1. Physical Science EOC Review
Marilyn Pendley, Instructor, CCCMC
Modified by R. Kittrell
Jan 2015 & 5Jan2016

3. Scientific Experimentation
controlled experiment
-Only one variable should be changed at a time.
Manipulated (independent) variable – changed by the experimenter.
Responding (dependent) variable – the effect that is measured.

4. Law vs. Theory Develop a law
Law: Summarizes the outcome of several experiments that occur repeatedly and consistently.
Example: The spoiled food served at lunch makes people sick with a stomachache.
Develop a theory
Theory: Explanation for why a law exists.
Example: It is the bacteria in the spoiled food that makes people ill.

5. Types of Measurements
1. Length
a. The distance from one point to another point.
b. Base unit is the meter (m).
c. Tool is the metric ruler.
2. Volume
a. The amount of space a substance occupies.
b. Base unit is the liter (L).
c. Tools: metric ruler for regular solids or graduated cylinder for liquids.

6. 3. Mass
a. The amount of matter in a substance.
b. Base unit - kilogram (kg).
c. Tool is the balance.
4. Weight
a. A measure of gravitational force on an object.
b. Unit is the newton (N).
c. Tool is the scale.

7. 5. Time
a. How long an event takes to occur.
b. Unit is the second (s).
c. Tool is the clock (stopwatch).
6. Temperature
a. The amount of kinetic energy a substance has.
b. SI unit is the Kelvin (K).
c. Tool is the thermometer.

8. 7. Density
a. How compacted the matter is in a substance.
b. Units can be g/mL, g/cm3, kg/m3.
c. Density is a derived unit (it is made up of other types of measurement).
d. D = m / v
e. Objects float if their density is less than the density of the fluid they are in.

9. Who is the Father of Atomic Theory?

10. Thomson’s Experiment:
In Thomson’s model of the atom, the negative charges are scattered throughout an atom filled with a positively charged mass of matter.
The “plum pudding” model

11. What did this experiment prove?
Beam of Alpha-Particles were
REPELED by Positive Charges in the nucleus

12. Atomic Theory: Who’s Model of the Atom?
Neils Bohr
The Bohr Model

13. Electron Cloud
An _________ _______ is a visual model of the most likely locations for electrons in an atom.
– Physical Science – Elements, Compounds, and Atoms
An Orbital is a region of space around the nucleus where an electron is likely to be found.
* An electron cloud is a good approximation of how
electrons behave in their orbitals.

14. Lewis Dot Diagram
An electron dot diagram uses the symbol of the element and dots to represent the outer level electrons.
Electron dot diagrams are used also to show how the electrons in the outer energy level are bonded when elements combine to form compounds.

15. Atom the smallest particle making up elements Proton = +
Neutron = neutral
Electron = -

16. Atomic Structure Basics:
Protons: positively charged particles, weighing 1 atomic mass unit (1.67x10-24 grams) and located in the nucleus.
Neutrons: neutrally charged particles, weighing approximately 1 atomic mass unit and located in the nucleus.
Electrons: negatively charged particles , weighing zero atomic mass units, located in orbitals of the energy levels found outside the atomic nucleus
From

17. Atomic Number:
The number of protons in an atom determines what element it is.
Add or subtract even one proton from an atom of any element and you no longer have the original element in any form. Now you have a different element!
Play the Name the Atom Game at:

18. C Drawing an Atom of Carbon 6 Atomic # = # of p+ and # of e-
12.011 6
Atomic #
= # of p+ and # of e-
Carbon has 6 p+ and 6 e-
Atomic Mass
minus Atomic # = # of n0
Carbon has 6 n0

19. Drawing an Atom of Carbone- e-
6 p+
6 n0

20. Periodic Table Basics:
Essential Question: What are Horizontal Rows called?
Answer: PERIODS

21. Electron Configuration
The “Period” number is equal to the number of energy levels in an atom
Remember: The number of electrons are equal to the number of protons in a neutral atom

22. What are Groups on the Periodic Table?
Essential Question: Groups are also known as Families of Elements.
They share chemical properties. WHY?
Answer: They have the same number of outer shell electrons.

23. Electron Configuration
For Groups IA – VIII the group numbers are equal to the number of outer shell electrons or valence electrons
Group “IA” has ONE valence electron
Group “IIA” has TWO valence electrons; etc.

24. Name that GROUP: The Alkali Metals IA = one outer shell electrons
therefore Oxidation state? +1

25. Name that GROUP: The Alkali Earth Metals
IIA = two outer shell electrons
Oxidation state? +2

26. Name that GROUP: The Noble Gases
VIIIA = eight outer shell electrons (except Helium which has 2 but is FULL)
therefore Oxidation state?
NOT!

27. Name that GROUP: The HALOGENS The Salt Formers
VIIA = SEVEN outer shell electrons
therefore Oxidation state? -1

28. Name that GROUP: The Transition Metals
B series = usually 2 or 3 outer shell electrons
therefore Oxidation state?
+2 or +3

29. Criss-Cross Method
Determine the charges/oxidation #’s for each element.
By criss-crossing the charges of the elements you can easily write the chemical formula
Example: Hydrogen + Oxygen
H + O  IONS = H O–2
Criss cross the oxidation #
just the numbers - not the + / - signs
Write the numbers as subscripts
bottom right of symbol

30. Criss Cross Method This becomes H+1 O-2 CrissCross the numbers H2O1
Final: H2O
Where is the 1 in the final formula?

31. Criss-Cross Method This becomes H+1 O-2 e- e- CrissCross the numbers
Final: H2O
Where is the 1 in the final formula?

32. Criss-Cross Method - -You Try it!
Mg + O
Ca + P
K + S
C + H
As + S
C + O

33. Criss-Cross Method You Try
Mg + O
Ca + P
K + S
C + H
As + S
C + O
 Mg2O2
 MgO
 Ca3P2
Just like with Fractions in math the Numbers will reduce!
 K2S
 CH4
 As2S3
 C2H4
 CO2

34. Criss-Cross & Polyatomic Ions
Sodium + Sulfate
Na + SO4
Na+1 + (SO4)-2
Do the Criss-Cross
Na2(SO4)1
Final: Na2(SO4)

35. Chemical Bonding: Ionic Ionic Bonding Covalent Metallic
Three types of bonding
Ionic Ionic Bonding
Covalent
Metallic
Game:
Bonding Animations and short clips
AWESOME MOVIE ON BONDING
30 minutes long

36. Ionic Bonding
Ionic Bonds: between oppositely charged atoms; usually on opposite sides of the periodic table (nonmetal and a metal)
transfer electrons
form networks, not molecules
conduct electricity

37. Covalent Bonds
Covalent Bonds: share electrons; usually between 2 elements close on the periodic table (2 nonmetals)
nonpolar covalent bond: e- shared equally
polar covalent bond: e- shared unequally

38. Metallic Bonding
“sea of electrons”: electrons can “float” freely between atoms; allows metals to conduct electricity well

39. Rules for naming and writing chemical formulas
1. Metal name comes first
2. Change the ending of the second element to “ide”
If you have two nonmetals, use the prefixes:
Mono – 1 Penta - 5
Di Hexa - 6
Tri Hepta - 7
Tetra – 4 Octa - 8

40. Which of the following is the correct name of a combination of sodium and iodine?
a) sodium chloride
b) sodium iodide
c) sodium iodine
d) iodine sodium

41. Transition Metal Naming
Transition metals show their charges as Roman Numerals because they can change charge!!
FeO = Fe+2 + O-2
Iron (II) Oxide
Fe2O3 = Fe+3 + O-2
Iron (III) Oxide

43. Chemical Reactions Types
Combustion: ALWAYS has O2 as a REACTANT!
AB + O AO + BO
Single-Replacement (single-displacement):
AX + B A + BX
Double-Replacement (double-displacement):
AX + BY AY + BX

44. Types of Chemical Reactions.
Type of Reaction
Definition
 Equation
Synthesis
Decomposition
Single Replacement
Double Replacement
Two or more elements or compounds combine to make a more complex substance
A + B → AB
Compounds break down
into simpler substances
AB → A + B
Occurs when one element replaces another one in a compound
AB + C → AC + B
Occurs when different atoms in two different compounds trade places
AB + CD → AC + BD
A = Red B = Blue C = Green D = Yellow

45. Identifying Chemical Reactions
Use colored pencils to circle the common atoms or compounds in each equation to help you determine the type of reaction it illustrates. Use the code below to classify each reaction.
S = Synthesis SR = Single Replacement
D = Decomposition DR = Double Replacement
____ P O2 → P4O10 ____ Mg O2 → MgO
____ HgO → Hg O2 ____ Al2O3 → Al O2
____ Cl NaBr → NaCl Br2 ____ H N2 → NH3

46. ____ Na + Br2 → NaBr ____ CuCl2 + H2S → CuS + HCl
____ HgO Cl2 → HgCl O2 ____ C H2 → CH4
____ KClO3  →   KCl  +  O2  ____ S F2 → SF6
____ BaCl2   +   Na2 SO4 →     NaCl   +   BaSO4

47. Acids & Bases Weak Acid/Base
The strength of an acid or base depends on how many acid or base particles dissociate into ions in water.
Strong Acid/Base
100% ions in water
strong electrolyte
HCl, HNO3, NaOH, LiOH
Weak Acid/Base
few ions in water
weak electrolyte
HC2H3O2, NH3 - + - +

48. pH Scale pH a measure of the concentration of H3O+ ions in solution
measured with a pH meter or an indicator with a wide color range

49. Atomic Structure:
How many neutrons in the following isotopes?
Hydrogen – 1
Helium – 4
Lithium – 6
Sodium – 22

50. More Isotope stuff… X H H (D) H (T) U A Z 1 2 3 235 92 238 Mass Number
Atomic Number
Element Symbol

51. Radioactive decay results in the emission [or release] of either:
an alpha particle (a),
a negative beta particle (electron) (b-),
a positive beta particle (positron) (b+),
or a gamma ray (g).
In a nuclear reaction the MASS and ATOMIC NUMBER must be the SAME on both sides of the equations

52. X Y + He Alpha Decay A Z A - 4 Z - 2 4 2
An alpha particle is identical to that of a helium nucleus.
It contains two protons and two neutrons. X A Z Y
A - 4
Z - 2 + He 4 2
unstable atom
alpha particle
more stable atom

53. X Y + e A Z Z + 1 -1 beta particle (electron) proton stays in nucleus
Beta Emission
A beta particle is a fast moving electron which is emitted from the nucleus of an atom undergoing radioactive decay.
Beta emission occurs when a neutron changes into a proton and an electron. X A Z Y
Z + 1 + e -1
beta particle
(electron)
proton stays
in nucleus

54. Gamma Decay
When atoms decay by emitting a or b particles to form a new atom, the nuclei of the new atom may still have too much energy to be completely stable. These unstable atoms will emit gamma rays to release that energy.
There is no change in mass or atomic number X A Z + g

55. Reaction What happens? Mass # Atomic # -4 -2 No change +1
Decay Summary
Reaction
What happens?
Mass #
Atomic #
Alpha Decay a
Lose Helium Nucleus -4 -2
Beta Decay b-
Lose electron from nucleus
(neutron turns into proton)
No change +1
Gammy Decay g
Emit high energy gamma ray and either a or b particle

56. The half-life of this element is 1 million years.
Test questions may involve
graphs like this one. The
Most common questions are:
"What is the half-life of this
element?"
Just remember, that at the end of one half-life, 50% of the element will remain. Find 50% on the vertical axis. Follow the blue line over to the red curve and drop straight down to find the answer:
The half-life of this element is 1 million years.

57. After 2 million years 25% of the original material will remain.
Another common question is: "What percent of the material originally present will remain after 2 million years?"
Find 2 million years on the bottom, horizontal axis. Then follow the green line up to the
red curve. Go to the left and find the answer.
After 2 million years 25% of the original material
will remain.

58. Nuclear Energy Essential Questions:
Why is it worth the RISK??
Tremendous OUTPUT of ENERGY!!
Fission or Fusion?
Fission! Atoms of U-235 are split
Use the link to see how Nuclear Fusion works:
Fusion! Atoms are joined or fused together.
McQuire Nuclear Power Station. The view from Hwy 16 in route to Charlotte. A “leak” would be a disaster for my sisters family as well as US!!

59. Heat energy:
Direction of Energy Flow?
HOT toward COLD

60. States of Matter
Watch what happens to molecules when heated by doing cool virtual experiments.
Click on the icon below to get started:

61. Change of Phase FIRST DO THIS Temperature Experiment By Clicking Here!
Phase change
Phase change
To Understand this Graph CLICK HERE

62. Chemical or Physical Change?
Chemical Change
Physical Change
New substances formed with new properties
Examples:
Rusting
Gas forming during a reaction (bubbles)
A precipitant forming during a reaction
No new substances formed
Examples:
Ice melting
Water evaporating
Dry ice subliming into Carbon dioxide
Salt or sugar dissolving in water

63. CLASSIFICATION OF MATTER

64. ELEMENTS contain only one type of atom building blocks of matter
115 known elements today, 90 which occur naturally
Found on periodic table
The first letter is always capitalized, the second letter is always lower case
Fluorine is F, not f
Cobalt is Co, not CO (which is carbon monoxide)

65. Properties – The way a chemical substance looks and behaves
Compounds
Compounds - 2 or more elements chemically combined to form a new substance with new properties
Properties – The way a chemical substance looks and behaves

66. Types of Matter:
Review basics about classifying matter by following the link below.
Watch the video clips!
Make sure you scroll all the way down to the chart to test your knowledge!

67. Mixtures and Pure Substances
A mixture has unlike parts and a composition that varies from sample to sample
A heterogeneous mixture has physically distinct parts with different properties.
A homogeneous mixture is the same throughout the sample
Pure substances are substances with a fixed composition

68. Matter
comes in 3 phases
Liquid
Solid
Gas

69. Solid
Definite Shape
Definite Volume

70. Liquid Indefinite Shape – takes the shape of the container
Definite Volume

71. Gas Indefinite Shape – takes the shape of the container.
Indefinite Volume – can expand and can be compressed.

72. Plasma Plasma: a high energy gaseous state of matter.
It is very unstable.
Particles are moving extremely fast, free energy
Most abundant phase of matter
Only present under extremely hot/energetic situations
Example: Sun

73. CHANGES IN STATE Melting: Solid to liquid Boiling: Liquid to gas
Sublimation: Solid to gas
The above three require input of energy
Condensation: Gas to liquid
Freezing: Liquid to solid
Deposition: Gas to solid
The above three release energy

75. PHYSICAL PROPERTIES
Characterize the physical state and physical behavior of a substance {appearance, smell, feel}
Each substance has unique physical properties
Examples
Sulfur appears as a yellow powder
The boiling point of water is 100 oC
Carbon monoxide is odorless

77. Solubility

78. Properties of Matter

79. Where is Magnetism Concentrated?
Magnetism is strongest at the
POLES

80. Magnetic Domains :
Not aligned:
Magnetic domains are ALIGNED in a permanent magnet :

81. What happens if you cut a magnet in half?
Each Part has a North and a south pole. S N S N

82. Electricity and Magnetism:
Electromagnetism

83. Get in line!

84. Electromagnets:
What Happens if you increase the number of coils in an electromagnet?
The magnet gets STRONGER!

85. Induction charging of two metal spheres:
from:

86. See http://www.physicsclassroom.com/Class/estatics/u8l2b.cfm

87. Potential Energy: PEgrav = mass • g • height
From
PEgrav = mass • g • height
Too hard to remember? Use the Reference Table!

88. Answer key: Note since PEgrav = m *• g • h
Doubling of the height will result in a doubling of the gravitational potential energy.
A tripling of the height will result in a tripling of the gravitational potential energy.
A: PE = 40 J (since the same mass is elevated to 4/5-ths height of the top stair)
B: PE = 30 J (since the same mass is elevated to 3/5-ths height of the top stair)
C: PE = 20 J (since the same mass is elevated to 2/5-ths height of the top stair)
D: PE = 10 J (since the same mass is elevated to 1/5-ths height of the top stair)
E and F: PE = 0 J (since the same mass is at the same zero height position as shown for the bottom stair
Fromhttp://

89. Physics Portion
Make a given table that lists the information you are given. BE SURE to include the item you are to find!
USE the Reference sheet! Find the equation that fits what you have.
Put the item you need to find on one side of the equals sign.
Add the other numbers and punch in the calculator.
Double check the answer from the calculator!