1. Basic Science Skills
Chapter 1

2. What is Science Science - What is Science? _________Science
There are 2 types of science
_________Science
Studying something to just to learn more about it
Why is the sky blue???
__________ Science
Studying something to make it better or fix a problem
Creating new Technology

3. Branches of Science end
Physical Science- the study of _______ & _________
end

4. Scientific Method Scientific Method Six Steps
An organized plan for gathering, organizing, and communicating information
The foundation of ALL modern science
Six Steps
________
Why are you going to do an experiment?
_________
Get background information
Has any one done this before?
end

5. Scientific Method ___________ __________
An educated prediction (educated guess)
What do you think is going to happen?
__________
Test your hypothesis
Look at your data and figured out what happened
Did your experiment prove or disprove your hypothesis?

6. THE METRIC SYSTEM

7. SI Units Scientists use a standard set of units for all measurements
What you are measuring
Unit
Symbol
Scientists use a standard set of units for all measurements
The SI Units
Same as the Metric System
end

8. Temperature There are 3 scales used to measure temperature
Fahrenheit (° ): Used in the U.S.
Celsius (° ): Used in all other countries in the world
Kelvin ( ): Used by scientists
To convert between them, use the following:
end

9. Temperature Temperatures you should know: °F °C K Water Boils
Human Body
Room Temp
Water Freezes
end

10. Temperature Convert the following temperatures: 26 °C = _____ °F
98 °F = _____ °C
34 °C = _____ K
end

11. Why do we use Scientific Notation???

12. Scientific Notation 300000000 = 503 = 10600 = 0.00086 = 0.1 ==
end

13. Scientific Notation 5.35 x 103 = 1.2 x 102 = 5.67 x 104 = 2.2 x 10-5 =
end

14. EOC BOOK REVIEW p p

15. CONVERSIONS
King
Henry
Died By
Drinking
Chocolate
Milk

16. EOC REVIEW BOOK p p

17. Properties and States of Matter
Chapters 2 and 3

18. Classifying Matter Matter: ____________________
Can be either a ___________ or a _____________
end

19. Classifying Matter-Pure Substance
Are either __________ or ____________
Ex: water, gold
end

20. Periodic Table of Elements
A list of all natural Elements

21. Classifying Matter- Pure Substance
Element
Ex: Gold (Au)
end

22. Classifying Matter- Pure Substance
Compound
Ex: Water (H2O)
end

23. Sugar Compound or Element?
Review:
Sugar
Compound or Element?

24. Oxygen Compound or Element?
Review:
Oxygen
Compound or Element?

25. Ice Compound or Element?
Review:
Ice
Compound or Element?

26. Carbon Dioxide Compound or Element?
Review:
Carbon Dioxide
Compound or Element?

27. Sodium Compound or Element?
Review:
Sodium
Compound or Element?

28. MIXTURES

29. Classifying Matter- Mixture
Mixtures
Either __________ or ________________
end

30. Classifying Matter- Mixtures
Homogeneous Mixtures
Everything looks __________
Called: _____________
1 substance dissolves in another
Ex: Tap Water, Kool-Aid, Steel

31. Mixtures Heterogeneous Mixtures Everything __________ look the same
Either a _______ or __________
Ex: Salad Dressing, Dirt

32. Separating Mixtures
2 Types of Filtration:
end

33. Matter

34. Physical & Chemical Properties

35. EOC BOOK REVIEW
p , 2, & 4

36. States and Phases
3 States of Matter
6 Phases of Matter

37. What you need today…. Notebook Paper Reference Tables Calculator
EOC Book
Ipad

38. Structure of the Atom Atoms are made up of 3 particles
___________, ___________, ___________
Called _________________ particles
You must identify them by mass, charge, and location
end

39. Structure of the Atom The Nucleus
Small, dense region in the center of an atom
Contains:
_____________ and ____________
All of an atom’s positive charge
Almost all of an atom’s _________ is held here.
end

40. Structure of the Atom Proton (____) Charge = ________
Found ____________
end

41. Structure of the Atom Electron (_____) Charge = ______
Found ______________
The number of electrons controls the electrical charge
end

42. Structure of the Atom Neutron (____) Charge = ____________
Found _____________
The number of neutrons controls the isotope
end

43. Structure of the Atom Atomic Number
The number of __________ & __________
Defines the element
Atomic Number
end

44. Structure of the Atom Mass Number
COMPLETE THE FORMULA
Mass # = (Atomic #) + (________________)
# of protons
end

45. Structure of the Atom
LABEL THE ELEMENT CORRECTLY

46. Isotope
Isotopes are the change in an atoms ___________ due to the change in _______________.
Elements on the periodic table show the ______________ mass of the atom.

47. Structure of the Atom Name Symb ol Proto ns Neutro ns Electr ons
COMPLETE CHART:
Name
Symb ol
Proto ns
Neutro ns
Electr ons
Atomi c Num ber
Mass Numb er
Carbon -12
end

48. Isotope
Carbon-14
Has how many protons, neutrons, and electrons?

49. Atomic Theories- Modern
In the Bohr Model:
_________ and __________form the nucleus
___________ are in rings around the nucleus
called energy levels

50. FILL IN THE BLANK
Each energy level can only hold a certain number of electrons
Energy Level # of electrons 1 2 3 4

51. Atomic Theories- Modern
WHAT ELEMENT IS THIS BOHR MODEL?
p = 3
n = 3
e = 3

52. Bohr Model Practice
Nitrogen

53. Nuclear Chemistry
Radioactivity

54. Nuclear Chemistry
Three types of radiation:
end

55. Nuclear Reactions Nuclear Equations Shows the transmutation
Atotal and Ztotal must be equal on each side of the equation
Fill in the equations
end

56. Nuclear Decay Complete Problems
If you had 25 g of gold-198 how much is left after it has gone through 12 half-lives?
You have 10.0 g of francium-210, which has a half-life of 5.2 minutes. How many half-lives must pass for about 1 g to be left? How much time has passed?
The half-life of radon-222 is 3.8 days. How much of a 100 g sample is left after 46.8 days?
end

57. Periodic Table Who created the Periodic Table?
How many original elements were there?

58. Periodic Table On the Periodic Table:
Columns are called: ____________________
Rows are called: _______________________

59. I am an element in Group 14, Period 2, who am I?
Find the Element
I am an element in Group 14, Period 2, who am I?

60. I have 4 protons, 5 neutrons, and 4 electrons, who am I?
Periodic Table
I have 4 protons, 5 neutrons, and 4 electrons, who am I?

61. I am the heaviest element in group 17, who am I?
Periodic Table
I am the heaviest element in group 17, who am I?

62. Periodic Table
I am the most reactive element on the periodic table, how many protons do I have?

63. Electron Configuration
Draw diagrams for the following: Sr
How many Valence electrons?
What is the charge of this electron?
end

64. Draw diagrams for the following:Si
How many Valence electrons?
What is the charge of this electron?

65. EOC BOOK REVIEW
P , 2, & 4

66. Chemical Compounds

67. Chemical Formulas How many total atoms are in each of these: H2SO4
Cu(NO3)2
end

68. Chemical Bonding
What are the 3 Types of Chemical Bond?
end

69. Chemical Bonding Identify the following as ionic or covalent
1) CaCl ) CO2
end

70. Chemical Bonding
Which element is the anion in this compound?
LiBr
end

71. Naming Ionic Compounds
Name the following:
MgF2
Ca3N2
end

72. Naming Ionic Compounds
Name the following:
NaC2H3O2
Sr3(PO4)2
end

73. Writing Ionic Formulas
Write the formulas for the following:
Beryllium Phosphide
Strontium Sulfide
end

74. Writing Ionic Formulas
Write the formula for the following:
Barium Chromate
Ammonium Sulfate
end

75. Transition Metals Silver (I) oxide Copper (II) bromide Iron (II) oxide
Write the formula for these Ionic Compounds:
Silver (I) oxide
Copper (II) bromide
Iron (II) oxide

76. Covalent Bonding Covalent Bond Bond between two:
____________and _______________
Atoms __________electrons 
end

77. 7 nonmetals that never exist by themselves.
Form pairs with each other
Called _________ (H, N, O, F, Cl, Br, I)

78. Naming Covalent Molecules
Name the following compounds:
As2O3 SO
end

79. Chemical Reactions
Chapter 7

80. Chemical Reactions
Examples of a Chemical Reaction:
end

81. Chemical Equations Chemical Equations The State of Matter is with:
2 parts:
Reactants
ON the
Products
The State of Matter is with:
( ), ( ), ( ), ( )
aq-
2 H2(g) + O2(g) 
2 H2O(l)
Yields/Forms/Produces
end

82. Chemical Equations The Law of Conservation of Matter
Matter CANNOT be created or destroyed!
Every atom at the start, must be at the end!
MUST BALANCE CHEMICAL EQUATIONS!!!
end

83. Chemical Equations Lets practice: ___ N2 + ___ H2  ___ NH3
___ KClO3  ___ KCl + ___ O2
end

84. Chemical Reactions
There are 5 basic chemical reactions:
end

85. Chemical Reactions A + B  AB
2 or more reactants combine to form 1 product
A + B  AB
end

86. Chemical Reactions AB  A + B
1 reactant breaks down into 2 or more products
AB  A + B
end

87. Chemical Reactions A + BC  AC + B
1 element replaces another element in a compound
A + BC  AC + B
end

88. Chemical Reactions AB + CD  AD + CB The reactants switch partners
Often produces water, a gas , or a solid
end

89. Chemical Reactions Combine with oxygen give off heat and light
Forms CO2(g) and H2O(l)
end

90. Chemical Reaction Classify the following: 2 H2 + O2  2 H2O
Zn + H2SO4  ZnSO4 + H2
2 HgO  2 Hg + O2
AgNO3 + NaCl  AgCl + NaNO3
2 C2H6 + 7 O2  4 CO2 + 6 H2O
end

91. EOC BOOK REVIEW p

92. Energy Changes
Chemical Energy
Exothermic
Endothermic
end

93. Reaction Rates Reaction Rate Speed of reactants becoming products
Ways to speed up:
end

94. EOC BOOK REVIEW p

95. Chapter 8: Solutions, Acids, Bases & pH

96. Solubility Solubility
Particles more attracted to solvent than each other
Measured in:
Changes with temperature
At 50 °C, the solubility of KNO3 is 80 g.
Can dissolve up to 80 g of KNO3 in 100 g of water
end

97. Solubility Solubility Curve What is the solubility of NH3 at 10 °C?
Solubility at different temps.
What is the solubility of NH3 at 10 °C?
~ ___ g of NH3 / 100 g of H2O
60 g of NH4Cl can be dissolved in 100 g of water at what temperature?
___ °C
end

98. Solubility
The amount of solute determines how a solution is classified:
_________________
end

99. Solubility Unsaturated Solutions Can dissolve more solute
__________ the Line
60 g of KNO3 are dissolved in 100 g of water at 50 °C?
Unsaturated Solution of KNO3
end

100. Solubility Saturated Solution Cannot dissolve any more ____ the Line
80 g of KNO3 are dissolved in 100 g of water at 50 °C?
Saturated Solution of KNO3
end

101. Solubility Supersaturated Solution
Supersaturated Solution of KNO3
Supersaturated Solution
Dissolved more than normally possible
_______ the Line
130 g of KNO3 are dissolved in 100 g of H2O at 50 °C?
end

102. Concentrations Concentration
The amount of solute in a given amount of solvent
Concentrated
lots of solute
Dilute
little solute
end

103. Acids and Bases
Acid
Chemical formulas start with an “___”
end

104. Acids and Bases
Base
Chemical formulas end with an ‘___’
end

105. Classify
Acid or Base?
NaOH,
Mg(OH)2,
HCl,
Al(OH)3

106. Strength of Acids and Bases
pH scale
0 - 6 = ____ 7 = ____ 8 – 14 = ____
end

107. EOC Book Reivew
p & 3

108. EOC BOOK REVIEW
p & 3 p
2-9, 11-14, 16-17

109. Review Sheet