Physical Science

Sidney Brandon Foster Mr. Adam Reinhart Clover High School

Spring 2011

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Table of Contents

Unit I Scientific Method Page 17 Hypothesis Page 18 Independent (Manipulated) Variable Page 18 Dependent Variable Page 18 Controlled Variable Page 18 DRY MIX Page 18 Metric System Page 18

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Table of Contents (Continued)

Unit II Protons Page 19 Neutrons Page 19 Electrons Page 19 Atomic Symbol Page 20 Atomic Number Page 20 Atomic Mass Page 20 Periods Page 21 Groups Page 21 Metal vs. Nonmetal vs. Metalloid Page 22 Ion Page 23

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Table of Contents (Continued)

Unit II Oxidation Number Page 23 Ion Symbol Page 23 Isotope Page 23 Isotope Symbol Page 23 Fission Page 24 Fusion Page 24

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Table of Contents (Continued)

Unit III Atom vs. Element Page 25 Compound vs. Molecule Page 25 Inorganic vs. Organic Compounds Page 25 Heterogeneous vs. Homogeneous Mixtures Page 25 Kinetic Theory Page 26 Solid vs. Liquid vs. Gas vs. Plasma Page 26 State Change Graph Page 27 Chemical Properties Page 28 Physical Properties Page 28 Increasing Rate of Solubility Page 28

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Table of Contents (Continued)

Unit III Acid and Bases Page 29 Neutralization Reaction Page 29

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Table of Contents (Continued)

Unit IV Ionic Bonds Page 30 Crystal Lattice Page 30 Writing Compounds Page 32 Naming Compounds Page 32 Covalent Bond Page 30 Synthesis Reaction Page 31 Decomposition Page 31 Single Replacement Reaction Page 31 Double Replacement Reaction Page 31 Increasing Rate of Reaction Page 33

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Table of Contents (Continued)

Unit IV Physical Change Page 33 Chemical Change Page 33 Endothermic Reaction Page 33 Exothermic Reaction Page 33 Law of Conservation of Mass Page 34 Balancing Chemical Equations Page 34

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Table of Contents (Continued)

Unit V Speed Page 35 Velocity Page 35 Instantaneous Velocity Page 35 Average Velocity Page 35 Graphing Velocity Page 35 Acceleration Page 35 Force Page 36 Newton's First, Second and Third Laws Page 36 Inertia Page 36

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Table of Contents (Continued)

Unit VI Energy Page 37 Law of Conservation of Energy Page 37 Potential Energy Page 37 Kinetic Energy Page 37 Roller Coasters Page 37 Pendulums Page 37 Energy Transformations Page 37 Work Page 37

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Table of Contents (Continued)

Unit VII Static Electricity Page 38 Friction Page 39 Induction Page 39 Lightning Page 38 Conduction Page 39 Ohm’s Law Page 38 Voltage Page 39 Resistance Page 39 Current Page 39 Alternating Current Page 40

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Table of Contents (Continued)

Unit VII Direct Current Page 40 Circuit Diagrams and Symbols Page 42 Closed vs. Open Circuits Page 40 Series Circuits Page 41 Parallel Circuits Page 41 Electromagnets Page 41 Electric Motors Page 41 Generators Page 41

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Table of Contents (Continued)

Unit VIII Mechanical Wave Page 44 Transverse Wave Page 44 Longitudinal Wave Page 44 Electromagnetic Wave Page 44 Amplitude Page 43 Wavelength Page 43 Frequency Page 43 Period Page 43 Wave Speed Page 45 Reflection Page 45

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Table of Contents (Continued)

Unit VIII Refraction Page 45 Diffraction Page 45 Constructive Interference Page 46 Destructive Interference Page 46 Sound Waves Page 47 Pitch Page 47 Echo Page 47 Doppler Effect Page 47

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Scientific Method A formal procedure in which the researcher can acquire new knowledge in an organized fashion.

Principles and procedures for the systematic pursuit of knowledge in-volving the recognition and formula-tion of a problem, the collection of data through observation and experi-ment, and the formulation and testing of hypotheses.

scientific method noun

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Dependent Variable What you measure in the experiment and what is affected during the experiment. The dependent variable responds to the independent variable.

Hypothesis A educated guess.

Independent Variable The variable in an experiment

Controlled Variable A variable which is not allowed to change

D-Dependent R-Responding Y-Y Axis M-Manipulated I-Independent X-X Axis

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Protons Protons are positively charged particles found within atomic nuclei.

Neutrons

Neutrons are uncharged particles found within atomic nuclei.

Electron

Electrons are negatively charged particles that surround the atom's nucleus.

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Atomic Number The amount of protons and

electrons in an atom. Atomic Symbol

A one or two letter interna-tionally agreed code for an

element.

Atomic Symbol

Atomic Mass The atomic mass is

the total mass of protons, neutrons

and electrons in a single atom.

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Rows of elements are called periods. The number of energy levels is equal to the period number.

Columns of elements are called groups. The number of valence electrons are equal to the group number.

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Characteristics of a metal: x� shiny x� good conductors of thermal

energy and electric current x� malleable x� ductile

Characteristics of a Nonmetal: x� has dullness x� poor conductors of

thermal energy and electric current

x� brittle

Characteristics of a Metalloid: x� has properties of both metals and

nonmetals

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Ion An ion is an atom or molecule in which the total number of electrons is not equal to the total number of protons.

Oxidation Number An oxidation number is a positive or negative number that indicates how many electrons an atom has gained, lost, or shared to become stable.

Isotope Isotopes are variants of atoms of a particular chemical element, which have differing numbers of neutrons.

Ion Example Fe2+

(Iron Atom that lost Electron)

Isotope Example Carbon-13

(Carbon Atom with the atomic mass of 13)

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Atom vs. Element Elements are made of multiple identical atoms.

Compound vs. Molecule Molecules are formed when two or more of the same atom combine while compounds are created with different types of elements.

Inorganic vs. Organic Compounds The difference between Inorganic and Organic Compounds are that Organic compounds have at least one carbon atom.

Heterogeneous vs. Homogeneous Mixture The difference between Heterogeneous and Homogeneous Mixtures is that in heterogene-ous mixtures, the scientist can see that the mixture is not evenly distributed.

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Kinetic Theory Kinetic Theory states that as the temperature of an atom increases, the atom will have more ki-netic energy.

Solid vs. Liquid vs. Gas vs. Plasma

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State Change Graph

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Chemical Properties A chemical property is any of a material's properties that becomes evident during a chemical reaction.

For an example:

Oxidation, Combustibility and Corrosion are all signs of chemical properties.

Physical Properties Physical properties can be observed or measured with-out changing the composition of matter. Examples: State, Viscosity, Conductivity, Density, Solubility.

Increasing Rate of Solubility Ways to increase the rate of solubility of a mixture are by increasing the surface area, temperature and by stirring the mixture.

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Acids and Bases Acid: A solution that has an ex-cess of H+ ions. It comes from the Latin word acidus that means "sharp" or "sour". Lemons. 6-0 on Ph scale. Sticky to touch. Base: A solution that has an ex-cess of OH- ions. Another word for base is alkali. Ammonia. 8-14 on Ph scale. Slippery to touch.

Neutralization Reaction

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Crystal Lattice

Covalent & Ionic Bond

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Types of Chemical Reactions x� Synthesis-two or more simple substances combine to form a more complex substance.

x� Decomposition-a more complex substance breaks down into its more simple parts.

x� Single Replacement-when one element trades places with another element. x� Double Replacement-when two elements switch places with two others.

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Increasing Rate of Reaction A scientist can increase the rate of a reaction by: x� Increasing the surface area x� Increasing the temperature x� Adding a catalyst

Physical Change When a physical change occurs the compound is not altered.

Chemical Change When a chemical change occurs a new substance is created. Odor, gas, color change, temperature change and precipitation are indicators.

Endothermic Reaction A reaction that absorbs heat.

Exothermic Reaction A chemical reaction that releases energy in the form of light or heat.

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Law of Conservation of Mass

The Law of Conservation of Mass states that mass must remain constant throughout a reaction.

Balancing Chemical Equations The product of a reaction must have the same amount of atoms as before the reaction took place. Therefore, scientist use coefficients to balance equations.

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Velocity Velocity is speed with a direction.

Speed The formula for speed is S=Distance/Time. Speed is

usually measured in meters per second.

Instantaneous Velocity Instantaneous speed is comparable to what a speedometer in a car

Average Velocity Average velocity is just net distance traveled divided by

time.

Acceleration Acceleration is the rate of

increase in velocity.

a = 'v / 't

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Force Force=Mass×Acceleration

The ability to move.

Inertia Inertia is the resistance of any physical object to a change in its

state of motion or rest, or the tendency of an object to resist any change in its motion

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Energy The ability to do work. Measured in Joules.

Law of Conservation of Energy States that energy cannot be either created

nor destroyed.

Potential Energy Stored energy.

Kinetic Energy Possessed energy while an object is in motion.

Work Work=Force×Distance

Energy Transformations Energy transformation is the process of energy

changing from one form to another.

Roller Coasters and Pendulums Both roller coasters and pendulums experience energy transformations. It

switches back and forth between kinetic energy and potential energy.

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Static Electricity Static Electricity is the build up

of excess electrons.

Lightning The discharge of electrons

Ohm’s  Law

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Mechanical Wave A disturbance that moves

through a medium.

Longitudinal Wave

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Wave Speed Wave Speed=Distance/Time

Reflection When Light is reflected, the angle

it hits the object is the same on both sides of the normal

Refraction When light enters a new medium, the ray angle

changes.

Diffraction– waves are able to bend around corners.

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Sound Waves Mechanical waves that require medium to travel.

Pitch Highness or lowness of sound characterized by the frequency

Echo The bouncing of sound waves against objects that create a

Doppler Effect Occurs when moving car

passes you.