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Chemistry Terms 1
| Question | Answer |
|---|---|
| absolute sero | The lowest possible temperature, written as 0 Kelvin or -273 degrees celsius |
| accuracy | The closeness of a measurement to an accepted value |
| activated Complex | The intermediate statebetween reactants and products in a chemical reaction; the peak of the potential energy diagram |
| addition polymerization | The joining of unsaturated monomers by a series of addition reactions. |
| addition reaction | The process in which a substance reacts across a double or triple bond in an organic compound. |
| alcohol | An organic compound containing a hydroxyl (-OH) group. |
| aldehyde | An organic compund containing a carbonyl group with at least one hydrogen atom attached to the carbonyl carbon. |
| alkali metal | Any group 1 element, excluding hydrogen. |
| alkaline earth element | Any group 2 element. |
| alkane | A hydrocarbon containing only single bonds between adjacent carbon atoms. |
| alkene | A hydrocarbon containing one double bond between two adjacent carbon atoms. |
| alkyl group | An open-chained hydrocarbon less one hydrogen atom; for example, CH3=methyl group, C2H5=ethyl group. Unspecified alkyl groups are designed by the letter R. |
| alkyne | A hydrocarbon containing one triple bond between two adjacent carbon atoms. |
| allotrope | A specific form of an element that can exist in more than one form; graphite and diamond are allotropes of the element carbon. |
| alloy | A solid metallic solution. |
| alpha decay | The radioactive process in which an alpha particle is emitted. |
| alpha particle | A helium-4 particle. |
| amide | An organic compound containing the CONH2 functional group. |
| amine | A hydrocarbon derivative containing an amino group. |
| amino acid | An organic compound containing an amino group. |
| anhydrous | Pertaining to a compound from which the water of crystallization has been removed. |
| anode | The electrode at which oxidation occurs. |
| aqueous | Pertaining to a solution in which water is the solvent. |
| aromatic hydrocarbon | Any ring hydrocarbon whose electronic structure is related to that of benzene. |
| arrenhius acid | Any substance that releases H+ ions in water. |
| arrenhius base | Any substance that releases OH- ions in the water. |
| atmospheric pressure | 1 standard atmospheric (atm)= 101.3 kilopascals. |
| atom | The basic unit of an element. |
| atomic mass | The weighted average of the masses of the isotopes of an element. |
| atomic mass unit (u) | One-twelfth the mass of a carbon-12 atom. |
| atomic number | The number of protons in the nucleus of an atom; the atomic number defines the element. |
| atomic radius | A measure of the size of an atom. |
| Avogadro's hypothesis | Equal volumes of gases, measured at the same temperature and pressure, contain equal numbers of particles. |
| Avogadro's numbers | The number of particles in 1 mole; 6.02 x 10^23. |
| battery | A commercial Voltaic cell. |
| benzene | C6H6; the parent hydrocarbon of all aromatic compounds. |
| beta decay | The radioactive process in which a beta particle is emitted. |
| beta (-) particle | An electron. |
| beta (+) particle | A positron. |
| binary compound | A compound containing two elements. |
| binding energy | The energy released when a nucleus is assembled from its nucleus. |
| boiling | The transition of liquid to gas; boiling occurs when the vapor pressure of a liquid equals the atmospheric pressure above the liquid. |
| boiling point | The temperature at which boiling occurs; the temperture at which liquid and vapor phases of a substance are in equilibrium. |
| boiling point elevation | The increase in the boiling point of a solvent due to the presence of solute particles. |
| bond energy | The energy needed to break a chemical bond. |
| Boyle's law | At constant temperature and mass, the pressure of an ideal gas is inversely proportional to it's volume; P1V1=P2V2. |
| breeder reactor | A fission reactor that generates it's own nuclear fuel. |
| bright-line spectrum | The lines of visible light emitted by elements as electrons fall to lower energy levels. |
| Bronsted-Lowry acid | A substance that can donate H+ ions. |
| Bronsted Lowry-base | A substance that can accept H+ ions. |
| carbonyl group | The functional group characteristic of aldehydes and ketones; C=O. |
| carboxyl group | The functional group characteristics of organic acids; -COOH. |
| catalyst | A substance that speeds a chemical reaction by lowering the activation energy of the reaction. |
| cathode | The electrode at which reduction occurs. |
| celsius (C) scale | The temperature scale on which the freezing and boiling points of water (at 1 atm) are set at 0 and 100, respectively. |
| chain reaction | A chemical or nuclear reaction in which one step supplies energy or reactants for the next step. |
| Charles's law | At constant pressure and mass, the volume of an ideal gas is directly proportional to the Kelvin temperature. V1/t1=V2/T2 |
| chemical bond | The stabilizing of two atoms by sharing or transferring electrons. |
| chemical equation | A shorthand listing of reactants, products and molar quantities in a chemical reaction. |
| chemical equilibrium | The state in which the rates of the forward reaction and reverse reaction are equal. |
| coefficient | A number in a chemical reaction that indicates how many particles of a reactant or product are required or formed in the reaction. |
| colligative property | A property that depends on the number of particles present rather than the type of particle. |
| combined (ideal) gas law | At constant mass, the products of the pressure and volume divided by the Kelvin temperature is constant; P1V1/T1=P2V2/T2. |
| compound | A combination of two or more elements with a fixed quantity of solute. |
| concentrated | Pertaining to a solution that contains a relatively large quantity of solute. |
| concentration | The "strength" of a solution; the quantity of solute relative to the quantity of solvent. |
| condensation | The change from gas to liquid. |
| condensation polymerization | The joining of monomers by a series of dehydration reactions. |
| condensation polymerization | The joining of monomers by a series of dehydration reactions. |
| control rod | The part of a fission reactor that controls the rate of fission by absorbing neutrons. |
| coordinate covalent bond | A single covalent bond in which the pair of electrons is supplied by one atom. |
| covalent bond | A chemical bond formed by the sharing of electrons. Between nonmetals to nonmetals. |
| cracking | The process of breaking large hydrocarbon molecules into smaller ones in order to increase yield of compounds such as gasoline. |
| crystal | A solid whose particles are arraged in a regulary repeating pattern. |
| decomposition | A reaction in which a compound forms two or more simpler substances. |
| density | Mass per unit volume; d=m/v. |
| deposition | The direct transition from gas to solid. |
| deuterium | The isotope of hydrogen with a mass number of 2. |
| diatomic molecule | A neutral particle consisting of two atoms; Br2 and CO are diatomic molecules. |
| diffusion | The movement of one substance through another. |
| dihydroxy alcohol | An organic compound with two hydroxyl groups. |
| dilute | (adj)Pertaining to a solution that contains a realtively small quantity of solute; (verb) to reduce the concentration of a solution by adding solvent. |
| dipole | An unsymmetrical charge distribution in a neutral molecule. |
| dipole-dipole attraction | The attractive force between two oppositely charged dipoles of neighboring polar molecules. |
| dissociation | The seperation of an ionic compound in a solution into positive and negative ions. |
| distillation | The simultaneous boiling of a liquid and condensation of it's vapor. |
| double bond | A covalent bond in which two pairs of electrons are shared by two adjacent atoms. |
| ductility | The property of a substance that allows it to be drawn into a wire; metallic substances possess ductility. |
| dynamic equilibrium | The state in which the rates of opposing processes are equal. |
| electrochemical cell | A device that produces usable electrical energy from a spontaneous redox reaction. |
| electrode | A conductor in a electrochemical or electrolytic cell that serves as the site of oxidation or reduction. |
| electrolysis | A nonspontaneous redox reaction driven by an external source of electricity. |
| electrolyte | A substance whose aqueous solution conducts electricity. |
| electrolytic cell | A device for carrying out electrolysis. |
| electron | The elementary unit of negative charge. |
| electronegativity | The measure of an atom's attraction for a bonded pair of electrons. |
| electroplating | The use of an electric current to deposit a layer of metal on a negatively charged object. |
| element | A substance all of whose atoms have the same atomic number. |
| empirical formula | A formula in which the elements are present in the smallest whole-number ratio; NO2 is a empirical formula, C2H4 is not. |
| endothermic reaction | A reaction that absorbs energyp; delta H is positive for an endothermic reaction. |
| end point | The point in a titration that signals that equilvalent quantities of reactions have been added. |
| energy | A quantity related to an object's capacity to do work. |
| enthalpy change (delta H) | The heat energy absorbed or released by a system at constant pressure. |
| entropy (S) | The measure of the randomness or disorder of a system. |
| entropy change (delta S) | An increase or decrease in the randomness of a system. |
| ester | The organic product of esterficaiton. |
| esterification | The reaction of an acid with an alcohol to produce an ester and water. |
| ethanoic acid | CH3COOH; acetic acid. |
| ethanol | CH3CH2OH; ethyl (grain) alcohol. |
| ethene | C2H4; ethylene; the partner of the alkene family of hydrocarbons. |
| ether | An organic compound containing the arrangement R-O-R. |
| ethyne | C2H2; acetylene; the parent of the alkyne family of hydrocarbons. |
| evaporation | The surface transition of liquid to gass |
| excted state | A condition in which one or more electrons in an atom are no longer in the lowest possible energy state. |
| exothermic reaction | A reaction that releases energy; delta H is negative for an exothermic reaction. |
| fermentation | The (anaerobic) oxidation of a sigar such as glucose to produce ethanol and carbon dioxide; the reaction is catalyzed by enzymes. |
| filtration | A method of seperating liquid from the particles suspended in it. |
| first ionization energy | The quantity of energy needed to remove the most loosely held electron from an isolated neutral atom. |
| fission | A nuclear reaction in which a heavy nuclide splits to form lighter nuclides and energy. |
| fission reactor | A device for producing electrical energy by means of a controlled fission reaction. |
| formula mass | The sum of the masses of the atoms in a formula; units are atomic mass units (u) or grams per mole (g/mol). |
| fractional distillation | The seperation of organic substances based on differences in their boiling points. |
| freezing | The transition from liquid to solid. |
| freezing point | The temperature at which freezing occurs. |
| freezing point depression (lowering) | The decrease in the freezing point of a solvent due to the presence of solute particles. |
| fuel rod | The part of a nuclear reactor that contains the fissionable material. |
| functional group | An atom or a group of atoms that confers specific properties on a organic molecule. |
| fusion | A synonym for melting; also, a nuclear process in which light nuclides join to form heavier nuclides and produce radiant energy. |
| fusion reactor | An experimental device for producing a controlled fusion reaction and generating electrical energy from it. |
| gas | The phase in which matter has neither definite shape nor definite volume. |
| gram-atomic mass | The molar mass of an element expressed in grams per mole (g/mol). |
| gram-molecular mass | The molar mass of a molecule. |
| ground state | The electron configuration of an atom in the lowest energy state. |
| group | The elements within a single vertical column of the Periodic Table. |
| half-cell | The pary of an electrochemical cell in which oxidation or reduction occurs. |
| half-life | The time needed for a substance to decay to one-half its initial mass. |
| half-reaction | The oxidation or reduction portion of a redox reaction. |
| halogen | An element in Group 17of the Periodic Tablep; F, Cl, Br, I. |
| heat energy | The energy released or absorbed by a system undergoing a change in temperature, in phase, or in composition. |
| heat of fusion | The heat energy absorbed when a unit mass of liquid changes to gas at its boiling point. |
| heat of reaction | The heat absorbed when or released as a result of a chemical reaction. |
| heat of vaporization | The heat energy absorbed when a unit mass of liquad changes to a gas at it's boiling point. |
| heavy water | A molecule of water in which the hydrogen atoms have a mass number of 2; deuterium oxide. |
| heterogeneous mixture | A nonuniform mixture. |
| homogeneous mixture | A mixture with a uniform distribution of particles; a solution is one example. |
| homologous series | A group of organic compounds with related structures and properties; each successive member of the series differs from the onw before it by a specific number of carbon and hydrogen atoms (usually CH2. |
| hydrate | A crystalline compound that has water molecules incorporated into it's crystal structure; common examples include CuSO4 5H2O and Na2SO4 * 10H2O. |
| hyrdration | The associationof water molecules with an ion or another molecule. |
| hydride | A binary compund of an active metal and hydrogen; the molecule. |
| hydrocarbon | An organic compound composed of carbon and hydrogen. |
| hydrogen bond | An unusually strong intermolecular attraction the results when hydrogen is bonded to a small, highly electronegative atome such a F,O or N. H-FON. |
| hydrolysis | A reaction in which a water molecule breaks a chemical bond; the reaction between certain salts and water to produce an excess of hydronium or hydroxide. |
| hydronium ion | H3O+; the conjugate acid of H2O; responsible for acidic properties in water solutions. |
| hydroxide ion | OH-; the conjugate base of H2O; responsible for basic properties in water solutions. |
| ideal gas | A model of gas in which the particles have no volume, do not attract or repel each other, and collide without the loss of energy; real gases approximate ideal gas behavior under conditions of low pressure and high temperature. |
| ideal gas law | The relationship obeyed by an ideal gas. |
| indicator | A substance that undergoes a color chane to signal a change in chemical conditions; acid-base indicators change color over specified pH ranges. |
| inert (noble) gas | An element in Group 18 of the Periodic Table; Ne, Ar, Kr, Xe, Rn. |
| inorganic compound | A compound that is not a hydrocarbon derivative. |
| ion | A particle in which the numbers of the protons and electrons are not equal. |
| ion-dipole attraction | The attractive force between an ion and the oppositely charged dipole of a neighboring polar molecule. |
| ionic bond | The electrostatic attraction of positive and negative ions in an ionic compound. |
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