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Honors Physical Science EOC Study Guide
EOC Test Date: June 3, 2016
There will be a total of 50 questions.
Experimental Design/Nature of Science:
SC.912.N.1.1 Define a problem based on a specific body of knowledge. For example: biology, chemistry, physics, and
earth/space science. (3 questions-2 moderate, 1 high)
o Define a problem based on a specific body of knowledge (biology, chemistry, physics, earth/space)
o Pose questions about the natural world using body of knowledge concepts
o Conduct systematic observations
o Examine books & other sources of information to see what is already known
o Review & discuss what is known in light of empirical evidence
o Lab safety protocols
o Observation vs inference (explain below)Observation—Qualitative (5 senses-descriptions) or Quantitative (measurements). Describing only what is
seen, heard, felt, smelled, tasted or measured. Elli’s shirt is Red. Inference—conclusion made based
on observation only. Elli’s favorite color is Red.
o Variables – Define:
Factors in an Experiment
Dependent (outcome) Variable: factor being measured (also called outcome variable), always indicated on the y axis when graphed
Independent (test) Variable: factor being altered (also called the test variable), always indicated on the x axis when graphed
Control: standard used for comparison to the experimental data
Constant: factor(s) that does not change so that a relationship between the independent and dependent variables can be established
Good experiments have many CONSTANTS and only change ONE variable at a time (test variable). This creates a FAIR
test and gives you more VALID data.
o Hypothesis—what MUST be included (explain below)If the type of light each plant grows under
increases in frequency turning it from
yellow to green (ROY G BIV), then the
growth of the plant will increase because
the plant will be receiving more energy.
*Hypotheses must include the test variable,
and the outcome variable. Constants are
unnecessary due to the number of
possible constants (also called controlled
variables).
Energy
SC.912.P.10.1 Differentiate among the various forms of energy and recognize that they can be transformed from one form
to others. (3 questions-1 low, 2 moderate)

Differentiate among the various forms of energy & recognize that they can be transformed from one for to another.
What are the 6 types of energy we discussed (include explanations)?
**This image has
Sound and
Mechanical
Separate, but
You get the
Gist.

Give 2 examples where multiple energy transformations occurs.
SC.912.P.10.18 Explore the theory of electromagnetism by comparing and contrasting the different parts of the
electromagnetic spectrum in terms of wavelength, frequency, and energy, and relate them to phenomena and applications.
(2 questions-1 low, 1 moderate)
 Explore the theory of electromagnetism by comparing and contrasting the different parts of the electromagnetic
spectrum in terms of:
o Wavelength—distance between crests or troughs (or compressions/rarefactions)—Longer WL = lower
frequency.
o Frequency--the number of waves passing a point in a certain time. We normally use a time of
one second, so this gives frequency the unit hertz (Hz), since one hertz is equal to one
wave per second.
o Energy—Electromagnetic. Higher frequency = more energy….same speed though!.
o Relate them to phenomena and applications—see below
Draw the Electromagnetic Spectrum below. Include the bullets above within the picture.
SC.912.P.12.7 Recognize that nothing travels faster than the speed of light in a vacuum which is the same for all observers
no matter how they or the light source are moving. (1 question-1 moderate)
 You will not be required to know the quantitative value for the speed of light, ONLY that nothing is faster!!!!!!
 You will NEED to know that regardless of the speed of an observer or source, in a vacuum, the speed of light is always
constant.
SC.912.P.10.15 Investigate and explain the relationships among current, voltage, resistance, and power. (2 questions-1
moderate, 1 high)
 Define the following electricity terms-- *Remember this slide from our PowerPoint (on Resources Tab).
o Power - Electric power is calculated from current and voltage: P = I x V
Also from our PowerPoint!!!!!------
Charge—Moving electrons give a charge to a circuit.
Circuit-- Electric circuit: a complete path through which charge (current) can flow
Transfer of energy within a circuit (explain)—Source (Battery-Chemical Energy), when closed, begins the flow of electrons
(the current) through the wires. The battery has a set voltage. The thickness and material of the wire determines the
amount of resistance in the circuit. The electrons move through the wires and metal components of each part of the circuit
because a conductor is necessary to maintain the flow of electricity. The electrons move through a light bulb, causing
friction and heat is produced. A light shines. The current and voltage determine how much power gets to the light bulb.
Light bulbs are designed to take in different amounts of Power depending on their Wattage.

Explain the relationship between current, voltage, resistance, and power
Current, voltage and resistance are related in a circuit according to
Ohm’s Law:
V  I R
Voltage  Current  Resistance
*If the resistance stays the same, what happens if the voltage increases?
 The current increases.
*If the voltage stays the same, what happens if the resistance increases?
 The current goes down.
Electric power is calculated from current and voltage: P = I x V
SC.912.P.10.3 Compare and contrast work and power qualitatively and quantitatively. (3 questions-1 low, 2 moderate)
*This is NEW!
 Compare and contrast work and power qualitatively and quantitatively (use the benchmark and contents above to
help you with this….they are VERY much related)-Power is a measure of how much work can be performed in a given amount of time.
Work is generally defined in terms of the lifting of a weight against the pull of gravity. The heavier the
weight and/or the higher it is lifted, the more work has been done. Work (when used in terms of force and
motion) is equal to force x distance.
In Electric Circuit, voltage is the specific work (or potential energy) per unit, while current is the rate at which
electric charges move through a conductor. Voltage (specific work) is viewed as the work done in lifting a
weight against the pull of gravity. Current (rate) is viewed as the speed at which that weight is lifted.
In electric circuits, power is a function of both voltage and current.
Power = Current (I) x Voltage (seen as WORK when in a circuit)
SC.912.P.10.14 Differentiate among conductors, semiconductors, and insulators. (2 questions-1 low, 1 moderate)
 Explain the difference between conductors, semiconductors, & insulators.
Conductor – Transfers heat and electricity easily; METALS, SOLIDS
Insulator – Prevents transfer of heat and electricity; NONMETALS, GASES
Semiconductor – Transfers some heat and electricity; METALLOIDS(such as silicon) When cooler, semiconductors are
insulators, when heated they are conductors.

How is energy transferred?
SC.912.P.10.21 Qualitatively describe the shift in frequency in sound or electromagnetic waves due to the relative motion of
a source or a receiver. (1 question-1 low)
Waves-Mechanical vs electromagnetic—Describe:
o
Transverse vs
longitudinal/compression
o
Wave characteristics (label the
parts of a wave)
o How energy is transferred?
--Transverse-Light---Needs no medium to transfer
--Longitudinal-Sound—HAS to have a medium in order to transfer
o Compare Sound vs. Light (speed in different media—vacuum, gas, liquid, solid)
Sound---Travels best through Solids where the medium (particles) are closest together, then liquid, then gas, and sound
does not travel through a vacuum.
Light—Travels best through a vacuum where there is no matter to slow it down. Then a gas, then liquid, then a solid. Light
cannot travel through Opaque solids, translucent lets little through, and transparent solids do allow the flow of light energy.
Light can also be reflected, refracted (bent when hits another medium….like gas to liquid), absorbed, or diffracted (or
scattered).
SC.912.P.10.5 Relate temperature to the average molecular kinetic energy. (2 questions-1 low, 1 moderate)
o Relate temperature to the average molecular kinetic energy (Kinetic Molecular Theory in terms of thermal
energy).
Temperature is the AVERAGE kinetic energy of all the particles in a substance. More KE, means a higher
temperature. Objects with higher temperatures will transfer some energy to objects they are in contact with. This
is HEAT and will happen until both objects are the same temperature.
SC.912.P.10.4 Describe heat as the energy transferred by convection, conduction, and radiation, and explain the
connection of heat to change in temperature or states of matter. (1 question-1 high)

Describe heat as the energy transferred by convection, conduction, and radiation.
Remember---Radiation is the initial transfer of heat to anything. Whatever has been heated transfers that heat through
fluids (liquids/gases) it is called convection. OR if that heat is transferred through solids, it is conduction.

Explain the connection of heat to change in temperature or states of matter.
All phase transitions occur at a constant temperature.
Once the sample of water reaches 100 degrees,
boiling occurs. Large bubbles of gas would be
observed forming throughout the bulk of the
liquid. The heat added to the liquid during this
stage causes a loosening of the attractions that
hold the water particles in the liquid state. The
temperature remains constant while the state of
water changes. Once all the water transitions
from the liquid to the gaseous state, the sample
of water (now in the gaseous state) begins to
increase its temperature again.
The energy absorbed by the water is used to loosen the attractions that hold one ice particle to another. Once all these attractions are
loosened, the ice would be observed to have entirely melted.

Explain the relationship between kinetic energy & heat.
Temperature changes are the result of the added energy causing the particles of to move more vigorously (or removing energy to
cause them to move more slowly). The addition of heat is causing an increase in the average kinetic energy of particles.
FORCES and MOTION
SC.912.P.12.3 Interpret and apply Newton's three laws of motion. (3 questions)
 Interpret & apply Newton’s three laws of motion (be able to solve for force)
o List Newton’s 3 Laws and give a real life example of each one.
SC.912.P.12.2 Analyze the motion of an object in terms of its position, velocity, and acceleration (with respect to a frame of
reference) as functions of time. (4 questions-1 low, 2 moderate, 1
high)

Analyze the motion of an object as functions in time in terms
of its:
o Position: See image to the right.
o Velocity (define)--- Speed in a given direction
*Calculated as Speed= Distance / Time
o Distance – Time Graph
 Measure and graph the movement of an object which travels at a constant speed
 Interpret the relationship of distance versus time
 Draw a distance vs. time graph and show constant speed. Explain it. Add a line with a different
color showing speed changing. Explain it. *Make a KEY!
Example
o Acceleration (with respect to a frame
of reference)—(define)— A change in
velocity (speed/direction) over time.
V2-V1 / Time (Final Velocity –
Initial Velocity) / Time
o Acceleration – Time Graph
 Measure and graph the movement of an object which travels at a constant speed
 Interpret the relationship of acceleration versus time.
 Draw a speed vs. time graph and show constant speed. Explain it. Add a line with a different color
showing positive acceleration, and one showing negative acceleration. Explain them. *Make a
KEY!
SC.912.P.12.4 Describe how the gravitational force between two objects depends on their masses and the distance
between them. (2 questions-1 low, 1 moderate)

Describe how the gravitational force between two objects depends on their masses & the distance between them
Mass ≠ Weight
o
o
o
o
Mass = amount of matter in a substance; measured in
kilograms (kg)
Weight = force on that matter by gravity; measured in
Newtons (N)
Gravity on Earth is 6 times greater than gravity on the
Moon. Weight changes when gravity changes. Mass does
not change.
GRAVITY changes based on distance and mass of the
objects. The CLOSER and MORE MASSIVE the objects are,
the MORE gravitational attraction there will be between
them.
SC.912.P.10.10 Compare the magnitude and range of the four fundamental forces (gravitational, electromagnetic, weak
nuclear, strong nuclear). (2 questions-1 moderate, 1 high)

What are the 4 fundamental forces (gravitational, electromagnetic, weak nuclear, strong nuclear)? Explain each
one. Which is the strongest?
Strongest ---Strong Nuclear force---This force holds the nucleus of an atom together. *Fusion. It is the strongest
force we know of as evidenced by the massive energy output when the nuclei is split.
Electromagnetic Force--Electromagnetism and the force that binds it is found in rainbows, lightning, and all
human-made devices using electric current. On an atomic level, it is essential in the bonding of molecules.
Weak nuclear Force is what is involved as the subatomic particles in an atom decay. *Fission
Weakest—Gravity—Binds the universe and attracts all bodies of matter to each other.
Honors Physical Science EOC Study Guide---Part 2
EOC Test Date: June 3, 2016
Chemistry
SC.912.P.8.2 Differentiate between physical and chemical properties and physical and chemical changes of matter. (1
question-high)

List 6 physical properties of matter and explain (define) them. Include 2 characteristic properties and explain why
they are characteristic properties.
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Color
Odor – how something smells
Luster - How shiny a substance is
Malleability - The ability of a substance to be beaten into thin sheets.
Ductility - The ability of a substance to be drawn into thin wires.
Thermal Conductivity - The ability of a substance to allow the flow of heat energy.
**Electrical Conductivity - The ability of a substance to allow the flow of electricity.
Magnetic Property – The ability of metals to be attracted to a magnet.
Hardness - How easily a substance can be scratched.
**Melting/Freezing Point - The temperature at which the solid and liquid phases of a substance
are in equilibrium at atmospheric pressure.
**Boiling Point - The temperature at which the vapor pressure of a liquid is equal to the
pressure on the liquid (generally atmospheric pressure).
**Density - The mass of a substance divided by its volume
Mass - A measurement of the amount of matter in a object (grams).
Weight - A measurement of the gravitational force of attraction of the earth acting on an object.
Volume - A measurement of the amount of space a substance occupies.
Length – How long and object is
**= Characteristic Properties because the amount of substance does not matter….those properties allow you to
identify the objects/substances. Ie., The density of water at sea level at 20 Degrees C is 1 g/mL, The boiling point
of water at sea level is 100 Degrees C, The Freezing/Melting point of water is 0 Degrees C at sea level.

List 3 chemical properties of matter and explain them (define).
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Flammability (the ability to catch on fire)
Reactivity with water (what happens when a substance reacts with water)
Reactivity with acids (what happens when a substance reacts with an acid)
Oxidation (the combination of a substance with oxygen)
Differentiate between physical and chemical changes of matter.
SC.912.P.12.11 Describe phase transitions in terms of kinetic molecular theory. (1 question-1 moderate)
**This is just states of matter (no plasma)! **Just fancy for moving molecules!
 State the Kinetic Molecular Theory (look this up, just for terminology).
Temperature is the AVERAGE kinetic energy of all the particles in a substance. More KE, means a higher temperature.
Objects with higher temperatures will transfer some energy to objects they are in contact with. This is HEAT and will
happen until both objects are the same temperature.

Describe phase transitions in terms of kinetic molecular theory. Include
temperature has to do with kinetic molecular movement.
Increase temperature, increase kinetic molecular movement.
SC.912.P.8.4 Explore the scientific theory of atoms (also known as atomic theory) by describing the structure of atoms in terms of
protons, neutrons and electrons, and differentiate among these particles in terms of their mass, electrical charges and locations within
the atom. (1 question-1 moderate)

Scientific Theory of Atoms (also known as Atomic
Theory)
o Structure of atoms in terms of protons,
neutrons, & electrons
o Differentiate among these particles in
terms of their mass, electrical charges,
& locations within the atom
The nucleus (protons (positive) + neutrons (neutral)) make us the majority of the mass of the atom. Hence, atomic mass =
#protons + #neutrons. This is located in the center of the atom. The charge of the nucleus is + and the nucleus is held
together by the strongest force known—Strong Nuclear Force. Because of that, the # of protons does not change unless
the entire element does. If neutrons vary, just by the nature of the make-up, the atom is called an isotope. The electrons
(negative) travel quickly in a cloud surrounding the atom. They are attracted to the positive nucleus of their own atom, but
can be shared or taken if another needs to share or take electrons in order to become stable.
SC.912.P.8.5 Relate properties of atoms and their position in the periodic table to the arrangement of their electrons. (3
questions-1 low, 1 moderate, 1 high)

Explain how the position of an atom on the periodic table directly relates to its electron
configuration.
 What
to
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
atoms/elements in the same group have in common?
Chemical Properties (and some physical). Ie., all of Group 1 are highly reactive Alkali Metals. As you move down
the groups, the more reactive the elements become.
What else does the group tell us?
Also, groups share the number of valence electrons used in bonding.
What does the period tell us?
The period number relates to the energy levels the atom has for its electrons. Ie., we know that period 6 has
more energy levels than period 2 and is therefore more reactive and also all have more mass.

Be able to determine the number of valence electrons.
Groups 1, 2, 13 (3), 14 (4), 15 (5), 16 (6), 17 (7), 18 (18) ----See above
SC.912.P.8.7 Interpret formula representations of molecules and compounds in terms of composition and structure. (2
questions-1 low, 1 moderate)

Interpret formula representations of molecules and compounds. How many atoms/elements/ions, etc. Give 4
different examples (atomic centers or exit pass) and break them apart to tell how many atoms, elements, if it is an
ion, etc. ie.,
H2SO4 ---how many of each atom?
H=2, S=1, O=4
Pb(NO3)2
1 Lead, 2 Nitrate Compound Molecules
Pb=1, N=2, O=6
elements=3
3PbI2
3 PbI2 compound molecules
Pb=3, I=6
elements=6
O=1, H=1
elements= 2
OH-
1 extra electron—Anion

How many different elements? 3
Be able to write a chemical formula for common substance when given the number of atoms (like your exit pass).
o Ie., 2 atoms of Hydrogen and 1 atom of Oxygen = H2O
o Covalent bonded molecule= (Between
which types of atoms usually?)
o Ionic bonded molecule = )Between
which types of atoms usually?)
SC.912.L.18.12 Discuss the special properties of water that contribute to Earth's suitability as an environment for life:
cohesive behavior, ability to moderate temperature, expansion upon freezing, and versatility as a solvent. (2 questions)
o Discuss the special properties of water that contribute to Earth’s suitability as an environment for life:

Cohesive behavior-Water is attracted to other water molecules due to the slight
charge when hydrogen and oxygen bond covalently.

Ability to moderate temperature—Water has a high specific
heat. This means that the amount of heat that must be
absorbed (or lost) by water in order to change 1 g g of water 1 degree is A LOT! SO…..areas
surrounded by water have a moderate climate because the water absorbs the heat without raising
the temperature of the water too significantly. At night, loss of heat from the water results in
warmer air. Our bodies work the same way! We need water in our bodies to regulate our
temperature and to maintain homeostasis.

Expansion upon freezing---Ice floats in liquid water because ice is less dense. Upon
freezing, the density of water decreases by about 9%. As water cools, there is less
molecular movement, thus the molecules loosen their bonds and begin to form steady
hydrogen bonds with their neighbors. This locks them into an organized pattern. And
BAM! ICE.

Versatility as a solvent—More substances
dissolve in water than any other chemical.
This is why it is known as the Universal
Solvent. However, it does not dissolve
EVERYTHING. Water is Polar. It has a
negative side (O) and a positive (H). Due to
this polarity, it can dissolve other polar
substances as well as charged (or ionic)
substances due to the unbalance. It will NOT dissolve NON-Polar substances (like oil).
SC.912.L.18.7 Identify the reactants, products, and basic functions of photosynthesis. (1 question-1 moderate)

Identify the reactants, products, & basic functions of photosynthesis---Write the equation and identify the reactants,
products, and basic functions. Be able to discuss the molecular formulas (amount of atoms, etc).
*Energy on the Reactant side
= ENDOTHERMIC
Plants absorb energy from sunlight to turn carbon dioxide and water into oxygen and glucose, which is a type of sugar
molecule. The energy is stored in the glucose molecules, ready to be used when needed.
SC.912.L.18.8 Identify the reactants, products, and basic functions of aerobic and anaerobic cellular respiration. (2
questions-1 low, 1 moderate)

Identify the reactants, products, & basic functions of aerobic & anaerobic cellular respiration--- Write the equation
and identify the reactants, products, and basic functions. Be able to discuss the molecular formulas (amount of
atoms, etc).
Most of the plant and animal cells use aerobic respiration. On the other hand, anaerobic bacteria, yeast cells,
prokaryotes, and muscle cells perform anaerobic respiration. ANAEROBIC does NOT have OXYGEN as a reactant
like AEROBIC
C6H12O6
2C2H5OH + CO2 + Energy
***Note---BOTH types of respiration have ENERGY on the PRODUCT side. Therefore, BOTH types of respiration are
considered EXOTHERMIC reactions (putting energy as being given OFF).
SC.912.P.10.7 Distinguish between endothermic and exothermic chemical processes. (2 questions-1 low, 1 moderate)
 Distinguish between endothermic & exothermic chemical processes (Explain the difference)When you think about exothermic and endothermic reactions, consider energy to be part of the reaction.
Forming Bonds = EXOTHERMIC
Reactions are exothermic when they release more energy to FORM THE NEW BONDS; release energy
Breaking Bonds = ENDOTHERMIC
Reactions are endothermic when they require more energy to BREAK BONDS; absorb energy
**See above info on Photosysthesis and Respiration as well as refer to our alka selzer lab and foaming mess lab.

How can you tell what the reaction will be when looking at the Chemical Equation? (Reactants and Products)
An exothermic reaction releases energy, so energy is on the product side of the chemical equation.
Exothermic Reaction=
Reactants
Products + Energy (Heat)
An endothermic reaction absorbs energy (taking energy to break bonds), so energy is on the reactant side of the
chemical equation.
Endothermic Reaction=
Reactants + Energy
Products
SC.912.P.8.8 Characterize types of chemical reactions. For example: redox, acid-base, synthesis, and single and double
replacement reactions. (2 questions-2 moderate)
 Explain the types of chemical reactions (Give examples):
Redox---- Both Synthesis and Decomposition reactions are considered Oxidation-Redox
reactions. Oxidation (redox) is a type of chemical reaction in which electrons are transferred
from one substance to another. For oxidation to occur, one substance must lose electrons and a
second substance must gain the lost electrons. The substance gaining electrons is said to
be reduced and the substance losing the electrons is said to be oxidized. Thus an oxidation
reaction is called a Redox reaction.
Acid-base AKA Neutralization---is a type of chemical reaction in which a strong acid and strong base react with each other to form
water and salt.
Acid-Base is a type of DOUBLE REPLACEMENT.
HBr + NaOH ---> NaBr + H2O
Synthesis-- A synthesis reaction is when two or more simple compounds combine to form a more complicated one.
General form: A +
B 
AB
2 Na
+
Cl2

2 NaCl
Decomposition----A decomposition reaction is the opposite of a synthesis reaction - a complex molecule breaks down to
make simpler ones.
2NI3
N2 + 3I2
Single replacement -- when one element trades places with another element in a compound
Double replacement-- when the anions and cations of two different molecules switch places, forming two entirely different
compounds.
SC.912.P.12.10 Interpret the behavior of ideal gases in terms of kinetic molecular theory. (1 question-1high)
***This is NEW! See website for help on this and on work/power.
 What is Kinetic Molecular Theory? (Repeat)
Interpret the behavior of ideal gases in terms of Kinetic Molecular Theory. *See
websites and videos below.
Great Gas Simulator on PHET:
https://phet.colorado.edu/en/simulation/gas-properties
Gas Videos:
https://www.youtube.com/watch?v=gmN2fRlQFp4
https://www.youtube.com/watch?v=EHxdVtygP1g

Think though….it isn’t too farfetched…
*Higher volume = Higher Temperature…..this makes sense! Thermal
energy causes molecules to spread out and take up more space!
*More space (high volume) = lower pressure as the molecules are not
compressed!
*In a CLOSED system, higher temperature = higher pressure as particles
bounce off the walls of the closed container and increase pressure.