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142 Cards in this Set
- Front
- Back
absolute zero
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the lowest possible temp, written as 0K or -273.15 C
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Accuracy
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the closeness of a measurement to an accepted value
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Acid Ionization Constant
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a constant whose value indicates the relative strength of an acid in aqueous solution.
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activated complex
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the intermediate state between reactants and products in a chemical reaction; the peak of potiental energy diagram
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activation energy
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the minimum energy needed to initiate a reaction
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addition polymerization
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the joining of unsaturated monomers by a series of addition reactions
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alcohol
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an organic compound containing a hydroxyl (-OH)group
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alkali metal
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any group 1 element excluding hydrogen H
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alkaline earth element
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any group 2 element
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alkyl group
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an open chained hydrocarbon less one hydrogen atom
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methyl group
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CH3
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ethyl group
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C2H5
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allotrope
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a specific form of an element that can exist in more than one form; graphite and diamond are allotropes pf the element carbon
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alloy
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a solid metallic solution
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alpha decay
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the radioactive process in which an alpha particle is emitted
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amino acid
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an organic compound containing at least one amino group and one carboxyl group
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amino group
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an ammonia group less than one hydrogen atom -NH2
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amphiprotic
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pertaining to a substance that can act as a Bronsted-Lowry acid or base by donating and accepting H+ ions
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anhydrous
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pertaining to a compound from which the water of crystallization has been removed
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anode
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the electrode at which oxidation occurs
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aqueous
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pertaining to a solution in which water is a solvent
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aromatic hydrocarbon
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any rong hydrocarbon whose electronic is related to that of benzene
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Arrhenius Acid
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any substance that releases H+ ion in water
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Arrhenius Base
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any substance that releases OH- ions in water
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Atom
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the basic unit of an element
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atomic mass
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the weighted average of the masses of the isotopes of an element
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atomic mass unit
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one twelfth the mass of a carbon-12 atom
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atomic number
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the # of protons in the nucleus of an atom the atomic number defines the element
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atomic radius
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a calculated estimate of the size of an atom
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avogadro's hypothesis
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equal volumes of gases, measured at the same temp and pressure, contain equal numbers of particles
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avogadro's #
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the # of particles in 1 mole; 6.02 x 10 [23]
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base ionization constant
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a constant whose value indicates the relative strength of a base in aqueous solution
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battery
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a commercial voltaic cell
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benzene
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C6H6; the parent hydrocarbon of all aromatic compounds
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beta decay
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the radioactive process in which a beta particle is emitted
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beta (-) particle
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an electron
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beta (+) particle
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a positron
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binary compound
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a compound containing two elements
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binding energy
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the energy realeased when a nucleus is assembled from its nucleons
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boiling
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the transition of a liquid to a gas; boiling occurs when a vapor pressure of a liquid equals the atmospheric pressure above the liquid
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boiling point
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the temp at which boiling occurs; the temp at which the liquid and vapor phases of a substance are in equilibrium
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boiling point elevation
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the increase in the boiling point of a solvent due to the presence of solute particles
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bond energy
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the energy needed to break a chemical bond
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Boyle's Law
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a constant temp and mass, the pressure of an ideal gas is inversely proportional to its volume; P1V1=P2V2
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breeder reactor
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a fission reactor that generates its own nuclear fuel
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bright line spectrum
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the lines of visible light emitted by elements as electrons fall to lower energy levels
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Bronsted Lowry acid
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a substance that can donate H+ ions.
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Bronsted Lowry base
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a substance that can accept H+ ions
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catalyst
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a substance that speeds a chemical reaction by lowering the activation energy of the reaction
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cathode
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the electrode at which reduction occurs
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chain reaction
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a chemical or nuclear reaction in which one step supplies energy or reactants for the next step
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charle's law
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at constant pressure and mass, the volume of an ideal gas is directly proportional to Kelvin temp; v/t=v/t
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chemical bond
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the stabilizing of two atoms by sharing or transferring electrons
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chemical energy
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the part of internal energy that is associated with te bonds and intermolecular attractions of substances
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chemical equation
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a shorthand listing of reactants, products and molar quantities in a chemical reaction
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chemical equilibrium
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the state in which the forward and reverse reactions are equal
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chemical property
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a property that describes the composition and reactivity of a substance
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chemical reaction
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a process in which one or more substances are converted into other substances
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chromatography
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the process in which the components of certain mixtures are separated because of their differences in solubility
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coefficient
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a # in a chemical equation that indicates how many particles of a reactant or product are required or formed in the reaction.
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colligative property
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a property that depends in the # of particles present rather than a type of a particle
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combined gas law
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at constant mass, the product of the pressure and volume divided by the kelvin temp is a constant PV/T=PT/T
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common ion effect
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an equilibrium shift caused by the addition of an ion present in a reaction
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compound
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a combination of two or more elements with a fixed composition by mass
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concentrated
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pertaining to a solution that contains relatively large quantity of solute
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concentration
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the "strength" of a solution; the of solute relative to the quantity of solvent
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condensation
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the change of gas to liquid
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condensation polymerization
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the joining of monomers by a series of dehydration reactions
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conjugate acid-base pair
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two particles that differ by a single H+
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constitutional isomers
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isomers that differ because their atoms are connected in different orders
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control rod
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a part of a fission reactor that controls the rate of fission by absorbing neutrons
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coordinate covalent bond
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a single covalent bond in which the pair of electrons is supplied by one atom
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covalent atomic radius
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the effective distance from the nucleus of a covalently bonded atom to its valence level
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covalent bond
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a chemical bond formed by the sharing of electrons
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cracking
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the process of breaking large hydrocarbon molecules into smaller ones in order to increase the yield of compounds such as gasoline
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crystallizaton
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the process in which a solute separates from its solution
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decomposition
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a reaction in which a compound forms two or more simpler substances
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deposition
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the direct transition from gas to solid
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diatomic molecules
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a neutral particle consisting of two atoms
ex Br2 and CO |
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diffusion
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the movement of one subtance to another
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dilute
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peratining to a solution that contains a relatively small quantity of solute; to reduce a concentration of a solution by adding solvent
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dipole
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an unsymmetrical charge distribution in a nuetral molecule
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dipole-dipole attraction
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the attractive force between two opposite charged dipoles of nieghboring polar molecules
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dipersion forces
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the attractive forces between nieghboring nonpolar molecules
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dissociation
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the separation of an ionic compound in solution into positive and negative ions
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distillation
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the simultaneous boiling of a liquid and condensation of its vapor
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ductility
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the property of a substance that allows it to be drawn into a wire; metallic substances possess ductility
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dynamic equilibrium
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the state in which the rates of opposing processes are equal
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effusion
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the escape pf gas from a small porous opening
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electrochemical cell
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a voltaic cell or an electrolytic cell
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electrode
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a conductor in an chemical or electrolytic cell that serves as a site of oxidation or reduction
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electrolysis
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a nonspontaneous redox reaction driven by an external source of electricity
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electrolyte
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a substance whose aqueous solution conducts electricity
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electrolytic cell
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a device for carrying out electrolysis
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electron
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the elementary unit or negative (-) charge
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electron affinity
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the energy change that occurs when an atom or ion gains an electron
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electronegativity
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the measure of an atom's attraction for a bonded pair of electrons
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electroplating
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the use of an electric current to deposit a layer of metal on a negatively charged object
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element
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a substance of all whose atoms have the same atomic #
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elementary reactions
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a series of simpler reactions that are "building blocks" of a more complex reaction
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empirical formula
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a formula in which the elements are present in the smallest whole-number ratio; NO2 is that but C2H4 is not
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endothermic reactions
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a reaction that absorbs energy
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energy
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a quantity related to an object's capacity to do work
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enthalpy change
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the heat energy absorbed or released by a system
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entropy
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the measure of randomness or disorder of a system
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ester
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the organic product of esterification
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esterfication
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the reaction of an acid with an alcohol to produce an ester and water
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evaporation
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the surface transitition of liquid to gas
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excited state
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a condition in which one or more electrons in an atom are no longer in the lowest possible energy state
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exothermic reaction
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a reaction that releases energy
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fermentation
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the (anaerobic) oxidation of a sugar such as glucose to produce ethanol and carbon dioxide; the reaction is catalyzed bby enyzmes
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filtration
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the process in which a precipitate is recovered from a mixture
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first ionization energy
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the quantity of energy needed to remove the most loosely held electron from an isolated neutral atom
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first law of thermodynamics
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energy is conserved in any process
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fission
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a nuclear reaction in ehich a heavy nuclide splits to form lighter nuclides and energy
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freezing
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the transition from liquid to solid
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freezing point
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the temp at which freezing occurs
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fusion
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a synonym for melting; also a nuclear process in which light nuclides join to form heavier nuclides and produce radiant energy
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gas
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the phase in which matter neither has definite shape nor volume
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graham's law of effusion
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at constant temp and pressure, the rate of effusion of a gas is inversely proportional to the square root of its molar mass or density
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ground state
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the electron configuration of an atom in the lowest energy state
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Haber process
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the commercial procedure by which ammonia is produced from nitrogen and hydrogen
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half cell
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the part of an electrochemical cell in which oxidation or reduction occurs
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halogen
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any element in group 17
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heat
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the energy transferred between two objects when they are at different temps
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heat of fusion
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heat absorbed when a unit mass of solid changes to liquid at its melting point
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heat of reaction
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the heat absorbed or released as a result of a chemical reaction
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heat of vaporization
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the hear absorbed when a unit mass of liquid changes to gas at its melting point
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Hess's Law
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the heat absorbed or released in a given reaction can be expressed as the sum of the heats associated with other reactions if these reactions can be "added" to produce the original reaction.
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heterogenous mixture
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a nonuniform mixture
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homogenous mixture
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a mixture with uniform distribution of particles
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homologous series
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group of organic compounds with related structures and properties; each successive member of the series differs from the one before it by a specific number of carbon and hydrogen atoms
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hybrid orbital
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an orbital formed by the "mixing" of individual atomic orbitals
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hydration
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the association of water molecules with an ion or another molecule
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hydrogen bond
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an unusually strong molecular attraction that results when hydrogen is bonded to a small, highly electronegative atom
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hydrolysis
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a reaction in which a water molecule breaks a chemical bond
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ideal gas
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a model of gas in which the particles have no volume, do not attract or repel each other, and collide without loss of energy
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indicator
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a substance that undergoes a color change to signal a change in chemical conditions
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inert gas
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any element in group 18
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ion
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a particle in which the numbers of protons and electrons are not equal
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ionic bond
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the electrostatic attraction of positive and negative ions in an ionic compound
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ionic compound
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substance whose particles consist of negative and positive ions.
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