Chemistry Comp – Flashcards

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Atom
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The smallest particle of life. Something cannot be broken down anymore from this point.
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Element
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One specific type of atom. Listed on periodic table.
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Mixture
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When two or more different atoms are combined but can still be separated.
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Compound
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When two or more different atoms are combined but can only be broken down with chemical reactions.
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Ionic Compound
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When atoms are held together by lost or gained electrons.
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Covalent Compound
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When atoms are held together by shared electrons.
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Homogeneous Mixture
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When the percent composition of each object in the mixture is the same.
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Heterogeneous Mixture
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When the percent composition of each object in the mixture is different.
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Proton
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Plus one charge. Subatomic particle. Located in the nucleus. Relative mass of one.
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Neutron
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No charge. Subatomic particle. Located in the nucleus. Relative mass of one. Can be lost or gained to form isotopes.
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Electron
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Minus one charge. Subatomic particle. Located in the electron cloud. Relative mass of zero. Can be gained or lost to form ions. Discovered in Milikan's Oil Drop experiment.
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Chemical Change
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When the chemical composition of an object is changes through a chemical reaction. (Ex: burning a log)
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Chemical Property
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Having to do with the chemical composition of objects.
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Physical Change
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When the chemical composition of an object remains the same but the object may look different. (Ex: shredding paper)
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Physical Property
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Having to do with the appearance of objects.
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Volume
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How much space something has inside.
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Mass
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How much matter an object has.
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Isotopes
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When the number of neutrons has changed. results in a different mass number.
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Ions
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When electrons are gained or lost. Either anion or cation. Have charge.
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Mole
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Unit for amount of substance. Count of the total number of particles in an atom.
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Cation
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When electrons are lost. Positive.
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Anion
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When electrons are gained. Negative.
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Robert Milikan
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Conducted Oil Drop experiment. Found the size of the electron's mass and charge.
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J.J. Thomson
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Conducted Cathode Ray Tube experiment. Plum Pudding model. Found that subatomic particles exist and mass to charge ratio of electrons.
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Dmitri Mendeleev
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Created earliest periodic table. Ordered elements by atomic mass.
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John Dalton
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Inspired by Democritus. Came up with atomic theory similar to today's.
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Aristotle
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Well known Greek philosopher of the time. Believed the earth was composed of four elements: Earth, Fire, Water, Wind. He disagreed with Democritus. Everyone agreed with him.
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Democritus
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Greek philosopher who first came up with the concept of an atom. No one believed him.
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Solid
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Organized particles, definite shape and volume.
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Liquid
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Unorganized particles, indefinite shape but definite volume.
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Gas
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Unorganized particles, indefinite shape and volume.
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Plasma
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Very fast and random particles, so much energy that electrons are liberated.
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Avagadro's Number
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6.022x1022
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AMU
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Atomic Mass Unit
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When balancing, add...
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Coeffecients
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When balancing, DON'T TOUCH...
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Subsripts
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Conservation of Mass
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Mass can't be created or destoyed.
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Why are equations balanced?
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To find an accurate and pricise measurement, along with correct atom counts.
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Reactants
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Left side
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Products
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Right Side
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Arrow
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Act as an equal sign in chemical reactions.
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Density
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D=M/V
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Endothermic Reaction
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When heat is released internally in a reaction.
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Exothermic Reaction
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When heat is released externally in a reaction.
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Luminous Intensity
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Candelas
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Electric Current
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Amperes
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Mass
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Kilograms
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Liquid
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Liters
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Time
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Seconds
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Temperature
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Kelvins
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Amount of Substance
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Moles
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Heisenberg Uncertainty Principle
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One cannot know the speed and location of an electron at the same time.
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Valence Level
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Highest energy level of atoms. This is where electrons are gained or lost.
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Monoatomic Ion
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An ion with only one element.
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Polyatomic Ion
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An ion with two or more elements.
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Plum Pudding Model
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J.J. Thompson's model of the atom. The electrons represent the plum pieces. Looks like a chocolate chip cookie if you don't know what plum pudding is.
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Quantum Model
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The most recent and current model of the atom.
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Solar System Model
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Bohr's model of the atom. Only valid with Hydrogen.
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Electron Spin
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When an electron spins in the opposite direction than that of the electron which it shares the orbital with.
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Octet
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Meaning eight electrons. When an atom has all orbitals filled completely.
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MINOH
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The recommended order of balancing equations. Metals, Polyatomic ions, Non-metals, Oxygen, Hydrogen
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Noble Gas Exception
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Noble gases are extremely stable and do not react.
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Noble Gas Notation
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When you only list the electron configuration of an element after its preceding Noble Gas.
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Bunsen Burner
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Used for a flame in labs.
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Parts of a Bunsen Burner
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Barrel, Air ports, Gas inlet, Base, Needle Valve
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Matter
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Anything which takes up space.
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Recommended flame to use in labs
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Noisy, blue, stable, cone-shaped flame.
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Ernest Rutherford
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Conducted Gold Foil experiment. Found the nucleus and that atoms are mostly empty space.
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Lewis Dot Symbols
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When you write the element symbol and draw dots around it symbolizing how many valence electrons it shares.
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Atomic Radius
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How close the electrons are pulled to the nucleus.
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Oil Drop Experiment
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Oil was dropped and then charged in the middle of its fall. Found the size of the mass and charge of the electron. Done by Millikan.
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Cathode Ray Tube Experiment
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Electrons were passed through a tube and then placed against a negative charge. Found out about subatomic particles and mass to charge ratio of electrons. Done by Thompson.
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Gold Foil Experiment
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Radioactive alfa-particles were shot into a piece of gold. Found that atoms were mostly empty space and that nuclei exist. Done by Rutherford.
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Chemistry
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The study of matter and the changes it undergoes.
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Freezing
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Liquid to solid.
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Melting
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Solid to liquid.
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Evaporation
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Liquid to gas.
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Sublimation
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Solid to gas.
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Deposition
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Gas to solid.
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Condensation
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Gas to liquid
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Ionization
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Gas to plasma.
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Deionization
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Plasma to gas.
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Orbit
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The path electrons travel.
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Orbital
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A mathematical representation of the space electrons take up.
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Electronegativity
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An electron's ability to attract other electrons.
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Molar Mass
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Mass per mole.
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Percent Composition
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Finding out the percentages that each compound has of each element.
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Ionization Energy
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The energy required to form ions.
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Isoelectronic
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2 species with the same electron configuration.
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Molecular Formula
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The number of atoms of each element.
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Empirical Formula
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Ratio of the atoms of each element.
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Electron Configuration
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A method of showing how many electrons an element has by means of orbitals.
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S
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2
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P
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6
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D
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10
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F
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14
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Lewis Structure
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A drawing which shows the sharing of electrons between elements in a covalent compound.
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Mole
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The number of atoms of each element present in a molecule.
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Boyle's Law
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k=PV
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Charles' Law
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k=v/t
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Gay-Lussac Law
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k=p/t
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Ideal Gas Law
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PV=nRT
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Combined Gas Law
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PV=kT
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R
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.082 L*atm/mol*k
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Percent Yield
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The percent of the calculated yield versus the actually obtained amount.
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Limiting Reactant
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The reactant that determines how much of a product can be formed.
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Acid
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A substance that has to do with hydrogen ions.
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Base
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A substance that has to do with hydroxide ions.
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pH
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Power of Hydrogen or the strength of an acid or base.
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Salt
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A neutral precipitate formed.
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Neutralization Reaction
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A reaction in which an acid and a base cancel each other out.
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Redox Reaction
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A reaction in which electrons are transferred among elements.
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Precipitate Reaction
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A reaction in which a solid precipitate is formed.
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Precipitate
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An insoluble solid at the bottom of water.
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