or solid at room temperature.

20. Physical Changes KC: How can physical changes be classified?
A: Physical changes can be classified as reversible or irreversible.

21. Reversible Phase changes Melting Freezing Sublimation Boiling
Condensation

22. Irreversible
Breaking
Tearing
Smashing
Cutting

23. Section 2.2
Mixtures
Page 44

24. Classifying Mixtures KC: How can mixtures be classified?
A: Mixtures can be calssified as either hetterogenous or homogenous.

25. Mixture A combination of two or more pure substance.
Can be made with different combinations of solid, liquids and gasses.

26. 2 Types of mixtures
1. Homogenous
2. Heterogenous

27. Heterogeneous Mixture
Not the same through out
More than one phase
(distinguishable parts)
ie:
Chicken noodle soup
Chex mix

28. Homogenous mixture Uniform composition; same through out AKA: Solution
Only one phase
ie:
Salt water
Tea
Olive oil
Vinegar
Alloy

29. Separating Mixtures KC: How can mixtures be seperated?
A: Differences in physical properties can be used to separate mixtures.

30. 5 ways to separate mixtures
Filtration
Distillation
Crystallization
Sublimation
Chromatography

31. Filtration
A technique which uses a pours barrier to separate a solid from a liquid

32. Distillation
A separation technique that is based on the differences in the boiling points of the mixed substances

33. Crystallization
A separation technique that results in the formation of pure solid particles of a substance from a solution containing the dissolved substance.

34. Sublimation
The process during which a solid changes to a vapor without going through the liquid phase

35. Chromatography
A technique that separates the components of a mixture (aka-mobile phase), based on the ability of each component to be drawn across the surface of another material (aka-stationary phase).

36. Section 2.3
Elements and Compounds

37. Distinguishing Elements and Compounds
KC: How are elements and compounds different?
A: Compounds can be broken down into simpler substances.

38. Examples of elements Ca Na H

39. Periodic Table
Organizes the elements into a grid of horizontal rows (aka-periods) and vertical columns (aka- groups/families).

40. Compounds
Two or more elements combined chemically

41. Breaking Down Compounds
Compounds can be broken down by chemical change
This process usually requires a an external energy source, such as heat or electricity

42. Properties of Compounds
The chemical and physical characteristics of a compound is very different than that of its constitute parts.

43. Example:
K + I  KI
Potassium & Iodine VS Potassium iodide

44. Potassium
A light silver metal that reacts with water

45. Iodine
A black solid that changes to a purple gas at room temperature.

46. Potassium iodide
A white salt

47. Distinguishing Substances and Mixtures
KC: How can substances and mixtures be distinguished?
A: If the composition of a material is fixed, the material is a substance. If the composition of the substance may vary, the material is a mixture.

48. Classification of matter
Ex: chex salt NaCl Na
mix water
(AKA: solutions)

49. Symbols and formulas
KC: What do chamists use to represent elements and compounds?
A: Chemists use chemical symbols to repersent elenents and chemical formulas to represent compounds

50. Chemical Symbol
One or two letters used to represent the name of an element.

51. Chemical Compounds

52. Section 2.4
Chemical Reactions

53. Chemical Changes
Key Concept: What always happens during a chemical change?
Answer: During a chemical change, the composition of matter changes
Example
combustion reaction

54. Examples: Fe to Rust Respiration
Combustion (candle burning vs. wax melting)

55. Words that indicate a chemical change:
-Decompose -Ferment -Tarnish
-Oxidize Burn Rust
-Corrode Rot Explode

56. Chemical Properties=
The ability (or inability) of a substance to combine with or change into one or more substances.

57. Chemical Change
One or more substances changes into one or more new substances.
AKA: Chemical reaction
Mg + HCl  H2 + MgCl

58. Reactants
The substance that are to be transformed.

59. Product
The substance(s) that are made

60. Recognizing Chemical Changes
Key Concept: What are the 4 possible clues that a chemical change has taken place?
Answer: Possible clues that a chemical reaction has taken place include: transfer of energy (heat or light), a change in color, the production of gas, or the formation of a precipitate.`

61. Precipitate=
The production of a solid.

62. Conservation of Mass
Key concept: How are the masses of the reactants and the masses of the products of a reaction related?
Answer: During any chemical reaction the mass of the reactants is always equal to the mass of the products.

63. Law of Conservation of Mass:
Massreactants=Massproducts

64. Mass of Magnesium oxide (g)
Practice Problems
2Mg + O2  2 MgO
Mass of Magnesium
(g)
Mass of Oxygen
Mass of Magnesium oxide (g) 5
3.3
8.3
6.5 A
10.8
13.6 9 B C
12.5
31.5

65. Words that indicate a chemical change:
-Decompose -Ferment -Tarnish
-Oxidize Burn Rust
-Corrode Rot Explode

66. Physical Changes=
A change which alters a substance without changing its composition.

67. Examples of physical changes:
Cutting
Braking
Phase Change=transition of mater from one state to another.

68. Chemical changes vs. physical changes
Alters a substance without changing its composition (arrangement of its atoms)
Does NOT change the arrangement of atoms
SAME substance!
Alters a substance by changing its composition (arrangement of its atoms)
DOES change the arrangement of atoms
NEW substance made!

69. Chemical/Physical changes Foldable