Term
|
Definition
| the temperature -273.15(degrees) celsius, given a value of zero in the Kelvin scale. |
|
|
Term
|
Definition
| the closeness of measurements to the correct or accepted value of the quantity measured. |
|
|
Term
|
Definition
| a compound whose color is sensitive to pH. |
|
|
Term
|
Definition
|
|
Term
|
Definition
| one of the 14 elements with atomic numbers from 90 (thorium, Th) through 103 (lawrencium, Lr) |
|
|
Term
|
Definition
| a transitional structure that results from an effective collision and that persists while old bonds are breaking and new bonds are forming. |
|
|
Term
|
Definition
| the minimum energy required to transform the reactants into an activated complex. |
|
|
Term
|
Definition
| a list of elements organized according to the ease with which the elements undergo certain chemical reactions |
|
|
Term
|
Definition
| the measured amount of a product obtained from a reaction |
|
|
Term
|
Definition
| a polymer formed by chain addition reactions between monomers that contain a double bond |
|
|
Term
|
Definition
| a reaction in which an atom or molecule is added to an unsaturated molecule and increases the saturation of the molecule |
|
|
Term
|
Definition
| an organic compund that contains one or more hydroxyl groups |
|
|
Term
|
Definition
| an organic compound in which a carbonyl group is attached to a carbon-atom chain |
|
|
Term
|
Definition
| one of the elements of Group 1 of the periodic table(lithium, sodium, potassium, rubidium, cesium, and francium) |
|
|
Term
|
Definition
| a solution in which a base has completely dissociated in water to yield aqueous OH- ions |
|
|
Term
|
Definition
| one of the elements of Group 2 of the periodic table( beryllium, magnesium, calcium, strontium, barium, and radium) |
|
|
Term
|
Definition
| a hydrocarbon that contains only single bonds |
|
|
Term
|
Definition
| a hydrocarbon that contains double covalent bonds |
|
|
Term
|
Definition
| a group of atoms that is formed when one hydrogen atom is removed from an alkane molecule |
|
|
Term
|
Definition
| an organic compound in which one or more halogen atoms- fluorine, chlorine, bromine, or iodine- are substituted for one or more hydrogen atom in a hydrocarbon |
|
|
Term
|
Definition
| a hydrocarbon with triple covalent bonds |
|
|
Term
|
Definition
| two protons and two neutrons bound together and emitted from the nucleus during some kinds of radioactive decay |
|
|
Term
|
Definition
| an organic compound that can be considered to be a derivative of ammonia, NH3 |
|
|
Term
|
Definition
| a solid in which the partivles are arranged randomly |
|
|
Term
|
Definition
| any species that can react as either an acid or a base |
|
|
Term
| angular momentum quantum number |
|
Definition
| the quantum number that indicated the shape of the orbital |
|
|
Term
|
Definition
|
|
Term
|
Definition
| the electrode where oxidation takes place |
|
|
Term
|
Definition
| a hydrocarbon with six-membered carbon rings and delocalized electrons |
|
|
Term
|
Definition
| a chemical compound that increases the concentration of hydrogen ions, H+, in aqueous solution |
|
|
Term
|
Definition
| a substance that increases the concentration of hydroxide ions, OH-, in aqueous solution |
|
|
Term
|
Definition
| bombarrdment of stable nuclei with charged and uncharged particles |
|
|
Term
|
Definition
| exactly equivalent to 760 mm Hg |
|
|
Term
|
Definition
| the smallest unit of an element that maintains the properties of that element |
|
|
Term
|
Definition
| a unit of mass that is exactly 1/12 the mass of a carbon-12 atom, or 1.660 540 * 10-27 kg |
|
|
Term
|
Definition
| a unit of mass that is exactly 1/12 the mass of a carbon-12 atom, or 1.660 540 * 10-27 kg |
|
|
Term
|
Definition
| one-half the distance between the nuclei of identical atoms that are bonded together |
|
|
Term
|
Definition
| an electron occupies the lowest- energy orbital that can receive it |
|
|
Term
|
Definition
| a process in which a substance acts s both an oxidizing agent and a reducing agent |
|
|
Term
|
Definition
| the weighted average of the atomic masses of the naturally occuring isotopes of an element |
|
|
Term
|
Definition
| equal volumes of gases at the same temperature and pressure contain equal numbers of molecules |
|
|
Term
|
Definition
| 6.022 1367 * 10(23); the number of particles in exactly one mole of a pure substance |
|
|
Term
|
Definition
| the stable nuclei cluster over a range of neutron- proton ratios |
|
|
Term
|
Definition
| a device used to measure atmospheric pressure |
|
|
Term
|
Definition
| the primary aromatic hydrocarbon |
|
|
Term
|
Definition
| an electron emitted from the nucleus during some kinds of radioactive decay |
|
|
Term
|
Definition
| an acid that contains only two different elements: hydrogen and one of the more-electronegative elements |
|
|
Term
|
Definition
| a compound composed of two different elements |
|
|
Term
| binding energy per nucleon |
|
Definition
| the binding energy of the nucleus divided by the number of nucleons it contains |
|
|
Term
|
Definition
| the conversion of a liquid as well as at its surface; occurs when the equilibrium vapor pressure of the liquid equals the atmospheric pressure |
|
|
Term
|
Definition
| the temperature at which the quilibrium vapor pressure of a liquid equals the atmospheric pressure |
|
|
Term
|
Definition
| the difference between the boiling point of a pure solvent, directly proportional to the molal concentration of the solution |
|
|
Term
|
Definition
| the energy require d to break a chemical bond and form neutral isolated atoms |
|
|
Term
|
Definition
| the distance between two bonded atoms at their minimum potential energy, that is, the average distance between two bonded atoms |
|
|
Term
|
Definition
| the volume of a fixed mass of gas varied inversely with pressure at constant temperature |
|
|
Term
|
Definition
| a molecule or ion that is a proton donor |
|
|
Term
| Bronsted-Lowry acid-base reaction |
|
Definition
| the transfer of protons from one reactant (the acid) to another (the base) |
|
|
Term
|
Definition
| a molecule or ion that is a proton acceptor |
|
|
Term
|
Definition
| a solution that can resist changes in pH |
|
|
Term
|
Definition
| a device used to measure the heat absorbed or released in a chemical or physical change |
|
|
Term
|
Definition
| the attraction of the surfac eof a liquid to the surface of a solid |
|
|
Term
|
Definition
| an organic compound that contains the carboxyl functional group |
|
|
Term
|
Definition
|
|
Term
|
Definition
| a substance that changes the rate if a chemical reaction without itself being permanently consumed |
|
|
Term
|
Definition
| the covalent binding of an element to itself to form chains or rings |
|
|
Term
|
Definition
| the electrode where reduction takes place |
|
|
Term
|
Definition
|
|
Term
|
Definition
| a reaction in which the material that starts the reaction is also one of the products and can start another reaction |
|
|
Term
|
Definition
| a physical change of a substance from one state to another |
|
|
Term
|
Definition
| a physical change of a substance from one state to another |
|
|
Term
|
Definition
| the volume of a fixed mass of gas at constant pressure varies directly with the Kelvin temperature |
|
|
Term
|
Definition
| any substance that has a definite composition |
|
|
Term
|
Definition
| any substance that has a definite composition |
|
|
Term
|
Definition
| any substance that has a definite composition |
|
|
Term
|
Definition
| a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together |
|
|
Term
|
Definition
| a change in which one or more substances are converted into different substances |
|
|
Term
|
Definition
| a representation, with symbols and formulas, of the identities and relative amounts of the reactants and products in a chemical reaction |
|
|
Term
|
Definition
| a state of balance in which the rate of a forward reaction equals the rate of its reverse reaction and the concentrations of its products and reactants remain unchanged |
|
|
Term
| chemical-equilibrium expression |
|
Definition
| the equation for the equilibrium constant, K |
|
|
Term
|
Definition
| a formula that indicated the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numerical subscripts |
|
|
Term
|
Definition
| the area of chemitry that is concerned with reaction rates and reaction mechanisms |
|
|
Term
|
Definition
| the ability of a substance to undergo a change that transforms it into a different substance |
|
|
Term
|
Definition
| a reaction in which one or more substances are converted into different substances |
|
|
Term
|
Definition
| the study of the composition, structure, and properties of matter and the changes it undergoes |
|
|
Term
|
Definition
| a small whole number that appears in front of a formula in a chemical reaction |
|
|
Term
|
Definition
| properties that depend on the concentration of solute particles but not on their identity |
|
|
Term
|
Definition
| the set of assumptions regarding collisions and reactions |
|
|
Term
|
Definition
| a mixture consisting of particles that are intermediate in size between those in solutions and suspensions forming mixtures known as colloid dipersions |
|
|
Term
|
Definition
| the relationship between the pressure, volume, and temperature of a fixed amount of gas |
|
|
Term
|
Definition
| a reaction in which a substance combines with oxygen, releasing a large amount of energy in the form of light and heat |
|
|
Term
|
Definition
| the phenomenon in which the addition of an ion common |
|
|
Term
|
Definition
| a reaction in which two or more substances combine to form a new compound |
|
|
Term
| composition stoichiometry |
|
Definition
| calculations involving the mass relationship of elements in compounds |
|
|
Term
|
Definition
| a substance that is made from the atoms of two or more elements that are chemically bonded |
|
|
Term
|
Definition
| a measure of the amount of solute in a given amount of solvent or solution |
|
|
Term
|
Definition
| the process by which a gas changes to a liquid |
|
|
Term
|
Definition
| a polymer formed by condensation reactions |
|
|
Term
|
Definition
| a reaction in which two molecules or parts of the same molecule combine |
|
|
Term
|
Definition
| the species that is formed when a Bronsted-Lowry base gains a proton |
|
|
Term
|
Definition
| the species that remains after a Bronsted-Lowry acid has given up a proton |
|
|
Term
|
Definition
| a neutron-absorbing rod that helps control a nuclear reaction by limiting the number of free neutrons |
|
|
Term
|
Definition
| a ratio derived from the equality between two different units that can be used to convert from one unit to the other |
|
|
Term
|
Definition
| a polymer made from two different monomers |
|
|
Term
|
Definition
| a chemical bond resulting from the sharing of an electron pair between two atoms |
|
|
Term
|
Definition
| the minimum amount of nuclide that providess the number of neutros needed to sustain a chain reaction |
|
|
Term
|
Definition
| indicates the critical temperature and critical pressure of a substance |
|
|
Term
|
Definition
| the lowest pressure at which a substance can exit as a liquid at the critical temperature |
|
|
Term
|
Definition
| the temperature above which a subtance cannot exist in the liquid state |
|
|
Term
|
Definition
| a substance in which the particles are arranged in an orderly, geometrix, repeating pattern |
|
|
Term
|
Definition
| the total three- dimensional arrangement of particles of a crystal |
|
|
Term
|
Definition
| a solid consisting of crystals |
|
|
Term
|
Definition
| an alkane in which the carbon atoms are arranged in a ring, or cyclic, structure |
|
|
Term
| Dalton's law of partial pressure |
|
Definition
| the total pressure of a mixture of gaes is equal to the sum of the partial pressures of the component gases |
|
|
Term
|
Definition
| a nuclide produced by the decay of a parent nuclide |
|
|
Term
|
Definition
| a series of radioactive nuclides producded by successive radioactive decay until a stable nuclide is reached |
|
|
Term
|
Definition
| a reaction in which a single compound produces two or more simpler substances |
|
|
Term
|
Definition
| an electron hared by more than two atoms |
|
|
Term
|
Definition
| the ratio of ma to volume or mas divided by volume |
|
|
Term
|
Definition
| the change of state from a gas directly to a solid |
|
|
Term
|
Definition
| a unit that is a combination of SI base units |
|
|
Term
|
Definition
| a colorless, crystalline, solid form of carbon |
|
|
Term
|
Definition
| a molecule containing only two atoms |
|
|
Term
|
Definition
| spontaneous mixing of the particles of two substances caused by their random motion |
|
|
Term
|
Definition
| equal but opposite charges that are separated by a short distance |
|
|
Term
|
Definition
| a force of attraction between polar molecules |
|
|
Term
|
Definition
| an acid that can donate two protons per molecule |
|
|
Term
|
Definition
| two quantities that give a constant value when one is divided by the other |
|
|
Term
|
Definition
| a reaction in which one element replaced a ssimilar element in a compound |
|
|
Term
|
Definition
| the separation of ions that occurs when an ionic compound dissolves |
|
|
Term
|
Definition
| a covalent bond produced by the sharing of two pairs of electrons between two atoms |
|
|
Term
| double-replacement reaction |
|
Definition
| a reaction in which the ions of two compounds exchange places in an aqueous solution to form two new compounds |
|
|
Term
|
Definition
| the ability of a substance to be drawn, pulled, or extruded through a small opening to produce a wire |
|
|
Term
|
Definition
| the rapid escape of a gas from the liquid in which it is dissolved |
|
|
Term
|
Definition
| a process by which gas particles under pressure pass trhough a tiny opening |
|
|
Term
|
Definition
| a collision between gas particles under pressure pass through a tiny opening |
|
|
Term
|
Definition
| a system of electrodess and electrolytes in which either chemical reaction produce electrical energy or an electric current produces chemical change |
|
|
Term
|
Definition
| the branch of chemitry that deals with electricity related applications of oxidation reduction reactions |
|
|
Term
|
Definition
| a conductor ued to establish electrical contact with a non metallic part of a circuit, such as an electrolyte |
|
|
Term
|
Definition
| the difference in npotential between an electrode and its solution |
|
|
Term
|
Definition
| the process in which an electric currrent is ued to produce an oxidation-reduction reaction; also the decomposition of a substance by an electric current |
|
|
Term
|
Definition
| a substance that dissolves in water to give a solution that conducts electric current |
|
|
Term
|
Definition
| an electrochemical cell in which electrical energy is required to produce a redox reaction and bring about a chemical change |
|
|
Term
| electromagnetic radiation |
|
Definition
| a form of energy that exhibits wavelike behavior as it travels through space |
|
|
Term
|
Definition
| all the forms of electromagnetic radiation |
|
|
Term
|
Definition
| the energy change that occurs when an electron is acquired by a neutral atom |
|
|
Term
|
Definition
| the process in which an inner orbital electron is captured by the nucleus of its own atom |
|
|
Term
|
Definition
| the arrangement of electrons in an atom |
|
|
Term
|
Definition
| an electron-configuration notation in which only the valence electrons of an towm of a particular element are shown, indicated by dots placed around the element's symbol |
|
|
Term
|
Definition
| measure of the ability of an atom in a chemical compound to attract electrons |
|
|
Term
|
Definition
| an electrolytic process in which a metal ion is reduced and olid metal is deposited on a surface |
|
|
Term
|
Definition
| a pure substance made of only one kind of atom |
|
|
Term
|
Definition
| a reaction in which a imple molecule, such as water or ammonis, is removed from adjacent carbon atoms of a larger molecule |
|
|
Term
|
Definition
| the symbols for the element comvined in a compound with suvscriiipts showing the smaller whole-number mole ratio of the different atoms in the compound |
|
|
Term
|
Definition
| the point in a titration at which an indicator changes color |
|
|
Term
|
Definition
| the heat ocntent of a system at constant pressure |
|
|
Term
|
Definition
| the amount of heat absorbed or lost by a ssustem during a process at constant pressure |
|
|
Term
|
Definition
| a measure of the degree of randomness of the particles, such as molecules, in a system |
|
|
Term
|
Definition
| a dynamis condition in which two opposing changes occur at equal rates in a closed system |
|
|
Term
|
Definition
| the ratio of the mathematical product of the centration of substances formed at quilibrium to the mathematical product of the concentration of the reacting substances. Each concentration is raised to a power equal to the coefficient of that substance in the chemical equation |
|
|
Term
| equilibrium vapor pressure |
|
Definition
| the pressure exerted by a vapor in quilibrium with its corresponding liquid at a given temperature |
|
|
Term
|
Definition
| the point at which the two solutions used in a titration are present in chemically equivalent amounts |
|
|
Term
|
Definition
| an organic compound with a carboxylic acid group in which the hydrogen of the hydroxyl group has been replaced by an alkyl group |
|
|
Term
|
Definition
| an organic compound in which two hydrocarbon groups are bonded to the same atom of oxygen |
|
|
Term
|
Definition
| the process by which particles escape from the surface of a nonboiling liquid and enter the gas state |
|
|
Term
|
Definition
| the substance that is not used up completely in a reaction |
|
|
Term
|
Definition
| a state in which an atom has a higher potential energy than it has in its ground state |
|
|
Term
|
Definition
| a property that depends on the amount of matter that is present |
|
|
Term
|
Definition
| a vertical column of the periodic table |
|
|
Term
|
Definition
| a device that uses exposure of film to measure the approximate radiation exposure of people working with radiations |
|
|
Term
|
Definition
| a substance than can flow and therefore takes the shape of its container, a liquid or a gas |
|
|
Term
|
Definition
| a representation of reactants and products of a chemical reaction by their symbols or formulas |
|
|
Term
|
Definition
| the sum of the average atomic masses of all the atoms represented in the formula of any molecule, formula, unit or ion |
|
|
Term
|
Definition
| the simplest cpllection of atoms from which an ionic compound's formula can be established |
|
|
Term
|
Definition
| distillation in which componenet of a mixture are separated on the basis of boiling point, by condensation of vapor in a fractionating column |
|
|
Term
|
Definition
| the combined enthalpy-entropy function of a system |
|
|
Term
|
Definition
| the difference between the change in enthalpy, (delta H, and the product of the Kelvin temperature and the entropy change, which is defined as T delta S, at a constant pressure and temperature |
|
|
Term
|
Definition
| the physical change of a liquid to a solid by the removal of heat |
|
|
Term
|
Definition
| the temperature at which a solid and liquid are in equilibrium at 1 atm(101.3 kPa) presure |
|
|
Term
| freezing-point depression |
|
Definition
| the difference between the freezing points of a pure solvent and a olution of a nonelectrolyte in that solvent; is directly proportional to the molal concentration of the solution |
|
|
Term
|
Definition
| the number of waves that pass a given point in a specific time, usually one second |
|
|
Term
|
Definition
| a dark-colored solid made of spherically networked carbon atom cages |
|
|
Term
|
Definition
| an atom or group of atoms that is responsible for the specific properties of an organic compound |
|
|
Term
|
Definition
| a high-energy electromagnetic wave emitted from a nucleus as it changes from an excited state to a ground energy state |
|
|
Term
|
Definition
| the state of matter in which a subtance has neither definite volume nor definite shape |
|
|
Term
|
Definition
| simple mathematical relationships between the volume, temperature, pressure, and quantity |
|
|
Term
|
Definition
| the pressure of a fixed mass of ga at constant voume varies directly eith the Kelvin temperature |
|
|
Term
| Gay-Lusac's law of ocmbining volumes and gases |
|
Definition
| at constant remperature and pressure, the volumes of gaseous reactants and products can be expressed as ratios of small whole numbers |
|
|
Term
|
Definition
| an instrument that detects radiation by counting electric pulses carried by gas ionized by radiation |
|
|
Term
|
Definition
| isomers in which the order of atom bonding is the same but the arrangement of atoms in space is different |
|
|
Term
|
Definition
| the rates of effusion of gases at the same temperature and pressure are inversely proportional to the squaure roots of their molar masses |
|
|
Term
|
Definition
| a soft, black, crystalline from of carbon that is a fair conductor of electricity |
|
|
Term
|
Definition
| the lowest energy state of an atom |
|
|
Term
|
Definition
| a vertical column of the periodic table |
|
|
Term
|
Definition
| a single electrode immersed in a solution of its ions |
|
|
Term
|
Definition
| the time required for half the atoms of a radioactive nuclide to decay |
|
|
Term
|
Definition
| the part of a reaction involving oxidation or reduction alone |
|
|
Term
|
Definition
| one of the elements of Group 17 (fluorine, chlorine, bromine, iodine, and astatine) |
|
|
Term
|
Definition
| the sum total of the kinetic energies of the particles in a sample of matter |
|
|
Term
|
Definition
| the sum total of the kinetic energies of the particles in a sample of matter |
|
|
Term
|
Definition
| heat released by the complete combustion of one mole of a substance |
|
|
Term
|
Definition
| the quantity of heat released or absorbed during a chemical reaction |
|
|
Term
|
Definition
| the amount of heat energy absorbed or released when a pecific amount of solute dissolves in a solvent |
|
|
Term
| heisenberg uncertainty principle |
|
Definition
| it is impossible to determine simultaneously both the position and velocity of an electron or any other particle |
|
|
Term
|
Definition
| the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid |
|
|
Term
|
Definition
| the overall enthalpy change in a reaction is equal to the sum of the enthalpy changes for the individual steps in the process |
|
|
Term
|
Definition
| a catalyst whose phase is different from that of the reactants |
|
|
Term
|
Definition
| a reaction involving reactants in two different phases |
|
|
Term
| highest occupied energy level |
|
Definition
| the electron-containing main energy level with the highest principal quantum number |
|
|
Term
|
Definition
| a reaction whose reactants and products exist in a single phase |
|
|
Term
|
Definition
| a series in which asjecent members differ by a constant unit |
|
|
Term
|
Definition
| orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electron sin a singly occupied orbitals must have the same spin |
|
|
Term
|
Definition
| orbitals of equial energy produced by the combination of two or more orbitals on the same atom |
|
|
Term
|
Definition
| the mixing of two or more atomic orbitals of similar energies on the same atom to produce new orbitals of equal energies |
|
|
Term
|
Definition
| a slution process with water as the solvent |
|
|
Term
|
Definition
| the simlest organic compound, composed of only carbon and hydrogen |
|
|
Term
|
Definition
| the intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule |
|
|
Term
|
Definition
| a reaction between water molecules and ions of a dissolved salt |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
| an imaginary gas that perfectly fills all the assumptions of the kinetic- molecular theory |
|
|
Term
|
Definition
| the constant R, 0.082 057 84 L atm/mol*K |
|
|
Term
|
Definition
| the mathematical relationhip of pressure, volume, temperature, and the number of moles of a gas |
|
|
Term
|
Definition
| liquid solutes and solvents that are not soluble in each other |
|
|
Term
|
Definition
| an electron that is not in the highest occupied energy level |
|
|
Term
|
Definition
| a property that does not depend on the amount of matter present |
|
|
Term
|
Definition
| a species that appears in some stps of a reaction but not in the net equation |
|
|
Term
|
Definition
| the force of attraction between molecules |
|
|
Term
|
Definition
| two quantities that have a constant mathematical product |
|
|
Term
|
Definition
| an atom orgroup of bonded atoms that has a positive or negative charge |
|
|
Term
|
Definition
| the chemical bond resulting from electrical attraction between large numbers of cations and anions |
|
|
Term
|
Definition
| a compound composed of positice and negative ions that are combined so that the numbers of poitive and negative charges are equal |
|
|
Term
|
Definition
| the formation of ions from solute molecules by the action of the solvent; any process that results in the formation of an ion |
|
|
Term
|
Definition
| the energy required to remove one electron form a neutal atom of an element |
|
|
Term
|
Definition
| compounds that have the same molecular formula but different structures |
|
|
Term
|
Definition
| atoms of the same elecemt that have different masses |
|
|
Term
|
Definition
| the SI unit of heat energy as well as all other forms of energy |
|
|
Term
|
Definition
| an organic compound in which a carbonyl group is attached to a carbon atom within the chain |
|
|
Term
| kinetic- molecular theory |
|
Definition
| a theory based on the idea that particles of matter are always in motion |
|
|
Term
| kinetic- molecular theory |
|
Definition
| a theory based on the idea that particles of matter are always in motion |
|
|
Term
|
Definition
| one of the 14 elements with atomic numbers from 58 (cerium, Ce) to 71 (lutetium,Lu) |
|
|
Term
| kinetic- molecular theory |
|
Definition
| a theory based on the idea that particles of matter are always in motion |
|
|
Term
| kinetic- molecular theory |
|
Definition
| a theory based on the idea that particles of matter are always in motion |
|
|
Term
|
Definition
| the energy released when on emole of an ionic crustalline compound is formed from gaseous ions |
|
|
Term
| law of conservation of mass |
|
Definition
| mass is neither created nor destroyed during ordinary chemical or physical reactions |
|
|
Term
| law of multiple proportions |
|
Definition
| a chemical compound contain the same element in exactly the same proportions by mass regardless of the size of the sample or the source of the compound |
|
|
Term
|
Definition
| when a system at equilibrium is disturbed by application of a stress, it attains a new equilibrium position that minimizes the stress |
|
|
Term
|
Definition
| an atom, ion, or molecule that accepts an electron pair to form a covalent bond |
|
|
Term
|
Definition
| the formation of one or more covalent bonds between an electron-pair donor and an electron-pair acceptor |
|
|
Term
|
Definition
| an aton, ion, or molecule that donates an electron pair to form a covalent bond |
|
|
Term
|
Definition
| a formula in whichi atomic symbols represent nuclei and inner-shell elctrons, dot-pairs or dashes between two atomic symbols represent electron pairs in covalent bonds, and dots adjacent to only one atomic symbol represent unshared electrons |
|
|
Term
|
Definition
| the reactant that limits the amounts of the other reactants that can combine- and the amount of product that can form- in a chemical reaction |
|
|
Term
|
Definition
| the state of matter in which the substance has a definite volume but an indefinite shape |
|
|
Term
|
Definition
| an intermolecular attraction resulting from the constant motion of electrons ans the creation of instateneous dipoles |
|
|
Term
|
Definition
| an intermolecular attraction resulting from the constant motion of electrons ans the creation of instateneous dipoles |
|
|
Term
|
Definition
| a pair of electrons that is not involved in bonding and that belongs exclusively to one atom |
|
|
Term
|
Definition
| the numbers of nucleons that represent completed nuclear energy levels-2,8,20,28,50,82, and 126 |
|
|
Term
|
Definition
| the quantum number that indicates the orientation of an orbital around the nucleus |
|
|
Term
|
Definition
| an element in the s-block or p-block |
|
|
Term
|
Definition
| the ability of a substance to be hammered or beaten into thin sheets |
|
|
Term
|
Definition
| a measure of the amount of matter |
|
|
Term
|
Definition
| the difference between the mass of an atom and the sum of the masses of its protons, nutreons, and electrons |
|
|
Term
|
Definition
| the total number of protons and electrons in the nucleus of an isotope |
|
|
Term
|
Definition
| anything that has mass and takes up space |
|
|
Term
|
Definition
| the physical change of a solid to a liquid by the addition of heat |
|
|
Term
|
Definition
| the temperature at which a solid becomes a liquid |
|
|
Term
|
Definition
| an element that is a good conductor of heat and electricity |
|
|
Term
|
Definition
| chemical bonding that results from the attraction between metal atoms and the surrounding sea of electrons |
|
|
Term
|
Definition
| an element that has osme characteritics of metals and some characteritics of nonmetals |
|
|
Term
|
Definition
| a common unit of pressure |
|
|
Term
|
Definition
| liquid solutes and solvents that are able to dissolve freely in one another in any proportion |
|
|
Term
|
Definition
| a blend of two or more kinds of matter, each of which retains it sown identity in any proportion |
|
|
Term
|
Definition
| an explanation of how phenomena occur and how data or events are related |
|
|
Term
|
Definition
| a material used op to sloow down the fast neutrons produced by fusion |
|
|
Term
| molal boiling-point constant |
|
Definition
| the boiling-point elevation of a solvent in a 1-molal solution of a non-volatile, nonelectrolyte solute |
|
|
Term
| molal freezing-point constant |
|
Definition
| the freezing-point depression of the solvent in a 1-molal solution of a non-volatile, nonelectrolyte solute |
|
|
Term
|
Definition
| the concentration of a solution expressed in moles of solute per kilogram of solvent |
|
|
Term
|
Definition
| the heat released or absorbed when one mole of a compound is formed by the combination of its elements |
|
|
Term
|
Definition
| the amount of heat energy required to melt one mole of solid at its melting point |
|
|
Term
| molal heat of vaporization |
|
Definition
| the amount of heat energy needed to vaporize one mole of liquid at its boiling point |
|
|
Term
|
Definition
| the mass of one mole of a pure subtance |
|
|
Term
|
Definition
| the number of moles of solute in one liter of solution |
|
|
Term
|
Definition
| the amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon |
|
|
Term
|
Definition
| a conversion factor that relates the amounts in moles of any two substances involved in a chemical reaction |
|
|
Term
|
Definition
| a chemical compound whose simplest units are molecules |
|
|
Term
|
Definition
| a formula showing the types and numbers of atoms combined in a single molecule of a molecular compound |
|
|
Term
|
Definition
| the uneven ditribution of molecular charge |
|
|
Term
|
Definition
| a neutral group of atoms that are held together by covalent bonds |
|
|
Term
|
Definition
| an ion formed from a sigle atom |
|
|
Term
|
Definition
| a small unit that joins with other to make a polymer |
|
|
Term
|
Definition
| an acid that can donate only one proton (hydrogen ion) per molecule |
|
|
Term
|
Definition
|
|
Term
|
Definition
| a fossil fuel composed primarily of alkanes containing one to four carbon atoms |
|
|
Term
|
Definition
| an equation that includes only those compounds and ions that undergo a chemical change in a reaction in aqueous solution |
|
|
Term
|
Definition
| the reaction of hydronium ions and hydroxide ions to form water molecules |
|
|
Term
|
Definition
| the SI unit for force; the force that will increae the speed of a one kilogram ma by one meter per second each second it is applied |
|
|
Term
|
Definition
| a Group 18 element(helium, neon, argon, krypton, xenon, and radon) |
|
|
Term
|
Definition
| an outer main energy level fullly occupied, in mot cases, by eight electrons |
|
|
Term
|
Definition
|
|
Term
|
Definition
| a substance that dissolves in water to give a solution that does not conduct an electric current |
|
|
Term
|
Definition
| an element that is a poor conductor of heat and electricity |
|
|
Term
|
Definition
| a covalent bond in which the bonding electrons are shared equally by the bodned atoms, resulting in a balanced distribution of electrical charge |
|
|
Term
|
Definition
| a substance that has little tendency to become a gas under existing conditions |
|
|
Term
|
Definition
| the energy released when a nucleus is formed from nucleons |
|
|
Term
|
Definition
| a process in which a heavy nucleus splite into more stable nuclei or intermediate mass |
|
|
Term
|
Definition
| a short-range proton-neutron, proton-proton, or neutron-neutron force that holds the nuclear particles together |
|
|
Term
|
Definition
| the combining of light mass nuclei to form a heavier, more stable nucleus |
|
|
Term
|
Definition
| a facility that uses heat from nuclear reactor to produce electrical energy |
|
|
Term
|
Definition
| the particles or electromagna=etic radiation emitted from the nucleus during radioactive decay |
|
|
Term
|
Definition
| a device that uses controlled-fission chain reactions to produce energy or radioactive nuclides |
|
|
Term
|
Definition
| nucleons exist in different energy levels, or shells, in the nucleus |
|
|
Term
|
Definition
|
|
Term
|
Definition
| the general term for any isotope of any element(77); another term for an atom that is identified by the number of protons and neutron in its nucleus |
|
|
Term
|
Definition
| a measure of a fuel's burning efficiency and its antiknock properties |
|
|
Term
|
Definition
| chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet of electrons in its highest occupied energy level |
|
|
Term
|
Definition
| a three- dimensional region around the nucleus that indicates the probable location of an electron |
|
|
Term
|
Definition
| a covlently bonded compound containing carbon, excluding carbonates and oxides |
|
|
Term
|
Definition
| the movement of solvent through a semipermeable membrane from the side of lower solute concentration to the side of higher solute concentration |
|
|
Term
|
Definition
| the external pressure that mut be applied to stop osmosis |
|
|
Term
|
Definition
| a reaction in which the atoms or ions of an element experience an increase in oxidation state |
|
|
Term
|
Definition
| a number assigned to an atom in a molecular compound or molecular ion that indicates the general distribution of electrons among the bonded atoms |
|
|
Term
| oxidation-reduction reaction |
|
Definition
| any chemical process in which elements undergo changes in oxidation number |
|
|
Term
|
Definition
| a number assigned to an atom in a molecular compound or ion that indicates the general distribution of electrons among the bonded atoms |
|
|
Term
|
Definition
| having experienced an increase in oxidation number |
|
|
Term
|
Definition
| a substance that has the potential to cause another substance to be oxidized |
|
|
Term
|
Definition
| an acid that is a compound of hydrogen, oxygen, and a third element, usually a non-metal |
|
|
Term
|
Definition
| a polyatomic ion that contains oxygen |
|
|
Term
|
Definition
| the negative of the common logarithm of the hydronium ion concentration of a solution |
|
|
Term
|
Definition
| a device used to determine the pH of a solution by measuring the voltage between the two electrodes that are placed in the solution |
|
|
Term
|
Definition
| the negative of the common logarithm of the hydroxide ion concentration of a solution |
|
|
Term
|
Definition
| the neaviest nuclide of each decay series |
|
|
Term
|
Definition
| the pressure of each gas in a mixture |
|
|
Term
|
Definition
| the pressure exerted by a force of one newton acting on an area of one square meter |
|
|
Term
| Pauli exclusion principle |
|
Definition
| no two electrons in the same atom can have the same set of four quantum numbers |
|
|
Term
|
Definition
| a value calculated by subtacting the experimental value from the accepted value, dividing from the difference of the accepted value, and then multiplying by 100 |
|
|
Term
|
Definition
| the ratio of the actual yield to the theoretical yield, multiplied by 100 |
|
|
Term
|
Definition
| the percentage by mass of each element in a compound |
|
|
Term
|
Definition
| a horizontal row of elements in the periodic table |
|
|
Term
|
Definition
| the physical and chemical properties of the elements are periodic function of their atomic numbers |
|
|
Term
|
Definition
| an arrangement of the elements in order of their atomic numbers so that elements with similar preperties fall in the same column, or group |
|
|
Term
|
Definition
| a complex mixture of different hydrocarnons that varies greatly in composition |
|
|
Term
|
Definition
| any part of a system that has unifrom composition and properties |
|
|
Term
|
Definition
| a graph of pressure versus temperature that shows the conditions under which the phases of a substance exist |
|
|
Term
|
Definition
| the emission of electons from a metal when light shines on the metal |
|
|
Term
|
Definition
| a particle of electromagnetic radiation that has zero rest mass and carries a quantum of energy |
|
|
Term
|
Definition
| a change in a substance that does not involve a change in identity of the substance |
|
|
Term
|
Definition
| a characteristic that can be observed or measured without changing the identity of the substance |
|
|
Term
|
Definition
| having an uneven distribution of charge |
|
|
Term
|
Definition
| a covalent bond in which the bonded atoms have an unequal attraction for the shared electrons |
|
|
Term
|
Definition
| a charged group of covalently bonded atoms |
|
|
Term
|
Definition
| a large molecule made of many small units joined to each other through organic reactions |
|
|
Term
|
Definition
| an acid that can donate more than one proton per molecule |
|
|
Term
|
Definition
| a particle that has the same mass as an electron but that has a positive charge, and is emitted from the nucleus during some kinds of radioactive decay |
|
|
Term
|
Definition
| a solid that is produced as a result of a chemical reaction in solution and that separates from the solution |
|
|
Term
|
Definition
| the closeness of a set of measurements of the same quantity made in the same way |
|
|
Term
|
Definition
| the force per unit area on a surface |
|
|
Term
|
Definition
| a highly purified solid compound ued to check the concentration of a known solution in a titration |
|
|
Term
|
Definition
| the quantum number that indicated the main energy level occupied by the electron |
|
|
Term
|
Definition
| a substance that is forned by a chemical change |
|
|
Term
|
Definition
| a substance that has a fixed composition and differs from a mixture in that every sample of a given pure substance has exactly the same characteristic properties and composition |
|
|
Term
|
Definition
| something that has magnitude, size, or amount |
|
|
Term
|
Definition
| the minimum quantity of energy that can be gained or lost by an atom |
|
|
Term
|
Definition
| a number that specifies the properties of atomic orbitals and the properties of electrons in orbitals |
|
|
Term
|
Definition
| a mathematical description of the wave properties of electrons and other very small particles |
|
|
Term
|
Definition
| the process by which the approximate age of an object is determined based on the maount of certain radioactive nuclides present |
|
|
Term
|
Definition
| the spontaneous disintegration of a nucleus into a slightly lighter and more stable nucleus, accompained by emission of particles, electromagnetic radiation, or both |
|
|
Term
|
Definition
| an unstable nucleus that undergoes radioactive decay |
|
|
Term
|
Definition
| an unstable nucleus that undergoes radioactive decay |
|
|
Term
|
Definition
| a radioactive atom that is incorporated into a substance so that movement of the substance can be followed by a radiationo detector |
|
|
Term
|
Definition
| the slowest rate step for a chemical reaction |
|
|
Term
|
Definition
| an equation that reacts in a chemical change |
|
|
Term
|
Definition
| the step-by-step sequence of reactions by which the overall chemical change occurs |
|
|
Term
|
Definition
| the change in concentration of reactants per unit time as a reaction proceeds |
|
|
Term
|
Definition
| calculations involving the mass relationships between reactant and products in a chemical reaction |
|
|
Term
|
Definition
| a gas that does not behave completelt according to the assumptions of the kinetic-molecular theory |
|
|
Term
|
Definition
| any chemical process in which the elements undergo changes in oxidation number |
|
|
Term
|
Definition
| having experienced a decreade in oxidation state |
|
|
Term
|
Definition
| a substance that has potential to cause another subtance to be reduced |
|
|
Term
|
Definition
| a reaction in which the oxidation state of an element decreases |
|
|
Term
|
Definition
| the measurement of the tendency for a half-reaction to occur as a resuction half-reaction in an electrochemical cell |
|
|
Term
|
Definition
| the quantity of ionizing radiation that does as much damage to human tissue as is done by 1 roentgen of high-voltage X rays |
|
|
Term
|
Definition
| the bonding in molecules or ions that cannot be correctly represented by a single Lewis structure |
|
|
Term
|
Definition
| the bonding in molecules or ions that cannot be correctly represented by a single Lewis structure |
|
|
Term
|
Definition
| a chemical reaction in which th eproducts re-from the origional reactants |
|
|
Term
|
Definition
| a unit used to measure nuclear radiation; equal to the amount of radiation that produces 2*10(9) ion pairs when it passes through 1 cm(3) of dry air |
|
|
Term
|
Definition
| an ionic compound composed of a cation and the anion from an acid(215); an ionic compound composed of a cation from a base and an anion from an acid |
|
|
Term
|
Definition
| a hydrocarbon in which each carbon atom in the molecule forms four single covalent bonds with other atoms |
|
|
Term
|
Definition
| a solution that contains the maximum amount of dissolved solute |
|
|
Term
|
Definition
| a logical approach to solving problems by obsercing and collecting data, formulating hypotheses, and formulating theories that are supported by data |
|
|
Term
|
Definition
| numbers written in the form M*10(n) where the factor M is a number greater than or qual to 1 but less than 10 and n is a whole number |
|
|
Term
|
Definition
| an instrument that converts scintillating light to an electic signal for detercting radiation |
|
|
Term
|
Definition
| an organic compound in which two hydrogen atoms of an ammonia molecule have been replaced by alkyl groups |
|
|
Term
|
Definition
| a process in which two water molecules produce a hydronium ion and a hydroxide ion by transfer of a proton |
|
|
Term
|
Definition
| a membrane that allows the movement of some particles while blocking the movement of others |
|
|
Term
|
Definition
| radiation-absorbing material that is used to decrease radiation exposure from nuclear reactors, especially gamma rays |
|
|
Term
|
Definition
| the measurement system accepted worldwide |
|
|
Term
|
Definition
| any digit in a measurement that is known with certainty plus one final digit, which is somewhat uncertain or is estimated |
|
|
Term
|
Definition
| a covalent bond produced by the sharing of one pair of electrons between two atoms |
|
|
Term
| single-replacement reaction |
|
Definition
| a reaction in which one element replaces a similar element in a compound |
|
|
Term
|
Definition
| the state of matter in which the substance has definite volume and definite shape |
|
|
Term
|
Definition
| the amount of a substance required to form a saturated solution with a specific amount of solvent at a specified temperature |
|
|
Term
| solubility product constant |
|
Definition
| the product of the molar concentrations of ions of a substance in a saturated solution, each raised to the power that is the coefficient of that ion in the chemical equation |
|
|
Term
|
Definition
| capable of being dissolved |
|
|
Term
|
Definition
| the substance dissolved in a solution |
|
|
Term
|
Definition
| a homogeneos mixture of two or more substances in a single phase |
|
|
Term
|
Definition
| the physical state in which the opposing processes of dissolution and crystallization of a solute occur at equal rates |
|
|
Term
|
Definition
| a solute particle that is surrounded by solvent molecules |
|
|
Term
|
Definition
| the dissolving medium in a solution |
|
|
Term
|
Definition
| the amount of heat energy requires to raise the temperature of one gram of substance by one celsius degree or one kelvin (1 K) |
|
|
Term
|
Definition
| an ion that does not take part in a chemical reaction and is found in solution both before and after the reaction |
|
|
Term
|
Definition
| the quantum number that has only two possible values, +1/2 and -1/2, which indicate the two fundamental spin states of an electron in an orbital |
|
|
Term
| standard electrode potential |
|
Definition
| a half cell potential measured relative toa potential of zero for the standard hydrogen electrode |
|
|
Term
| standard molar volume of a gas |
|
Definition
| the volume occupied by one mole of a gas at STP, 22.414 10 L |
|
|
Term
|
Definition
| a solution that contains a precisely known concentration of a solute |
|
|
Term
| standard temperature and pressure |
|
Definition
| the agreed-upon standard conditions of exactly 1 atm pressure and 0 degrees celsius |
|
|
Term
|
Definition
| an acid that ionizes completely in aqueous solution |
|
|
Term
|
Definition
| any compound of which all or almost all of the dissolved compound ezists as ions in aqueous solution |
|
|
Term
|
Definition
| a formula that indicated the number and types of atoms present in a molecule and also show the bonding arrangement and bonds but not the unshared electron pairs of the atoms in a molecule |
|
|
Term
|
Definition
| isomers in which the atoms ar ebonded together in different orders |
|
|
Term
|
Definition
| the change of state from a solid directly to a gas |
|
|
Term
|
Definition
| a reaction in which one or more atoms replace another atom or group of atoms in a molecule |
|
|
Term
|
Definition
| a substnace that retains certain liquid properties even at temperatures at which it appears to be solid |
|
|
Term
|
Definition
| a solution that ocntains more dissolved solute than a aturated solution ocntains under the same conditions |
|
|
Term
|
Definition
| a force that tends to pull adjacent parts of a liquid's surface together, thereby decreasing urface area to the smallest possible size |
|
|
Term
|
Definition
| a reaction in which two or more substances combine to form a new compound |
|
|
Term
|
Definition
| a specific portion of matter in a given region of space that has been selected for study during an experiment or observation |
|
|
Term
|
Definition
| a measure of the average kinetic energy of the particles in a sample of matter |
|
|
Term
|
Definition
| an organic compound in which all three hydrogen atoms of an ammonia molecule have been replaced by alkyl groups |
|
|
Term
|
Definition
| the maximum amount of product that can be produced from a gicen amount of reactant |
|
|
Term
|
Definition
| a broad generalization that explains a body of facts or phenonema |
|
|
Term
|
Definition
| an equation that includes the quantity of heat released or absorbed during the reaction a written |
|
|
Term
|
Definition
| the study of the changes in heat energy that accompany chemical reactions and physical changes |
|
|
Term
|
Definition
| a polymer that melts when heated and can be reshaped many times |
|
|
Term
|
Definition
| a polymer that does not melt when heated but keeps its origional shape |
|
|
Term
|
Definition
| the controlled addition and measurement of the maount of a solution of known concentration required to react completely with a measured amount of a solution of unknown concentration |
|
|
Term
|
Definition
| one of the d-block elements that is a metal, with typical metallic properties |
|
|
Term
|
Definition
| the pH range over which an indicator changes color |
|
|
Term
|
Definition
| a change in the identity of a nucleus as a result of a change in the number of its protons |
|
|
Term
|
Definition
| an element with more than 92 protons in its nucleus |
|
|
Term
|
Definition
| a covalent bond produced by the sharing of three pairs of electrons between two atoms |
|
|
Term
|
Definition
| the temperature and pressure conditions at which the solid, liquid, and vapor of a substance can coexist at equilibrium |
|
|
Term
|
Definition
| an acid able to donate three protons per molecule |
|
|
Term
|
Definition
| the smallest portion of a crystal lattice that shows the three dimensional pattern to the entire lattice |
|
|
Term
|
Definition
| a hydrocarbon in which not all carbon have four single covalent bonds |
|
|
Term
|
Definition
| a solution that contains less solute than a aturated solution under the existing conditions |
|
|
Term
|
Definition
| a pair of electrons that is not involved in bonding and that belongs exclusively to one atom |
|
|
Term
|
Definition
| an electron that is aveilable to be lost, gained, or shared in the formation of chemical compounds |
|
|
Term
|
Definition
| the proces by which a liquid or solid changes to a gas |
|
|
Term
|
Definition
| a liquid that evaporates readily |
|
|
Term
|
Definition
| an electrochemical cell in which the redox reaction occurs naturally and produces electrical energy |
|
|
Term
|
Definition
| the amount of space occupied by an object |
|
|
Term
|
Definition
| repulsion between the sets of valence-level electrons surrounding an atom causes there sets to be oriented as far apart as possible |
|
|
Term
|
Definition
| a corss-linking process between adjacent polyioprene molecules that occurs when the molecules are heated with sulfur atoms |
|
|
Term
|
Definition
| the distance between corresponding points on adjacent waves |
|
|
Term
|
Definition
| an acid that is a weak electrolyte |
|
|
Term
|
Definition
| a compound of which a relatively small amount of the dissolved compound ezists as ions in an aqueous solution |
|
|
Term
|
Definition
| a measure of the gravitational pull on matter |
|
|
Term
|
Definition
| an equation in which the reactants and productss in a chemical reaction are represented by words |
|
|
