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PHYSICAL SCIENCE EOCT
Study Guide KEY
Nature of Science: Chapter 1
1.) What do scientific models represent? Objects too large or too small to put
inside a lab.
2.) What is the scientific method : Procedure for an organized investigation
3.) What is a hypothesis? Educated prediction of outcome of experiment
4.) Fill in the SI prefixes for the following phrase.
Kilo- 1000-King
Hecta-100-Henry
deci-1/10-Drinking
Deca-10-Died
Centi-1/100-Chocolate
Base-1-By
Milli-1/1000-Milk
5.) Calculate the conversions below:
1 meter  100 cm
100 grams  0.100 kilograms
10 ft 120 inches
1200 seconds  20 minutes
6.) Name the instrument used to measure mass? Triple Beam Balance
Volume? Graduated Cylinder
7.) Scientific Notation (The problems on the student copy should have been different. Just draw in arrows on your paper and
disregard the blanks after the numbers.)
102,000,000

1.02 x 108
0.000000000089  8.9 x 10-11
9.07 x 104
1 x 10-4
 90,700
 0.0001
8. Charts on next 2 pages of key will be analyzed during class.
CHEMISTRY:
(I.)Classification of Matter Ch. 2/3
STATE OF
MATTER
Solid
Liquid
EXPLANATION
Definite volume and shape
Definite volume and shape
of container
Gas
No definite volume or shape
1.) Place the following in order from big to small: atom, element, matter,
molecule
Matter Molecule Element  Atom
2.) What is the difference between compound, element, and mixture?
Compound: chemically bonded atoms
Element: basic building blocks
Mixture: substances blended together with no specific formula
3.) List the difference between a heterogeneous or a homogenous mixture,
and pure substance:
Substance
Heterogeneous
mixture
Homogeneous
Mixture
Pure
substance
Label examples:
Define
Mixture that all
components are seen
Mixture that all
components are blended
and looks like one
Specific chemical
formula
Example
pizza
tea, coffee
water H2O
a.) salt water: homogeneous
b.) garden salad: heterogeneous
c.) water: pure substance H2O
Know and understand the phase changes.
4.) Identify solvent, solute, solution for the list below:
a. Chocolate milk:solution
b. Milk: solvent
c. Chocolate: solute
5.) Answer: Weight is the result of gravity on mass; mass is how much matter
is in a substance measured in grams.
6.) Label a physical change or a chemical change:
a. melting: physical
b.combustion: _chemical
c. metabolism: chemical
d.boiling: physical
e. dissolving: physical
f. rusting: chemical
7.) Briefly state the Law of Conservation of Mass. (Ch. 7)
When a chemical reaction takes place the reactants must equal the
product. Matter cannot be created or destroyed.
8.) Briefly list the Kinetic Theory: (Ch.3)
a. All matter is made up of atoms
b. Atoms are always in motion
c. Atoms are always colliding
9.) Label the following SI units. (Ch. 1)
Quantity
Units of
Measure
Volume
Liters (L)
Density
Kg/mL or
Kg/cm3
Temperature Kelvin or
Celsius
Mass
Grams (g)
Acceleration Meters/seconds2
( m/s2)
Force
Newtons (N)
Power
Watts (W)
Resistance Ohms (Ω)
Speed
Meters/second
(m/s)
Energy
Joules (J)
Length
Meters (m)
Time
Seconds (s)
Current
Amperes (A)
(II.) ATOMS/ELEMENTS/BONDS
Chapter 4
Components Charge Location
1.) protons
+
Nucleus
2.) electrons
Energy
levels
3.) neutrons No
Nucleus
charge
4.) Nucleus
+
Center
of atom
1.) List the particles in the nucleus Protons and neutrons
2.) Where are valence electrons located in the atom and why are they
important for bonding?
Valence electrons are on the outermost energy level of the atom and the
number of Valence electrons determines which elements can bond
3.) List the number of valence electrons for:
Group 1: 1
Group 2: 2
Group 16: 6
Group 17 7
Group 18: 8 = complete; full outer energy level; no
OUTER energy level can hold more than 8 electrons
(valence electrons)
4.) What is special about the noble gases? They do not bond b/c their
outer orbital is full with 8 valence electrons.
5.) How are the elements placed on the periodic table? By atomic
number
6.) If an atom loses an electron it becomes an ion with a positive
charge.
7.) If an atom gains an electron it becomes an ion with a negative
charge.
8.) If an atom has the same number of protons but different number of
neutrons it becomes an isotope.
32
Ge
72.61
9.) What is the atomic number? 32 What does the atomic number represent?
Number of protons
10.) What is the atomic mass number? 73 What does atomic mass number
represent? Number of protons plus the number of neutrons.
11) Give the following for Ge: Protons:32 Neutrons: 73 – 32 = 41
Electrons: 32
Period:4 Group 14 Type of element metalloid
REMEMBER APE! ATOMIC # = PROTON NUMBER = ELECTRON #
12.) As the elements go across the Periodic Table, what happens to the size
and mass of the atoms? The atoms get bigger; atomic # & mass get
larger
13.) Fill in the Families of Elements:
Label each family or group on a blank periodic table (or go back to the graphic
organizer that we did 1st semester)
Family
Alkali
Metals
Alkaline
Earth
Metals
Transition
Metals
Semi
conductors
Non metals
Properties
Highly reactive
1 valence electron
Highly reactive
2 valence electrons
Group
1
2
Varied valence electrons 3-12
(metalloids) properties of
metals and non-metals
Touch
zig-zag
line
Poor conductors, brittle, Right of
low luster
stairsteps
Inert-non-reactive, happy 18
Noble
Gases
Chapter 6
14.) Explain the difference between the following bonds
What happens Give the type of
BOND
IONIC
to the
electrons?
transfer
COVALENT Share pair of
electrons
METALLIC
Share a pool
of electrons
elements that
bond
NaCl - Salt,
metal +
non- metal
Water- H2Onon - metal +
non - metal
Metal with metal
15.) organic compounds contain carbon
16.) # of valence electrons
17.) Write the chemical formula for the following:
Aluminum Oxide: Al2O3
Magnesium Bromide: MgBr2
Dihydrogen Monoxide: H2O HexaCalcium PentaManganese: Ca6Mn5
Calcium Fluoride: CaF2
18.) Define diatomic atoms and give an example?
Molecule made up of 2 of the same type of atoms that share electrons equally.
Ex: H2 N2 O2 Cl2 Br2 I2 F2
19. Polar molecule – a molecule with a polar bond in which electrons are not
shared equally; a non-polar molecule has a polar bond or bonds that are
shared equally
III. Chemical Reactions: Ch. 7
1.) Balance the following equations. Label Reactant and Product. Label the
type of reaction taking place:
a. __CH4 + 2 O2  __CO2 + 2 H2O
Combustion
b. 3 CuCl2 + 2Al  2AlCl3 + 3Cu
c. 8 Ag2S  16 Ag +__ S8
Single Displacement
Decomposition
d. 2 NaBr + __ Ca(OH) 2  __ CaBr 2 +2 NaOH
e. 2 NH3 + __ H2 SO4  __ (NH4)2SO4
Double displacement
Synthesis
Reactants are on the left; products are on the right. For example: for letter a,
the Reactants are: CH4 + 2 O2 and the Products: CO2 + 2 H2O
2.) Moles of oxygen on product side of a: two; (there are 4 total ATOMS of O)
3) Compare endothermic to exothermic?
Endothermic – feels cooler, Epsom salts, absorb heat
Exothermic - feels warmer, firecracker, release heat
4) How many Aluminum Chloride molecules are there in B after balancing? 2
5) How many molecules of Silver Sulfide are in C after balancing? 8
6) Define Equilibrium: Balance between reactant and product
7) What factors cause chemical reactions to go faster? Heat, increase
surface area, stirring, change concentration of reactants, use a catalyst
IV. Radioactivity: Ch. 10
1.) How do elements become radioactive? When an unstable atomic
nucleus emits charged particles and energy.
2.) Explain the 3 types of radiation:
TYPE
Alpha
Particles
Beta
Particles
Gamma
Rays
EXPLANATION/STRENGTH CHARGE
4
Helium particle – low
2 He
+ 4 charge
energy
0
Electron particle
-1 e
-1 charge
∞
Energy – high energy
0 charge
3.) Define Half-Life: Time it takes for a substance to decay in half.
4.) Describe the difference between fission and fusion:
Fission - division of nucleus
Fusion - combining of nuclei
5) Define isotope? Atom with same number of protons but different
number of neutrons.
6.) Write the Equation for U-238 (atomic number of 92) when it goes through
each type of decay.
Alpha:
238
92
U 
234
90
Th +
4
2 He
______________________________________________________________
Beta:
238
238
0
92 U
93 Np + -1 e
_______________________________________________________________
V. Matter/Acid & Bases: Ch. 8
1.) Label the following Heterogeneous/Homogeneous/Pure Substance:
a.) Salad: Heterogeneous e.) Milk: Homogeneous
b.) Egg: Heterogeneous
f.) Carbon: Pure Substance
c.) Water: Pure Substance
g.) dirt: Heterogeneous
d.) Salt water: Homogeneous h.) sugar: Pure Substance
2.) What is the difference between miscible and immiscible? Dissolvable vs
not dissolvable
3.) What is the universal solvent: water.
4.) Name 3 ways to speed up the dissolving process:
1. Stir
2. Heat
3. Crush - greater surface area exposed on smaller
particles
5.) Describe the difference between unsaturated and saturated:
See # 9 & 10 below
6.) Understand the pH Scale: Label Acid side and Base side and give
examples from page 247.
Acids pH 0 – 6.9 Neutral - 7
Bases 8 – 14
strong acid- 0 to 2
strong Base- 12 - 14
0 1 2 3 4 5 6 7 8 9 10 11 12 13 14
lemon
vinegar
bar soap
Drano
7.) What is the neutral substance on the pH scale? Water- pH of 7
8.) How do soaps work: (hint-emulsifier) Allow water and oil to mix
9.) Define saturated solutions. Contains as much solute as the solvent
can normally hold at a given temperature
10.) Describe unsaturated Solutions: Solutions that can dissolve more
solute
11.) What is the difference between Non-polar and Polar Molecules?
Non-polar molecules do not have a positive and negative side. Polar
molecules have a negative and positive side.
12.) Bases contain OH -1 ions and turn litmus (pH) paper blue.
Acids contain H3O+1 ions and turn litmus (pH) paper red.
VI. MOTION and FORCE: Ch. 11/12
1.) What is the difference between speed and velocity?
Speed is distance divided by time which is m/s and velocity is
speed with direction.
2.) What is the acceleration at:
a. constant speed: 0 m/s2
b. gravity: 9.8 m/s2
3.) What is the speed of aardvark in m/s that runs 10 meters every hour?
(convert hours to seconds!) 10m/3600s = 0.0028 m/s
4.) What is the acceleration of a car that goes from 0 to 60 m/s in 30
seconds? (remember units) 60m/s - 0m/s = 2m/s2
30s
5.) Define Net Force: overall force acting on an object after all
forces are combined
6.) If the Net Force is 0, the objects have balanced forces, which do not
move.
7.) What’s the difference between friction and air resistance? Friction is
the opposition to motion. Air resistance is the opposition to
motion in the air.
8.) Newton’s Laws:
Law Explanation
Write the
Equation & Ex.
1st Inertia-objects will
None; desk
remain at rest until
sitting still;
acted on by a force
planet in motion
2nd Acceleration is based Force is equal to
on force and mass
mass times
acceleration
3rd For every action
Rocket
there is an equal and launching
opposite reaction
VII. WORK and ENERGY: Ch. 14/15
1.) Fill in Table:
CONCEPT EXPLANATION
Work
Cause change
Power
Rate of work
Mechanical how much help
Advantage a machine will
do
Potential
Energy
Kinetic
Energy
Force
Weight
UNITS
Joules
watts
none
Stored energy
Joules
Energy of
motion
Push or pull on
an object
Force of gravity
on an object
Joules
EQUATION
w= F x D
P= w/t
Effort
distance
resistance
dist.
Hxgxm
½ mass x
(v)2
newtons F=mass x
acceleration
Newtons Wt= m x g
g = 9.8m/s2
4.) Simple Machines LEVERS and INCLINED PLANES
SIMPLE
Explanation
MACHINE
Levers
1st Class: fulcrum in
the middle
2nd Class: fulcrum at
one end, resistance in
middle
3rd Class: fulcrum at
one end and effort in
middle
Pulleys
Multiple or movable
pulleys increase the
mechanical advantage.
(count supporting
ropes for mechanical
advantage)
Wheel and Large wheel turns
axle
smaller axle
Examples
Inclined
Planes
Ramp
Multiply and redirect
the force
1st: see/saw-hammer
2nd: wheelbarrow
3rd:bat, broom , golf club
Block and tackle
Steering wheel
Wedge
Multiplies force and
redirects outward
Axe
Screw
Inclined plane
wrapped around a
cylinder
Drill bit
5.) The sum of kinetic and potential energy is the Mechanical energy.
6.) The source of all energy comes from the Sun.
7.) Law of Conservation of Energy states: Energy cannot be created or
destroyed but it can be transformed into another form
VIII. Heat: Ch. 16
1.) What is Absolute 0? All atoms stop moving. Has not happened.
2.) Fill in the Energy Transfer table:
Energy
Explanation
Transfer
Conduction Transfer of energy by contact
Convection Transfer of energy by the movement
of fluids (air) (currents)
Example
Lizard on a heated rock
Boiling water
Radiation
Transfer of energy by electromagnetic Sun
waves
3.) Define Specific Heat: The amount of heat needed to raise the
temperature of 1 kg of a substance by 1K.
4.) Which substance has the higher specific heat between iron and water:
water. Which substance will heat up the slowest? water
5.) If a substance is a good conductor then the specific heat is lower
because it heats up quickly.
6.) Label the parts of the equation: Heat Energy = c ∙ m ∙ ∆t
Joules = specific heat X mass X (final temperature – initial temperature)
IX. Waves: Ch. 17/18
Type of Wave Definition
DRAW
Electromagnetic From Long to
Wave
Short
wavelength
R, M, I, V, UV,
X, G
Longitudinal
Energy and
medium go in
same direction
Transverse
Medium moves
perpendicular
to the energy
1.) What types of waves do NOT require a medium: electromagnetic
2.) What type of waves do require a medium: mechanical (sound)
3.) Label the following Transverse Waves: (Insert center line)
Amplitude/Crest/Trough/Wavelength
Crest – Top of the wave
Trough – bottom of the wave
amplitude - distance from the rest position to the top of the crest or to the
bottom of the trough
wavelength - distance from crest to crest, trough to trough, or from the starting
point on one wave to the same point on the next wave
4.) Define and give an example:
a. Reflection: bouncing of waves; Ex: flat mirror
b. Refraction: bending of waves between mediums; Ex: pencil in
a glass of water
c. Diffraction: bending of waves around an object; Ex: hearing a
sound coming from around a corner of a building
d. Constructive Interference: waves overlap and make a stronger
wave; Ex: a musical note becomes
stronger when two separate instruments play the same note
5.) Compare frequency and pitch? The higher the frequency the higher
the pitch (higher musical note)
6.) Explain the properties of Sound:
a. Ultrasound (greater than 20,000Hz): sounds higher that humans can
hear; Ex: dog whistle or imaging for medical reasons
b. Infrasound (less than 20 Hz): sounds too low for humans to
hear; Ex: sounds coming from earthquakes that normally
not heard by humans; faulty electrical equipment
7.) Compare the speed of light and sound as they travel through a gas into
a liquid to a solid? The speed of LIGHT decreases as it travels from a gas
to a liquid, then decreases again as it travels from a liquid to a solid. The
speed of SOUND increases as it travels from a gas to a liquid, then
increases again as it travels from a liquid to a solid
(sound waves/mechanical waves MUST have a medium)
8.) Understand the diagram at the bottom of p. 9 on your review.
X. Electricity/Magnetism
Ch. 20/21
1. What type of circuit is this: parallel circuit
2. What type of cell is a car battery? Wet cell (electrolyte)
3.
4.
What determines the brightness of a light bulb’s filament: number of
coils and resistance
What is the unit for the following:
a. Resistance:
b. Potential Difference(voltage):
c. Current:
d. Power:
ohms
volts
amperes
watts
5. What is Ohm’s Law?
R= V/I - Resistance is related to volts and amperes.
6. What are two ways to transfer electrons to create a charge for static
electricity?
Induction and conduction
7. Put the following in order from least resistance to most resistance:
Conductors, insulators, superconductors, and semiconductors.
Superconductor, conductor, semiconductor, insulator
8. Lights connected in a single pathway are considered a series circuit.
9. Draw a schematic drawing of a simple circuit:
10.
What is the difference b/t AC and DC? Alternating current - current
reverses; direct current – travels in one direction
11.
If a 250 W heater has a current of 5.00 A, what is the resistance of the
heating element?
a. Remember the formula for power is P = I x V so P/I = V.
P
/ I = V;
250W/5 A = x V
50 V = x
V is the unknown so
b. Then you will need to plug the V (voltage) found into the Ohm’s law formula
to find resistance: R = V/I
R = 50V/5A
R = 10 Ω (ohms)
12.
Draw a magnet showing random magnetic domains.
weak magnet
13.
Draw a magnet showing the aligned magnetic domains.
strong magnet
14.
15.
What is an electromagnet? Magnet that becomes magnetized when
powered by an electrical source
Draw a bar magnet and label the field lines?
16. What are the differences between a motor and a generator?
Motor
Generator
1. Electrical energy to
1. Mechanical energy to
Mechanical
electrical energy
2. Needs power to run
2. Produces electricity
3. Example - fans
3. Example – turbines producing
electricity for homes
17.
What is the difference b/t a step up and step down transformer?
A step up transformer raises the amount of power flowing thru
the line and a step down transformer lowers the amount of
power flowing thru the line.