Honors Physical Science EOC Study GuideEOC Test Date: 5/25/17

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 conceptso Conduct systematic observationso Examine books & other sources of information to see what is already knowno Review & discuss what is known in light of empirical evidenceo Lab safety protocolso 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:

o Hypothesis—what MUST be included (explain below)-

If the type of light each plant grows underincreases 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

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.

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 hasSound 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:

*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

V=I×RVoltage=Current×Resistance

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/compressiono 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 Mass = amount of matter in a substance; measured in kilograms (kg)

o Weight = force on that matter by gravity; measured in Newtons (N)

o Gravity on Earth is 6 times greater than gravity on the Moon. Weight changes when gravity changes. Mass does not change.

o 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. 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.

Weakest—Gravity—Binds the universe and attracts all bodies of matter to each other.

Honors Physical Science EOC Study Guide---Part 2EOC 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.

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). 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 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 How many different elements? 3

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

OH- 1 extra electron—Anion O=1, H=1 elements= 2

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 = EXOTHERMICReactions are exothermic when they release more energy to FORM THE NEW BONDS; release energy

Breaking Bonds = ENDOTHERMICReactions 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.

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.

2 Na + Cl2 2 NaCl

General form: A + B AB

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=gmN2fRlQFp4https://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.