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76 Cards in this Set
- Front
- Back
Scientific Method
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1. Make observations
2. Develop hypothesis 3. Test hypothesis to prove or disprove |
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Exact Measurement
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Counted or defined
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Measurement number
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A number with attached Units. An instrument must be used to obtain a measurement, so some error or uncertainty is involved.
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Mass
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Measure of the amount of matter an object possesses; usually reported in grams
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Volume
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amount of space occupied by a substance. Usually measure in Liters
1 mL=1 cm3 |
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English Volume Relationships
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1 gallon=4 quarts
1 quarts=2 pints 1 pint=2 cups |
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Guidelines for Significant Digits
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1. Non-Zero numbers are always significant
2. Zeros between numbers are significant 3. Place holder zeros are not significant Zeros at the end of a number and after a decimal point are significant |
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Metric system
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A decimal system of measurements that uses the following basic units.
meter, gram, Liter, second |
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Metric Prefixes
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Kilo= 3
Deci=-1 Centi=-2 mili=-3 |
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Volume Conversions
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1 mL=1 cm3= 1 cc
1 L= 1000 mL= 1000 cm3 |
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Volume by Caculation
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Volume= Length x width x thickness
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Volume by Displacement
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The volume of an object can be measure by adding the object to a container holding water and finding the difference between the two water levels.
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Density Concept
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The amount of mass in a unit volume of Matter
Density= Mass/Volume Units: g/cm3 or g/ mL or g/L Density of Water 1.00 g/cm3 |
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Temperature
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Measure of the average energy of a single particle in a system.
Hotness or coolness of a substance is determined by the average energy of the molecules in a system. Hot molecules move master and have higher energy. |
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Boiling and Freezing point of water for 3 temperature scales
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F=212 boiling, 32 Freezing
C=100 boiling, 0 Freezing K= 373 boiling, 273 Freezing |
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Heat
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Measure of total energy of all particles in a system
Heat transfers from a system at a higher temperature to one at a lower temperature. Heat always transfers from a hotter to the cooler object. |
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Specific heat
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The amount of heat needed to raise the temperature of 1 gram of a substance by 1 degree C.
The higher the specific heat of a substance, the more heat it can absorb before its temperature begins to raise. |
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Matter
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Anything that has Mass and Occupies space.
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Gas
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Particles are far apart and are in constant random motion.
Gases assume the shape of the container. If volume increases, particles move apart to fill entire container. If volume decreases, particles move closer together. |
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Liquid
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Particles are close together but are free to move past one another.
Liquid assume the shape of the container. Volume is constant. |
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Solid
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Particles are packed tightly together; these particles vibrate but remain in their place. Solids have a definite, fixed shape. Volume is constant.
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Four changes in physical state
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Condensing-gas to liquid
Vaporizing-liquid to gas Deposition-gas to Solid Sublimination- solid to gas |
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Pure Substance
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consist of a single chemical with a fixed composition and distinct properties.
Two types of pure substances:element and compound |
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element
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consist of only one type of atom
a substance that cannot be broken down further by chemical reaction |
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compound
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consist of two or more element and has a specific formula
a substance that can be chemically separated into its elements |
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Mixture
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Consist of two or more compounds, but has no specific formula.
has variable composition with definite or varying properties. |
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Metals
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shiny appearance
malleable, ductile density-usually high good conductors of heat and electricity |
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Nonmetals
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dull appearance
brittle density-usually low poor conductors. |
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Semimetals
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have properties intermediate between metals and nonmetals.
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Normal Physical State of Elements
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Mercury and Bromine are liquids
H2, N2, F2, O2, Cl2, and all Noble Gases are gases. All other elements are solids |
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Diatomic Molecules
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H2, N2, F2, O2, I2, Cl2, Br2
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Law of Definite Composition
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Compounds always contain the same elements in the same proportion by mass
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Physical Properties
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physical state (solid, liquid, gas)
color density melting and boiling points solubility hardness odor electrical and heat conductivity |
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Chemical Properties
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Describes have a substance reacts with other substances
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Physical Change
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A process that does not alter the chemical composition of the substance
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Chemical Change
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A process that changes the chemical composition of the substance
Burning or rusting, fizzing, precipitation, release of heat or light, change in color or odor. |
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Law of conservation of Mass
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matter is neither created nor destroyed in a chemical reaction.
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Kinetic energy
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Energy resulting from motion
As temperature increases, the particles move faster |
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Potential Energy
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stored energy that matter possesses due to its position or its chemical bonds.
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H
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Hydrogen
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He
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Helium
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Li
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Lithium
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Be
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Beryllium
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B
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Boron
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C
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Carbon
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N
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Nitrogen
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O
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Oxygen
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F
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Fluorine
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Ne
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Neon
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Na
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Sodium
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Mg
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Magnesium
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Al
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Aluminum
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Si
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Silicon
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P
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Phosphorus
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S
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Sulfur
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Cl
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Chlorine
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Ar
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Argon
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K
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Potassium
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Ca
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Calcium
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Sc
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Scandium
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Ti
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Titanium
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Mn
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Manganese
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Fe
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Iron
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Co
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Cobalt
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Ni
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Nickel
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Cu
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Copper
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Zn
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Ainc
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Br
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Bromine
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Ag
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Silver
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Sn
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Tin
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I
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Iodine
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Ba
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Barium
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Au
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Gold
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Hg
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Mercury
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Pb
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Lead
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Bi
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Bismuth
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