Absolute Zero
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0 K or -273.15°C. This is the temperature at which molecular motion is at a minimum.
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| Accuracy |
How close a particular measurement is to the true value.
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Acid
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A chemical that can act as a proton donor (Bronsted-Lowry theory) or is an electron acceptor (Lewis theory)
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Acid Ionization Constant (Ka)
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Equilibrium constant for a Bronsted-Lowry acid given by the formula Ka = [H]*[A] / [HA]
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Actinide
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Element in the 2nd row of the f-block elements.
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Activation Energy (Ea)
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The amount of energy that must be put into a reaction for it to proceed.
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Active Site
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The specific area in an enzyme where the enzyme can perform a catalytic function.
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Activity Series
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An ordered list of chemicals based on how easily they can be oxidized.
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Actual Yield
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How much product was actually made in a reaction - determined by measurement.
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Adduct
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Generic name for a compound formed by the combination of a Lewis acid and a Lewis base.
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Alcohol
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Any organic compound that contains a -OH functional group.
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Aldehyde
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Any organic compound that contains a carbonyl (C=O) attached to a H. -CHO
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Alkali Metal
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Any element from the first column of the periodic table (group 1)
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Alkaline Earth Metal
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Any element from the second column of the periodic table (group 2)
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Alkane
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A single bond between carbon atoms, with each carbon bonded to three other atoms. Given by the general formula CnH(2n+2)
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Alkene
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A double bond between carbon atoms, with each carbon bonded to two other atoms.
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Alkyne
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A triple bond between carbon atoms, with each carbon bonded to one other atom.
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Alloy
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Mixture of 2 or more metals
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Amalgam
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A solution of a metal in mercury (Hg)
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Amide
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Any organic compound that contains a carbonyl (C=O) attached to a -NH- group.
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Amine
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A chemical that looks like ammonia (NH3) but where any or all of the N-H bonds can be replaced with a N-C bond.
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Amino Acid
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A chemical that contains both a carboxylic acid (-CO2H) and an amine (-NH2)
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Ampere
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Most common unit to measure electric current.
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Amphiprotic
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A chemical that can act as both a proton donor and a proton acceptor.
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Amplitude
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The height of a wave. See "peak-to-peak amplitude" and "peak amplitude".
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Anion
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Any chemical ion that contains a negative charge (ex. I-)
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Anode
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In an electrical system, the electrode where oxidation occurs.
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Antibonding Orbital
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An orbital involved in molecular orbital (MO) bonding theory which is less stable (higher energy) than the atomic orbitals from which it was formed.
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Aqueous
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Any solution that uses water as the solvent.
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Arrhenius Equation
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Equation used in kinetics that describes how rate constants depend on temperature and activation energy. k = Ae-Ea/RT
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Atmosphere (atm)
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A common unit of pressure that is based on normal pressure at sea level where pressure = 1atm.
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Atom
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The most basic unit of chemical matter containing both a nucleus of protons and neutrons, and electrons.
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Atomic Number (Z)
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The number of protons in an atom's nucleus.
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Atomic Orbital
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Describes the areas of electron density around an atoms nucleus
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Atomic Radius
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The distance from the center of an atoms nucleus to the farthest electron(s) of that atom.
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Atomic Symbol
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The letters assigned to a particular element (ex. chlorine = Cl)
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Atomic Theory
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The theory that all matter is composed of atoms, which can not change their basic properties (ex. lead can not be turned into gold)
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Aufbau Principle
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The most stable form of an atom comes from placing electrons in the lowest energy, available, atomic orbital.
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Avogadro's Constant
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The number of atoms contained in 1 mole. 6.022142 x 1023 particles/mole
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Azimuthal Quantum Number (l)
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Describes the shape of an atomic orbital and can range from 0 to n-1.
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