2.01 motion physical science eoc review. motion motion – a change of position. all motion is...

2.01 Motion

Physical Science EOC Review

Motion

• Motion – a change of position.• All motion is relative – Point of Reference

Reference point – A place or object used for comparison to determine if an object is in motion.

Distance vs. Displacement

• Distance is how far an object has traveled during its motion.

• Displacement is a how far an object is from where it started.

Speed vs. Velocity

• Speed is "how fast an object is moving."

• Velocity is Speed… except velocity includes direction.Velocity is "the rate at which an object changes its position."

Average vs. Instantaneous Speed

• Average Speed is the average over an entire trip.

• Instantaneous Speed is the speed at one instant…

Instantaneous speed is what your speedometer reads.

Average vs. Instantaneous Speed

Motion

• Using graphical analysis, solve for distance, time, and average velocity.

Unit: m/stdv

Motion

• Using graphical analysis, solve for distance, time, and average velocity. Also analyze conceptual trends in the distance vs. time graphs such as constant velocity and acceleration.

Speed (Velocity) Acceleration

Accelerated Motion

• Investigate how acceleration is a relationship between velocity and time:

Unit: m/s/s tvv

tva if

Accelerated Motion

• Investigate how acceleration is a relationship between velocity and time:

Accelerated Motion

• Using graphical analysis, solve for velocity, time, and average acceleration.

Accelerated Motion

• Using graphical analysis, solve for velocity, time, and average acceleration. Also analyze conceptual trends in the velocity vs. time graphs such as constant velocity and acceleration.

Constant Speed(straight lines)

Accelerated Speed(curved line)

Accelerated Motion

• Investigate acceleration due to gravity as an example of uniformly changing velocity: g = 9.8m/s/s.

2.02 Force


Weight vs. Mass

• Weight is different from mass – Mass is how much matter makes up an object– Weight includes the force of acceleration due

to gravity and mass of an object:.

2.02 Force

• Mathematically and graphically analyze weight as the relationship between the acceleration due to gravity and mass of an object:

Unit: Newton

mgFg

2.02 Force

• Investigate force mathematically and graphically with respect to acceleration as a change in motion.

Unit: Newton

F ma

2.02 Force

• Investigate balanced and unbalanced forces using the equation: . Unit: Newton

F ma

Force

• A force is a push or a pull– Balanced Forces

– Unbalanced Forces

Inertia

• Inertia is related to mass.– Which would have more inertia… a bowling

ball, or a volley ball of the same size? (Which one would roll the farthest?)

Newton’s Three Laws of Motion

1. Law of Inertia: – An object in motion will stay in motion and– An object at rest will stay at rest unless– A force acts on it

2. F = ma3. For every Action there is an equal and

opposite Reaction.

2.02 Force

• Analyze Newton’s Third Law as the relationship described by

Force of Object A on Object B = Force of Object B on Object A

2.02 Force

• Investigate friction as force that opposes the motion of an object.

Friction

• Friction is a force that opposes the motion of an object.– Static Friction– Sliding Friction

– Rolling Friction

– Fluid Friction

3.01 Energy


Energy

• Types of Energy:– Kinetic Energy – The energy of Motion– Thermal Energy – Heat Energy – Related to

Kinetic Energy (Movement of Molecules)– Potential Energy – The energy of Position

• Elastic Potential Energy– Chemical Energy – Energy stored in chemical

bonds – Related to Potential Energy– Nuclear Energy – Energy in the atom’s nucleus– Electric Energy

Energy

• Law of Conservation of Energy: – Energy is neither created nor destroyed– One type of energy can be converted into

another type of energy

Energy

• Potential Energy can be converted to Kinetic Energy… and back to PE!– Example: Roller Coaster

– Example Pendulum

Energy

Electric Energy can be formed by Kinetic Energy:

Energy

Electric Energy can be formed by Potential Energy:

Energy

Kinetic Energy can be formed by Chemical Energy:

Gasoline Engine

Energy

Kinetic Energy can be formed by Electrical Energy:

Energy

Thermal Energy can be formed by Nuclear Energy:

Energy

Sometimes, Thermal Energy is a form of waste energy:

Energy

• Calculate kinetic energy:

Unit: Joule (J)

KE mv12

2

Energy

• Predict change in kinetic energy when mass or velocity change.

Unit: Joule (J)

KE mv12

2

Energy

• Calculate gravitational potential energy:

Unit: Joule (J)

hFmghPE g

Energy

• Predict change in gravitational potential energy when mass or height change.

Unit: Joule (J)

hFmghPE g

Energy

• Use conceptual analysis to investigate the characteristics of a substance-such as mass, specific heat capacity, and temperature-that affect its ability to absorb or release thermal energy.

3.02 Work and Power


Work

• Work • In order for work to be done by a force, the

force must be in the direction of movement. No movement… No Work!

• Calculate work:Unit: Joule (Newton ● Meter)

W F d

Power

• Power • Power is the rate of doing work.• Calculate power:

Unit: Watt

WP t

3.03 Thermal Energy


Heat Energy

• Differentiate among conduction, convection, and radiation energy transfers.

List the examples of conduction, convection and radiation shown in the picture.

Heat Energy

• Investigate the interaction between substances of different temperatures.

Heat Energy

• Explain why no machine can be 100% efficient.

What is being lost? Energy

Heat Energy


Why is energy being lost? Friction

Heat Energy


What do the arrows represent?

Waste Energy lost because of Friction

Heat Energy


No machine is 100 percent efficient because energy is always lost due to heat or friction.

Heat Energy

• Differentiate between heat and temperature.

Heat Energy

• Temperature is the measure of the average kinetic energy of the molecules of a substance.(Units: ºC, ºF, Kelvin)

Heat Energy

• Heat is the kinetic energy of the moleculesUnits: Joules

Heat Energy

• Convection currents investigation: by adding drops of food coloring to warm and cold water.

DemonstrationWhat you need:

Two clear containers, about the same size 2 dark colors of food coloring Warm and cold water

What to do:1. Put the two containers next to each other. Pour cold

water into one container until it is about ¾ of the way full. Then pour warm water in the other one up to the same level.

2. Take a dropper of food coloring in each hand and add two drops of food coloring to each glass at the same time.

3. Watch how the food coloring spreads through the containers. Which glass does it spread through faster?

3.04 Waves


Transverse Wave

• Identify the basic characteristics of a transverse wave: trough, crest, amplitude, and wavelength.

Trough

Crest

Amplitude

Wavelength

TransverseWave

Compressional Wave

• Identify the basic characteristics of a longitudinal (compressional) wave: amplitude, rarefaction, and compression.

Rarefaction (where lines are spaced farther apart)

Compression

CompressionalWave

Waves

• Explore the differences between compression and transverse waves.

Period and Frequency

• Recognize the relationship between period and frequency. Conceptual understanding of inverse relationship.

1 second

Period = 1 cycle = 1/3 second

Frequency = 3 cycles per second = 3 Hz

Wave Problems

• Use the relationships among velocity, frequency, and wavelength to solve wave problems:

Unit: m/s

fvw Wave speed = frequency x wavelength

Wave Energy

• Understand that a wave's energy is related to its amplitude.

Sound

• Investigate how the velocity of a sound wave varies through different mediums.

Electromagnetic Spectrum

• Interpret the electromagnetic spectrum (use reference tables) to determine relationships among energy, frequency, and wavelength.

Electromagnetic Spectrum

• Relate wave energies to possible health risks.

Electricity


4.01 Static Electricity

• Investigate and analyze the transfer of electrons to charge objects.

Electroscope charged by Induction

++++

+

-

----

Electroscope charged by Conduction

-

----

-

----


• Investigate and analyze the transfer of electrons to charge objects.

-

-

-

-

-

- -- -

- -

--

-- -- - -

- - -- -- - --


• Demonstrate that opposite charges attract and like charges repel.

Both are neutral

“Opposites” attract

“Like Charges” repel

“Like Charges” repel


• Compare and contrast the three methods of charging objects:


• Conduction – by touching.

Electroscope charged by Conduction

-

--

--

-

---

-


• Friction – by rubbing.


• Induction – without touching.

Electroscope charged by Induction

+ ++

+

+

-

--

--

4.02 Circuits

• Interpret simple circuit diagrams using symbols.

4.02 Circuits

• Investigate open and closed circuits.

4.02 Circuits

• Apply Ohm’s Law and the power equation to simple DC circuits: and V IRP VI

4.02 Circuits

• Distinguish between series and parallel circuits.

4.02 Circuits

• Conceptually explore the flow of electricity in series and parallel circuits.

4.02 Circuits

• Explain how the flow of electricity through series and parallel circuits is affected by voltage and resistance.

Units:V – VoltI – AmpR - Ohm

V IR

4.03 Magnetism

• Describe the characteristics and behaviors of magnetic domains.

4.03 Magnetism

• Investigate the attraction of unlike poles and the repulsion of like poles.

4.03 Magnetism

• Magnetic Field Lines

4.03 Magnetism

• Investigate the strength of an electromagnet by varying the number of coils, varying current, or core material.

4.03 Magnetism

• Develop an understanding of the relationship between electricity and magnetism in practical applications such as generators and motors.

Chemistry


5.01 Atomic Theory

• Illustrate how observations and conclusions from experimentation changed atomic theory over time.

5.01 Atomic Theory

• Explain Dalton’s atomic theory, which states the following:– Chemical elements are made up of atoms.– The atoms of an element are identical in their

masses. (This was shown to be false with the discovery of isotopes.)

– Atoms of different elements have different masses.

– Atoms only combine in small, whole number ratios such as 1:1, 1:2, 2:3 and so on.

5.01 Atomic Theory

• Explain and illustrate J. J. Thomson’s plum pudding model.

5.01 Atomic Theory

• Explain Rutherford’s gold foil experimental conclusions. The atom is mainly empty space with a dense positively charged center.

5.01 Atomic Theory

• Explain Bohr’s model. Show how electrons are arranged in energy levels. Illustrate models with electrons in energy orbits.

5.01 Atomic Theory

• Describe the electron cloud model and identify the number of electrons in each level (2n2), focusing on the following levels: 2, 8, 18, and 32.

5.02 Atomic Structure

• Describe the charge, relative mass, and the location of protons, electrons, and neutrons within an atom.

Proton: +1 Charge / 1 amuNeutron: no Charge / 1 amu

Electron: -1 Charge / amu20001

Nucleus:

Around Nucleus:


• Calculate the number of protons, neutrons, electrons, and mass number in neutral atoms and ions.

Atomic Number

Atomic Mass

Number of ProtonsNumber of Electrons

Number of Protons + Neutrons

# p+ = 11# e- = 11

# p+ + # n0 = 23# n0 = 23 – 11# n0 = 12


• Explain how the different mass numbers of isotopes contributes to the average atomic mass for a given element.

Average Atomic Mass – the average of all the isotopes of Hydrogen found in nature


• Write the symbols for various isotopes examples:Carbon-12Carbon-14

Hydrogen-1Hydrogen-2Hydrogen-3

C126

C146

H11H21H31

C-12C-14

H-1H-2H-3

in


• Draw Bohr models from hydrogen to argon including common isotopes.

H11H21H31

neutron in the nucleus

5.03 Physical Properties

• Define and explain physical properties.• Physical properties can be tested without

changing what the substance is.• Physical changes are reversible.

Examples:An iron rod is magnetized.Water is frozen.


• Calculate the density of different substances (solids, liquids, and gases)

D mV


• Recognize that phase changes are physical changes.


• Investigate phase changes.– Graph, label and analyze heating/cooling

curves for various substances.


• Determine the identity of various substances by comparing properties with known substances.

6.01 Periodic Trends• Define group (family) and period.• Locate the following on the periodic table: alkali metals,

alkaline earth metals, transition metals, halogens, noble gases, metals, nonmetals, metalloids.

• Compare and contrast the physical and chemical properties of metals, nonmetals, and metalloids. (Properties should include but not be limited to reactivity, physical state, melting and boiling point, ductility, malleability, conductivity, and luster.)

• Analyze the periodic trend for atomic radius (left to right and top to bottom on periodic table).

6.01 Periodic Trends

• Define group (family) and period.


• Locate the following on the periodic table: alkali metals, alkaline earth metals, transition metals, halogens, noble gases, metals, nonmetals, metalloids.

Metals / Nonmetals

Transition Metals

Alkali Metals

Alkaline Earth Metals

Halogens

Noble Gases


• Compare and contrast the physical and chemical properties of metals, nonmetals, and metalloids. (Properties should include but not be limited to reactivity, physical state, melting and boiling point, ductility, malleability, conductivity, and luster.)


• Metals– Normally Solids– High Melting Points– High Boiling Points– Good Conductors of heat and electricity– Durable– Malleable– Ductile– Metallic Luster (shiny)


• Non-Metals– Normally Solids– High Melting Points– High Boiling Points– Poor Conductors of heat and electricity– Brittle– Non-metallic luster (dull)


• Metalloids– Characteristics of both metallic and non-

metallic elements


• Analyze the periodic trend for atomic radius (left to right and top to bottom on periodic table).

6.02 Forming and Naming Compounds

• Describe how ions form


• Describe how ionic, covalent, and metallic bonds form and provide examples of substances that exhibit each type of bonding.


• Represent elements, ions, and simple compounds with electron dot diagrams.


• Predict an element’s oxidation number based on its position in the periodic table and valence electrons, excluding the transition elements.


• Name and write formulas for simple binary compounds.


• Name and write formulas of compounds using polyatomic ions given in the reference table.

6.03 Chemical Reactions

• Identify the reactants and products of a simple chemical equation.

Reactant + Reactant → Product


• Use coefficients to balance simple chemical equations.

H2 + Cl2 HCl


• Use coefficients to balance simple chemical equations.

H2 + Cl2 2 HCl


• Recognize that chemical equations must be balanced because of the law of conservation of matter.

CaCl2 + Na2SO4 → CaSO4 + NaClCaCl2 + Na2SO4 → CaSO4 + 2 NaCl


• Classify chemical reactions as one of four types: single replacement, double replacement, decomposition, and synthesis. (Neutralization reaction is a type of double replacement reaction.)

A + B → AB SynthesisAB → A + B DecompositionA + BC → AC + B Single ReplacementAB + CD → AD + CB Double Replacement

6.04 Indicators of Chemical Change

• Observe a process and describe the indicator(s) of chemical change it exhibits.


• Differentiate between exothermic and endothermic reactions.


• (Color change is sometimes an indicator of chemical change-sometimes physical-discuss examples.)

6.05 Solutions

• Give examples of solutions containing solutes and solvents of various phases such as alloys and carbonated drinks.

6.05 Solutions

• Explain the polar nature of water (The phrase “like dissolves like” is often used to explain why substance dissolves another which is an over simplification of the process).

6.05 Solutions

• Investigate the factors that affect the rate of solution of a solid including concentration, stirring, temperature, and surface area.

6.05 Solutions

• Compare and contrast electrical conductivity of solutions containing ionic and covalent solutes.

6.05 Solutions

• Interpret the solubility curves for solids (concentration vs temperature). Investigate various concentrations unsaturated through supersaturated.

6.05 Solutions

• Conduct an experiment to illustrate trends in solubility.

6.05 Solutions

• Identify the acid, base, and salt in a neutralization reaction. (See 6.03)

6.05 Solutions

• Compare and contrast the physical and chemical characteristics of acids, bases, and neutral substances.

6.05 Solutions

• Develop an understanding of the concentration of ions in the organization of the pH scale.

6.05 Solutions

• Investigate the pH of various substances using various indicators: litmus paper, phenolphthalein, and pH paper.

Radioactivity

• Compare and contrast the characteristics of alpha and beta particles and gamma rays.

Radioactivity

• Compare and contrast the alpha, beta, and gamma decay processes.

Radioactivity

• Compare and contrast the processes of fission and fusion.

Radioactivity

• Describe various means of dealing with nuclear waste over time.

Figure 6. Air-source heat pump in cooling mode.

Figure 7. Air-source heat pump in heating mode.

2.01 motion physical science eoc review. motion motion – a change of position. all motion is...

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