1. Unit 1. Matter and Change

2. Do Now:
What are the parts of the scientific method and explain each part?

3. Objective Identify the common steps of scientific methods
Identify types of variables
Describe the difference between a theory and a scientific law
Identify the characteristics of a substance
Distinguish between physical and chemical properties
Differentiate among the physical states of matter

4. Objectives Continued Activities:
Define physical and chemical changes and list common changes
Apply the law of conservation of mass to chemical reactions
Activities:
Q&A
Solve problems
Exit Ticket

5. Scientific Method (p12) Systematic approach used in scientific study
Method for scientists to verify the work of others

6. Steps of Scientific Method
Observation
Hypothesis
Experiments
Conclusion
Theory/ Scientific Law

7. Observation Act of gathering information
Qualitative Data- color, shape, odor other physical characteristics
Quantitative Data – some type of measurement. It is numerical. Ex. Height, weight, how fast, how slow etc.

8. Hypothesis
Tentative explanation for what has been observed.

9. Experiment Set of controlled observations used to test the hypothesis
Must carefully plan and set up one or more laboratory experiments in order to change and test one variable at a time.
Independent Variable – Variable that you plan to change. ( what you can control)
Dependent Variable – variable that changes based on the independent variable

10. Conclusion
Judgment based on the information obtained

11. I. Kinetic Molecular Theory States of Matter
Ch. 3 - Matter I.
Kinetic Molecular Theory
States of Matter

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

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

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

15. Three States of Matter
Gases
high KE - particles can separate and move throughout container
variable shape
variable volume
Vapor- Gaseous state of a substance that is a solid or liquid at room temperature.

16. Matter and its Properties
It’s Classified!

17. Physical vs. Chemical Physical Property Chemical Property
can be observed without changing the identity of the substance
Extensive or intensive properties
Chemical Property
describes the ability of a substance to undergo changes in identity

18. Extensive vs. Intensive
Extensive Property
depends on the amount of matter present
ex,.-
Intensive Property
depends on the identity of substance, not the amount
Ex.-

19. Extensive vs. Intensive
Extensive Property
depends on the amount of matter present
ex,.- Volume, mass, Energy
Intensive Property
depends on the identity of substance, not the amount
Ex.- melting point, boiling point, conduct electricity or heat
WHAT ABOUT DENSITY??

20. A. Extensive vs. Intensive
Examples:
boiling point
volume
mass
density
conductivity

21. A. Extensive vs. Intensive
Examples:
boiling point…… intensive
Volume …. extensive
Mass ….. extensive
Density ….. intensive
Conductivity ….. intensive

22. Physical vs. Chemical Physical Change Chemical Change
changes the form of a substance without changing its identity
properties remain the same
Chemical Change
changes the identity of a substance
products have different properties

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

24. B. Physical vs. Chemical Examples: melting point physical flammable
density
magnetic
tarnishes in air
physical
chemical

25. B. Physical vs. Chemical Examples: melting point physical flammable
density
magnetic
tarnishes in air
physical
chemical

26. B. Physical vs. Chemical rusting iron dissolving in water
Examples:
rusting iron
dissolving in water
burning a log
melting ice
grinding spices

27. B. Physical vs. Chemical chemical rusting iron physical
Examples:
rusting iron
dissolving in water
burning a log
melting ice
grinding spices

28. Law of Conservation of Mass
Mass is neither created nor destroyed during a chemical reaction. It is conserved
In a chemical reaction, the mass of the reactants must equal the mass of the products

29. Law of Conservation of Mass
Pg. 78 #7 A student carefully placed 15.6 g of sodium in a reactor supplied with an exess quantity of chlorine gas. When the reaction was complete, the student obtained 39.7f of sodium chloride. Calculate how many grams of chlorine gas reacted. How many grams of sodium reacted?

30. Law of Conservation of Mass
Pg. 78 #7 A student carefully placed 15.6 g of sodium in a reactor supplied with an exess quantity of chlorine gas. When the reaction was complete, the student obtained 39.7f of sodium chloride. Calculate how many grams of chlorine gas reacted. How many grams of sodium reacted? 24.1 g of chlorine gas, 15.6 of sodium

31. Law of Conservation of Mass
Pg. 78 #7 A student carefully placed 15.6 g of sodium in a reactor supplied with an exess quantity of chlorine gas. When the reaction was complete, the student obtained 39.7f of sodium chloride. Calculate how many grams of chlorine gas reacted. How many grams of sodium reacted? 24.1 g of chlorine gas, 15.6 of sodium

32. HW
Pg 79 (10 and 13 only)

33. Do Now: DO NOW: What is a solution?
Describe the difference between a heterogeneous and homogenous mixture
Calculate % by Mass

34. Objective: SWBAT: Activities Contrast Mixtures and substances
Classify mixtures as homogeneous or heterogeneous
List and describe several techniques used to separate mixtures.
Distinguish between elements and compounds
Activities
Q&A
Solve problems
Exit Ticket

35. Objective:
Activities:

36. 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
Colloids
Suspensions

37. A. Matter Flowchart graphite pepper sugar (sucrose) paint soda
Examples:
graphite
pepper
sugar (sucrose)
paint
soda

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

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

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

41. Pure Substances 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.

42. Two different compounds, each has a definite composition.
Pure Substances
For example…
Two different compounds, each has a definite composition.

43. 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

44. Diatomic Elements Hydrogen Nitrogen Oxygen Fluorine Chlorine Bromine
Iodine
There are 7 diatomic elements
These atoms are never alone, if they are the pair up with the same atom

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

46. C. Mixtures Solution homogeneous very small particles
no Tyndall effect
Tyndall Effect

47. C. Mixtures Colloid heterogeneous medium-sized particles
Tyndall effect
particles don’t settle
EX: milk

48. C. Mixtures Suspension heterogeneous large particles Tyndall effect
particles settle
EX: fresh-squeezed lemonade

49. Mixtures (variable composition)
Homogeneous – Solutions
evenly distributed
Heterogeneous
not evenly distributed

50. Tea – Homogeneous Mixture

51. Air – Homogeneous Mixture

52. Alloys – Homogeneous Mixtures

53. Cereal – Heterogeneous Mixture

54. Sand – Heterogeneous Mixture

55. C. Mixtures mayonnaise muddy water fog saltwater
Examples:
mayonnaise
muddy water
fog
saltwater
Italian salad dressing

56. C. Mixtures colloid mayonnaise suspension muddy water fog solution
Examples:
mayonnaise
muddy water
fog
saltwater
Italian salad dressing

57. % by Mass = Percent by Mass
AKA % composition

58. Example
P 88 # 19
A 78.0 g sample of an unknown compounds contains 12.4 g of hydrogen. What is the present by mass of hydrogen in the compound?

59. Example
P 88 # 19
A 78.0 g sample of an unknown compounds contains 12.4 g of hydrogen. What is the present by mass of hydrogen in the compound?
% mass = (12.4/78.0) * 100 = 15.9%

60. Extra problems:
Pg 88 (# 22-23)

61. HW
Pg 90 (28)
Pg 94 (32, 37, 38, 40, 42, 43,44,50,52, 57,58,60, 62, 64, 76, 92)

62. Do Now: Look at your periodic table.
What important information can you get from the PTOE?

63. Objectives Activities Find patterns in the Periodic Table
Classify elements as metals, non-metals or metalloids
Distinguish between metals, non-metals or metalloids
Activities
PPT
Group work

64. The Periodic Table

65. A. Mendeleev Dmitri Mendeleev (1869, Russian)
Organized elements by increasing atomic mass.
Elements with similar properties were grouped together.
There were some discrepancies.
C. Johannesson

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

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

68. How PTOE is organized
Metals
Nonmetals
Metalloids
C. Johannesson

69. B. Blocks Main Group Elements Transition Metals
Inner Transition Metals
C. Johannesson

70. 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.
Families: vertical rows of elements, aka groups
Each group contains similar chemical properties

71. Types of Elements METALS: Shiny Conductors of heat and electricity
Most metals are malleable (can be pounded into thin sheets; a sugar cube sized chunk of gold can be pounded into a thin sheet which will cover a football field),
Most metals are ductile (can be drawn out into a thin wire).
All are solids at room temp (except Mercury, which is a 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.

72. Types of Elements Vary greatly in appearance Non-lustrous
NON- METALS:
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)
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)

73. Types of Elements
Metalloids:
Elements may share properties of metals and non-metals.

74. Exit Ticket: 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

75. Review of Unit
List topics we have covered.
Study for test!