Chemistry Terminology化学术语

BMA004

Absolute Entropy (of a substance)
The increase in the entropy of a substance as it goes from a perfectly ordered crystalline form at 0 °K (where its entropy is zero) to the temperature in question.
Absolute Zero
The zero point on the absolute temperature scale; -273.15°C or 0 K; theoretically， the temperature at which molecular motion ceases.
Absorption Spectrum
Spectrum associated with absorption of electromagnetic radiation by atoms (or other species) resulting from transitions from lower to higher energy states.
Accuracy
How closely a measured value agrees with the correct value.
Acid
A substance that produces H+(aq) ions in aqueous solution. Strong acids ionize completely or almost completely in dilute aqueous solution. Weak acids ionize only slightly.
Acid Anhydride
The oxide of a nonmetal that reacts with water to form an acid.
Acid Anhydride
Compound produced by dehydration of a carbonic acid; general formula is R--C--O--C--R
Acidic Salt
A salt containing an ionizable hydrogen atom; does not necessarily produce acidic solutions.


Activation Energy
Amount of energy that must be absorbed by reactants in their ground states to reach the transition state so that a reaction can occur.
Active Metal
Metal with low ionization energy that loses electrons readily to form cations.
Activity (of a component of ideal mixture)
A dimensionless quantity whose magnitude is: equal to molar concentration in an ideal solution; equal to partial pressure in an ideal gas mixture; and defined as 1 for pure solids or liquids.
Activity Series
A listing of metals (and hydrogen) in order of decreasing activity
Actual Yield
Amount of a specified pure product actually obtained from a given reaction. Compare with Theoretical Yield.
Actinides
Elements 90 to 103 (after actinium)
Acyl Group
Compound derived from a carbonic acid by replacing the --OH group with a halogen (X)， usually --Cl; general formula is O R--C--X
Addition Reaction
A reaction in which two atoms or groups of atoms are added to a molecule， one on each side of a double or triple bond
Adhesive Forces
Forces of attraction between a liquid and another surface.
Adsorption
Adhesion of a species onto the surfaces of particles
Alcohol
Hydrocarbon derivative containing an --OH group attached to a carbon atom not in an aromatic ring.
Aldehyde
Compound in which an alkyl or aryl group and a hydrogen atom are attached to a carbonyl group and a hydrogen atom are attached to a carbonyl group; general formula， O-R-C-H
Alkali Metals
Metals of Group IA (Na， K， Rb).
Alkaline Battery
A dry cell in which the electrolyte contains KOH.
Alkaline Earth Metals
Group IIA metals
Alkenes (Olefins)
Unsaturated hydrocarbons that contain one or more carbon-carbon double bonds.
Alkyl Group
A group of atoms derived from an alkane by the removal of one hydrogen atom.
Alkylbenzene
A compound containing an alkyl group bonded to a benzene ring.
Alkynes
Unsaturated hydrocarbons that contain one or more carbon-carbon triple bonds.
Allotropes
Different forms of the same element in the same physical state.
Allotropic Modifications (Allotropes)
Different forms of the same element in the same physical state.
Alloying
Mixing of metal with other substances (usually other metals) to modify its properties.
Alpha Particle
A helium nucleus.
Alpha (a) Particle
Helium ion with 2+ charge; an assembly of two protons and two neutrons.
Alums
Hydrated sulfates of the general formula M+M3+(SO4)2.12H2).
Amide
Compound containing the O-C-N group.
Compound that can be considered a derivative of ammonia in which one or more hydrogens are replaced by a alkyl or aryl groups.
Amine
Derivatives of ammonia in which one or more hydrogen atoms have been replaced by organic groups.
Amine Complexes
Complex species that contain ammonia molecules bonded to metal ions.
Amino Acid
Compound containing both an amino and a carboxylic acid group.The --NH2 group.
For more information see:Amino Acids
Amorphous Solid
A noncrystalline solid with no well-defined ordered structure.
Ampere
Unit of electrical current; one ampere equals one coulomb per second.


Amphiprotism
Ability of a substance to exhibit amphiprotism by accepting donated protons.
Amphoterism
The ability to react with both acids and bases.
Ability of substance to act as either an acid or a base.
Anion
A negative ion; an atom or goup of atoms that has gained one or more electrons.
Anode
In a cathode ray tube， the positive electrode.
Electrode at which oxidation occurs.
Antibonding Orbital
A molecular orbital higher in energy than any of the atomic orbitals from which it is derived; lends instability to a molecule or ion when populated with electrons; denoted with a star (*) superscript or symbol.
Aromatic Hydrocarbons
Benzene and its derivatives.
Artificial Transmutation
An artificially induced nuclear reaction caused by the bombardment of a nucleus with subatomic particiles or small nucei.
Aryl Group
Group of atoms remaining after a hydrogen atom is removed from the aromatic system.


Associated Ions
Short-lived species formed by the collision of dissolved ions of opposite charges.
Atmosphere
A unit of pressure; the pressure that will support a column of mercury 760 mm high at 0 °C.
Atom
The smallest particle of an element
Atomic Mass Unit (amu)
One twelfth of a mass of an atom of the carbon-12 isotope; a unit used for stating atomic and formula weights; also called dalton.
Atomic Number
Integral number of protons in the nucleus; defines the identity of element.
Atomic Orbital
Region or volume in space in which the probability of finding electrons is highest.
Atomic Radius
Radius of an atom.
Atomic Weight
Weighted average of the masses of the constituent isotopes of an element; The relative masses of atoms of different elements.


Aufbau ('building up') Principle
Describes the order in which electrons fill orbitals in atoms.
Autoionization
An ionization reaction between identical molecules.
Avogadro's Law
At the same temperature and pressure， equal volumes of all gases contain the same number of molecules.


Avogadro's Number
The number (6.022x10^23) of atoms， molecules or particles found in exactly 1 mole of substance.


Background Radiation
Ratiation extraneous to an experiment. Usually the low-level natural radiation form cosmic rays and trace radioactive substances present in our environment.

Band
A series of very closely spaced， nearly continuous molecular orbitals that belong to the crystal as a whole.

Band of Stability
Band containing nonradioactive nuclides in a plot of number of neutrons versus atomic number.

Band Theory of Metals
Theory that accounts for the bonding and properties of metallic solids.

Barometer
A device for measuring pressure.

Base
A substance that produces OH (aq) ions in aqueous solution. Strong soluable bases are soluble in water and are completely dissociated. Weak bases ionize only slightly.

Basic Anhydride
The oxide of a metal that reacts with water to form a base.

Basic Salt
A salt containing an ionizable OH group.

Beta Particle
Electron emitted from the nucleus when a neuton decays to a proton and an electron.

Biodegradability
The ability of a substance to be broken down into simpler substances by bacteria.

Binary Acid
A binary compound in which H is bonded to one or more of the more electronegative nonmetals.

Binary Compound
A compound consisting of two elements; may be ionic or covalent.

Binding Energy (nuclear binding energy)
The energy equivalent (E = mc^2) of the mass deficiency of an atom.
where: E = is the energy in joules， m is the mass in kilograms， and c is the speed of light in m/s^2

Boiling Point
The temperature at which the vapor pressure of a liquid is equal to the applied pressure; also the condensation point

Boiling Point Elevation
The increase in the boiling point of a solvent caused by the dissolution of a nonvolatile solute.


Bomb Calorimeter
A device used to measure the heat transfer between system and surroundings at constant volume.
For more information see Analytical Chemistry

Bond Energy
The amount of energy necessary to break one mole of bonds of a given kind (in gas phase).
The amount of energy necessary to break one mole of bonds in a substance， dissociating the sustance in the gaseous state into atoms of its elements in the gaseous state.


Bond Order
Half the numbers of electrons in bonding orbitals minus half the number of electrons in antibonding orbitals.

Bonding Orbital
A molecular orbit lower in energy than any of the atomic orbitals from which it is derived; lends stability to a molecule or ion when populated with electron

Bonding Pair
Pair of electrons involved in a covalent bond.

Boron Hydrides
Binary compounds of boron and hydrogen.

Born-Haber Cycle
A series of reactions (and accompanying enthalpy changes) which， when summed， represents the hypothetical one-step reaction by which elements in their standard states are converted into crystals of ionic compounds (and the accompanying enthalpy changes.)


Boyle's Law
At constant temperature the volume occupied by a definite mass of a gas is inversely proportional to the applied pressure.

Breeder Reactor
A nuclear reactor that produces more fissionable nuclear fuel than it consumes.

Bronsted-Lowry Acid
A proton donor.

Bronsted-Lowry Base
A proton acceptor

Buffer Solution
Solution that resists change in pH; contains either a weak acid and a soluble ionic salt of the acid or a weak base and a soluble ionic salt of the base.

Buret

A piece of volumetric glassware， usually graduated in 0.1-mL intervals， that is used to deliver solutions to be used in titrations in a quantitative (dropwise) manner.

BMA004

l         Calorie

l         The amount of heat required to raise the temperature of one gram of water from 14.5°C to 15.5°C. 1 calorie = 4.184 joules.

l         Calorimeter

l         A device used to measure the heat transfer between system and surroundings.

l         For further information see Analytical Chemistry

l         Canal Ray

l         Stream of positively charged particles (cations) that moves toward the negative electrode in cathode ray tubes; observed to pass through canals in the negative electrode.

l         Capillary

l         A tube having a very small inside diameter.

l         Capillary Action

l         The drawing of a liquid up the inside of a small-bore tube when adhesive forces exceed cohesive forces， or the depression of the surface of the liquid when cohesive forces exceed the adhesive forces.

l         Carbanion

l         An organic ion carrying a negative charge on a carbon atom.

l         Carbonium ion

l         An orgainic ion carrying a positive charge on a carbon atom.

l         Carcinogen

l         A substance capable of causing or producing cancer in mammals.

l         Catalyst

l         A substance that speeds up a chemical reaction without being consumed itself in the reaction.

l         A substance that alters (usually increases) the rate at which a reaction occurs.

l         Catenation

l         Bonding of atoms of the same element into chains or rings.

l         The bonding together of atoms of the same element to form chains.

l         The ability of an element to bond to itself.

l         Cathode

l         Electrode at which reduction occurs

l         In a cathode ray tube， the negative electrode.

l         Cathodic Protection

l         Protection of a metal (making ir a cathode) against corrosion by attaching it to a sacrifical anode of a more easily oxidized metal.

l         Cathode Ray Tube

l         Closed glass tube containing a gas under low pressure， with electrodes near the ends and a luminescent screen at the end near the positive electrode; produces cathode rays when high voltage is applied.

l         Cation

l         A positive ion; an atom or group of atoms that has lost one or more electrons.

l         Cell Potential

l         Potential difference， Ecell， between oxidation and reduction half-cells under nonstandard conditions.

l         Central Atom

l         An atom in a molecule or polyatomic ion that is bonded to more than one other atom.

l         Chain Reaction

l         A reaction that， once initiated， sustains itself and expands.

l         This is a reaction in which reactive species， such as radicals， are produced in more than one step. These reactive species， radicals， propagate the chain reaction.

l         Chain Termination Step

l         The combination of two radicals， which removes the reactive species that propagate the change reaction.

l         Charle's Law

l         At constant pressure the volume occupied by a definite mass of gas is directly proportional to its absolute temperature.

l         Chemical Bonds

l         The attractive forces that hold atoms together in elements or compounds.

l         Chemical Change

l         A change in which one or more new substances are formed.

l         Chemical Equation

l         Description of a chemical reaction by placing the formulas of the reactants on the left and the formulas of products on the right of an arrow.

l         Chemical Equilibrium

l         A state of dynamic balance in which the rates of forward and reverse reactions are equal; there is no net change in concentrations of reactants or products while a system is at equilibrium.

l         Chemical Hygiene Officer (CHO)

l         A person or employee who is qualified by training or experience to provide technical guidance in the development and implementations of the provisions of a Chemical Hygiene Plan (CHP)

l         Chemical Hygiene Plan (CHP)

l         A written program developed and implemented by an employer designating proceedures， equipment， personal protective equipment， and work practices that are capable of protecting employees from the health hazards presented by hazardous chemicals usid in that particular workplace.

l         Chemical Kinetics

l         The study of rates and mechanisms of chemical reactions and of the factors on which they depend.

l         Chemical Periodicity

l         The variations in properties of elements with their position in the periodic table

l         Cis-

l         The prefix used to indicate that groups are located on the same side of a bon about which rotation is restricted.

l         Cis-Trans Isomerism

l         A type of geometrical isomerism related to the angles between like ligands.

l         Clay

l         A class of silicate and aluminosilicate minerals with sheet-like structures that have enormous surface areas that can absorb large amounts of water.

l         Cloud Chamber

l         A device for observing the paths of speeding particiles as vapor molecules condense on them to form foglike tracks.

l         Coefficient of expansion

l         The ratio of the change in length or volumen of a body to the original lengthor volume for a unit change in temperature.

l         Cohesive Forces

l         All the forces of attraction among particles of a liquid.

l         Coke

l         An impure form of carbon obtained by destructive distillation of coal or petroleum.

l         Colligative Properties

l         Physical properties of solutions that depend upon the number but not the kind of solute particles present.

l         Collision Theory

l         Theory of reaction rates that states that effective collisions between reactant molecules must occur in order for the reaction to occur.

l         Colloid

l         A heterogeneous mixture in which solute-like particles do not settle out.

l         Combination Reaction

l         Reaction in which two substances ( elements or compounds ) combine to form one compound.

l         Reaction of a substance with oxygen in a highly exothermic reaction， usually with a visible flame.

l         Combustible

l         Classification of liquid substances that will burn on the basis of flash points. A combustible liquid means any liquid having a flash point at or above 37.8°C (100°F) but below 93.3°C (200°F)， except any mixture having components with flash points of 93.3°C (200°F) or higher， the total of which makes up 99 percent or more of the total volume of the mixture.

l         Common Ion Effect

l         Suppression of ionization of a weak electrolyte by the presence in the same solution of a strong electrolyte containing one of the same ions as the weak electrolyte.

l         Complex Ions

l         Ions resulting from the formation of coordinate covalent bonds between simple ions and other ions or molecules.

l         Composition Stoichiometry

l         Descibes the quantitative (mass) relationships among elements in compounds.

l         Compound

l         A substance of two or more elements in fixed proportions. Compounds can be decomposed into their constituent elements.

l         For more Information see Compounds

l         Compressed Gas

l         A gas or mixture of gases having， in a container an absolute pressure exceeding 40 psi at 21.1°C (70°F)

l         A gass or mixture having in a container， an absolute pressure exceeding 104 psi at 54.4°C (130°F) regardless of the pressure at (21.1°C (70°F)

l         A liquid having a vapour pressure exceeding 40 psi at 37.8°C (70°F) as determined by ASTM D-323-72.

l         Concentration

l         Amount of solute per unit volume or mass of solvent or of solution.

l         Condensation

l         Liquefaction of vapor.

l         Condensed Phases

l         The liquid and solid phases; phases in which particles interact strongly.

l         Condensed States

l         The solid and liquid states.

l         Conduction Band

l         A partially filled band or a band of vacant energy levels just higher in energy than a filled band; a band within which， or into which， electrons must be promoted to allow electrical conduction to occur in a solid.

l         Conjugate Acid-base Pair

l         In Bronsted-Lowry terminology， a reactant and product that differ by a proton， H+.

l         Conformations

l         Structures of a compound that differ by the extent of rotation about a single bond.

l         Continuous Spectrum

l         Spectrum that contains all wave-lengths in a specified region of the electromagnetic spectrum.

l         Control Rods

l         Rods of materials such as cadmium or boron steel that act as neutron obsorbers (not merely moderaters) used in nuclear reactors to control neutron fluxes and therfore rates of fission.

l         Conjugated Double Bonds

l         Double bonds that are separated from each other by one single bond -C=C-C=C-.

l         Contact Process

l         Industrial process by which sulfur trioxide and sulfuric acid are produced from sulfur dioxide.

l         Coordinate Covalent Bond

l         Covalent bond in which both shared electrons are furnished by the same species; bond between a Lewis acid and Lewis base.

l         Coordinate Covalent Bond

l         A covalent bond in which both shared electrons are donated by the same atom; a bond between a Lewis base and a Lewis acid.

l         Coordination Compound or Complex

l         A compound containing coordinate covalent bonds.

l         Coordination Isomers

l         Isomers involving exchanges of ligands between complex cation and complex anion of the same compound.

l         Coordination Number

l         In describing crystals， the number of nearest neighbours of an atom or ion.

l         The number of donor atoms coordinated to a metal.

l         Coordination Sphere

l         The metal ion and its coordinating ligands but not any uncoordinated counter-ions.

l         Corrosion

l         Oxidation of metals in the presence of air and moisture.

l         For more information see Corrosion

l         Coulomb

l         Unit of electrical charge.

l         Coulometry

l         The quantitative application of Faraday's Law to the analysis of materials. The current and time are the usual variables measured.

l         Covalent Bond

l         Chemical bond formed by the sharing of one or more electron pairs between two atoms.

l         Covalent Compounds

l         Compounds containing predominantly covalent bonds.

l         Critical Mass

l         The minimum mass of a particular fissionable nuclide in a given volume required to sustain a nuclear chain reaction.

l         Critical Point

l         The combination of critical temperature and critical pressure of a substance.

l         Critical Pressure

l         The pressure required to liquefy a gas (vapor) at its critical temperature.

l         Critical Temperature

l         The temperature above which a gas cannot be liquefied; the temperature above which a substance cannot exhibit distinct gas and liquid phases.

l         Crystal Field Stabilization Energy

l         A measure of the net energy of stabilization gained by a metal ion's nonbonding d electrons as a result of complex formation.

l         For more information see Crystallography

l         Crystal Field Theory

l         Theory of bonding in transition metal complexes in which ligands and metal ions are treated as point charges; a purely ionic model; ligand point charges represent the crystal (electrical) field perturbing the metal?s d orbitals containing nonbonding electrons.

l         For more information see Crystallography

l         Crystal Lattice

l         A pattern of arrangement of particles in a crystal.

l         For more information see Crystallography

l         Crystal Lattice Energy

l         Amount of energy that holds a crystal together; the energy change when a mole of solid is formed from its constituent molecules or ions (for ionic compounds) in their gaseous state.

l         The energy charge when one mole of formula units of a crystalline solid is formed from its ions， atoms， or molecules in the gas phase; always negative.

l         For more information see Crystallography

l         Crystalline Solid

l         A solid characterized by a regular， ordered arrangement of particles.

l         For more information see Crystallography

l         Curie (Ci)

l         The basic unit used to describe the intensity of radioactivity in a sample of material. One curie equals 37 billion disintegrations per second or approximately the amount of radioactivty given off by 1 gram of radium.

l         Cyclotron

l         A device for accelerating charged particles along a spiral path.



l         Daughter Nuclide

l         Nuclide that is produced in a nuclear decay.

l         Debye

l         The unit used to express dipole moments.

l         Degenerate

l         Of the same energy.

l         Delocalization

l         Of electrons; refers to bonding electrons that are distributed among more than two atoms that are bonded together; occurs in species that exhibit resonance.

l         The formation of a set of molecular orbitals that extend over more than two atoms; important in species that valence bond theory describes in terms of resonance.

l         Denaturation

l         A process pertaining to a change in structure of a protein form regular to irregular arrangement of the polypeptide chains.

l         Denatured

l         A commercial term used to describe ethanol that has been rendered unfit for human consumption because of the addition of harmful ingredients to make it sales tax-expempt.

l         Density

l         Mass per unit Volume: D=MV

l         Deposition

l         The direct solidification of a vapor by cooling; the reverse of sublimation.

l         Derivative

l         A compound that can be imagined to arise from a partent compound by replacement of one atom with another atom or group of atoms. Used extensively in orgainic chemistry to assist in identifying compounds.

l         Dermal toxicity

l         Adverse health effects resulting from skin exposure ot a substance.

l         Designated area

l         An area that may be used for work with carcinogens， reproductive toxins， or substances that have a high degree of acute toxicity. A designated area may be the entire laboratory， an area of a laboratory， or a device such as a loboratory hood.

l         Detergent

l         A soap-like emulsifer that contains a sulfate， SO3 or a phosphate group instead of a carboxylate group.

l         Deuterium

l         An isotope of hydrogen whose atoms are twice as massive as ordinary hydrogen;deuterion atoms contain both a proton and a neutron in the nucleus.

l         Dextrorotatory

l         Refers to an optically active substance that rotates the plane of plane polarized light clockwise; also called dextro.

l         Diagonal Similarities

l         Refers to chemical similarities in the Periodic Table of elements of Period 2 to elements of Period 3 one group to the right; especially evident toward the left of the periodic table.

l         Diamagnetism

l         Weak repulsion by a magnetic field.

l         Differential Scanning Calorimetry (DSC)

l         A technique for measuring the temperature， direction， and magnitude of thermal transitions in a sample material by heating/cooling and comparing the amount of energy required to maintain its rate of temperature increase or decrease with an inert reference material under similar conditions.

l         Differential Thermal Analysis (DTA)

l         A technique for observing the temperature， direction， and magnitude of thermally induced transitions in a material by heating/cooling a sample and comparing its temperature with that of an inert reference material under similar conditions.

l         Differential Thermometer

l         A thermometer used for accurate measurement of very small changes in temperature.

l         Dilution

l         Process of reducing the concentration of a solute in solution， usually simply by mixing with more solvent.

l         Dimer

l         Molecule formed by combination of two smaller (identical) molecules.

l         Dipole

l         Refers to the separation of charge between two covalently bonded atoms

l         Dipole-dipole Interactions

l         Attractive interactions between polar molecules， that is， between molecules with permanent dipoles.

l         Dipole Moment

l         The product of the distance separating opposite charges of equal magnitude of the charge; a measure of the polarity of a bond or molecule; a measured dipole moment refers to the dipole moment of an entire molecule.

l         Dispersing Medium

l         The solvent-like phase in a colloid

l         Dispersed Phase

l         The solute-like species in a colloid

l         Displacement Reactions

l         Reactions in which one element displaces another from a compound.

l         Disproportionation Reactions

l         Redox reactions in which the oxidizing agent and the reducing agent are the same species.

l         Dissociation

l         In aqueous solution， the process in which a solid ionic compound separates into its ions.

l         Dissociation Constant

l         Equilibrium constant that applies to the dissociation of a comples ion into a simple ion and coordinating species (ligands).

l         Distilland

l         The material in a distillation apparatus that is to be distilled.

l         Distillate

l         The material in a distillation apparatus that is collected in the receiver.

l         Distillation

l         The separation of a liquid mixture into its components on the basis of differences in boiling points.

l         The process in which components of a mixture are separated by boiling away the more volitile liquid.

l         Domain

l         A cluster of atoms in a ferromagnetic substance， all of which align in the same direction in the presence of an external magnetic field.

l         Donor Atom

l         A ligand atom whose electrons are shared with a Lewis acid.

l         D-Orbitals

l         Beginning in the third energy level， aset of five degenerate orbitals per energy level， higher in energy than s and p orbitals of the same energy level.

l         Dosimeter

l         A small， calibrated electroscope worn by laboratory personnel and designated to detect and measure incident ionizing radiation or chemical exposure.

l         Double Bond

l         Covalent bond resulting from the sharing of four electrons (two pairs) between two atoms.

l         Double Salt

l         Solid consisting of two co-crystallized salts.

l         Doublet

l         Two peaks or bands of about equal intensity appearing close together on a spectrogram.

l         Downs Cell

l         Electrolytic cell for the commercial electrolysis of molten sodium chloride.

l         For further information see Electrochemistry or Fuel Cells

l         DP number

l         The degree of polymerization; the average number of monomer units per polymer unit.

l         Dry Cells

l         Ordinary batteries (voltaic cells) for flashlights. radios， and so on; many are Leclanche cells.

l         For further information see Electrochemistry or Fuel Cells

l         D -Transition elements (metals)

l         B Group elements except IIB in the periodic table; sometimes called simply transition elements EX. Fe， Ni， Cu， Ti .

l         For further information see Metals

l         Dumas Method

l         A method used to determine the molecular weights of volatile liquids.

l         Dynamic Equilibrium

l         An equilibrium in which processes occur continuously， with no net change.

l         When two (or more) processes occur at the same rate so that no net change occurs.



l         Effective Collisons

l         Collision between molecules resulting in a reaction; one in which the molecules collide with proper relative orientations and sufficient energy to react.

l         Effective Molality

l         The sum of the molalities of all solute particles in a solution.

l         Effective Nuclear Charge

l         The nuclear charge experienced by the outermost electrons of an atom; the actual nuclear charge minus the effects of shielding due to inner-shell electrons.

l         Example: Set of dx2-y2 and dz2 orbitals; those d orbitals within a set with lobes directed along the x-， y-， and z-axes.

l         Electrical Conductivity

l         Ability to conduct electricity.

l         Electrochemistry

l         Study of chemical changes produced by electrical current and the production of electricity by chemical reactions.

l         Electrodes

l         Surfaces upon which oxidation and reduction half-reactions; occur in electrochemical cells.

l         Electrode, Potentials

l         Potentials， E， of half-reactions as reductions versus the standard hydrogen electrode.

l         Electrolysis

l         Process that occurs in electrolytic cells.

l         Electrolyte

l         A substance whose aqueous solutions conduct electricity.

l         Electrolytic Cells

l         Electrochemical cells in which electrical energy causes nospontaneous redox reactions to occur.

l         An electrochemical cell in which chemical reactions are forced to occur by the application of an outside source of electrical energy.

l         Electrolytic Conduction

l         Conduction of electrical current by ions through a solution or pure liquid.

l         Electromagnetic Radiation

l         Energy that is propagated by means of electric and magnetic fields that oscillate in directions perpendicular to the direction of travel of the energy.

l         Electromotive Series

l         The relative order of tendencies for elements and their simple ions to act as oxidizing or reducing agents; also called the activity series.

l         Electron

l         A subatomic particle having a mass of 0.00054858 amu and a charge of 1-.

l         Electron Affinity

l         The amount of energy absorbed in the process in which an electron is added to a neutral isolated gaseous atom to form a gaseous ion with a 1- charge; has a negative value if energy is released.

l         Electron Configuration

l         Specific distribution of electrons in atomic orbitals of atoms or ions.

l         Electron Deficient Compounds

l         Compounds that contain at least one atom (other than H) that shares fewer than eight electrons

l         Electronic Transition

l         The transfer of an electron from one energy level to another.

l         Electronegativity

l         A measure of the relative tendency of an atom to attract electrons to itself when chemically combined with another atom.

l         Electronic Geometry

l         The geometric arrangement of orbitals containing the shared and unshared electron pairs surrounding the central atom of a molecule or polyatomic ion.

l         Electrophile

l         Positively charged or electron-deficient.

l         Electrophoresis

l         A technique for separation of ions by rate and direction of migration in an electric field.

l         Electroplating

l         Plating a metal onto a (cathodic) surface by electrolysis.

l         Element

l         A substance that cannot be decomposed into simpler substances by chemical means.

l         Eluant or eluent

l         The solvent used in the process of elution， as in liquid chromatography.

l         Eluate

l         Solvent (or mobile phase) which passes through a chromatographic column and removes the sample components from the stationary phase.

l         Emission Spectrum

l         Spectrum associated with emission of electromagnetic radiation by atoms (or other species) resulting from electronic transitions from higher to lower energy states.

l         Emulsifying Agent

l         A sustance that coats the particles of the dispersed phase and prevents coagulation of colloidal particles; an emulsifier.

l         Emulsion

l         Colloidal suspension of a liquid in a liquid.

l         Enantiomer

l         One of the two mirror-image forms of an optically active molecule.

l         Endothermic

l         Describes processes that absorb heat energy.

l         Endothermicity

l         The absorption of heat by a system as the process occurs.

l         End Point

l         The point at which an indicator changes colour and a titration is stopped.

l         Energy

l         The capacity to do work or transfer heat.

l         Enthalpy

l         The heat content of a specific amount of substance; defined as E= PV.

l         Entropy

l         A thermodynamic state or property that measures the degree of disorder or randomness of a system.

l         For more information see Thermochemistry

l         Enzyme

l         A protein that acts as a catalyst in biological systems.

l         Equation of State

l         An equation that describes the behavior of matter in a given state; the van der Waals equation describes the behavior of the gaseous state.

l         Equilibrium or Chemical Equilibrium

l         A state of dynamic balance in which the rates of forward and reverse reactions are equal; the state of a system when neither forward or reverse reaction is thermodynamically favored.

l         Equilibrium Constant

l         A quantity that characterizes the position of equilibrium for a reversible reaction; its magnitude is equal to the mass action expression at equilibrium. K varies with temperature.

l         Equivalence Point

l         The point at which chemically equivalent amounts of reactants have reacted.

l         Equivalent Weight

l         An oxidizing or reducing agent， who's mass gains (oxidizing agents) or loses (reducing agents) 6.022 x 1023 electrons in a redox reaction.

l         The mass of an acid or base that furnishes or reacts with 6.022 x 1023 H3O+ or OH- ions.

l         Essential Oil

l         A plant extract that has a distinctive odour or flavour.

l         Ester

l         A Compound of the general formula R-C-O-R1 where R and R1 may be the same or different， and may be either aliphatic or aromatic.

l         Ether

l         Compound in which an oxygen atom is bonded to two alkyl or two aryl groups， or one alkyl and one aryl group.

l         Eutrophication

l         The undesirable overgrowth of vegetation caused by high concentrates of plant nutrients in bodies of water.

l         Evaporization

l         Vaporization of a liquid below its boiling point.

l         Evaporation Rate

l         The rate at which a particular substance will vapourize (evaporate) when compared to the rate of a known substance such as ethyl ether. This term is especially useful for health and fire-hazard considerations.

l         Excited State

l         Any state other than the ground state of an atom or molecule.

l         Exothermic

l         Describes processes that release heat energy.

l         Exothermicity

l         The release of heat by a system as a process occurs.

l         Explosive

l         A chemical or compound that causes a sudden， almost instantaneous release or pressure， gas， heat and light when subjected to sudden shock， pressure， high temperature or applied potential.

l         Explosive limits

l         The range of concentrations over which a flammable vapour mixed with proper ratios of air will ignite or explode if a source of ignitions is provided.

l         Extensive Property

l         A property that depends upon the amount of material in a sample.

l         Extrapolate

l        To estimate the value of a result outside the range of a series of known values. Technique used in standard additions calibration procedure.

BMA004

Ø         Faraday

Ø         One faraday of electricity corresponds to the charge on 6.022 x 10 23 electrons， or 96，487 coulombs.

Ø         Faraday's Law of Electrolysis

Ø         One equivalent weight of a substance is produced at each electrode during the passage of 96，487 coulombs of charge through an electrolytic cell.

Ø         Fast Neutron

Ø         A neutron ejected at high kinetic energy in a nuclear reaction.

Ø         Fat

Ø         Solid triester of glycerol and (mostly) saturated fatty acids.

Ø         Fatty Acids

Ø         An aliphatic acid; many can obtained from animal fats.

Ø         Ferromagnetism

Ø         The ability of a substance to become permanently magnetized by exposure to an external magnetic field.

Ø         Film badge

Ø         A small patch of photographic film worn on clothing to detect and measure accumulated incident ionizing radiation.

Ø         Flammable

Ø         A liquid as defined by NFPD and DOT as having a flash point below 37.8°C (100°F).

Ø         Flash Point

Ø         The temperature at which a liquid will yield enough flamable vapour to ignite. There are various recognized industrial testing methods; therefore the method used must be stated.

Ø         Fluorescence

Ø         Absorption of high energy radiation by a substance and subsequent emission of visible light.

Ø         Fossil Fuels

Ø         Substances consisting largely of hydrocarbons， derived from decay of organic materials under geological conditions of high pressure and temperature (metamorphism) include coal， petroleum， natural gas， peat and oil shale.

Ø         For further information see Fuel Chemistry

Ø         Frasch Process

Ø         Method by which elemental sulfur is mined or extracted. Sulfur is melted with superheated water (at 170°C under high pressure) and forced to the surface of the earth as a slurry.

Ø         First Law of Thermodynamics

Ø         The total amount of energy in the universe is constant (also known as the Law of Conservation of Energy) energy is neither created nor destroyed in ordinary chemical reactions and physical changes.

Ø         For further information see Thermochemistry

Ø         Flotation

Ø         Method by which hydrophobic (water-repelling) particles of an ore are separated from hydrophilic (water-attracting) particles of a metallurgical pretreatment process.

Ø         Fluids

Ø         Substances that flow freely; gases and liquids.

Ø         Flotation

Ø         Flux

Ø         A substance added to react with the charge， or a product of its reduction， in metallurgy; usually added to lower a melting point.

Ø         Foam

Ø         Colloidal suspension of a gas in a liquid.

Ø         Forbidden Zone

Ø         A relatively large energy separation between an insulator's highest filled electron energy band and the next higher energy vacant band. Beginning in the fourth energy level， a set of seven degenerate orbitals per energy level， higher in energy than s， p， and d orbitals of the same energy level.

Ø         Formal Charge

Ø         A method of counting electrons in a covalently bonded molecule or ion; counts bonding electrons as though they were equally shared between the two atoms.

Ø         Formula

Ø         Combination of symbols that indicates the chemical composition of a substance.

Ø         Formula Unit

Ø         The smallest repeating unit of a substance. The molecule for nonionic substances

Ø         Formula Weight

Ø         The mass of one formula unit of a substance in atomic mass units.

Ø         Fractional Distillation

Ø         The process in which a fractioning column is used in distillation apparatus to separate components of a liquid mixture that have different boiling points.

Ø         Fractional Precipitation

Ø         Removal of some ions from solution by precipitation while leaving other ions with similar properties in solution.

Ø         Free Energy， Gibbs Free Energy

Ø         The thermodynamic state function of a system that indicates the amount of energy available for the system to do useful work at constant T and P.

Ø         Free Energy Change

Ø         The indicator of spontaneity of a process at constnt T and P. If delta-G is negative， the process is spontaneous.

Ø         Free Radical

Ø         A highly reactive chemical species carrying no charge and having a single unpaired electron in an orbital.

Ø         Freezing Point Depression

Ø         The decrease in the freezing point of a solvent caused by the presence of a solute.

Ø         Frequency

Ø         The number of repeating corresponding points on a wave that pass a given observation point per unit time.

Ø         Fuel Cells

Ø         Voltaic cells in which the reactants (usually gases) are supplied continuously.

Ø         A voltaic cell that converts the chemical energy of a fuel and an oxidizing agent directly into electriacl energy on a continuous basis.

Ø         Functional Group

Ø         A group of atoms that represents a potential reaction site in an organic compound.

Ø         Chemistry Terminology G



Ø         Gamma Ray

Ø         High energy electromagnetic radiation.

Ø         A highly penetrating type of nuclear radiation similar to x-ray radiation， except that it comes from within the nucleus of an atom and has a higher energy. Energywise， very similar to cosmic ray except that cosmic rays originate from outer space.

Ø         For more information see Electrochemistry

Ø         Galvanizing

Ø         Placing a thin layer of zinc on a ferrous material to protect the underlying surface from corrosion.

Ø         Gangue

Ø         Sand， rock， and other impurities surrounding the mineral of interest in an ore.

Ø         Geiger counter

Ø         A gas filled tube which discharges electriaclly when ionizing radiation passes through it.

Ø         Gel

Ø         Colloidal suspension of a solid dispersed in a liquid; a semirigid solid.

Ø         Gem-dimethyl group

Ø         Two methyl groups of the same carbon atom.

Ø         Geometrical Isomers

Ø         Compounds with different arrangements of groups on either side of a bond with restricted rotation， such as a double bond or a single bond in a ring; for example cis-trans isomers of certain alkenes.

Ø         Stereoisomers that are not mirror images of each other; also known as position isomers.

Ø         Graham's Law

Ø         The rates of effusion of gases are inversely proportional to the square roots of their molecular weights or densities.

Ø         Greenhouse Effect

Ø         Trapping of heat at the surface of the earth by carbon dioxide and water vapour in the atmosphere.

Ø         Ground State

Ø         The lowest energy state or most stable state of an atom， molecule or ion.

Ø         Group

Ø         A vertical column in the periodic table; also called a family.

Ø         For more information see Periodic Tables

Ø         Chemistry Terminology H

Ø         Haber Process

Ø         A process for the catalyzed industrial production of ammonia from N2 and H2 at high temperature and pressure.

Ø         Half-Cell

Ø         Compartment in which the oxidation or reduction half-reaction occurs in a voltaic cell.

Ø         Half-Life

Ø         The time required for half of a reactant to be converted into product(s).

Ø         The time required for half of a given sample to undergo radioactive decay.

Ø         Half-Reaction

Ø         Either the oxidation part or the reduction part of a redox reaction.

Ø         Halogens

Ø         Group VIIA elements: F， Cl， Br， I

Ø         Hard Water

Ø         Water containing Fe3+， Ca2+， and Mg2+ ions， which forms precipates with soap.

Ø         Heat

Ø         A form of energy that flows between two samples of matter because of their differences in temperature.

Ø         Heat Capacity

Ø         The amount of heat required to raise the temperature of a body (of any mass) one degree Celsius.

Ø         Heat of Condensation

Ø         The amount of heat that must be removed from one gram of a vapor at it's condensation point to condense the vapour with no change in temperature.

Ø         Heat of Crystallization

Ø         The amount of heat that must be removed from one gram of a liquid at its freezing point to freeze it with no change in temperature.

Ø         Heat of Fusion

Ø         The amount of heat required to melt one gram of solid at its melting point with no change in temperature. Usually expressed in J/g. The molar heat of fusion is the amount of heat required to melt one mole of a solid at its melting point with no change in temperature and is usually expressed in kJ/mol.

Ø         Heat of Solution

Ø         The amount of heat absorbed in the formation of solution that contains one mole of solute; the value is positive if heat is absorbed (endothermic) and negative if heat is released (exothermic).

Ø         Heat of Vaporization

Ø &, nbsp;       The amount of heat required to vaporize one gram of a liquid at its boiling point with no change in temperature. Usually expressed in J/g. The molar heat of vaporization is the amount of heat required to vaporize one mole of liquid at its boiling point with no change in temperature and usually expressed ion kJ/mol.

Ø         Heavy Water

Ø         Water containing deuterium， a heavy isotope of hydrogen.

Ø         Heisenberg Uncertainty Principle

Ø         It is impossible to determine accurately both the momentum and position of an electron simultaneously.

Ø         Henry's Law

Ø         The pressure of the gas above a solution is proportional to the concentration of the gas in the solution.

Ø         Hess' Law of Heat Summation

Ø         The enthalpy change for a reaction is the same whether it occurs in one step or a series of steps.

Ø         Heterocyclic Amine

Ø         Amine in which the nitrogen is part of a ring.

Ø         For further information see Heterocyclic Chemistry

Ø         Heterogeneous Catalyst

Ø         A catalyst that exists in a different phase (solid， liquid or gas) from the reactants; a contact catalyst.

Ø         Heterogeneous Equilibria

Ø         Equilibria involving species in more than one phase.

Ø         Heterogeneous Mixture

Ø         A mixture that does not have uniform composition and properties throughout.

Ø         Heteronuclear

Ø         Consisting of different elements.

Ø         High Spin Complex

Ø         Crystal field designation for an outer orbital complex; all t2g and eg orbitals are singly occupied before any pairing occurs.

Ø         Homogeneous Catalyst

Ø         A catalyst that exists in the same phase (solid， liquid or gas) as the reactants.

Ø         For more information see Catalysis

Ø         Homogeneous Equilibria

Ø         Equilibria involving only one species in a single phase. For example， all gases， all liquids or all solids.

Ø         Homogeneous Mixture

Ø         A mixture which has uniform composition and properties throughout.

Ø         Homologous Series

Ø         A series of compounds in which each member differs from the next by a specific number and kind of atoms.

Ø         Homonuclear

Ø         Consisting of only one element.

Ø         Hund's Rule

Ø         All orbitals of a given sublevel must be occupied by single electrons before pairing begins (see Aufbau Principle)

Ø         Hybridization

Ø         Mixing a set of atomic orbitals to form a new set of atomic orbitals with the same total electron capacity and with properties and energies intermediate between those of the original unhybridized orbitals.

Ø         Hydrate

Ø         A solid compound that contains a definite percentage of bound water.

Ø         Hydrate Isomers

Ø         Isomers of crystalline complexes that differ in whether water is present inside or outside the coordination sphere

Ø         Hydration

Ø         Reaction of a substance with water.

Ø         Hydration Energy

Ø         The energy change accompanying the hydration of a mole of gase and ions.

Ø         Hydride

Ø         A binary compound of hydrogen

Ø         Hydrocarbons

Ø         Compounds that contain only carbon and hydrogen

Ø         Hydrogen Bond

Ø         A fairly strong dipole-dipole interaction (but still considerably weaker than the covalent or ionic bonds) between molecules containing hydrogen directly bonded to a small， highly electronegative atom， such as N， O， or F.

Ø         Hydrogenation

Ø         The reaction in which hydrogen adds across a double or triple bond.

Ø         Hydrogen-Oxygen Fuel Cell

Ø         Fuel cell in which hydrogen is the fuel (reducing agent) and oxygen is the oxidizing agent.

Ø         Hydrolysis

Ø         The reaction of a substance with water or its ions.

Ø         Hydrolysis Constant

Ø         An equilibrium constant for a hydrolysis reaction.

Ø         Hydrometer

Ø         A device used to measure the densities of liquids and solutions.

Ø         Hydrophilic Colloids

Ø         Colloidal particles that repel water molecules.

Ø         For more information see Colloidal Chemistry

BMA004

n             Chemistry Terminology I



n             Inner Orbital Complex

n             Valence bond designation for a complex in which the metal ion utilizes d orbitals for one shell inside the outermost occupied shell in its hybridization.

n             Isomers

n             Different substances that have the same formula.

n             Ionization Isomers

n             Isomers that result from the interchange of ions inside and outside the coordination sphere.

n             Inert s-pair Effect

n             Characteristic of the post-transition minerals; tendency of the outermost s electrons to remain nonionized or un shared in compounds.

n             Insoluble Compound

n             A very slightly soluble compound.

n             Indicators

n             For acid-base titrations， organic compounds that exhibit different colors in solutions of different acidities; used to determine the point at which reaction between two solutes is complete.

n             Ionization Constant

n             Equilibrium constant for the ionization of a weak electrolyte.

n             Ion Product for Water

n             Equilibrium constant for the ionization of water， Kw = [H3O+][OH-] =1.00 x 10-14 at 25 °C.

n             Inhibitory Catalyst

n             An inhibitor， a catalyst that decreases the rate of reaction.

n             For more information see Catalysis

n             Integrated Rate Equation

n             An equation giving the concentration of a reactant remaining after a specified time; has different mathematical form for different orders of reactants.

n             Ioniztion

n             The breaking up of a compound into separate ions.

n             Ideal Solution

n             A solution that obeys Raoult"s Law exactly.

n             Insulator

n             Poor electric and heat conductor.

n             Intermolecular Forces

n             Forces between individual particles (atoms， molecules， ions) of a substance.

n             Isomorphous

n             Refers to crystals having the same atomic arrangement.

n             For more information see Crystallograph

n             Ideal Gas

n             A hypothetical gas that obeys exactly all postulates of the kinetic-molecular theory.

n             Ideal Gas Law

n             The product of pressure and the volume of an ideal gas is directly proportional to the number of moles of the gas and the absolute temperature.

n             Ionization

n             In aqueous solution， the process in which a molecular compound reacts with water and forms ions.

n             Ionic Bonding

n             Chemical bonding resulting from the transfer of one or more electrons from one atom or a group of atoms to another.

n             Ionic Compunds

n             Compounds containing predominantly ionic bonding.

n             Ionic Geometry

n             The arrangement of atoms (not lone pairs of electrons) about the central atom of a polyatomic ion.

n             Isoelectric

n             Having the same electronic configurations

n             Ionization Energy

n             The minimum amount of energy required to remove the most loosely held electron of an isolated gaseous atom or ion.

n             Isotopes

n             Two or more forms of atoms of the same element with different masses; atoms containing the same number of protons but different numbers of neutrons.

n             Ion

n             An atom or a group of atoms that carries an electric charge.

n             Chemistry Terminology J

n             Joule

n             A unit of energy in the SI system. One joule is 1 kg. m2/s2 which is also 0.2390 calorie.

n             Chemistry Terminology K

n             K Capture

n             Absorption of a K shell (n=1) electron by a proton as it is converted to a neutron.

n             Ketone

n             Compound in which a carbonyl group is bound to two alkyl or two aryl groups， or to one alkyl and one aryl group.

n             Kinetic Energy

n             Energy that matter processes by virtue of its motion.

n             Kinetic-molecular Theory

n             A theory， that attempts to explain macroscopic observations on gases in microscopic observations on gases in microscopic observations on gases in microscopic or molecular terms.

n             Chemistry Terminology L

n             Lanthanides

n             Elements 58 to 71 (after lanthanum)

n             Lanthanide Contraction

n             A decrease in the radii of the elements following the lanthanides compared to what would be expected if there were no f-transition metals.

n             Law of Combining Volumes (Gay-Lussac"s Law)

n             At constant temperature and pressure， the volumes of reacting gases ( and any gaseous products) can be expressed as ratios of small whole numbers;

n             Law of Conservation of Energy

n             Energy cannot be created or destroyed; it may be changed from one form to another.

n             Law of Conservation of Matter

n             There is no detectable change in the quantity of matter during an ordinary chemical reaction.

n             Law of Conservation of Matter and Energy

n             The total amount of matter and energy available in the universe is fixed.

n             Law of Definite Proportions (Law of Constant Composition)

n             Different samples of a pure compound always contain the same elements in the same proportions by mass.

n             Law of Partial Pressures (Dalton"s Law)

n             The total pressure exerted by a mixature of gases is the sum of the partial pressures of the individual gases.

n             Lead Storage Battery

n             Secondary voltaic cell used in most automobiles.

n             Leclanche Cell

n             A common type of dry cell.

n             Le Chatelier"s Principle

n             States that a system at equilibrium， or striving to attain equilibrium， responds in such a way as to counteract any stress placed upon it.

n             If a stress (change of conditions) is applied to a system at equilibrium， the system shifts in the direction that reduces stress.

n             Leveling Effect

n             Effect by which all acids stronger than the acid that is characteristic of the solvent react with solvent to produce that acid; similar statement applies to bases. The strongest acid (base) that can exist in a given solvent is the acid (base) characteristic of the solvent.

n             Levorotatory

n             Refers to an optically active substance that rotates the plane of plane polarized light counterclockwise; also called levo.

n             Lewis Acid

n             Any species that can accept a share in an electron pair.

n             Lewis Base

n             Any species that can make available a share in an electron pair.

n             Lewis Dot Formula (Electron Dot Formula)

n             Representation of a molecule， ion or formula unit by showing atomic symbols and only outer shell electrons

n             Ligand

n             A Lewis base in a coordination compound.

n             Limiting Reactant

n             Substance that stoichiometrically limits the amount of product(s) that can be formed.

n             Linear Accelerator

n             A device used for accelerating charged particles along a straight line path.

n             Line Spectrum

n             An atomic emission or absorption spectrum.

n             Linkage Isomers

n             Isomers in which a particular ligand bonds to a metal ion through different donor atoms.

n             Liquid Aerosol

n             Colloidal suspension of liquid in gas.

n             London Forces

n             Very weak and very short-range attractive forces between short-lived temporary (induced) dipoles; also called dispersion Forces.

n             Lone Pair

n             Pair of electrons residing on one atom and not shared by other atoms; unshared pair.

n             Low Spin Complex

n             Crystal field designation for an inner orbital complex; contains electrons paired t2g orbitals before eg orbitals are occupied in octahedral complexes.

BMA004

Ø           Chemistry Terminology M



Ø           Magnetic Quantum Number (mc)

Ø           Quantum mechanical solution to a wave equation that designates the particular orbital within a given set (s， p， d， f ) in which a electron resides.

Ø           Manometer

Ø           A two-armed barometer.

Ø           Mass

Ø           A measure of the amount of matter in an object. Mass is usually measured in grams or kilograms.

Ø           Mass Action Expression

Ø           For a reversible reaction， aA + bB cC + dD the product of the concentrations of the products (species on the right)， each raised to the power that corresponds to its coefficient in the balanced chemical equation， divided by the product of the concentrations of reactants (species on the left)， each raised to the power that corresponds to its coefficient in the balanced chemical equation. At equilibrium the mass action expression is equal to K; at other times it is Q.[C]c[D]d [A]a[B]b = Q， or at equilibrium K

Ø           Mass Deficiency

Ø           The amount of matter that would be converted into energy if an atom were formed from constituent particles.

Ø           Mass Number

Ø           The sum of the numbers of protons and neutrons in an atom; an integer.

Ø           Mass Spectrometer

Ø           An instrument that measures the charge-to-mass ratio of charged particles.

Ø           For further information see Mass Spectrometry

Ø           Matter

Ø           Anything that has mass and occupies space.

Ø           Mechanism

Ø           The sequence of steps by which reactants are converted into products.

Ø           Melting Point

Ø           The temperature at which liquid and solid coexist in equilibrium; also the freezing point.

Ø           Meniscus

Ø           The shape assumed by the surface of a liquid in a cylindrical container.

Ø           Metal

Ø           An element below and to the left of the stepwise division (metalloids) in the upper right corner of the periodic table; about 80% of the known elements are metals.

Ø           Metallic Bonding

Ø           Bonding within metals due to the electrical attraction of positively charges metal ions for mobile electrons that belong to the crystal as a whole.

Ø           Metallic Conduction

Ø           Conduction of electrical current through a metal or along a metallic surface.

Ø           Metalloids

Ø           Elements with properties intermediate between metals and nonmetals: B， Al， Si， Ge， As， Sb， Te， Po， and At.

Ø           Metallurgy

Ø           Refers to the overall processes by which metals are extracted from ores.

Ø           Metathesis Reactions

Ø           Reactions in which two compounds react to form two new compounds， with no changes in oxidation number. Reactions in which the ions of two compounds exchange partners.

Ø           Method of Initial Rates

Ø           Method of determining the rate-law expression by carrying out a reaction with different initial concentrations and analyzing the resultant changes in initial rates.

Ø           Miscibility

Ø           The ability of one liquid to mix with (dissolve in) another liquid.

Ø           Mixture

Ø           A sample of matter composed of two or more substances， each of which retains its identity and properties.

Ø           Moderator

Ø           A substance such as hydrogen， deuterium， oxygen or paraffin capable of slowing fast nuetrons upon collision.

Ø           Molality

Ø           Concentration expressed as number of moles of solute per kilogram of solvent.

Ø           Molarity

Ø           Number of moles of solute per litre of solution.

Ø           Molar Solubility

Ø           Number of moles of a solute that dissolve to produce a litre of saturated solution.

Ø           Molecular Equation

Ø           Equation for a chemical reaction in which all formulas are written as if all substances existed as molecules; only complete formulas are used.

Ø           Molecular Formula

Ø           Formula that indicates the actual number of atoms present in a molecule of a molecular substance.

Ø           Molecular Geometry

Ø           The arrangement of atoms (not lone pairs of electrons) around a central atom of a molecule or polyatomic ion.

Ø           Molecular Orbital

Ø           An orbit resulting from overlap and mixing of atomic orbitals on different atoms. An MO belongs to the molecule as a whole.

Ø           Molecular Orbital Theory

Ø           A theory of chemical bonding based upon the postulated existence of molecular orbitals.

Ø           Molecular Weight

Ø           The mass of one molecule of a nonionic substance in atomic mass units.

Ø           Molecule

Ø           The smallest particle of an element or compound capable of a stable， independent existence.

Ø           Mole Fraction

Ø           The number of moles of a component of a mixture divided by the total number of moles in the mixture.

Ø           Monoprotic Acid

Ø           Acid that can form only one hydronium ion per molecule; may be strong or weak.

Ø           Acid that contains one ionizable hydrogen atom per formula unit.

Ø           Mother Nuclide

Ø           Nuclide that undergoes nuclear decay.

Ø           Chemistry Terminology N

Ø           Native State

Ø           Refers to the occurrence of an element in an uncombined or free state in nature.

Ø           Natural Radioactivity

Ø           Spontaneous decomposition of an atom.

Ø           Nernst Equation

Ø           Corrects standard electrode potentials for nonstandard conditions.

Ø           Net Ionic Equation

Ø           Equation that results from canceling spectator ions and eliminating brackets from a total ionic equation.

Ø           Neutralization

Ø           The reaction of an acid with a base to form a salt and water. Usually， the reaction of hydrogen ions with hydrogen ions to form water molecules.

Ø           Neutron

Ø           A neutral subatomic particle having a mass of 1.0087 amu.

Ø           Nickel-cadmium cell (Nicad battery)

Ø           A dry cell in which the anode is Cd， the cathode is NiO2， and the electrolyte is basic.

Ø           Nitrogenases

Ø           A class of enzymes found in bacteria within root nodules in some plants， which catalyze reactions by which N2 molecules from the air are converted to ammonia.

Ø           For more information see Enzymes

Ø           Nitrogen Cycle

Ø           The complex series of reactions by which nitrogen is slowly but continually recycled in the atmosphere， lithosphere and hydrosphere.

Ø           Noble Gases (Rare Gases)

Ø           Elements of the periodic Group 0; also called rare gases; formerly called inert gases， He，Ne，Ar， Kr， Xe， Rn.

Ø           Nodal Plane

Ø           A region in which the probability of finding an electron is zero.

Ø           Nonbonding Orbital

Ø           A molecular orbital derived only from an atomic orbital of one atom; lends neither stability nor instability to a molecule or ion when populated with electrons.

Ø           Nonelectrolyte

Ø           A substance whose aqueous solutions do not conduct electricity.

Ø           Nonpolar Bond

Ø           Covalent bond in which electron density is symmetrically distributed

Ø           Nuclear Binding Energy

Ø           Energy equivalent of the mass deficiency; energy released in the formation of an atom from the subatomic particles.

Ø           Nuclear Fission

Ø           The process in which a heavy nucleus splits into nuclei of intermediate masses and one or more protons are emitted.

Ø           Nuclear Reaction

Ø           Involves a change in the composition of a nucleus and can evolve or absorb an extraordinarily large amount of energy

Ø           Nuclear Reactor

Ø           A system in which controlled nuclear fisson reactions generate heat energy on a large scale， which is subsequently converted into electrical energy.

Ø           Nucleons

Ø           Particles comprising the nucleus; protons and neutrons.

Ø           Nucleus

Ø           The very small， very dense， positively charged center of an atom containing protons and neutrons， as well as other subatomic particles.

Ø           Nuclides

Ø           Refers to different atomic forms of all elements in contrast to ?isotopes?， which refer only to different atomic forms of a single element.

Ø           Nuclide Symbol

Ø           Symbol for an atom A/Z E， in which E is the symbol of an element， Z is its atomic number， and A is its mass number.



Ø           Chemistry Terminology O



Ø           Octahedral

Ø           A term used to describe molecules and polyatomic ions that have one atom in the center and six atoms at the corners of a octahedron.

Ø           Octane Number

Ø           A number that indicates how smoothly a gasoline burns.

Ø           Octet Rule

Ø           Many representative elements attain at least a share of eight electrons in their valence shells when they form molecular or ionic compounds; there are some limitations.

Ø           Oil

Ø           Liquid triester of glycerol and unsaturated fatty acids.

Ø           Open Sextet

Ø           Refers to species that have only six electrons in the highest energy level of the central element (many Lewis acids).

Ø           Optical Activity

Ø           The rotation of plane polarized light by one of a pair of optical isomers.

Ø           Optical Isomers

Ø           Stereoisomers that differ only by being nonsuperimposable mirror images of each other， like right and left hands， also called enantiomers.

Ø           Ore

Ø           A natural deposit containing a mineral of an element to be extracted.

Ø           Organic Chemistry

Ø           The chemistry of substances that contain carbon-hydrogen bonds.

Ø           Osmosis

Ø           The process by which solvent molecules pass through a semipermable membrane from a dilute solution into a more concentrated solution.

Ø           Osmotic Pressure

Ø           The hydrostatic pressure produced on the surface of a semipermable membrane by osmosis.

Ø           Ostwald Process

Ø           A process for the industrial production of nitrogen oxide and nitric acid from ammonia and oxygen.

Ø           Outer Orbital Complex

Ø           Valence bond designation for a complex in which the metal ion utilizes d orbitals in the outermost (occupied) shell in hybridization.

Ø           Overlap

Ø           The interaction of orbitals on different atoms in the same region of space.

Ø           Oxidation

Ø           An algebraic increase in the oxidation number; may correspond to a loss of electrons.

Ø           Oxidation Numbers

Ø           Arbitrary numbers that can be used as mechanical aids in writing formulas and balancing equations; for single- atom ions they correspond to the charge on the ion; more electronegative atoms are assigned negative oxidation numbers (also called Oxidation states).

Ø           Oxidation-reduction Reactions

Ø           Reactions in which oxidation and reduction occur; also called redox reactions.

Ø           Oxide

Ø           A binary compound of oxygen.

Ø           Oxidizing Agent

Ø           The substance that oxidizes another substance and is reduced.

Ø           Chemistry Terminology P

Ø           Pairing

Ø           A favourable interaction of two electrons with opposite m ， values in the same orbital.

Ø           Pairing Energy

Ø           Energy required to pair two electrons in the same orbital.

Ø           Paramagnetism

Ø           Attraction toward a magnetic field， stronger than diamagnetism， but still weak compared to ferromagnetism.

Ø           Partial Pressure

Ø           The pressure exerted by one gas in a mixture of gases.

Ø           Particulate Matter

Ø           Fine divided solid particles suspended in polluted air.

Ø           Pauli Exclusion Principle

Ø           No two electrons in the same atom may have identical sets of four quantum numbers.

Ø           Percentage Ionization

Ø           The percentage of the weak electrolyte that ionizes in a solution of given concentration.

Ø           Percent by Mass

Ø           100% times the actual yield divided by theoretical yield.

Ø           Percent Composition

Ø           The mass percent of each element in a compound.

Ø           Percent Purity

Ø           The percent of a specified compound or element in an impure sample.

Ø           Period

Ø           The elements in a horizontal row of the periodic table

Ø           Periodicity

Ø           Regular periodic variations of properties of elements with atomic number (and position in the periodic table).

Ø           Periodic Law

Ø           The properties of the elements are periodic functions of their atomic numbers.

Ø           Periodic Table

Ø           An arrangement of elements in order of increasing atomic numbers that also emphasizes periodicity.

Ø           Peroxide

Ø           A compound containing oxygen in the -1 oxidation state. Metal peroxides contain the peroxide ion， O22-

Ø           pH

Ø           Negative logarithm of the concentration (mol/L) of the H3O+[H+] ion; scale is commonly used over a range 0 to 14.

Ø           Phase Diagram

Ø           Diagram that shows equilibrium temperature-pressure relationships for different phases of a substance.

Ø           Phenol

Ø           Hydrocarbon derivative containing an [OH] group bound to an aromatic raing.

Ø           Photochemical Oxidants

Ø           Photochemically produced oxidizing agents capable of causing damage to plants and animals.

Ø           Photochemical Smog

Ø           A brownish smog occurring in urban areas receiving large amounts of sunlight; caused by photochemical (light-induced) reactions among nitrogen oxides， hydrocarbons and other components of polluted air that produce photochemical oxidants.

Ø           Photoelectric Effect

Ø           Emission of an electron from the surface of a metal caused by impinging electromagnetic radiation of certain minimum energy; current increases with increasing intensity of radiation.

Ø           Photon

Ø           A packet of light or electromagnetic radiation; also called quantum of light

Ø           Physical Change

Ø           A change in which a substance changes from one physical state to another but no substances with different composition are formed. Example Gas to Liquid - Solid.

Ø           Plasma

Ø           A physical state of matter which exists at extremely high temperatures in which all molecules are dissociated and most atoms are ionized.

Ø           Polar Bond

Ø           Covalent bond in which there is an unsymmetrical distribution of electron density.

Ø           Polarimeter

Ø           A device used to measure optical activity.

Ø           Polarization

Ø           The buildup of a product of oxidation or a reduction of an electrode， preventing further reaction.

Ø           Polydentate

Ø           Refers to ligands with more than one donor atom.

Ø           Polyene

Ø           A compound that contains more than one double bond per molecule.

Ø           Polymerization

Ø           The combination of many small molecules to form large molecules.

Ø           Polymer

Ø           A large molecule consisting of chains or rings of linked monomer units， usually characterized by high melting and boiling points.

Ø           Polymorphous

Ø           Refers to substances that crystallize in more than one crystalline arrangement.

Ø           Polyprotic Acid

Ø           An Acid that can form two or more hydronium ions per molecule; often a least one step of ionization is weak.

Ø           Positron

Ø           A Nuclear particle with the mass of an electron but opposite charge.

Ø           Potential Energy

Ø           Energy that matter possesses by virtue of its position， condition or composition.

Ø           Precipitate

Ø           An insoluble solid formed by mixing in solution the constituent ions of a slightly soluble solution.

Ø           Primary Standard

Ø           A substance of a known high degree of purity that undergoes one invariable reaction with the other reactant of interest.

Ø           Primary Voltaic Cells

Ø           Voltaic cells that cannot be recharged; no further chemical reaction is possible once the reactants are consumed.

Ø           Proton

Ø           A subatomic particle having a mass of 1.0073 amu and a charge of +1， found in thew nuclei of atoms.

Ø           PseudobinaryIonic Compounds

Ø           Compounds that contain more than two elements but are named like binary compounds.



Ø           Chemistry Terminology Q



Ø           Quantum Mechanics

Ø           Mathematical method of treating particles on the basis of quantum theory， which assumes that energy (of small particles) is not infinitely divisible.

Ø           Quantum Numbers

Ø           Numbers that describe the energies of electrons in atoms; derived from quantum mechanical treatment.

Ø           Chemistry Terminology R

Ø           Radiation

Ø           High energy particles or rays emitted during the nuclear decay processes.

Ø           Radical

Ø           An atom or group of atoms that contains one or more unpaired electrons (usually very reactive species)

Ø           Radioactive Dating

Ø           Method of dating ancient objects by determining the ratio of amounts of mother and daughter nuclides present in an object and relating the ratio to the object?s age via half-life calculations.

Ø           Radioactive Tracer

Ø           A small amount of radioisotope replacing a nonradioactive isotope of the element in a compound whose path (for example， in the body) or whose decomposition products are to be monitored by detection of radioctivity; also called a radioactive label.

Ø           Radioactivity

Ø           The spontaneous disintegration of atomic nuclei.

Ø           Raoult's Law

Ø           The vapor pressure of a solvent in an ideal solution decreases as its mole fraction decreases.

Ø           Rate-determining Step

Ø           The slowest step in a mechanism; the step that determines the overall rate of reaction.

Ø           Rate-law Expression

Ø           Equation relating the rate of a reaction to the concentrations of the reactants and the specific rate of the constant.

Ø           Rate of Reaction

Ø           Change in the concentration of a reactant or product per unit time.

Ø           Reactants

Ø           Substances consumed in a chemical reaction.

Ø           Reaction Quotient

Ø           The mass action expression under any set of conditions (not necessarily equlibrium); its magnitude relative to K determines the direction in which the reaction must occur to establish equilibrium.

Ø           Reaction Ratio

Ø           The relative amounts of reactants and products involved in a reaction; maybe the ratio of moles. millimoles， or masses.

Ø           Reaction Stoichiometry

Ø           Description of the quantitative relationships among substances as they participate in chemical reactions.

Ø           Reducing Agent

Ø           The substance that reduces another substance and is oxidized.

Ø           Resonance

Ø           The concept in which two or more equivalent dot formulas for the same arrangement of atoms (resonance structures) are necessary to describe the bonding in a molecule or ion.

Ø           Reverse Osmosis

Ø           Forcing solvent molecules to flow through a semipermable membrane from a concentated solution into a dilute solution by the application of greater hydrostatic pressure on concentrated side than the osmotic pressure opposing it.

Ø           Reversible Reaction

Ø           Reactions that do not go to completion and occur in both the forward and reverse direction.

Ø           Chemistry Terminology S

Ø           Salt Bridge

Ø           A U-shaped tube containing electrolyte， which connects two half-cells of a voltaic cell.

Ø           Saponification

Ø           Hydrolysis of esters in the presence of strong soluable bases.

Ø           Saturated Hydrocarbons

Ø           Hydrocarbons that contain only single bonds. They are also called alkanes or paraffin hydrocarbons.

Ø           Saturated Solution

Ø           Solution in which no more solute will dissolve.

Ø           Second Law of Thermodynamics

Ø           The universe tends toward a state of greater diorder in spontaneous processes.

Ø           Secondary Standard

Ø           a solution that has been titrated against a primary standard. A standard solution is a secondary standard.

Ø           Secondary Voltaic Cells

Ø           Voltaic cells that can be recharged; original reactanats can be regenerated be reversing the direction of the current flow.

Ø           Semiconductor

Ø           A substance that does not conduct electricity at low temperatures but does so at higher temperatures.

Ø           Semipermable Membrane

Ø           A thin partition between two solutions through which certain molecules can pass but others cannot.

Ø           Shielding Effect

Ø           Electrons in filled sets of s ， p orbitals between the nucleus and outer shell electrons shield the outer shell electrons somewhat from the effect of protons in the nucleus; also called screening effect.

Ø           Sigma Bonds

Ø           Bonds resulting from the head-on overlap of atomic orbitals， in which the region of electron sharing is along and (cylindrically) symmetrical to the imaginary line connecting the bonded atoms.

Ø           Sigma Orbital

Ø           Molecular orbital resulting from head-on overlap of two atomic orbitals.

Ø           Silicones

Ø           Polymeric organosilicon compounds; contain individual or cross-linked Si-O chains or rings in which some oxygens of SiO4 tetrahedra are replaced by other groups.

Ø           Single Bond

Ø           Covalent bond resulting from the sharing of two electrons (one pair) between two atoms.

Ø           Solubility Product Constant

Ø           Equilibrium constant that applies to the dissolution of a slightly soluble compound.

Ø           Solubility Product Principle

Ø           The solubility product constant expression for a slightly soluble compound is the product of the concentrations of the constituent ions， each raised to the power that corresponds to the number of ions in one formula unit.

Ø           Solute

Ø           The dispersed (dissolved) phase of a solution.

Ø           Solution

Ø           Homogeneous mixture of two or more substances.

Ø           Solvation

Ø           The process by which solvent molecules surround and interact with solute ions or molecules.

Ø           Solvent

Ø           The dispersing medium of a solution.

Ø           Solvolysis

Ø           The reaction of a substance with the solvent in which it is dissolved.

Ø           S Orbital

Ø           A spherically symmetrical atomic orbital; one per energy level.

Ø           Specific Gravity

Ø           The ratio of the density of a substance to the density of water.

Ø           Specific Heat

Ø           The amount of heat required to raise the temperature of one gram of substance one degree Celsius.

Ø           Specific Rate Constant

Ø           An experimentally determined (proportionality) constant， which is different for different reactions and which changes only with temperature; k in the rate-law expression: Rate = k [A] x [B]v.

Ø           Spectator Ions

Ø           Ions in a solution that do not participate in a chemical reaction.

Ø           Spectral Line

Ø           Any of a number of lines corresponding to definite wavelengths of an atomic emission or absorption spectrum; represents the energy difference between two energy levels.

Ø           Spectrochemical Series

Ø           Arrangement of ligands in order of increasing ligand field strength.

Ø           Spectrum

Ø           Display of component wavelengths (colours) of electromagnetic radiation.

Ø           Square Planar

Ø           A term used to describe molecules and polyatomic ions that have one atom in the center and four atoms at the corners of a square.

Ø           Square Planar Complex

Ø           Complex in which the metal is in the center of a square plane， with ligand donor atoms at each of the four corners

Ø        &n, bsp;  Standard Electrodes

Ø           Half-cells in which the oxidized and reduced forms of a species are present at unit activity; 1.0M solutions of dissolved ions， 1.0atm partial pressure of gases， and pure solids and liquids.

Ø           Standard Electrode Potential

Ø           By convention ， potential， Eo， of a half-reaction as a reduction relative to the standard hydrogen electrode when all species are present at unit activity.

Ø           Standard Entropy

Ø           The absolute entropy of a substance in its standard state at 298 K.

Ø           Standard Molar Enthalphy of Formation

Ø           The amount of heat absorbed in the formation of one mole of a substance in a specified state from its elements in their standard states.

Ø           Standard Molar Volume

Ø           The volume occupied by one mole of an ideal gas under standard conditions; 22.4liters.

Ø           Standard Reaction

Ø           A reaction in which the numbers of moles of reactants shown in the balanced equation， all in their standard states， are completely converted to the numbers of moles of products shown in the balanced equation， also sall at their standard state.

Ø           Stereoisomers

Ø           Isomers that differ only in the way that atoms are oriented in space; consist of geometrical and optical isomers.

Ø           Stoichiometry

Ø           Description of the quantitative relationships among elements and compounds as they undergo chemical changes.

Ø           Strong Electrolyte

Ø           A substance that conducts electricity well in a dilute aqueous solution.

Ø           Strong Field Ligand

Ø           Ligand that exerts a strong crystal or ligand electrical field and generally forms low spin complexes with metal ions when possible.

Ø           Structural Isomers

Ø           Compounds that contain the same number of the same kinds of atoms in different geometric arrangements.

Ø           Sublimation

Ø           The direct vaporization of a sold by heating without passing through the liquid state.

Ø           Substance

Ø           Any kind of matter all specimens of which have the same chemical composition and physical properties.

Ø           Substitution Reaction

Ø           A reaction in which an atom or a group of atoms is replaced by another atom or group of atoms.

Ø           Supercooled Liquids

Ø           Liquids that， when cooled， apparently solidify but actually continue to flow very slowly under the influence of gravity.

Ø           Supercritical Fluid

Ø           A substance at temperature above its critical temperature.

Ø           Supersaturated Solution

Ø           A solution that contains a higher than saturation concentration of solute; slight disturbance or seeding causes crystallization of excess solute.

Ø           Suspension

Ø           A heterogeneous mixture in which solute-like particles settle out of solvent-like phase some time after their introduction.



Ø           Chemistry Terminology T



Ø           Temperature

Ø           A measure of the intensity of heat， i.e. the hotness or coldness of a sample. or object.

Ø           Ternary Acid

Ø           A ternary compound containing H， O， and another element， often a nonmetal.

Ø           Ternary Compound

Ø           A compound consisting of three elements; may be ionic or covalent.

Ø           Tetrahedral

Ø           A term used to describe molecules and polyatomic ions that have one atom in center and four atoms at the corners of a tetrahedron.

Ø           Theoretical Yield

Ø           Maximum amount of a specified product that could be obtained from specified amounts of reactants， assuming complete consumption of limiting reactant according to only one reaction and complete recovery of product. (Compare with Actual Yield)

Ø           Thermal Cracking

Ø           Decomposition by heating a substance in the presence of a catalyst and in the absence of air.

Ø           Thermodynamics

Ø           The study of the energy transfers accompanying physical and chemical processes.

Ø           Thermonuclear Energy

Ø           Energy from nuclear fusion reactions.

Ø           Third Law of Thermodynamics

Ø           The entropy of a hypothetical pure， perfect， crystalline sustance at absolute zero temperature is zero.

Ø           Titration

Ø           A Procedure in which one solution is added to another solution until the chemical reaction between the two solutes is complete; the concentration of one solution is known and that of the other is unknown.

Ø           Total Ionic Equation

Ø           Equation for a chemical reaction written to show the predominant form of all species in aqueous solution or in contact with water.

Ø           Transition State Theory

Ø           Theory of reaction rates that states that reactants pass through high-energy transition states before forming products.

Ø           Tyndall Effect

Ø           The scattering of light by colloidal particles.

Ø           Chemistry Terminology U

Ø           Unsaturated Hydrocarbons

Ø           Hydrocarbons that contain double or triple carbon-carbon bonds.

Ø           Chemistry Terminology V

Ø           Valence Bond Theory

Ø           Assumes that covalent bonds are formed when atomic orbitals on different atoms overlap and the electrons are shared.

Ø           Valence Electrons

Ø           Outermost electrons of atoms; usually those involved in bonding.

Ø           Valence Shell Electron Pair Repulsion Theory

Ø           Assumes that electron pairs are arranged around the central element of a molecule or polyatomic ion so that there is maximum separation (and minimum repulsion) among regions of high electron density.

Ø           van der Waals' Equation

Ø           An equation of state that extends the ideal gas law to real gases by inclusion of two empirically determined parameters， which are different for different gases.

Ø           Vapor

Ø           A gas formed by boiling or evaporating a liquid.

Ø           Vapor Pressure

Ø           The particle pressure of a vapor at the surface of its parent liquid.

Ø           Voltage

Ø           Potential difference between two electrodes; a measure of the chemical potential for a redox reaction to occur.

Ø           Voltaic Cells

Ø           Electrochemical cells in which spontaneous chemical reactions produce electricity; also called galvanic cells.

Ø           Chemistry Terminology W

Ø           Water Equivalent

Ø           The amount of water that would absorb the same amount of heat as the calorimeter per degree temperature increase.

Ø           Weak Electrolyte

Ø           A substance that conducts electricity poorly in a dilute aqueous solution.

Ø           Weak Field Ligand

Ø           A Ligand that exerts a weak crystal or ligand field and ge- nerally forms high spin complexes with metals.

Ø           Chemistry Terminology Z

Ø           Zone Refining

Ø           A method of purifying a bar of metal by passing it through an induction heater; this causes impurties to move along a melted portion.

alenkhoo

Thanks. good info