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123 Cards in this Set
- Front
- Back
Matter
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Physical material of the universe- anything that has a mass and occupies space
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Elements
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Very basic or elementary substances
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Atoms
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The almost infinitesimally small building blocks of matter
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Molecules
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Two or more atoms are joined together in specific shapes
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States of Matter
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Gas, liquid, or solid
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Liquid
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Has a distinct volume independent of its contaner but has no specific shape
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Gas
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Has no fixed volume or shape
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Solid
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Has a definite shape and volume
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Pure Substance
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Matter thatas distinct properties and a composition that doesn't vary from sample to sample.
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Elements
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Cannot be decomposed into simpler substances
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Compounds
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Substances composed of twoor more elements
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Mixtures
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combinateions of two or more substances in which each substance retains its own chemical identity
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Law of Constant Composition
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The observaion that the elemental composition of a pure compound is always the same
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Solutions
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Homogenous mixtures
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Physical Properties
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Properties that can be measured without changing the identity and composition of the substance.
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Chemical Properties
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Properties hat describe the way a substance may change or reat to form other substances
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Intensive Properties
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Propeties that do not depend on the amount of the sample being examined.
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Extensive Properties
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Properties of substances that depend on the quantity of the sample and include measurements of mass and volume.
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Physical Changes
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A change in which a substance changes its physical appearance, but not its composition.
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Changes of State
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Physical changes from different states (for example: liquid to solid)
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Chemical Changes
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Changes nwhich a substance is transformed into a chemically different substance.
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Metric System
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The units of measurement used for scientific measurements.
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Precision
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Ameasure of how closely individual measurements agree with one another
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Accuracy
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How closely individual measurements agree with the correct value
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Conversion Factor
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A fraction whose numerator and denominator are the same quantity expressed in different units
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Scientific Method
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A dynamic process used to answe questions about our physical world
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Atoms
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The basic building blocks of matter; the smallest units ofan element that can combine with other elments
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Subatomic particles
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Comprise atoms; some are charged
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Cathode rays
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Their behavior in magnetic and electrical fields led to the discovery of the electron
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Radioactivity
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The spontaneos emission of radiation by atoms
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Nucleus
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The dense, positively charged center of a atom
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Protons
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Positively charged subatomic particle
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Neutrons
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Neutral subatomic particle
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Electons
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Negatively charged subatomic particle
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Atomic Number
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The number of protons
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Isotopes
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Atoms of a given element that differ in the number of nuetrons, and consequently in mass
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Mass Number
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Total number of protons plue neutrons in the atom
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Nuclide
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An atom of a specific isotope
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Atomic Weight
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Average atomic mass of each element
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Periodic Table
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The arrangelment of elements in order of increasing atomic number
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Group
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The elements in a column of the periodic table
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Metallic Elements
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All the elements on the lef side and in the middle of the periodic table
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Molecule
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An assembly of two or moe atoms tightly bound together
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Diatomic Molecule
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A molecule that is made up of two atoms
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Molecular Formulas
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Chemical formulas tha indicate the actual numbers and types of atoms in a molecule
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Empirical Formulas
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Chemical formulas that give only the relative number of atoms of each type in a molecule
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Structural Formula
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Shows which atoms are attached to which within the molecule
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Ion
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A charged particle
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Cation
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An ion with a positive charge
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Anion
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An ion with a negative charge
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Ionic Compound
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A compound that contains both positively and negatively charged ions
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Chemical Nomenclature
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The naming of substances
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Organic Chemistry
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The sudy of compounds of carbon
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Hydrocarbons
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Organic compounds only containing carbon and hydrogren
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Stoichiometry
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The study of the quantitative relationships between chemical formulas and chemical equations
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Law of Conservation of Mass
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The total mass of the products of a chemical reacton is the same as the total mass of the reactants.
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Chemical Equation
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Shows the equal numbers of atoms of each element oneach side of the equation
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Combination Reactions
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Two reactants combine to form one product
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Decomposition Reaction
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A single reactant forms two or more products
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Combustion Reaction
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A reaction in which a hydrocarbon reacts with oxygen to form carbon dioxide and water.
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Formula Weight
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Weight of the compound that equals the sum of the atomic weighs of the atoms in its formula
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Mole
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Avogradro's number of formula units of that substanc
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Avogadro's Number
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6.02 x 10^23
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Limiting Reactant
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The reactant that is completey consumed in a reaction
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Theoretical Yield
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The quantity of product calculated to form when all of the limiting reagent reacts
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Aqueous Solutions
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Solutions in which water is the dissolving medium
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Solvent
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The component of the solution that is in the greater quantity
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Solutes
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All other components of a solution
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Electrolyte
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Any substance whose aqueos soluton contains ions
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Nonelectrolyte
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Any substance that forms a solution contaiing no ions
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Strong Electrolytes
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Those electrolytes that are present in solution entirely as ions
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Weak Electrolytes
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Those electrolytes that are present partly as molecules
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Precipitation reactions
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Those in which an insoluble product forms
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Precipitate
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An insoluble product
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Solubility
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The amount of a substnc that dissolves in a given quantity of solvent
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Metahesis reactions
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Reaction such as precipitation reaction, in which cations and annions appear to exchange partners
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Moleclar equation
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Used when the complete chemical formulas of all reactants and products are used
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Complete Ionic Equation
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Shows all dissolved strong electrolytes as their component ions
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Net Ionic Equation
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An equation in which those ions that go through te reaction unchanged are omitted
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Acids
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Proton donors
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Bases
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Proton acceptors
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Oxidation
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The loss of electrons by a substance
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Reductions
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The gain of electrons by a substance
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Displacement Reactions
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The redox reactions between metals and acides and between metals and salts
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Activity Series
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A list of metals arranged in order of decreasing ease of oxidation
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Molarity
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The number of moles of solute per liter of solution
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Titration
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Combine a solution on known concentration with a solution of unknown concentration
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Thermodynamics
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The study of energy and its transformations
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Thermochemistry
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The transformations of enrgy- especially heat- during chemical reactions
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Kinetic Energy
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Energy due to the motion of the object
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Kintetic Energy
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Energy due to the motion of the object
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Potential Enrgy
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Energy that an object possesses by virtue of its position relative to other objects
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Calorie
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The quantity of energy necessary to increase the temperateure of 1g of water by 1 degree C
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System
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Specific amount of matter
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Surroundings
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Everything outside of a system
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Work
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Energy expanded to move an object against a force
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Heat
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The enrgy that is transferred from a hotter object to a colder one
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Energy
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The capacity to do work or transfer heat
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Interal energy
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The sum of all the kinetic and potential energies of its component parts
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First Law of Thermodynamics
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The change in the internal system of a system is the sum of the heat transferred into or out of the system and the work, done on or by the system
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Endothermic
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Process in which the system absorbs heatfrom the surroundings
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Exothermic
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Process in which the system releases heat to the surroundings
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Pressure-volume work
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Performed when a gas is produced or consumed in a chemical reaction occuring at constant pressure
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Enthalpy of reaction
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The enthalpy of the products minus the enthalpy of the reactants
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Calorimeter
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Measures the temperature change accompanying a process
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Heat Capacity
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The amount of heat required to raise its temperature by I degree kelvin
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Molar Heat Capacity
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The heat capacity of one mole of a pure substance
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Specific het
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The heat capacity of one gram of a substance
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Bomb Calorimeer
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Used to measure the heat evolved in combustion reactions
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Hess's Law
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If a reaction is carried out in aseries of stems, the change in heat for the reaction will be equal tothe sum of enthalpy changes for the steps.
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Enthalpy of Formation
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The enthalpy change for the reaction in which the substance is formed from its constituent elements
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Standard Enthapy
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Enthalpy change when all reactants and productes are at 1 atm pressure and a specific temperature
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Standard Enthalpy of Formation
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The chang in enthalpy for the reaction that forms 1 mol of the substance from its elements with all reactants and products at 1 atm pressure and usually 298 K
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Electronic Structure
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Describes the energies and arrangement of electrons around the atom.
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Quantum of Energy
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The minimum amount of radiant energy that an object can gain or lose
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Planck's Constant
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h= 6.63 x 10^-34 J-s
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Photoelectric Effect
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The emission of electrons from metal surfaces from light
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Spectrum
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Produced by a dispersion of radiation into its component wavelengths
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Continuous Spectrum
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If a sepctrum contains all wavelengths
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Line Spectrum
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If a spectrum only contains specific wavelengths
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Ground State
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The lowest energy of a hydrogen atom
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Heisenberg's Uncertainty Principle
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There is an inheret limit to the accuracy with which the position of momentum of a particle can be measured simultaneously.
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Wave functions
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Mathematical functions that describe the behavior of the electron in the quantum mechanical model of the hydrogen atom
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