Term
|
Definition
a temp scale on which absolute zero (0K) is the lowest temp
(kelvin temp scale) |
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Term
|
Definition
| theoretically the lowest attainable temp |
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Term
|
Definition
| the closeness of a measurement to the true value of the quantity that is being measured |
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Term
|
Definition
| a substance that yields hydrogen ions (H+) when dissolved in water |
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Term
| acid ionization constant (Ka) |
|
Definition
| the equilibrium constant for acid ionization |
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Term
|
Definition
| elements that have incompletely filled 5f subshells or readily give rise to cations that have incompletely filled 5f subshells |
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Term
|
Definition
| the species temporarily formed by reactant molecules as a result of a collision before they form the product |
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Term
|
Definition
| the minimum amount of energy required to initiate a chemical reaction |
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Term
|
Definition
| a summary of the results of many possible displacement reactions |
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Term
|
Definition
| the amount of product actually obtained in a reaction |
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Term
|
Definition
| a reaction in which one molecule is added to another |
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Term
|
Definition
| attraction between unlike molecules |
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Term
|
Definition
| an organic compound containing the hydroxyl group (-OH) |
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Term
|
Definition
| compounds with a carbonyl functional group and the general formula RCHO in which R is an H atom, an alkyl, or an aromatic hydrocarbon group |
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Term
|
Definition
| hydrocarbons that do not contain the benzene group or the benzene ring |
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Term
|
Definition
| the group 1A elements (Li, Na, K, Rb, Cs, and Fr) |
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Term
|
Definition
| the group 2A elements (Be, Mg, Ca, Sr, Ba, and Ra) |
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Term
|
Definition
| hydrocarbons having the general formula CnH2n+2, in which n=1,2... |
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Term
|
Definition
| hydrocarbons that contain one or more carbon-carbon double bounds. They have the general formula CnH2n in which n=2,3... |
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Term
|
Definition
| hydrocarbons that contain one or more carbon-carbon triple bonds. they have the general formula CnH2n-2 in which n=2,3... |
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Term
|
Definition
| two or more forms of the same element that differ significantly in chemical and physical properties |
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Term
alpha particles
alpha rays |
|
Definition
| helium ions with a charge of +2 |
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Term
|
Definition
| organic bases that have the functional group -NR2 in which R may be H, and alkyl group, or an aromatic hydrocarbon group |
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Term
|
Definition
| a special kind or carboxylic acid that contains at least one carboxyl group (-COOH) and at least one amino group (-NH2) |
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Term
|
Definition
| A solid that lacks a regular three-dimensional arrangement of atoms or molecules |
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Term
|
Definition
| an oxide that exhibits both acidic and basic properties |
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Term
|
Definition
| the vertical distance from the middle of a wave to the peak or trough |
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Term
|
Definition
| an ion with a net negative charge |
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Term
|
Definition
| the electrode at which oxidation occurs |
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Term
| antibonding molecular orbital |
|
Definition
| a molecular orbital that is of higher energy and lower staility than the atomic orbitals from which it was formed |
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Term
|
Definition
| a solution in which the solvent is water |
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Term
|
Definition
| a hydrocarbon that contains one or more benzene rings |
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Term
|
Definition
| the pressure exerted by earth's atmosphere |
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Term
|
Definition
| the basic unit of an element that can enter into chemical combination |
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Term
|
Definition
| the mass of an atom in atomic mass units |
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Term
|
Definition
| a mass exactly equal to one-twelfith the mass of one carbon-12 atom |
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Term
|
Definition
| the number of protons in the nucleus of an atom |
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Term
|
Definition
| the wave function of an electron in an atom |
|
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Term
|
Definition
| one-half the distance between the nuclei in two adjacent atoms of the same element in a metal. for elements that exist as diatomic units, the atomic radius is one-half the distance between the nuclei of two atoms in a particular molecule |
|
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Term
|
Definition
| as protons are added one by one to the nucleus to build up the elements, electrons similarly are added to the atomic orbitals |
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Term
|
Definition
| at constant pressure and temperature, the volume of a gas is directly proportional to the number of moles of the gas present |
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Term
|
Definition
| 6.022 X 1023; the number of particles in a mole |
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Term
|
Definition
| an instrument that measures atmospheric pressure |
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Term
|
Definition
| a substance that yields hydroxide ions (OH-) when dissolved in water |
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|
Term
| base ionization constant (Kb) |
|
Definition
| the equilibrium constant for the ionization of a base |
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Term
|
Definition
| a galvanic cell or a series of several connected galvanic cells that can be used as a source of direct electric current at a constant voltage |
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|
Term
beta particles
beta rays B |
|
Definition
| streams of electrons emitted during the decay of certain radioactive substances |
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Term
|
Definition
| an elementary step involving two molecules that is part of a reaction mechanism |
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Term
|
Definition
| compounds containing just two elements |
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Term
|
Definition
| the temperature at which the vapor pressure of a liquid is equal to the external atmospheric pressure |
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Term
|
Definition
| the boiling pt of the son (Tb) minus the boiling pt of the pure solvent (Tb°) |
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Term
|
Definition
| the enthalpy change required to break a bond in a mole of gaseous molecules |
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Term
|
Definition
| the distance between the centers of two bonded atoms in a molecule |
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Term
|
Definition
| the difference between the number of electrons in bonding molecular orbitals and anibonding molecular orbitals, divided by two |
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|
Term
| bonding molecular orbital |
|
Definition
| a molecular orbital that is of lower energy and greater stability than the atomic orbitals form wihich it was formed |
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Term
|
Definition
| the cycle that relates lattice energies of ionic compounds to ionization energies, electron affinities, and other atomic and molecular properties |
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Term
|
Definition
| diagram of the region containing about 90 percent of the electron density in an atomic orbital |
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Term
|
Definition
| the volume of a fixed amount of gas is inversely proportional to the gas pressure at constant temp. |
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Term
|
Definition
| a nuclear reactor that produces more fissionable material than it uses |
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Term
|
Definition
| a substance capable of donating a proton in a reaction |
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Term
|
Definition
| a substance capable of accepting a proton in a reaction |
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Term
|
Definition
| a solution of a weak acid or a base its salt; both components must be present. a buffer solution has the ability to resist changes in pH when small amounts of either acid or base are added to it |
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Term
|
Definition
| the measurnment of heat changes |
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Term
|
Definition
| acids that contain the carboxyl group (-COOH) |
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Term
|
Definition
| a substance that increasese the rate of a chemical reaction by providing an alternate reaction pathway without being consumed during the reaction |
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Term
|
Definition
| the electrode at which reduction occurs |
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Term
|
Definition
| an ion with a net positive charge |
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Term
|
Definition
| difference in electrical potential between the anode and the cathode of a galvanic cell |
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Term
Charles's and Gay-Lussac's law
Charles's law |
|
Definition
| the volume of a fixed amount of gas is directly proportional to the absolute temp of the gas when the pressure is held constant |
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Term
|
Definition
| a substance that forms complex ions with metal ions in solution |
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Term
|
Definition
| energy stored within the structural units of chemical substances |
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Term
|
Definition
| an equation that uses chemical symbols to show what happens during a chemical reaction |
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Term
|
Definition
| a state in which the rates of the forward and reverse reactions are equal and no net changes can be observed |
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Term
|
Definition
| an expression showing the chemical composition of a compound in terms of the symbols for the atoms of the elements involved |
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Term
|
Definition
| the area of chemistry concerned with the speeds or rates at which chemical reactions occur |
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Term
|
Definition
| any property of a substance that cannot be studied without converting the substance into some other substance |
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Term
|
Definition
|
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Term
|
Definition
| the science that studies the properties of substances and how substances react with one another |
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Term
|
Definition
| compounds or ions that are not superimposable with their mirror images |
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Term
|
Definition
| a system that allows the exchange of energy (usually in the form of heat) but not mass with its surroundings |
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Term
|
Definition
| the most efficient arrangements for packing atoms molecules, or ions in a crystal |
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Term
|
Definition
| the intermolecular attraction between like molecules |
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Term
|
Definition
| properties of solutions that depend on the number of solute particles in solution and not on the nature of the solute |
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Term
|
Definition
| a reaction in which two or more substances combine to form a single product |
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Term
|
Definition
| a reaction in which a substance reacts with oxygen, usually with the release of heat and light to produce a flame |
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Term
|
Definition
| an ion containing a central metal cation bonded to one or more molecules or ions |
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Term
|
Definition
| a substance composed of two or more elements chemically united in fixed proportions |
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Term
| concentration of a solution |
|
Definition
| the amount of solute present in a given quantity of solution |
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Term
|
Definition
| the phenomenon of going from the gaseous state to the liquid state |
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Term
|
Definition
| the joining of two molecules and teh elimination of a small molecule, usually water |
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Term
|
Definition
| different spatial arrangements of a molecule that are generated by rotation about single bonds |
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Term
|
Definition
| an acid and its conjugate base or a base and its conjugate acid |
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Term
|
Definition
| a bond in which the pair of electrons is supplied by one of the two bonded atoms |
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Term
|
Definition
| a neutral species containing a complex ion |
|
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Term
|
Definition
| in a crystal lattice it is defined as the number of atoms (or ions) surrounding an atom (or ion) in coordination compounds it is defined as the number of donor atoms surroundinng the central metal atom in a complex |
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Term
|
Definition
| a polymer containing two or more different monomers |
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Term
|
Definition
| the deterioration of metals by an electrochemical process |
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Term
|
Definition
| the potential energy between two ions is directly proportional to the product of their charges and inversely proportional to the distance between them |
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Term
|
Definition
| a bond in which two electrons are shared by two atoms |
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Term
|
Definition
| compounds containing only covalent bonds |
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Term
|
Definition
| the minimum mass of fissionable material required to generate a sefl-sustaining nuclear chain reaction |
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Term
|
Definition
| the minimum pressure necessary to bring about liquefaction at the critical temp |
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Term
|
Definition
| the temp above which a gas will not liquefy |
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Term
|
Definition
| the energy difference between two sets of d orbitals of a metal atom in the presence of ligands |
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Term
|
Definition
| a solid that possesses rigid and long-range structural order; its atoms, molecules, or ions occupy specific positions |
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Term
|
Definition
| the process in which dissolved solute comes out of solution and forms crystals |
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Term
|
Definition
| hydrocarbons having the general formula CnH2n in which n=3,4... |
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Term
| dalton's law of partial pressures |
|
Definition
| the total pressure of a mixture of gases is just the sum of the pressures that each gas would exert if it were present alone |
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Term
|
Definition
| the breakdown of a compound into two or more components |
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Term
| delocalized molecular orbital |
|
Definition
| a molecular orbital that is not confined between two adjacent bonding atoms but actually extends over three or more atoms |
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Term
|
Definition
| protein that does not exhibit normal biological activities |
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Term
|
Definition
| the mass of substance divided by its volume |
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Term
| deoxyribonucleic acid (DNA) |
|
Definition
|
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Term
|
Definition
| the process in which vapor molecules are converted directly to the solid phase |
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Term
|
Definition
| similarities between pairs of elements in different groups and periods of the periodic table |
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Term
|
Definition
| repelled by a magnet; a diamagnetic substance contains only paired electrons |
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Term
|
Definition
| a molecule that consists of two atoms |
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Term
|
Definition
| the gradual mixing of molecules of one gas with the molecules of another by virtue of their kinetic properties |
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Term
|
Definition
| a procedure for preparing a less concentrated solution from a more concentrated solution |
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Term
|
Definition
| the product of charge and the distance between the charges in a molecule |
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Term
|
Definition
| forces that act between polar molecules |
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Term
|
Definition
| each unit of the acid yields two hydrogen ions |
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Term
|
Definition
| the attractive forces that arise as a result of temporary dipoles induced in the atoms or molecules |
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Term
|
Definition
| a reaction in which an atom or an ion in a compound is replaced by an atom of another element |
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Term
|
Definition
| the atom in a ligand that is bonded directly to the metal atom |
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Term
|
Definition
| a covalent bond in which two atoms share two pairs of electrons |
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Term
|
Definition
| the condition in which the rate of a forward process is exactly balanced by the rate of the reverse process |
|
|
Term
| effective nuclear charge (Zeff) |
|
Definition
| the nuclear charge felt by an electron when both the actual charge (Z) and the repulsive effect (shielding) of the other electrons are taken into account |
|
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Term
|
Definition
| the process by which a gas under pressure escapes from one compartment of a container to another by passing through a small opening |
|
|
Term
|
Definition
| the branch of chemistry that deals with the interconversion of electrical energy and chemical energy |
|
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Term
|
Definition
| a process in which electrical energy is used to bring about a nonspontaneous chemical reaction |
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Term
|
Definition
| an apparatus for carrying out electrolysis |
|
|
Term
| electromagnetic radiation |
|
Definition
| the emission and transmission of energy in the form of electromagnetic waves |
|
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Term
|
Definition
| a wave that has an electric field component and a mutually perpendicular magnetic field component |
|
|
Term
| electromotive force (emf) (E) |
|
Definition
| the voltage difference between electrodes |
|
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Term
|
Definition
| a subatomic particle that has a very low mass and carries a single negative electric charge |
|
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Term
|
Definition
| the negative of the energy change that takes place when an electron is accepted by an atom (or an ion) inthe gaseous state |
|
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Term
|
Definition
| the distribution of electrons amoung the various orbitals in an atom or molecule |
|
|
Term
|
Definition
| the probability that an electron will be found at a particular region in an atomic orbital |
|
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Term
|
Definition
| the ability of an atom to attrract electrons toward itself in a chemical bond |
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Term
|
Definition
| a substance that cannot be separated into simpler substances by reaction at teh molecular level |
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Term
|
Definition
| a series of simple reactions that represent the overall progress of a reaction at the molecular level |
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Term
|
Definition
| the continuous or line spectrum of electromagnetic radiation emitted by a substance |
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Term
|
Definition
| an expression using chemical symbolys to show the types of elements in a substance and the simplest ratios of the different kinds of atoms |
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Term
|
Definition
| compounds and their nonsuperimposable mirror images |
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Term
|
Definition
| occurs in a titration when the indicator changes color |
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Term
|
Definition
| processes that absorb heat from the surroundings |
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Term
|
Definition
| the capacity to do work or to produce change |
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Term
|
Definition
| a thermodynamic puantity used to describe heat changes taking place at constant pressure |
|
|
Term
| enthalpy of reaction (ΔH) |
|
Definition
| the difference between the enthalpies of the products and the enthalpies of the reactants |
|
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Term
|
Definition
| a measure of how spread out or dispersed the energy of a system is amoung the different possible ways that the system can contain energy |
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|
Term
|
Definition
|
|
Term
|
Definition
| a number equal to the ratio of the equilibrium concentrations of products to the equilibrium concentrations of reactants, each raised to the power of its stoichiometric coefficient |
|
|
Term
| equilibrium vapor pressure |
|
Definition
| the vapor pressure measured for a dynamic equilibrium of condensation and evaporation |
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Term
|
Definition
| the point at which an acid is completely reacted with or neurtralized by a base |
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Term
|
Definition
| compounds that have the general formula RCOOR', in which R can be H or an alkyl group or an aromatic hydrocarbon group and R' is an alkyl group of an aromatic hydrocarbon group |
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Term
|
Definition
| an organic compound containing the R-O-R' linkage, in which R and R' are alkyl and/or aromatic hydrocarbon groups |
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Term
|
Definition
| the escape of molecules from the surface of a liquid; also called vaporization |
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Term
|
Definition
| a reactant present in a quantity greater than necessary to react with the amount of the limiting reagent present |
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Term
|
Definition
| a state that has higher energy than the ground state of teh system |
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Term
|
Definition
| processes that give off heat to the surroundings |
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Term
|
Definition
| a property that depends on how much matter is being considered |
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Term
|
Definition
| the elements in a vertical column of the periodic table |
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Term
|
Definition
| charge contained in 1 mole of electrons, equivalent to 96,485 coulombs |
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|
Term
| first law of thermodynamics |
|
Definition
| energy can be converted from one form to another, but cannot be created or destroyed |
|
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Term
|
Definition
| a reaction whose rate depends on reactant concentration raised to the first power |
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Term
|
Definition
| the electrical charge difference between the number of valence electrons in an isolated atom and the number of electrons in an isolated atom and the number of electrons assigned to that atom in a lewis structure |
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Term
|
Definition
| the equilibrium constant for the complex ion formation |
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Term
|
Definition
| the energy available to do useful work |
|
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Term
|
Definition
| the number of waves that pass through a particular point per unit time |
|
|
Term
|
Definition
| a galvanic cell that requires a continuous supply of reactants to keep functioning |
|
|
Term
|
Definition
| that part of a molecule characterized by a special arrangement of atoms that is largely responsible for the chemical behavior of the parent molecule |
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Term
|
Definition
| an electrochemical cell that generates electricity by means of a spontaneous redox reaction |
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Term
|
Definition
|
|
Term
|
Definition
| the constant that appears in the ideal gas equation (PV=nRT). it is expressed as 0.08206L X atm/K X mol, or 8.314 J/K X mol |
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Term
|
Definition
| compounds with the same type of number of atoms and the same chmical bonds but different spatial arrangements; such isomers cannot be interconverted without breaking a chemical bond |
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Term
|
Definition
see free energy
(G) the energy available to do useful work |
|
|
Term
| Graham's law of diffusion |
|
Definition
| Under the same conditions of temp and pressure, the rates of diffusion of gases are inversely proportional to the square roots of their molar masses |
|
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Term
|
Definition
| as experimental procedure that involves the measurenment of mass to identify an unknown component of a substance |
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Term
|
Definition
| the lowest energy state of a system |
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Term
|
Definition
| the elements in a vertical column of the periodic table |
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Term
|
Definition
| oxidation and reduction reactions that occur at the electrodes |
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Term
|
Definition
| the time required for the concentration of a reactant to decrease to half its initial concentration |
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|
Term
|
Definition
| a reaction that explicityly shows electrons involved in either oxidation or reduction |
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Term
|
Definition
| the nonmetallic elements in group 7A (F, Cl, Br, I, and At) |
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Term
|
Definition
| transfer of energy between two bodies that are at different temps |
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Term
|
Definition
| the amount of heat required to raise the temp of a given quantity of a substance by one degree celsius |
|
|
Term
| Heisenberg uncertainty principle |
|
Definition
| it is impossible to know simultaneouslty both the momentum and teh position of a particle with certainty |
|
|
Term
|
Definition
| the solubility of a gas in a liquid is proportional to the pressure of the gas over the solution |
|
|
Term
|
Definition
| when reactants are converted to products, the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps |
|
|
Term
| heterogeneous equilibrium |
|
Definition
| an equilibrium state in which the reacting species are not all in the same phase |
|
|
Term
|
Definition
| the individual components of such a mixture remain physically separate and can be seen as separate components |
|
|
Term
|
Definition
| an equilibrium condition in which all reacting species are in the same phase |
|
|
Term
|
Definition
| the composition of themixture is the same throughout the solution |
|
|
Term
| homonuclear diatomic molecule |
|
Definition
| a diatomic molecule containing atoms of the same element |
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|
Term
|
Definition
| a polymer that is made of only one type of monomer |
|
|
Term
|
Definition
| the most stable arrangement of electrons in atomic subshells is the one with the greatest number of parallel spins |
|
|
Term
|
Definition
| atomic orbitals obtained when two or more nonequivalent orbitals of the same atom combine before covalent bond formation |
|
|
Term
|
Definition
| the process of mixing the atomic orbitals in an atom (usually eht central atom) to generate a set of new atomic orbitals before covalent bond formation |
|
|
Term
|
Definition
| compounds that have a specific number of water molecules attached to them |
|
|
Term
|
Definition
| a process in which an ion or a molecule is surrounded by water molecules arranged in a specific manner |
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|
Term
|
Definition
| compounds made up of only carbon and hydrogen |
|
|
Term
|
Definition
| a special type of dipole-dipole interaction between the hydrogen atom bonded to an atom of a very electronegative element (F, N, O) and another atom of one of the three electronegative elements |
|
|
Term
|
Definition
| the addition of hydrogen, especially to compounds with double and triple carbon-carbon bonds |
|
|
Term
|
Definition
|
|
Term
|
Definition
| a tentative explanation for a set of observations |
|
|
Term
|
Definition
| a hypothetical gas whose pressure-volume-tem behavior can be completely accounted for by the ideal gas equation |
|
|
Term
|
Definition
| an equation expressing thte relationships among pressure, volume, temp, and amount of gas (PV=nRT, in which r is the gas constant) |
|
|
Term
|
Definition
| any solution that obeys Raoult's law |
|
|
Term
|
Definition
| substances that have distiinctly different colors in acidic and basic media |
|
|
Term
|
Definition
| the separation of positive and negative charges in an atom (or a nonpolar molecule) casued by the proximity of an ion or a polar molecule |
|
|
Term
|
Definition
| a complex ion that undergoes very slow ligand exchange reactions |
|
|
Term
|
Definition
| a property that does not depend on how much matter is being considered |
|
|
Term
|
Definition
| a species that appears in the mechanism of the reaction (that is, in the elementary steps ) but not in the oeverall balanced equation |
|
|
Term
|
Definition
| attractive forces that exist among molecules |
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|
Term
| International system of units |
|
Definition
| a revised metric system (abbreviated SI) that is widely used in scientific research |
|
|
Term
|
Definition
| forces that hold atoms together in a molecule |
|
|
Term
|
Definition
| an atom or group of atoms that has a net positive or negative charge |
|
|
Term
|
Definition
| a species made up of at least one cation and at least one anion held together by electrostatic forces |
|
|
Term
|
Definition
| forces that operate between an ion and a dipole |
|
|
Term
|
Definition
| the electrostatic force that holds ions together in an ionic compound |
|
|
Term
|
Definition
| any neutral compound containing cations and anions |
|
|
Term
|
Definition
| an equation that shows dissolved ionic compounds in terms of their free ions |
|
|
Term
|
Definition
| the radius of a cation or an anion as measured in an ionic compound |
|
|
Term
|
Definition
| the minimum energy required to remove an electron from an isolated atom (or an ion) in its ground state |
|
|
Term
|
Definition
| product of hydrogen ion concentration and hydroxide ion concentration (both in molarity) at a particular temp |
|
|
Term
|
Definition
| a system that does not allow the transfer of either mass or energy to or from its surroundings |
|
|
Term
|
Definition
| atoms having the same atomic number but different mass numbers |
|
|
Term
|
Definition
| unit of energy given by newtons X meters |
|
|
Term
|
Definition
see absolute temp scale
...a temp scale on which absolute zero (0k) is the lowest temp |
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|
Term
|
Definition
| compounds with a carbonyl functional group and the general formula RR'CO in wich R and R' are alkyl and /or aromatic hydrocarbon groups |
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|
Term
| kinetic energy (KE) energy available because of the motion of an object |
|
Definition
|
|
Term
| kinetic molecular theory of gases |
|
Definition
| a theory that describes the physical behavior of gases at the molecular level |
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Term
|
Definition
| complexes that undergo rapid ligand exchange reactions |
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Term
|
Definition
| elements that have incompletely filled 4f subshells or readily give rise to cations that hve incompletely filled 4f subshells |
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|
Term
|
Definition
| the energy required to completely separate one mole of a solid ionic compound into gaseous ions |
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Term
|
Definition
| the positions occupied by atoms, molecules, or ionst that define the geometry of a unit cell |
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|
Term
|
Definition
| a concise verbal or mathematical statement of a relationship between phenomena that is always the same under the same conditions |
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|
Term
| law of conservation of energy |
|
Definition
| the total quantity of energy in the univers is constant |
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|
Term
| law of conservation of mass |
|
Definition
| matter can be neither created nor destroyed |
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|
Term
| law of definite proportions |
|
Definition
| different smaples of teh same compoud always contain its constituent elements in the same proportions by mass |
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|
Term
| law of multiple prroportions |
|
Definition
| if two elements can combine to form more than one type of compound, the masses of one element that combine with a fixed mass of the other elemtne are in ratios of small whole numbers |
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Term
|
Definition
| if an extermal stress is applied to a system at equilibrium, the system will adjust itself in such a way as to partially offset the stress |
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Term
|
Definition
| a substance that can donate a pair of electrons |
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|
Term
|
Definition
| a substance that can donate a pair of electrons |
|
|
Term
|
Definition
| the symbol of an element with one or more dots that represent the number of valence electrons in an atom of the element |
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|
Term
|
Definition
| a representation of covalent bonding using lewis symbolys. shared electron pairs are shown either as lines or as pairs of dots between two atoms, and lone pairs are shown as pairs of dots on individual atoms |
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Term
|
Definition
| a molecule or an ion that is bonded to the metal ion in a complex ion |
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Term
|
Definition
| the reactant used up first in a reaction |
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Term
|
Definition
| spectrum produced when radiation is absorbed or emitted by a substance only at some wavelengths |
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Term
|
Definition
| the volume occupied by 1 cubic decimeter |
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Term
|
Definition
| valence electrons that are not involved in covalent bond formation |
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Term
|
Definition
| properties that can be measured directly |
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Term
|
Definition
| a device used to measure the pressure of gases |
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Term
|
Definition
| atoms that contain two or more electrons |
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|
Term
|
Definition
| a measure of the quantity of matter contained in an object |
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|
Term
|
Definition
| the difference between the mass of an atom and the sum of the masses of its protons, neutrons, and electrons |
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|
Term
|
Definition
| the total number of neutrons and protons present in the nucleus of an atom |
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|
Term
|
Definition
| anything that occupies space and possesses mass |
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Term
|
Definition
| the temp at whcih solid and liquid phases coexist in equilibrium |
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|
Term
|
Definition
| an element with properties intermediate between those of metals and nonmetals |
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|
Term
|
Definition
| elements that are good conductors of heat and electricity and have the tendency to form positive ions in ionic compounds |
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|
Term
|
Definition
| a reaction that involves the exchange of parts between two compounds |
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Term
|
Definition
| properties that must be measured indirectly with the aid of a microscope or other special instrument |
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|
Term
|
Definition
| two liquids that are completely soluble in each other in all proportions are said to be miscible |
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|
Term
|
Definition
| a combination of two or more substances in which the substances retain their identities |
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|
Term
|
Definition
| a substance that can reduce teh kinetic energy of neutrons |
|
|
Term
|
Definition
| the number of moles of solute dissolved in 1 kilogram of solvent |
|
|
Term
|
Definition
see molarity
...(M) the number of moles of solute in 1 liter of solution |
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|
Term
| molar heat of fusion (ΔHfus) |
|
Definition
| the energy (in kilojoules) required to melt 1 mole of a solid |
|
|
Term
| molar heat of sublimation (ΔHsub) |
|
Definition
| the energy (in kilojoules) required to vaporize 1 mole of a liquid |
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|
Term
| molar heat of vaporization (ΔHvap) |
|
Definition
| the energy (in kilojoules) required to baporize 1 mole of liquid |
|
|
Term
|
Definition
| the mass (in grams or kilograms) of 1 mole of atoms, molecules, or other particles |
|
|
Term
|
Definition
| the number of moles of solute in 1 liter of saturated solution (mol/L) |
|
|
Term
|
Definition
| the number of moles of solute in 1 liter of solution |
|
|
Term
|
Definition
| the amount of substance that contains as many elementary entities (atoms, molecules, or other particles) as there are atoms in exactly 12 grams (or 0.012 kilograms) of the carbon-12 isotope |
|
|
Term
|
Definition
| ratio of the number of moles of one component of mixture to the total number of moles of all components in the mixture |
|
|
Term
|
Definition
| an approach for determining the amount of product formed in a reaction |
|
|
Term
|
Definition
| equations in which the formulas of the compounds are written as though all species existed as molecules or whole units |
|
|
Term
|
Definition
| an expression showing the exact numbers of atoms of each element in a molecule |
|
|
Term
|
Definition
| the sum of the atomic masses (in amu) present in a given molecule |
|
|
Term
|
Definition
| an orbital that results from the interaction of atomic orbitals of the bonding atoms |
|
|
Term
| moleculartiy of a reactino |
|
Definition
| the number of molecules reating in an elementary step |
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|
Term
|
Definition
| an aggregate of at least two atoms in a definite arrangement held together by special forces |
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|
Term
|
Definition
| an ion that contains only one atom |
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|
Term
|
Definition
| simple repeating units in a polymer |
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|
Term
|
Definition
| each unit of the acid yields one hydgrogen ion |
|
|
Term
|
Definition
| bonds formed when two atoms share two or moe pairs of electrons |
|
|
Term
|
Definition
| the relation between teh emf of a galvanic cell and the standard emf and the concentrations of the oxidizing and reducing agents |
|
|
Term
|
Definition
| an equation that includes only the ionic species that actually take part in athe reaction |
|
|
Term
|
Definition
| a reaction between an acid and a base |
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|
Term
|
Definition
| a subatomic particle that bears no net electric charge. its mass is slightly greater than a proton's |
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|
Term
|
Definition
|
|
Term
|
Definition
| the noble gas that most nearly precedes the elemtne being considered; used in writing electron configurations |
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|
Term
|
Definition
| nonmetallic elemtnes in group 8A (He, Ne, Ar, Kr, We, and Rn) |
|
|
Term
|
Definition
| a point at which the amplitude of a wave is zero |
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|
Term
|
Definition
| a substance that, when dissolved in water, gives a solution that is not electrically conducting |
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|
Term
|
Definition
| elements that are usually poor conductors of heat and electricity |
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|
Term
|
Definition
| a molecule that does not possess a diple moment |
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|
Term
|
Definition
| does not have a measurable vapor pressure |
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|
Term
|
Definition
| the energy required to break up a nucleus into protons and neutrons |
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|
Term
|
Definition
| a self-sustaining sequence of nuclear fission reactions |
|
|
Term
|
Definition
| the process in which a heavy nucleus (mass number > 200) divides to form small nuclei of intermediate mass and one or more neutrons |
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|
Term
|
Definition
| the combining of small nuclei into larger ones |
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|
Term
|
Definition
| a reaction involving change in an atomic nucleus |
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|
Term
|
Definition
| the change undergone by a nucleus as a result of bonbardment by neutrons or other particles |
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|
Term
|
Definition
| high molar mass polymers that play an essential role in protein synthesis |
|
|
Term
|
Definition
| the repeating unit in each strand of a DNA molecule which consists of a base-deoxyribose-phosphate group |
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|
Term
|
Definition
| the cnetral core of an atom |
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|
Term
|
Definition
| an atom other than hydrogen tends to form bonds until it is surrounded by eight valence electrons |
|
|
Term
|
Definition
| a system that can exchange mass and energy (usually in the form of heat) with its surroundings |
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|
Term
|
Definition
| the branch of chem that deals w carbon compounds |
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|
Term
|
Definition
| the net movement of solvent molecules through a semipermeable membrane from a pure solvent or from a dilute solution to a more concentrated solution |
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|
Term
|
Definition
| the pressure required to stop osmosis |
|
|
Term
|
Definition
| the additional boltage required to cause electrolysis |
|
|
Term
|
Definition
| the number of charges an atom would have in a molecule if electrons were transferred completely in the direction indicatied by the difference in electronegativity |
|
|
Term
|
Definition
| the half-reaction that represents the loss of electrons in a redox process |
|
|
Term
|
Definition
see oxidation number
...the number of charges an atom would have in a molecule if electrons were transferred ckompletely in the direction indicated by the difference in electronegativity |
|
|
Term
| oxidation-reduction reaction |
|
Definition
see redox reaxtion
...a eraction in which there is either a transfer of electrons or change in teh oxidation number os the substances taking part in teh reaction |
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|
Term
|
Definition
| a substance that can accept electrons from another substaance or increase the oxidation number os another substance |
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|
Term
|
Definition
| an acid containing hydrogen, oxygen, and another elemetn (the central element) |
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|
Term
|
Definition
| an anion derived form an oxoacid |
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|
Term
|
Definition
| attracted to a magnet. a paramagnetic substance contains one or more unpaired electrons |
|
|
Term
|
Definition
| the pressure of one component in a mixture of gases |
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|
Term
|
Definition
| a pressure of on newton per square meter (1 N/m2) |
|
|
Term
| pauli exclusion principle |
|
Definition
| no two electrons in an atom can have the same four quantum numbers |
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|
Term
|
Definition
| the percent by mass of each element in a compound |
|
|
Term
|
Definition
| the ratio of ionized acid concentration at equilibrium tot he initial concentration of acid |
|
|
Term
|
Definition
| the ratio of the mass of a solute to the mass of the solution multiplied by 100% |
|
|
Term
|
Definition
| the ration of the actual yeild of a reaction to the theoretical yield, multiplied by 100% |
|
|
Term
|
Definition
| the horizontal row of the periodic table |
|
|
Term
|
Definition
| a tabular arrangement of the elements by similarities in properties and by increasing atomic number |
|
|
Term
|
Definition
| the negative logarithm of the hydrogen ion concentration in an aqueous solution |
|
|
Term
|
Definition
| a homogeneous part of a system that is in contact with other parts of the system but separated form them by a well-ddefined boundary |
|
|
Term
|
Definition
| transformation form one phase to another |
|
|
Term
|
Definition
| a diagramshowing the conditioins at which a substance exists as a solid, liquid, and vapor |
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|
Term
|
Definition
| a phenomenon in whcih electrons are ejected form the surface of certain metals exposed to light of at least a certain minimum frequency |
|
|
Term
|
Definition
|
|
Term
|
Definition
| an equilibrium in which only physical properties change |
|
|
Term
|
Definition
| any property of a substance that can be observed without transforming the substance into some other substance |
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|
Term
|
Definition
| a covalent bond formed by sideways overlapping orbitals; its electron density is concentrated above and below the plane of the nuclei of the bonding atoms |
|
|
Term
|
Definition
| a molecular orbital in wich the electron density is concentrated above and below the line joining the two nuclei of the bonding atoms |
|
|
Term
|
Definition
| a gaseous state of matter consisting of positive ions and electrons |
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|
Term
|
Definition
| in such a bond, the electrons spend more timein the vicinity of one atom than the other |
|
|
Term
|
Definition
| a molecule that possesses a dipole moment |
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|
Term
|
Definition
| the instrumetn for studying interaction between plane-polarized light and chiral molecules |
|
|
Term
|
Definition
| the ease with which the electron distribution in the atom (or molecule)can be distorted |
|
|
Term
|
Definition
| an ion that contains more that one atom |
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|
Term
|
Definition
| a molecule that consist of more than two atoms |
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|
Term
|
Definition
| a molecular compound distinguished by a high molar mass and made up of many repeating units |
|
|
Term
|
Definition
| a particle that has the same mass as the electron but bears a +1 charge |
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|
Term
|
Definition
| energy available by vertue of an object's position |
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|
Term
|
Definition
| an insoluble solid that separates fro a supersaturated solution |
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|
Term
|
Definition
| a reaction characterized by the formation of a precipitate |
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|
Term
|
Definition
| the closeness of agreement of two or more measurements of the same quantity |
|
|
Term
|
Definition
| force applied per unit area |
|
|
Term
|
Definition
| the substance formed as a result of a chemical reaction |
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|
Term
|
Definition
|
|
Term
|
Definition
| a subatomic particle having a single positive electric charge. the mass of a proton is about 1840 times that of an electron |
|
|
Term
|
Definition
| consisting of general observations about the system |
|
|
Term
|
Definition
| the determination of the types of ions present in a solution |
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|
Term
|
Definition
| comprising numbers obtained by various measurements of the system |
|
|
Term
|
Definition
| the smallest quantity of energy that can be emitted or absorbed in teh form of electromagnetic radiation |
|
|
Term
|
Definition
| numbers that describe the distribution of electrons in atoms |
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|
Term
|
Definition
| an equimolar mixture of two enantiomers |
|
|
Term
|
Definition
| energy transmitted in the form of waves |
|
|
Term
|
Definition
| the emission and transmission of energy through space in the form of particles and/or waves |
|
|
Term
|
Definition
| a species that contains an unpaired electron |
|
|
Term
|
Definition
| a sequence of nuclear reactions that ultimately result in thet formation of a stable isotope |
|
|
Term
|
Definition
| the spontaneous breakdown of a nucleus by the emission of particles and/or radiation |
|
|
Term
|
Definition
| the partial pressure of the solvent over a solution is given by the produce of teh vapor pressure of the pure solvent and teh mole fraction of the solvent in the solution |
|
|
Term
|
Definition
see lanthanide series
...elements that have incompletely filled 4f subshells or readily give ries to cations that have incompletely filled 4f subshells |
|
|
Term
|
Definition
see noble gases
...nonmetallic elemetns in group 8A (He, Ne, Ar, Kr, Xe, and Rn) |
|
|
Term
|
Definition
| proportionality constant relating reaction rate to the concentrations of reactants |
|
|
Term
|
Definition
| an expression relating teh rate of a reaction to the rate constant and teh concentrations of the reactants |
|
|
Term
|
Definition
| the slowest step in the sequence of steps leading to the formation of products |
|
|
Term
|
Definition
| the starting substances in a chemical reaction |
|
|
Term
|
Definition
| the sequence of elementary steps that leads to product formation |
|
|
Term
|
Definition
| the sum of the powers to which all reactant concentrations appearing in the rate law are raised |
|
|
Term
|
Definition
| a number equal to the ratio of product concentrations, each raised to the power of its stoichiometric coefficient at some point other than equilibrium |
|
|
Term
|
Definition
| the change in concentration of reactant or product with time |
|
|
Term
|
Definition
| a reaction in which there is either a transfer of electrons or a change in teh oxidation numbers of the substances taking part in teh reaction. also called oxidation-reduction reaction |
|
|
Term
|
Definition
| a substance that can donate electrons to another substance or decrease teh oxidation numbers in another substance |
|
|
Term
|
Definition
| the half-reaction that represents the gain of electrons in a redox process |
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|
Term
|
Definition
| elements in groups 1A through 7 A all of which have at least an incompletely filled s or p subshell of the highest principal quantum number |
|
|
Term
|
Definition
| the use of two or more lewis structures to represent a particular molecule |
|
|
Term
|
Definition
| one of two or more alternative lewis structures for a single molecule that cannot be described fully with a single lewis structure |
|
|
Term
|
Definition
| a reaction that can occur in both directions |
|
|
Term
|
Definition
|
|
Term
| root-mean-square (rms) speed (urms) |
|
Definition
| a measure of the average molecular speed at a given temp |
|
|
Term
|
Definition
| an ionic compound made up of a cation other than H+ and an anion other that OH- or O2- |
|
|
Term
|
Definition
| the reaction of the anion or cation or both of a salt with water |
|
|
Term
|
Definition
|
|
Term
|
Definition
| gydrocarbons that contain only single covalent bonds |
|
|
Term
|
Definition
| at a given temp, the solution that results when the maximum amount of a substacne has dissolved in a solvent |
|
|
Term
|
Definition
| a systematic approach to research |
|
|
Term
|
Definition
| a reaction whose reate depends on teh concentration of one reactnat raised to the second power or on teh concentration of two different reactants, each raissed to the first power |
|
|
Term
|
Definition
| a membrane that allows solvent molecules to pass through, but blocks the movement of solute molecules |
|
|
Term
|
Definition
| a conbalent bond formed by orbitals overlapping end-to-end; its electron density is concentrated betweent he nuclei of the bonding atoms |
|
|
Term
|
Definition
| a molecular orbital in which the electron density is concentrated around a line between the two nuclei of teh bonding atoms |
|
|
Term
|
Definition
| the number of meaningful digits in a measured or calculated quanitity |
|
|
Term
|
Definition
| two atoms held together by one electron pair are joined by a singel bond |
|
|
Term
|
Definition
| the maximum amt of solute that can be dissolved in a given quantity of solvent at a specific temp |
|
|
Term
|
Definition
| the product of teh molar concentrations of constituent ions, each raised to the power of its stoichiometric coefficient in the equilibrium equation |
|
|
Term
|
Definition
| the substance present in the smaller amount in a solution |
|
|
Term
|
Definition
| a homogeneous mixture of two or more substances |
|
|
Term
|
Definition
| the process in which an ion or molecule is surrounded by solvent molecules arranged in an ordered manner |
|
|
Term
|
Definition
| the substance present in the larger amount in a solution |
|
|
Term
|
Definition
| the amount of heat energy required to raise temp of one gram of substance by one degree C |
|
|
Term
|
Definition
| ions that are not involved in the overall reaction |
|
|
Term
|
Definition
| a list of ligands arranged in order of their abilities to split the d-orbital energies |
|
|
Term
| standard atmospheric pressuer (1atm) |
|
Definition
| the pressure that supports a column of mercury exactly 76 cm high at 0 degree C at sea level |
|
|
Term
|
Definition
| the difference of the standard reduction potentials of teh substance that undergoes reduction and teh substance that undergoes oxidation in a redox process |
|
|
Term
| standard enthalpy of formation (ΔH°f) |
|
Definition
| the heat change that results when 1 mole of a compound is formed from its elements in their standard states |
|
|
Term
| standard enthalpy of reaction (ΔH°rxn) |
|
Definition
| the enthalpy change that occurs when the reaction is carried out under standard-state conditions |
|
|
Term
| standard entropy of reaction (ΔS°rxn) |
|
Definition
| the entropy change when the reaction is carried out under standard-state conditions |
|
|
Term
| standard free energy of reaction (ΔG°rxn) |
|
Definition
| the free energy change when the reaction is carried out under standard-state conditions |
|
|
Term
| standard free energy of formation (ΔG°f) |
|
Definition
| the free-energy change when 1 mole of a compound is synthesized from its elements in their standart-state conditions |
|
|
Term
| standard reduction potential |
|
Definition
| the voltage measured as a reduction reaction occurs at the electrode when all solutes are 1 M and all gases are at 1 atm |
|
|
Term
|
Definition
| a solution of accurately known concentration |
|
|
Term
|
Definition
| the condition of 1 atm of pressure |
|
|
Term
| standard temperature and pressure (STP) |
|
Definition
|
|
Term
|
Definition
| a property that is determined by the state of the system |
|
|
Term
|
Definition
| the values of all pertinent macroscopic variables (for example, composition, volume, pressure, and temp) of a system |
|
|
Term
|
Definition
| compounds that are made up of the same types and numbers of atoms bonded together in the same sequence but with different spatial arrangements |
|
|
Term
|
Definition
| the exact molar amounts of reactants and products that appear in a balanced chemical equation |
|
|
Term
|
Definition
| the mass relationships among reactants and products in chemical reactions |
|
|
Term
|
Definition
| an acid that is a strong electrolyte |
|
|
Term
|
Definition
| a base that is a strong electrolyte |
|
|
Term
|
Definition
| a representation that shows how atoms are bonded ot one another in a molecule |
|
|
Term
|
Definition
| molecules that havet he same molecular formula but different structures |
|
|
Term
|
Definition
| the process in which molecules go directly from the solid phase into the vapor phase |
|
|
Term
|
Definition
| a form of matter that has a definite or constant composition (the number and type of basic units present) and distinct properties |
|
|
Term
|
Definition
| a solution that contains more of the solute than is present in a saturated solution |
|
|
Term
|
Definition
| the amount of energy required to stretch or increase the surface of a liquid by a unit area |
|
|
Term
|
Definition
| the rest of the univers outside a system |
|
|
Term
|
Definition
| any specific part of the universe that is of interest to us |
|
|
Term
|
Definition
| an elementarystep involving three molecules |
|
|
Term
|
Definition
| compounds consisting of three elements |
|
|
Term
|
Definition
| the amount of product predicted by the balanced equation when all of the limiting reagent has reacted |
|
|
Term
|
Definition
| a unifying principle that explains a body of facts and/or those laws that are based on them |
|
|
Term
|
Definition
| energy associated with the random motion of atoms and molecules |
|
|
Term
|
Definition
| the heating of the environment to temperatures that are harmful to its living inhabitants |
|
|
Term
|
Definition
| an equation that shows both the mass and enthalpy relations |
|
|
Term
|
Definition
| the study of heat changes in chemical reactions |
|
|
Term
|
Definition
| the scientific study of teh interconversion of heat and other forms of energy |
|
|
Term
|
Definition
| nuclear fusion reactions that occur at very high temperatures |
|
|
Term
| third law of thermodynamics |
|
Definition
| the entropy of a perfect crystalline substance is zero at the absolute zero of temperature |
|
|
Term
|
Definition
| the gradual addition of a solution af accurately known concentration to another solution of unkown concentration until the chemical reaction between the two solutions is complete |
|
|
Term
|
Definition
| isotopes, especially radioactive isotopes, that are used to trace the path of the atoms of an element in a chemical or biological process |
|
|
Term
|
Definition
| elements that have incompletely filled d subshells or readily give rise to cations that have incompletely filled d subshells |
|
|
Term
|
Definition
see activated complex
...the species temporarily formed by reactant molecules as a result of a collision before they form the product |
|
|
Term
|
Definition
| elements with atomic numbers greater than 92 |
|
|
Term
|
Definition
| a covalent bond in which two atoms share three pairs of electrons |
|
|
Term
|
Definition
| the point at which the vapor, liquid, and solid states of a substance are in equilibrium |
|
|
Term
|
Definition
| eaach unit of the acid yeilds three hydrogen ions |
|
|
Term
|
Definition
| an elementary step involving one molecule |
|
|
Term
|
Definition
| the basic repeating unit of the arrangement of atoms, molecules, or ions in a crystalline solid |
|
|
Term
|
Definition
| hydrocarbons that contain carbon-carbon double bonds or carbon-carbon triple bonds |
|
|
Term
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Definition
| a solution that contains less solute than it has the capacity to dissolve |
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Definition
| The outer electrons of an atom, which are the ones involved in chemical bonding |
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Definition
| The outermost electron-occupied shell of an atom, which holds the electrons that are usually involved in bonding |
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Term
Valence Shell Electron Pair Repulsion
(VSEPR) |
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Definition
| A model that accounts for the geometrical arrangements of shared and unshared electron pairs around a central atom in terms of the repulsive forces between electron pairs |
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Term
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Definition
| An equation that describes the relationships among P, V, n, and T for a nonideal gas |
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Term
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Definition
| The collectrive name for certain attractive forces between atoms and molecules, namely, dipole-dipole, dipole-induced dipole, and dispersion forces |
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Term
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Definition
| The escape of molecules from the surface of aliquid; also called evaporation |
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Term
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Definition
| A measure of a fluid's resistance to flow |
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Term
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Definition
| Having measurable vapor pressure |
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Term
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Definition
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Term
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Definition
| A vibrating disturbance by which energy is transmitted |
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Term
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Definition
| The distance between identical points on successive waves |
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Term
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Definition
| An acid that is a weak electrolyte |
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Term
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Definition
| A base that is a weak electrolyte |
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Term
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Definition
| The force that gravity exerts on an object |
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Term
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Definition
| Directed energy change resulting from a process |
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Term
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Definition
| The scattering of X rays by the units of a regular crystalline solid |
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