1. Unit 1. Matter and Change
This lesson is 8 days long

2. Objectives: Define the term “chemistry”
Describe the difference branches of Chemistry.
Describe the difference between a physical change and a chemical change and give several examples of each.
Describe different characteristics of the three states matter.
Classify a mixture as homogeneous or heterogeneous.
Classify a pure substance as an element or a compound.

3. Chemistry is a Physical Science

4. Both living and nonliving matter have
Chemistry is the study of matter and the changes that it undergoes.
Biological
Science
Physical
Sciences
Chemistry
Both living and nonliving matter have
a chemical structure.

5. Chemistry deals with:
What is material made of?
What is the makeup and internal arrangement of the atoms?
How does it behave when heated, cooled or mixed with other materials?

6. Branches of Chemistry
Organic chemistry – the study of carbon containing compounds.
Inorganic chemistry – the study of substances that do not contain carbon (metals and gases).
Physical chemistry – the study of the properties and changes of matter and their relation to energy.
Introduction Video

7. Analytical chemistry – the identification of the components and composition of materials.
Biochemistry – the study of the processes occurring in living systems.

8. Do Now:
What are the states of matter?

9. States of Matter There are FOUR states of matter → Solid Liquid Gas
Plasma
State of matter depends on Kinetic Energy between the particles

10. Kinetic Molecular Theory (KMT)
Particles of matter are always in motion.
The kinetic energy (speed) of these particles increases as temperature increases.

11. Solids Three States of Matter
very low KE - particles vibrate but can’t move around
fixed shape
fixed volume

12. Liquids Three States of Matter
low KE - particles can move around but are still close together
variable shape
fixed volume

13. Gases Three States of Matter
high KE - particles can separate and move throughout container
variable shape
variable volume

14. Objectives: Distinguish between: intensive & extensive properties
Physical & chemical changes
Classify matter

15. Extensive vs. Intensive
Extensive Property
depends on the amount of matter present
ex: length, mass, weight, volume

16. Extensive vs. Intensive
Intensive Property
A property that depends on the type of matter, not how much there is!
ex: color, odor, luster, conductivity, melting point, boiling point, & Density

17. Let’s Practice! Extensive vs. Intensive
boiling point
Volume
Mass
Density
Conductivity

18. Let’s Practice! Extensive vs. Intensive
boiling point…… intensive
Volume …. extensive
Mass ….. extensive
Density ….. intensive
Conductivity ….. intensive

19. Do Now Define the word chemistry.
2. Name the five branches of chemistry.
3. Define basic and applied research.

20. Physical vs. Chemical Properties
Physical Property
can be observed without changing the identity of the substance

21. Physical vs. Chemical Properties
Chemical Property
describes the ability of a substance to undergo changes in it’s identity

22. Let’s Practice! Physical vs. Chemical
melting point
flammable
density
magnetic
tarnishes in air

23. Let’s Practice! Physical vs. Chemical
melting point
flammable
density
magnetic
tarnishes in air
physical
chemical

24. Physical vs. Chemical CHANGE
Physical Change
changes the form of a substance without changing its identity
properties remain the same

25. Physical vs. Chemical CHANGE
changes the identity of a substance
products have different properties

26. Signs of a Chemical Change →
change in color or odor
formation of a gas
formation of a precipitate (solid)
change in light or heat

27. Properties and Changes in Matter
In the example of burning of charcoal, carbon and oxygen are the reactants in the combustion reaction. Carbon dioxide is the product.
carbon oxygen → carbon dioxide
C O CO2
(reactants) (product)

28. Let’s Practice! Physical vs. Chemical Change
rusting iron
dissolving in water
burning a log
melting ice
grinding spices

29. Let’s Practice! Physical vs. Chemical Change
rusting iron
dissolving in water
burning a log or charcoal
melting ice
grinding spices

30. SOLUTIONS & MIXTURES

31. Do Now What would you consider a pure substance?
What would you consider a mixture?

32. Do Now What is a solution?
Describe the difference between a heterogeneous and homogenous mixture

33. Element Pure Substances composed of identical atoms
EX: copper wire, aluminum foil

34. Compound Pure Substances
composed of 2 or more elements in a fixed ratio
properties differ from those of individual elements
EX: table salt (NaCl)

35. Law of Definite Composition
A given compound always contains the same, fixed ratio of elements.
Law of Multiple Proportions
Elements can combine in different ratios to form different compounds.

36. Two different compounds, each has a definite composition.
For example…
Two different compounds, each has a definite composition.

37. Pure Substances - (constant composition)
Elements
Listed on the Periodic Table
Cannot be broken down into unique components
Na, Cl, Al, O2, S8
Compounds
Made of elements that are chemically joined
Can be broken down
NaCl, H2O, AlCl3, H2SO4

38. Mixtures Variable combination of 2 or more pure substances.
Heterogeneous
Homogeneous

39. Mixtures - (variable composition)
Homogeneous
evenly distributed
Heterogeneous
not evenly distributed

40. a homogeneous solution usually contains very small particles
Mixtures continued…
a homogeneous solution usually contains very small particles

41. Colloid solutions are heterogeneous and usually contain medium-sized particles
These particles don’t settle
EX: milk, cosmetics, fog, detergents, blood, & paint

42. Suspension solutions are heterogeneous and contain large particles.
These particles settle at the bottom
EX: fresh-squeezed lemonade

43. Let’s Practice! mayonnaise muddy water fog saltwater
Italian salad dressing

44. Let’s Practice! colloid mayonnaise suspension muddy water fog solution
saltwater
Italian salad dressing

45. Can it be physically separated?
Matter Flowchart
MATTER
yes no
Can it be physically separated?
Is the composition uniform? no
yes
Is it made of more than one type of atom? no
yes

46. Can it be physically separated?
Matter Flowchart
MATTER
yes no
Can it be physically separated?
MIXTURE
PURE SUBSTANCE
Is the composition uniform? no
yes
Is it made of more than one type of atom? no
yes

47. Can it be physically separated?
Matter Flowchart
MATTER
yes no
Can it be physically separated?
MIXTURE
PURE SUBSTANCE
Is the composition uniform? no
yes
Is it made of more than one type of atom? no
yes
Homogeneous Mixture
(solution)
Heterogeneous Mixture

48. Can it be physically separated?
Matter Flowchart
MATTER
yes no
Can it be physically separated?
MIXTURE
PURE SUBSTANCE
Is the composition uniform? no
yes
Is it made of more than one type of atom? no
yes
Homogeneous Mixture
(solution)
Heterogeneous Mixture
Colloids
Suspensions

49. Can it be physically separated?
Matter Flowchart
MATTER
yes no
Can it be physically separated?
MIXTURE
PURE SUBSTANCE
Is the composition uniform? no
yes
Is it made of more than one type of atom? no
yes
Homogeneous Mixture
(solution)
Heterogeneous Mixture
Compound
Element
Colloids
Suspensions

50. Let’s Practice! graphite pepper sugar (sucrose) paint soda
How do we categorize the following?
graphite
pepper
sugar (sucrose)
paint
soda

51. Let’s Practice! element graphite hetero. mixture pepper compound
homo mixture
Homo mixture
graphite
pepper
sugar (sucrose)
paint
soda

52. Tea – Homogeneous Mixture

53. Air – Homogeneous Mixture

54. Alloys – Homogeneous Mixtures

55. Cereal – Heterogeneous Mixture

56. Sand – Heterogeneous Mixture

57. Separating Mixtures Only a physical change- no new matter
Filtration - separate solids from liquids with a barrier (filter paper)
Distillation - separate liquids because of different boiling points. Solutions is heated and vapor is caught in a cooled area.
Chromatography - different substances are attracted to paper or gel, so move at different speeds

59. Do Now - Identify the type of substance
1. ice tea
2. carbon
3. carbon dioxide
4. foul water
5. foul water after separation
6. milk

61. Do Now
List as many elements as you can from the periodic table WITHOUT LOOKING ☺

62. Objectives
1. SWBAT determine if an element is a metal, nonmetal, or metalloid.
2. SWBAT differentiate between main elements and transition elements
3. SWBAT draw and explain molecular models of mixtures, solutions, elements, and compounds.

63. The
Periodic
Table

65. Dmitri Mendeleev (1869, Russian)
Organized elements by increasing atomic mass.
Elements with similar properties were grouped together.

66. Dmitri Mendeleev (1869, Russian)
Predicted properties of undiscovered elements.

67. Henry Moseley (1913, British)
Organized elements by increasing atomic number.
Resolved discrepancies in Mendeleev’s arrangement.

68. Organization of the Elements

69. Metallic Character
Metals
Nonmetals
Metalloids

70. Get 3 colored pencils. Make a key!

71. Blocks
Main Group Elements
Transition Metals
Inner Transition Metals

72. Periods and Families Periods: horizontal rows on the periodic table
physical and chemical properties change somewhat regularly across a row.
Elements closer to each other in the same period tend to be similar than those that are farther apart.
Groups: vertical rows of elements, AKA families
Each group contains similar chemical properties

74. Do Now: Au Si Br Classify the following as either a
METAL, NON-METAL or METALLOID: Au Si Br

75. METALS : Types of Elements Shiny Conductors of heat and electricity
Most metals are ductile (can be drawn out into a thin wire).
Most metals are malleable (can be pounded into thin sheets like tin foil)
a sugar cube sized chunk of gold can be pounded into a thin sheet which will cover a football field!

76. METALS Continued....
All are solids at room temp (except Mercury, which is liquid)
Metals tend to have low ionization energies, and typically lose electrons (i.e. are oxidized) when they undergo chemical reactions
Alkali metals are always 1+ (lose the electron in s subshell)
Alkaline earth metals are always 2+ (lose both electrons in s subshell)
Compounds of metals with non-metals tend to be ionic in nature.

77. Add in ionization!

78. NON- METALS : Types of Elements Vary greatly in appearance
Non-lustrous
Poor conductors of heat and electricity
The melting points of non-metals are generally lower than metals
Seven non-metals exist under standard conditions as diatomic molecules: H2(g) N2(g) O2(g) F2(g) Cl2(g) Br2(l) I2(l) (volatile liquid - evaporates readily)

79. Nonmetal + Metal -> Salt
NON- METALS continued...
Nonmetals, when reacting with metals, tend to gain electrons (typically attaining noble gas electron configuration) and become anions:
Nonmetal + Metal -> Salt
Compounds composed entirely of nonmetals are molecular substances (not ionic)

80. Metalloids: Types of Elements
Elements may share properties of metals and non-metals.
A stair-step line separates the metals from the nonmetals on the periodic table

81. Metalloids continued... Properties:
All metalloids are solids at room temperature.
Less malleable than metals but not as brittle as nonmetals.
Metalloids tend to be semiconductors of electricity. (intermediate between metals and nonmetals).
Used in semiconducting materials found in computers, calculators, televisions and radios.

82. Noble Gases Types of Elements
Elements in Group 18 of the periodic table.
They are considered nonmetals.
These elements are generally unreactive.
All are gases at room temperature.
Examples: neon, argon, krypton, xenon (all used in lighting) and helium.

83. Do Now: Classify the following as either a:
METAL, NON-METAL or METALLOID: Au Si Br
An element that is brittle and conducts electricity
An element that is malleable
An element that has tendency to become an anion