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. Matter
comes in 3 phases
Liquid
Solid
Gas

10. Solid
Definite Shape
Definite Volume

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

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

13. 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

14. 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

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

16. PHYSICAL and CHEMICAL PROPERTIES
Property of a substance that does not change even if substance is altered.
Examples- melting point, odor, color, etc.
Chemical:
Property of a substance that can only be observed because substance is changed.
Examples- combustibility, reaction with acid

17. 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

18. Properties of Matter

19. CLASSIFICATION OF MATTER

20. 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)

21. 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

22. 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

24. 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.

25. 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.

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

27. 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

28. 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:

29. 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

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

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

32. 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

33. 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.

34. 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.

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

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

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

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

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

40. 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

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

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

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

44. 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

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

46. 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

47. 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

48. 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

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

50. 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

51. 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

52. 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

54. 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

55. 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

56. 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

57. ____ 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

59. Solubility

60. 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 - + - +

61. 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

62. Isotopes- Forms of an element with different numbers of neutrons (different masses)
Isotopes of Hydrogen
Protium- A#1 M#1 #N=0
Deuterium- A#1 M#2 #N=1
Tritium- A#1 M#3 #N=2

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

64. 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

65. 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

66. 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

67. 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

68. 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

69. 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.

70. 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.

71. 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!!

72. Electromagnetic Energy
Types of Energy
Mechanical Energy
Kinetic (motion) and Potential (stored)
Heat Energy
Chemical Energy
Nuclear Energy
Electromagnetic Energy
Light, Sound, Electricity, Magnetism

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

75. Calculating Q Q= Mass (m) X DT (change in temp) X Cp (Specific Heat)
Mass- in grams (or an equivalent unit to the mass in Cp)
DTemperature- (End Temp Co) – (Beg. Temp Co)
Cp- J/g X Co (a chart with CP values will be provided or you will be given the Cp value in the problem)

76. Q Practice Problem
If the temperature of 34.4 g of ethanol increases from 25 C to 78.8 C, how much heat has been absorbed by the ethanol? (The Cp of Ethanol is 2.44 J/g . C).
Q= 34.4 g X ( ) X 2.44 J/g . C
Q= J ~ 4.52 X 103 J
Why is subtracting end temp – beg temp SO IMPORTANT?
To know if heat is being lost (-) or absorbed (+)

77. Three Ways to Transfer Heat
Conduction
Direct contact
Convection
Cyclic Movement
Radiation
Through empty space

78. Explain how an object can have a zero or negative displacement.
Dist. Vs. Disp.
Distance
Actual path that an object takes
Cannot be negative
Displacement
Straight line from start to finish
Can be negative or zero
Think about your charts made to calculate distance and displacement on the grid.
Explain how an object can have a zero or negative displacement.

79. Speed and Velocity Speed: the rate at which an object changes position
m/s : SI unit for speed

80. Instantaneous vs. Average
Instantaneous Speed:
speed at a particular point in time
Ex: Speedometer of a car
Average Speed:
speed taken over a distance traveled
Ex: Calculating your speed over an entire trip

82. How is velocity different than speed?
Velocity is speed with a direction.
Ex: traveling 60 km/hr North
Two ways to change velocity:
1. Change speed (speed up/slow down)
2. Change direction (turn)

83. Acceleration Acceleration: is the rate of change in velocity
Acceleration = change in velocity
time
a = ve – vb
SI unit of acceleration = m/s/s or m/s2

84. Ways to Change Acceleration
Change Speed
Change Direction
Can you have negative acceleration?

85. Speed and Time Graphs

86. Forces
A force causes an object to move, accelerate, change speed, or direction
The unit of force is the Newton (N).
1 N = 1 kg x m/s/s

87. Balanced & Unbalanced Forces
Balanced forces – opposite and equal forces acting on the same object
result in NO motion of the object
Unbalanced forces – two or more forces of unequal strength or direction acting upon on an object
results in motion of the object

88. Types of Forces
Gravity
Friction
Fluid Pressure Forces
Air Pressure

89. Falling Objects
A falling object will accelerate downward at 9.8 m/s/s (in a vacuum). However, in real life air resistance will gradually slow it down.
Terminal velocity is the top speed reached by a falling object. At terminal velocity air resistance is equal to gravitational pull.

90. Circular Motion
According to Newton's 1st Law, an object will move in a straight line unless a net force causes it to do otherwise.
Therefore, an object moving in a curved or circular path, like a tetherball, must have a force pulling it in a circle.

91. Work
Work is done on an object when a force is exerted on an object that causes the object to move some distance.
No work without motion
No work without force in the same direction

92. Direction and force
Horse does not work on the rider – force not in same direction
Horse does work on the cart - force and motion in the same direction
Force on person
Force on cart
motion
motion

93. Calculating work Work = Force X Distance Force units = Newton, N
Distance units = meter, m
Work units = Joule, J
J = N*m

94. 4. Calculating Work
4. A woman lifts her 100-newton child up one meter and carries her for a distance of 50 meters to the child’s bedroom. How much work does the woman do?
Work
100 N X 1 m= 100 N-m
(the 50 meter carry is not in the upward direction the force is applied)

95. Mechanical advantage
Mechanical Advantage is used to determine if using a simple machine would be better to accomplish work than not using a simple machine.
Example- would it be better to dig a hole with your hands or a shovel?
If M.A. > 1 than using the simple machine was beneficial.
If M.A. < 1 than it would have been better to NOT use the simple machine.

96. Mechanical advantage
There are TWO ways to calculate Mechanical Advantage:
Ideal Mechanical Advantage (IMA) which uses distances to determine.
Actual Mechanical Advantage (AMA) which uses force to determine.

97. The 6 Simple Machines Movable Machines Non-movable Machines Pulley
Wheel and Axle
Lever
Non-movable Machines
Wedge
Inclined Plane
Screw

98. What does a simple machine do?
Make work easier by
Changing the applied force
Changing the distance over which the force is applied
Changing the direction of the effort force
What does a simple machine NOT do?
You cannot get more work output than work input!

99. R- 2nd Class- Resistance E- 3rd Class- Effort
3 Classes of Levers:
Remember what is in the middle:
F- 1st Class-Fulcrum
R- 2nd Class- Resistance
E- 3rd Class- Effort

100. Transverse waves
A transverse wave is one in which the disturbance is perpendicular to the direction of travel of the wave.
Examples: Light wave, waves on a guitar string.

101. Longitudinal Waves
Longitudinal wave is one in which the disturbance is parallel to the line of travel of the wave.
Example: Sound wave in air is a longitudinal wave.

102. The Nature of Sound Longitudinal Sound Waves
Sound in air is a longitudinal wave that is created by a vibrating object, such as a guitar string, the human vocal cords, or the diaphragm of a loudspeaker.

103. Constructive Interference of Sound Waves
Wavelength = λ = 1 m
Path difference = 0

104. Destructive Interference
Wavelength = λ = 1 m
Path difference = λ/2= 0.5 m

105. Doppler effect Change in frequency and pitch of a sound.
Due to the motion of either the sound source or the observer.
Listen!

106. Doppler effect of sound

107. Electromagnetic Waves
Transverse waves without a medium!
(They can travel through empty space)

108. Electromagnetic waves travel VERY FAST – around 300,000 kilometres per second (the speed of light).
At this speed they can go around the world 8 times in one second.

109. Waves or Particles?
Electromagnetic radiation has properties of waves but also can be thought of as a stream of particles.
Example: Light
Light as a wave: Light behaves as a transverse wave which we can filter using polarized lenses.
Light as particles (photons): When directed at a substance light can knock electrons off of a substance (Photoelectric effect)

110. Notice the wavelength is
long (Radio waves) and gets shorter (Gamma Rays)

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

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

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

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

115. Get in line!

116. Ways to charge an object: 1. Conduction- direct touching 2
Ways to charge an object: 1. Conduction- direct touching 2. Induction- getting inside field but not touching 3. Friction-rubbing two objects together (forms static electricity)
from:

117. 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://

118. 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!