EOCT Review

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EOCT Review

Physics

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Section 1: Motion, Forces, and Energy

SPS 7. Students will relate transformations and flow of energy within a system.SPS 8. Students will determine relationships among force, mass, and motion.

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Speed and Velocity: SPS 8a. Calculate velocity and acceleration.

• Speed is how fast an object is going with respect to an object. • Velocity is a measure of the speed in a given direction. • You can say the top speed of an airplane is 300 kilometers per

hour (kph). But its velocity is 300 kph in a northeast direction.

Calculating speed or velocity• Speed= distance/ time • velocity= distance/time; directions

Calculate the following:1. Bob travels 300 km in 10 hrs towards the store.2. Ashley swims 50 m in 10 seconds.

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Acceleration: SPS 8a. Calculate velocity and acceleration.

• Acceleration is the increase of velocity over a period of time. • Deceleration is the decrease of velocity.• Acceleration = final velocity- initial velocity/ time or

a = vf- vi/ t

Change in acceleration:• Caused by a change in speed• Caused by a change in direction

Calculate the acceleration1. A train traveling 20 meters per second takes 10 seconds to stop.2. A boy gains a speed of 5 m/s after running for 20 seconds.

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Newton’s Laws of Motion: SPS 8b. Apply Newton’s 3 Laws to everyday situations by explaining the following: inertia, relationship between force, mass, and

acceleration, and equal and opposite forces.

• Newton’s 1st Law: An object at rest stays at rest, and an object in motion stays in motion, with the same direction and speed unless acted on by unbalanced force. (Also called the Law of Inertia)

• Newton’s 2nd Law: F= ma• Newton’s 3rd Law: For every action there is an

equal and opposite reaction. Forces are found in pairs.

http://www.physics4kids.com/files/motion_velocity.html

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Newton’s 1st Law

• The ladder continues to move forward even though the truck stops.

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Newton’s 2nd Law

• F= ma

• The force required to move the car is 50N.

m

F

a

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Newton’s 3rd Law

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Forces and Gravitation: SPS 8c. Relate falling objects to gravitational force.

Gravity is the force that pulls objects toward the Earth. It is affected by mass and distance. • The equation for the force of gravity is F or W = mg.

Acceleration due to gravityThe acceleration due to the force of gravity on Earth is g: 9.8 m/s2 .

WeightThe weight of an object is the measurement of the force of gravity on that object. You weigh something on a scale, according to the force that the Earth pulls it down: w = mg; where w is the weight in Newtons (N)

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Mass and Weight: SPS 8d. Explain the difference between mass and weight.

• Mass is a measure of how much matter an object has. • Weight is a measure of how strongly gravity pulls on that

matter. • Mass is constant, but the weight may change.

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Section 2: Work and Mechanical Advantage:

SPS 8e. Calculate amounts of work and mechanical advantage using simple

machines.

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Simple Machines

• Machines are devices that make work easier. • Machines do work ( W = F • d ) with just one

movement • Compound machines require more than one

movement to do work. • There are six simple machines: lever, pulley,

wheel and axle, inclined plane, wedge, and screw.

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Simple Machines• Since a machine has

parts that are in contact with other things, friction is produced. So in the real world, a machine can never be 100% efficient.

• Efficiency = Work output/ Work input x 100%

Wheel and axle

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Mechanical AdvantageSPS 8e. Calculate amounts of work and mechanical advantage using simple machines.

Formula for Force• MA =Resistance force (Fr)

Effort force (Fe)

• MA= 100kg/50 kg– MA= 2

Formula for Distance• MA = Input distance (slope)

Output distance (height) • MA= 12m/6m

MA= 2

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Section 3: Energy and Energy Transformations

SPS 7. Students will relate transformations and flow of energy within a system.

SPS 7a. Identify energy transformations within a system (e.g. lighting of a match.)

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Energy: SPS 7. Students will relate transformations and flow of energy within a system.SPS 7a. Identify energy transformations within a system (e.g. lighting of a match.)

Types of EnergyPotential energy Stored energy due to position Kinetic energy Energy of motionChemical Energy A form of potential energy and it is possessed by things such as

food, fuels and batteriesThermal Energy HeatMechanical Energy Sum of potential and kinetic energy in a systemElectromagnetic Energy

The energy source required to transmit information (in the form of waves) Some types of electromagnetic energy include: radio waves, microwaves, infrared waves, visible light, ultraviolet light, x-rays, and gamma rays. All electromagnetic forms of energy travel at the speed of light which is very fast.

Gravitational Potential energy

Energy stored within an object due to its height above the surface of the Earth.

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Energy TransformationConsuming food Chemical energy to mechanical energy

Car engine Chemical energy to mechanical energy

Light bulb Electrical energy to light and heat

Windmills Energy of the wind into mechanical energy of the blades and then into electrical energy

Solar panels Light energy from the sun into electrical energy

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3 Methods of Heat TransferSPS 7b. Investigate molecular motion as it relates to thermal energy changes in terms of conduction, convection, and radiation.

Method of heat transfer

Description Example

Conduction Heat transfer by direct contact

Burning your hand by touching a hot pan.

Convection Heat transfer through fluids (gas or liquid)

Wind currents.Heating and cooling system in our homes and buildings.

Radiation Heat transfer through open space (vacuum)

The hood of a car getting hot on a summer day.

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Conduction

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Convection

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Radiation

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Insulator vs. ConductorInsulator Conductor

Material that does not allow heat/charge to pass easily.

Material that allows heat/charge to pass easily.

Examples: wood, plastic, rubber, air, fiberglass, fleece, thermal underwear

Examples: Metals such as copper, silver, gold, aluminum

Poor conductor Poor insulator

Heat travels from a warmer material to a colder material.

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Calculating Specific HeatSPS 7c. Determine the heat capacity of a substance using

mass, specific heat, and temperature.

• The amount of energy needed to raise 1kg of a substance by 1 K

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Section 4: Waves, Electricity, and Magnetism

SPS9- Students will investigate the properties of wavesSPS10: Students will investigate the properties of electricity and magnetism.

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SPS9a. Recognize that all waves transfer energy.

• A wave is a disturbance that transfers energy through matter or through space.

• Some waves, like sound waves, must travel through matter, these waves are called mechanical waves.

• Other waves, like light do not require a medium and can travel through space. These waves are called electromagnetic waves.

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SPS9e. Relate the speed of sound to different mediums

2 Different Types of WavesMechanical Electromagnetic

• (requires a medium: solid, liquid, or gas)

• (does not require a medium/ can travel in a vacuum)

• Sound waves require air (gas)

• Radio waves

• Water waves require water (liquid)

• Infrared Light

• Earthquake (seismic waves) requires earth (solid)

• Gamma rays

.

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SPS9e. Relate the speed of sound to different mediums

Wave Speed through different mediums• Sound travels fastest in solids.• Sounds travels slowest in gases?Sound travels faster in solids because particles are closer together in solids than in gases, and therefore energy moves faster!

LiquidGas Solid

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Longitudinal vs. Transverse

• Waves can be either longitudinal (compression) or transverse.

Label the parts of the wave below.

Longitudinal

Transverse

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Relating Frequency and Wavelength: SPS 9b. Relate frequency and wavelength

to the electromagnetic waves and mechanical waves.

Frequency is how fast the wave is moving. If you stand in one spot and watch a wave go by, it is the number of crests that go by in a second.

• Waves with long wavelengths have a low frequency. Waves with short wavelengths have a high frequency. The higher the frequency, the more energy a wave has.

• The speed or velocity of a wave depends on the wavelength and the frequency. The formula for wave speed is:

• Speed = wavelength x frequency

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Frequency vs. Wavelength

• What happens to the wavelength as the frequency decreases?

• Which wave has more energy? Why?

A.

B.

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THE ELECTROMAGNETIC SPECTRUM: SPS 9c. Compare and contrast the characteristics of electromagnetic and mechanical (sound waves).

• The electromagnetic spectrum is a set of electromagnetic waves in order of wavelength and frequency. – a long wavelength has a low frequency– a short wavelength has a high frequency.

• What happens to frequency as you move from left to right? Wavelengths? Energy?

• Which wave has the longest wavelength? Shortest?• Which wave has the highest frequency? Lowest?• Which wave has the most energy? Least?• F

RabbitsMate

InVery

UnusualX-tra

Gardens

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Wave Interactions: SPS 9d. Students will investigate the phenomenon of reflection, refraction, diffraction, and

interference.

• When a wave hits a piece of matter, the wave can be absorbed or it can be reflected.

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Wave Interaction

Reflection• The bouncing back after a

wave strikes an object that it cannot pass through.

Refraction• The bending of waves due

to a change in speed.• Examples include prisms,

lenses like glasses and contacts, and a mirage.

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Wave Interaction

Diffraction

• The bending of waves around a barrier. When it encounters a barrier, the wave can go around it.

• Examples include sound waves bending to come around a corner, or underneath a door

Interference

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Doppler Effect SPS 9f. Explain the Doppler Effect in terms of everyday interactions.

• Who hears a higher pitched sound? Why?

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Electricity

Electricity & Magnetism: SPS10: Students will investigate the properties of

electricity and magnetismSPS10a. Investigate static electricity in terms of

friction, induction, and conduction.

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Static Electricity

• Static - some of the outer electrons are held very loosely.

• They can move from one atom to another. • An atom that loses electrons has more protons

than electrons. It is positively charged- cation • An atom that gains electrons has more electrons

than protons. It has a negative charge- anion. • A charged atom is called an "ion."

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Static Electricity

• Static electricity is the imbalance of positive and negative charges.

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Current Electricity:

SPS10b Explain the flow of electrons in terms of alternating and direct current;

the relationship between voltage, resistance and current; simple, series,

and parallel circuits

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Electricity

• To make "something" (refrigerator, light, computer, radio controlled car, sewing machine......) turn on we need:– an appropriate source of electricity (battery/outlet), – metal wires insulated with plastic,– a switch – and the “thing”.

• We connect them in a distinct sequence for the thing to work.

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Source of Energy

• In the case of DC (Direct Current – (battery) current flows in one direction only), it has a limited life than is unusable so we throw it away.

• -In the case of AC (alternating Current – (wall plug) current flows back and forth (changes direction)) the power company provides the electricity, it is far closer to limitless as an energy source.

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Electric Current

• The flow of electrons is called a current, an electric current

• Current flows from high to low energy. • The formula for calculating voltage is:

– V = R x I

•

R

V

I

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CircuitsSeries Circuits

• The current must flow through one device to get to the next device. This means that the rate of current flow through all devices is the same.

• 1 loop

Parallel Circuits

• In a parallel circuit each device is directly connected to the power source. This means that each device receives the same voltage.

• 2+ loops

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Series Circuit vs. Parallel CircuitsSeries

1. Has a single loop for electrons to travel round

2. Components are connected one after another

3. Current has to travel through all components

Parallel

1. Has two or more paths for electrons to flow down

2. Current is shared between the branches

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Magnetism

SPS 10c: Investigate applications of magnetism and/or its relationship to the movement of

electrical charge as it relates to electromagnets; simple motors; and permanent magnets.

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MagnetismSPS 10c: Investigate applications of magnetism and/or its relationship to the movement of electrical charge as it relates to electromagnets; simple motors; and permanent magnets.

• Magnetism is a universal force like gravity. • A magnet always has two poles - north and

south. • Like poles repel each other and opposite poles

attract.

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Temporary Magnet vs. Permanent Magnet

Temporary Magnet• Has magnetic properties for

a short time.• Ex: electromagnet

Permanent Magnet• A magnet that maintains its

magnetic properties forever.• Ex: magnetite and

lodestone

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Electromagnetism

• Electricity can produce a magnetic field and magnetism can produce an electric current.

• An electromagnet is a temporary magnet. • As long as there is a current flowing, a magnetic field is present. • A simple electromagnet consists of a

– battery,– copper wire– iron nail

• The strength of the electromagnet depends on:– the number of turns in the wire coil– and the size of the iron core– The amount of voltage.

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Electrical Machines

Motor • Converts electric energy to

mechanical energy• Ex: battery, drill

Generator• Converts mechanical energy

to electrical energy• Ex: windmill, turbine

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EOCT Review

Chemistry

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Section 5: Properties of MatterSPS2. Students will explore the nature of matter, its classifications, and its system for naming types of matter.

SPS 5. Students will compare and contrast the phases of matter as they relate to atomic and molecular motion. SPS 5a. Compare and contrast the atomic/molecular motion of solids, liquids, gases and plasmas.

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Physical Properties and Changes

Physical PropertyCharacteristic that can be

observed or measured using the 5 senses.

Physical ChangeChange in the form of

matter but not in identity.

DensityShapeColorOdor

TextureViscosity

ConductivityMalleabilityHardness

Melting and Boiling Points

Phase changes(melting, freezing)

Beating an eggStirring milkBending wire

Folding a paperCrushing sugar

DissolvingSlicing a tomato

Boiling water

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Density

• Density is a measure of the amount of mass in a certain volume.

• The heavier an object, the more dense it is.

• This physical property is often used to identify and classify substances.

• It is measured in g/cm3.

• SAMPLE PROBLEM: What is the density of a billiard ball that has a volume of 100 cm3 and a mass of 250 g?

d

m

v

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Chemical Properties and Changes

Chemical PropertyWay a substance reacts with

another substance to produce a new substance

Chemical ChangeOccurs when a substance reacts and forms one or more new substances

ReactivityFlammabilityCombustion

FermentationOxidationCorrosion

Baking a cakeMixing baking soda and

vinegarBurning a candle

Iron rustingMaking wine Milk souring

Banana ripening/rottingDigestionBreathing

Evidence of chemical

change: 1. change in color

2. production of a gas3. formation of

precipitate

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States (Phases) of Matter: SPS 5a. Compare and contrast the atomic/molecular motion of solids, liquids, gases and plasmas.

Common States of Matter

Volume Shape Molecular Attraction

Examples

Solids yes yes strong Gold, silver, carbon

Liquids yes no medium Mercury, bromine

Gases no no weak Nitrogen, hydrogen, oxyygen

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States of Matter

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Phase Change

• Label the phase changes below. Tell which reactions are endothermic and which are exothermic.

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Gas LawsFactors that affect Gas Pressure

1. Temperaturea) Increase in temperature

increases pressure.2. Volume

a) Decrease in volume increases pressure

3. Number of particlesa) Increase in the number of

particles increases pressure.

3 Gas Laws

1. Charles’s Law (pressure)2. Boyle’s Law (temperature)3. Gay- Lusaac (volume)

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Gas Laws SPS 5b. Relate temperature, pressure, and volume of gases to the behavior of gases.

Charles Law- When Pressure is constant, temperature and volume are directly proportional.

Boyle’s Law

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Boyle’s Law- When Temperature is constant, pressure and volume are inversely (opposite) proportional.

Boyle’s Law

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Gay Lusaac’s Law- When volume is constant, pressure and temperature are directly proportional.

Boyle’s Law

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Section 6: Atomic Theory and the Periodic Table

SPS1. Students will investigate our current understanding of the atom. a. Examine the structure of the atom in terms of • proton, electron, and neutron locations. • atomic mass and atomic number. • atoms with different numbers of neutrons (isotopes). • explain the relationship of the proton number to the element’s

identity. b. Compare and contrast ionic and covalent bonds in terms of electron movement.

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Structure of the Atom

SPS1. Students will investigate our current understanding of the atom..

• All matter is made up of atoms.

Subatomic Particle Charge Location Size

Proton (p+) 1+ Nucleus Equal to size of neutron

Neutron (n) 0 Nucleus Equal to size of proton

Electron (e-) 1- Outside nucleus Smallest subatomic particle

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SPS1. Students will investigate our current understanding of the atom. a. Examine the structure of the atom in terms of proton, electron, and neutron locations.

• Protons (+) equals Electrons (-)• charge) and protons (+ charge) to make the atom

electrically neutral.

Protons(+) Electrons (-)

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a. Examine the structure of the atom in terms of atomic mass and atomic number.

• The atomic number of an element is what distinguishes it from all other elements.

• The atomic number is the number of protons there are in the nucleus.

• Hydrogen's atomic number is 1. • Helium's atomic number is 2.

1

H

Hydrogen

1.0079

2

He

Helium

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Atomic NumberAtomic Number

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a. Examine the structure of the atom in terms of atomic mass and atomic number.

• The mass number is the number of neutrons added to the number of protons.

• In other words, the total number of particles in the nucleus.

Mass Number

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SPS1. Students will investigate our current understanding of the atom. -atoms with different numbers of neutrons (isotopes).

• Isotopes are atoms of the same element that have different numbers of neutrons and different mass numbers.

• To distinguish one isotope from another, the isotopes are referred by their mass numbers.

hydrogen

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Section 7: Periodic TableSPS4. Students will investigate the arrangement

of the Periodic Table.

a. Determine the trends of the following:• Number of valence electrons• Location of metals, nonmetals, and metalloids• Phases at room temperature

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Periodic Table

• The Periodic Table is organized into– Rows (periods)– Columns (groups)

Each row in the table of elements is a period.• Elements in period 1 have one energy level.• Elements in period 2 have two energy levels.• Elements in period 3 have three energy levels.• Elements in period 4 have four energy levels.• Elements in period 5 have five energy levels.• Elements in period 6 have six energy levels.• Elements in period 7 have seven energy levels.

Periods- Total of 7

Horizontally Into Periods

Groups Each column in the periodic table is called a group.

• The elements in a group have the same number of valence electrons.

• Therefore members of a group in the periodic table have similar chemical properties.

There are 18 GROUPS Vertically into Groups

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• Elements in group 1 have one valence electron.• Elements in group 2 have two valence electrons.• Elements in group 13 have three valence electrons.• Elements in group 14 have four valence electrons.• Elements in group 15 have five valence electrons.• Elements in group 16 have six valence electrons.• Elements in group 17 have seven valence electrons.• Elements in group 18 have eight valence electrons;

except Helium (2).

Vertically into Groups

The Periodic Law

Atomic Mass UnitsThe mass of an atom in grams is extremely small. In order to have a convenient way to compare the masses of atoms, scientists chose one isotope to serve as a standard.

• Scientists assigned 12 atomic mass units to the carbon-12 atom, which has 6 protons and 6 neutrons.

• An atomic mass unit (amu) is defined as one twelfth the mass of a carbon-12 atom.

Atomic Mass

There are four pieces of information for each element.

Atomic Mass

1. Atomic number

2. Element symbol

3. Element name

4. Atomic mass

What categories are used to classify elements on the periodic table?

Classes of Elements

Elements are classified as metals, nonmetals, and metalloids.

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• Elements to the left of the blue stair case line are metals.

• Elements to the right of the staircase line are nonmetals

• Elements along the staircase line are metalloids/semi-conductors.

MetalsThe majority of the elements on the periodic table are classified as metals. Metals are elements that are good conductors of electric current and heat.

• Except for mercury (liquid), metals are solids at room temperature.

• Most metals are malleable. • Many metals are ductile; that is, they can be drawn

into thin wires.

Classes of Elements

The metals in groups 3 through 12 are called transition metals. Transition metals are elements that form a bridge between the elements on the left and right sides of the table.

• Transition elements, such as copper and silver, were among the first elements discovered.

• One property of many transition metals is their ability to form compounds with distinctive colors.

Classes of Elements

NonmetalsNonmetals generally have properties opposite to those of metals.

• Nonmetals are elements that are poor conductors of heat and electric current.

• Nonmetals have low boiling points–many nonmetals are gases at room temperature.

• Nonmetals that are solids at room temperature tend to be brittle. If they are hit with a hammer, they shatter or crumble.

Classes of Elements

MetalloidsMetalloid elements are located on the periodic table between metals and nonmetals.

• Metalloids are elements with properties that fall between those of metals and nonmetals.

• For example, a metalloid’s ability to conduct electric current varies with temperature. Silicon (Si) and germanium (Ge) are good insulators at low temperatures and good conductors at high temperatures.

Classes of Elements

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Group Names

• Some groups have specific names– Group 1- alkali metals (most reactive metals)– Group 2- alkaline earth metals– Groups 3-12- transition metals– Group 17- halogens (most reactive nonmetals)– Group 18- noble gases (unreactive)

• Group 1 and Group 17 are the most reactive elements.

• Group 18, the noble gases, are unreactive.

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