Vinnitsa National Pirogov Memorial Medical UniversityBiological and General Chemistry Department

Medical chemistry course

CHEMISTRY DICTIONARY

Vinnitsa 2010

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Systematic course is approved by academic council of Pirogov National Medical Universityof Vinnitsa (minutes № 5 from 2.03.2011)

Authors:Assistant Professor Smirnova O.V.

Assistant Professor Chervyak M.M.Assist. Shunkov V.S.

Reviewer:

Azarov O.S.- Candidate of chemistry science, assistant professorDepartment of Biological and General Chemistry VNMU

Marchak T.V.- Candidate of chemistry science, assistant professorDepartment of Physiological Agriculture and Live Stock

Breeding and Chemistry VNAU

Shitova T.V. – Senior-lecturerDepartment of Russian and Ukrainian languages

Head of English language courses VNMU

Printing group VNMU:Text editor – Shunkov V.S.

Computer editor – Shunkov V.S.Secretary Koroleva N.D.

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Contents:

1) Chemistry Dictionary ……………………………………………………………………….42) Products: Complete List…………………………………………………………………….47

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AAbsolute Entropy (of a substance)The increase in the entropy of a substance as it goes from a perfectly ordered crystalline form at0 °K (where its entropy is zero) to the temperature in question.

Absolute ZeroThe zero point on the absolute temperature scale; -273.15°C or 0 K; theoretically, thetemperature at which molecular motion ceases.

Absorption SpectrumSpectrum associated with absorption of electromagnetic radiation by atoms (or other species)resulting from transitions from lower to higher energy states.

AccuracyHow closely a measured value agrees with the correct value.

AcidA substance that produces H+(aq) ions in aqueous solution. Strong acids ionize completely oralmost completely in dilute aqueous solution. Weak acids ionize only slightly.

Acid AnhydrideThe oxide of a nonmetal that reacts with water to form an acid.

Acid AnhydrideCompound produced by dehydration of a carbonic acid; general formula is R--C--O--C--R

Acidic SaltA salt containing an ionizable hydrogen atom; does not necessarily produce acidic solutions.

Activation EnergyAmount of energy that must be absorbed by reactants in their ground states to reach thetransition state so that a reaction can occur.

Active MetalMetal 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 SeriesA listing of metals (and hydrogen) in order of decreasing activity

Actual YieldAmount of a specified pure product actually obtained from a given reaction. Compare withTheoretical Yield.

ActinidesElements 90 to 103 (after actinium)

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Acyl GroupCompound derived from a carbonic acid by replacing the --OH group with a halogen (X),usually --Cl; general formula is O R--C--X

Addition ReactionA reaction in which two atoms or groups of atoms are added to a molecule, one on each side of adouble or triple bond

Adhesive ForcesForces of attraction between a liquid and another surface.

AdsorptionAdhesion of a species onto the surfaces of particles

AlcoholHydrocarbon derivative containing an --OH group attached to a carbon atom not in an aromaticring.

AldehydeCompound in which an alkyl or aryl group and a hydrogen atom are attached to a carbonyl groupand a hydrogen atom are attached to a carbonyl group; general formula, O-R-C-H

Alkali MetalsMetals of Group IA (Na, K, Rb).

Alkaline BatteryA dry cell in which the electrolyte contains KOH.

Alkaline Earth MetalsGroup IIA metals

Alkenes (Olefins)Unsaturated hydrocarbons that contain one or more carbon-carbon double bonds.

Alkyl GroupA group of atoms derived from an alkane by the removal of one hydrogen atom.

AlkylbenzeneA compound containing an alkyl group bonded to a benzene ring.

AlkynesUnsaturated hydrocarbons that contain one or more carbon-carbon triple bonds.

AllotropesDifferent forms of the same element in the same physical state.

Allotropic Modifications (Allotropes)Different forms of the same element in the same physical state.

AlloyingMixing of metal with other substances (usually other metals) to modify its properties.

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Alpha ParticleA helium nucleus.

Alpha (a) ParticleHelium ion with 2+ charge; an assembly of two protons and two neutrons.

AlumsHydrated sulfates of the general formula M+M3+(SO4)2 *12H2).

AmideCompound containing the O-C-N group.Compound that can be considered a derivative of ammonia in which one or more hydrogens arereplaced by a alkyl or aryl groups.

AmineDerivatives of ammonia in which one or more hydrogen atoms have been replaced by organicgroups.

Amine ComplexesComplex species that contain ammonia molecules bonded to metal ions.

Amino AcidCompound containing both an amino and a carboxylic acid group.The --NH2 group.

Amorphous SolidA noncrystalline solid with no well-defined ordered structure.

AmpereUnit of electrical current; one ampere equals one coulomb per second.

AmphiprotismAbility of a substance to exhibit amphiprotism by accepting donated protons.

AmphoterismThe ability to react with both acids and bases. Ability of substance to act as either an acid or abase.

AnionA negative ion; an atom or goup of atoms that has gained one or more electrons.

AnodeIn a cathode ray tube, the positive electrode. Electrode at which oxidation occurs.

Antibonding OrbitalA 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 HydrocarbonsBenzene and its derivatives.

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Artificial TransmutationAn artificially induced nuclear reaction caused by the bombardment of a nucleus with subatomicparticiles or small nucei.

Aryl GroupGroup of atoms remaining after a hydrogen atom is removed from the aromatic system.

Associated IonsShort-lived species formed by the collision of dissolved ions of opposite charges.

AtmosphereA unit of pressure; the pressure that will support a column of mercury 760 mm high at 0 °C.

AtomThe 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 andformula weights; also called dalton.

Atomic NumberIntegral number of protons in the nucleus; defines the identity of element.

Atomic OrbitalRegion or volume in space in which the probability of finding electrons is highest.

Atomic RadiusRadius of an atom.

Atomic WeightWeighted average of the masses of the constituent isotopes of an element; The relative masses ofatoms of different elements.

Aufbau ('building up') PrincipleDescribes the order in which electrons fill orbitals in atoms.

AutoionizationAn ionization reaction between identical molecules.

Avogadro's LawAt the same temperature and pressure, equal volumes of all gases contain the same number ofmolecules.

Avogadro's NumberThe number (6.022x1023) of atoms, molecules or particles found in exactly 1 mole of substance.

BBackground RadiationRatiation extraneous to an experiment. Usually the low-level natural radiation form cosmic raysand trace radioactive substances present in our environment.

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BandA series of very closely spaced, nearly continuous molecular orbitals that belong to the crystal asa whole.

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

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

BarometerA device for measuring pressure.

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

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

Basic SaltA salt containing an ionizable OH group.

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

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

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

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

Binding Energy (nuclear binding energy)The energy equivalent (E = mc2) 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/s2

Boiling PointThe temperature at which the vapor pressure of a liquid is equal to the applied pressure; also thecondensation point

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

Bomb CalorimeterA device used to measure the heat transfer between system and surroundings at constant volume.

Bond EnergyThe amount of energy necessary to break one mole of bonds of a given kind (in gas phase).

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The amount of energy necessary to break one mole of bonds in a substance, dissociating thesustance in the gaseous state into atoms of its elements in the gaseous state.

Bond OrderHalf the numbers of electrons in bonding orbitals minus half the number of electrons inantibonding orbitals.

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

Bonding PairPair of electrons involved in a covalent bond.

Boron HydridesBinary compounds of boron and hydrogen.

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

Boyle's LawAt constant temperature the volume occupied by a definite mass of a gas is inverselyproportional to the applied pressure.

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

Bronsted-Lowry AcidA proton donor.

Bronsted-Lowry BaseA proton acceptor

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

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

CCalorieThe amount of heat required to raise the temperature of one gram of water from 14.5°C to15.5°C. 1 calorie = 4.184 joules.

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

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Canal RayStream of positively charged particles (cations) that moves toward the negative electrode incathode ray tubes; observed to pass through canals in the negative electrode.

CapillaryA tube having a very small inside diameter.

Capillary ActionThe drawing of a liquid up the inside of a small-bore tube when adhesive forces exceed cohesiveforces, or the depression of the surface of the liquid when cohesive forces exceed the adhesiveforces.

CarbanionAn organic ion carrying a negative charge on a carbon atom.

Carbonium ionAn orgainic ion carrying a positive charge on a carbon atom.

CarcinogenA substance capable of causing or producing cancer in mammals.

CatalystA substance that speeds up a chemical reaction without being consumed itself in the reaction.A substance that alters (usually increases) the rate at which a reaction occurs.

CatenationBonding of atoms of the same element into chains or rings. The bonding together of atoms of thesame element to form chains. The ability of an element to bond to itself.

CathodeElectrode at which reduction occurs. In a cathode ray tube, the negative electrode.

Cathodic ProtectionProtection of a metal (making ir a cathode) against corrosion by attaching it to a sacrifical anodeof a more easily oxidized metal.

Cathode Ray TubeClosed glass tube containing a gas under low pressure, with electrodes near the ends and aluminescent screen at the end near the positive electrode; produces cathode rays when highvoltage is applied.

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

Cell PotentialPotential difference, Ecell, between oxidation and reduction half-cells under nonstandardconditions.

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

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Chain ReactionA reaction that, once initiated, sustains itself and expands. This is a reaction in which reactivespecies, such as radicals, are produced in more than one step. These reactive species, radicals,propagate the chain reaction.

Chain Termination StepThe combination of two radicals, which removes the reactive species that propagate the changereaction.

Charle's LawAt constant pressure the volume occupied by a definite mass of gas is directly proportional to itsabsolute temperature.

Chemical BondsThe attractive forces that hold atoms together in elements or compounds.

Chemical ChangeA change in which one or more new substances are formed.

Chemical EquationDescription of a chemical reaction by placing the formulas of the reactants on the left and theformulas of products on the right of an arrow.

Chemical EquilibriumA state of dynamic balance in which the rates of forward and reverse reactions are equal; there isno net change in concentrations of reactants or products while a system is at equilibrium.

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

Chemical Hygiene Plan (CHP)A written program developed and implemented by an employer designating proceedures,equipment, personal protective equipment, and work practices that are capable of protectingemployees from the health hazards presented by hazardous chemicals usid in that particularworkplace.

Chemical KineticsThe study of rates and mechanisms of chemical reactions and of the factors on which theydepend.

Chemical PeriodicityThe variations in properties of elements with their position in the periodic tableCis- The prefix used to indicate that groups are located on the same side of a bon about whichrotation is restricted.Cis-Trans IsomerismA type of geometrical isomerism related to the angles between like ligands.

ClayA class of silicate and aluminosilicate minerals with sheet-like structures that have enormoussurface areas that can absorb large amounts of water.

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Cloud ChamberA device for observing the paths of speeding particiles as vapor molecules condense on them toform foglike tracks.

Coefficient of expansionThe ratio of the change in length or volumen of a body to the original lengthor volume for a unitchange in temperature.

Cohesive ForcesAll the forces of attraction among particles of a liquid.

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

Colligative PropertiesPhysical properties of solutions that depend upon the number but not the kind of solute particlespresent.

Collision TheoryTheory of reaction rates that states that effective collisions between reactant molecules mustoccur in order for the reaction to occur.

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

Combination ReactionReaction in which two substances ( elements or compounds ) combine to form one compound.Reaction of a substance with oxygen in a highly exothermic reaction, usually with a visibleflame.

CombustibleClassification of liquid substances that will burn on the basis of flash points. A combustibleliquid 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.

Common Ion EffectSuppression of ionization of a weak electrolyte by the presence in the same solution of a strongelectrolyte containing one of the same ions as the weak electrolyte.

Complex IonsIons resulting from the formation of coordinate covalent bonds between simple ions and otherions or molecules.

Composition StoichiometryDescibes the quantitative (mass) relationships among elements in compounds.

CompoundA substance of two or more elements in fixed proportions. Compounds can be decomposed intotheir constituent elements.

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Compressed GasA gas or mixture of gases having, in a container an absolute pressure exceeding 40 psi at 21.1°C(70°F)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)A liquid having a vapour pressure exceeding 40 psi at 37.8°C (70°F) as determined by ASTM D-323-72.

ConcentrationAmount of solute per unit volume or mass of solvent or of solution.

CondensationLiquefaction of vapor.

Condensed PhasesThe liquid and solid phases; phases in which particles interact strongly.

Condensed StatesThe solid and liquid states.

Conduction BandA 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 tooccur in a solid.

Conjugate Acid-base PairIn Bronsted-Lowry terminology, a reactant and product that differ by a proton, H+.

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

Continuous SpectrumSpectrum that contains all wave-lengths in a specified region of the electromagnetic spectrum.

Control RodsRods of materials such as cadmium or boron steel that act as neutron obsorbers (not merelymoderaters) used in nuclear reactors to control neutron fluxes and therfore rates of fission.

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

Contact ProcessIndustrial process by which sulfur trioxide and sulfuric acid are produced from sulfur dioxide.

Coordinate Covalent BondA covalent bond in which both shared electrons are donated by the same atom; a bond between aLewis base and a Lewis acid.

Coordination Compound or ComplexA compound containing coordinate covalent bonds.

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Coordination IsomersIsomers involving exchanges of ligands between complex cation and complex anion of the samecompound.

Coordination NumberIn describing crystals, the number of nearest neighbours of an atom or ion.The number of donor atoms coordinated to a metal.

Coordination SphereThe metal ion and its coordinating ligands but not any uncoordinated counter-ions.

CorrosionOxidation of metals in the presence of air and moisture.

CoulombUnit of electrical charge.

CoulometryThe quantitative application of Faraday's Law to the analysis of materials. The current and timeare the usual variables measured.

Covalent BondChemical bond formed by the sharing of one or more electron pairs between two atoms.

Covalent CompoundsCompounds containing predominantly covalent bonds.

Critical MassThe minimum mass of a particular fissionable nuclide in a given volume required to sustain anuclear chain reaction.

Critical PointThe combination of critical temperature and critical pressure of a substance.

Critical PressureThe pressure required to liquefy a gas (vapor) at its critical temperature.

Critical TemperatureThe temperature above which a gas cannot be liquefied; the temperature above which asubstance cannot exhibit distinct gas and liquid phases.

Crystal Field Stabilization EnergyA measure of the net energy of stabilization gained by a metal ion's nonbonding d electrons as aresult of complex formation.

Crystal Field TheoryTheory of bonding in transition metal complexes in which ligands and metal ions are treated aspoint charges; a purely ionic model; ligand point charges represent the crystal (electrical) fieldperturbing the metals d orbitals containing nonbonding electrons.

Crystal LatticeA pattern of arrangement of particles in a crystal.

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Crystal Lattice EnergyAmount of energy that holds a crystal together; the energy change when a mole of solid isformed from its constituent molecules or ions (for ionic compounds) in their gaseous state.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.

Crystalline SolidA solid characterized by a regular, ordered arrangement of particles.

Curie (Ci)The basic unit used to describe the intensity of radioactivity in a sample of material. One curieequals 37 billion disintegrations per second or approximately the amount of radioactivty givenoff by 1 gram of radium.

CyclotronA device for accelerating charged particles along a spiral path.

DDaughter NuclideNuclide that is produced in a nuclear decay.

DebyeThe unit used to express dipole moments.

DegenerateOf the same energy.

DelocalizationOf electrons; refers to bonding electrons that are distributed among more than two atoms that arebonded together; occurs in species that exhibit resonance.The formation of a set of molecular orbitals that extend over more than two atoms; important inspecies that valence bond theory describes in terms of resonance.

DenaturationA process pertaining to a change in structure of a protein form regular to irregular arrangementof the polypeptide chains.

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

DensityMass per unit Volume: D=MV

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

DerivativeA compound that can be imagined to arise from a partent compound by replacement of one atomwith another atom or group of atoms. Used extensively in orgainic chemistry to assist inidentifying compounds.

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Dermal toxicityAdverse health effects resulting from skin exposure ot a substance.

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

DetergentA soap-like emulsifer that contains a sulfate, SO3 or a phosphate group instead of a carboxylategroup.

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

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

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

DiamagnetismWeak repulsion by a magnetic field.

Differential Scanning Calorimetry (DSC)A technique for measuring the temperature, direction, and magnitude of thermal transitions in asample material by heating/cooling and comparing the amount of energy required to maintain itsrate of temperature increase or decrease with an inert reference material under similar conditions.

Differential Thermal Analysis (DTA)A technique for observing the temperature, direction, and magnitude of thermally inducedtransitions in a material by heating/cooling a sample and comparing its temperature with that ofan inert reference material under similar conditions.

Differential ThermometerA thermometer used for accurate measurement of very small changes in temperature.

DilutionProcess of reducing the concentration of a solute in solution, usually simply by mixing withmore solvent.

DimerMolecule formed by combination of two smaller (identical) molecules.

DipoleRefers to the separation of charge between two covalently bonded atoms

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Dipole-dipole InteractionsAttractive interactions between polar molecules, that is, between molecules with permanentdipoles.

Dipole MomentThe product of the distance separating opposite charges of equal magnitude of the charge; ameasure of the polarity of a bond or molecule; a measured dipole moment refers to the dipolemoment of an entire molecule.

Dispersing MediumThe solvent-like phase in a colloid.

Dispersed PhaseThe solute-like species in a colloid.

Displacement ReactionsReactions in which one element displaces another from a compound.

Disproportionation ReactionsRedox reactions in which the oxidizing agent and the reducing agent are the same species.

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

Dissociation ConstantEquilibrium constant that applies to the dissociation of a comples ion into a simple ion andcoordinating species (ligands).

DistillandThe material in a distillation apparatus that is to be distilled.

DistillateThe material in a distillation apparatus that is collected in the receiver.

DistillationThe separation of a liquid mixture into its components on the basis of differences in boilingpoints.The process in which components of a mixture are separated by boiling away the more volitileliquid.

DomainA cluster of atoms in a ferromagnetic substance, all of which align in the same direction in thepresence of an external magnetic field.

Donor AtomA ligand atom whose electrons are shared with a Lewis acid.

D-OrbitalsBeginning in the third energy level, aset of five degenerate orbitals per energy level, higher inenergy than s and p orbitals of the same energy level.

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DosimeterA small, calibrated electroscope worn by laboratory personnel and designated to detect andmeasure incident ionizing radiation or chemical exposure.

Double BondCovalent bond resulting from the sharing of four electrons (two pairs) between two atoms.

Double SaltSolid consisting of two co-crystallized salts.

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

Downs CellElectrolytic cell for the commercial electrolysis of molten sodium chloride.

DP numberThe degree of polymerization; the average number of monomer units per polymer unit.

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

D -Transition elements (metals)B Group elements except IIB in the periodic table; sometimes called simply transition elementsEX. Fe, Ni, Cu, Ti .

Dumas MethodA method used to determine the molecular weights of volatile liquids.

Dynamic EquilibriumAn equilibrium in which processes occur continuously, with no net change.When two (or more) processes occur at the same rate so that no net change occurs.

EEffective CollisonsCollision between molecules resulting in a reaction; one in which the molecules collide withproper relative orientations and sufficient energy to react.

Effective MolalityThe sum of the molalities of all solute particles in a solution.

Effective Nuclear ChargeThe nuclear charge experienced by the outermost electrons of an atom; the actual nuclear chargeminus the effects of shielding due to inner-shell electrons.Example: Set of dx2-y2 and dz2 orbitals; those d orbitals within a set with lobes directed alongthe x-, y-, and z-axes.

Electrical ConductivityAbility to conduct electricity.

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ElectrochemistryStudy of chemical changes produced by electrical current and the production of electricity bychemical reactions.

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

Electrode PotentialsPotentials, E, of half-reactions as reductions versus the standard hydrogen electrode.

ElectrolysisProcess that occurs in electrolytic cells.

ElectrolyteA substance whose aqueous solutions conduct electricity.

Electrolytic CellsElectrochemical cells in which electrical energy causes nospontaneous redox reactions to occur.An electrochemical cell in which chemical reactions are forced to occur by the application of anoutside source of electrical energy.

Electrolytic ConductionConduction of electrical current by ions through a solution or pure liquid.

Electromagnetic RadiationEnergy that is propagated by means of electric and magnetic fields that oscillate in directionsperpendicular to the direction of travel of the energy.

Electromotive SeriesThe relative order of tendencies for elements and their simple ions to act as oxidizing or reducingagents; also called the activity series.

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

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

Electron ConfigurationSpecific distribution of electrons in atomic orbitals of atoms or ions.

Electron Deficient CompoundsCompounds that contain at least one atom (other than H+) that shares fewer than eight electrons

Electronic TransitionThe transfer of an electron from one energy level to another.

ElectronegativityA measure of the relative tendency of an atom to attract electrons to itself when chemicallycombined with another atom.

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Electronic GeometryThe geometric arrangement of orbitals containing the shared and unshared electron pairssurrounding the central atom of a molecule or polyatomic ion.

ElectrophilePositively charged or electron-deficient.

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

ElectroplatingPlating a metal onto a (cathodic) surface by electrolysis.

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

Eluant or eluentThe solvent used in the process of elution, as in liquid chromatography.

EluateSolvent (or mobile phase) which passes through a chromatographic column and removes thesample components from the stationary phase.

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

Emulsifying AgentA sustance that coats the particles of the dispersed phase and prevents coagulation of colloidalparticles; an emulsifier.

EmulsionColloidal suspension of a liquid in a liquid.

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

EndothermicDescribes processes that absorb heat energy.

EndothermicityThe absorption of heat by a system as the process occurs.

End PointThe point at which an indicator changes colour and a titration is stopped.

EnergyThe capacity to do work or transfer heat.

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

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EntropyA thermodynamic state or property that measures the degree of disorder or randomness of asystem.

EnzymeA protein that acts as a catalyst in biological systems.

Equation of StateAn equation that describes the behavior of matter in a given state; the van der Waals equationdescribes the behavior of the gaseous state.

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

Equilibrium ConstantA quantity that characterizes the position of equilibrium for a reversible reaction; its magnitudeis equal to the mass action expression at equilibrium. K varies with temperature.

Equivalence PointThe point at which chemically equivalent amounts of reactants have reacted.

Equivalent WeightAn oxidizing or reducing agent, who's mass gains (oxidizing agents) or loses (reducing agents)6.022 x 1023 electrons in a redox reaction.The mass of an acid or base that furnishes or reacts with 6.022 x 1023 H3O+ or OH- ions.

Essential OilA plant extract that has a distinctive odour or flavour.

EsterA 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.

EtherCompound in which an oxygen atom is bonded to two alkyl or two aryl groups, or one alkyl andone aryl group.

EutrophicationThe undesirable overgrowth of vegetation caused by high concentrates of plant nutrients inbodies of water.

EvaporizationVaporization of a liquid below its boiling point.

Evaporation RateThe rate at which a particular substance will vapourize (evaporate) when compared to the rate ofa known substance such as ethyl ether. This term is especially useful for health and fire-hazardconsiderations.

Excited StateAny state other than the ground state of an atom or molecule.

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ExothermicDescribes processes that release heat energy.

ExothermicityThe release of heat by a system as a process occurs.

ExplosiveA 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.

Explosive limitsThe range of concentrations over which a flammable vapour mixed with proper ratios of air willignite or explode if a source of ignitions is provided.

Extensive PropertyA property that depends upon the amount of material in a sample.

ExtrapolateTo estimate the value of a result outside the range of a series of known values. Technique used instandard additions calibration procedure.

FFaradayOne faraday of electricity corresponds to the charge on 6.022 x 1023 electrons, or 96,487coulombs.

Faraday's Law of ElectrolysisOne equivalent weight of a substance is produced at each electrode during the passage of 96,487coulombs of charge through an electrolytic cell.

Fast NeutronA neutron ejected at high kinetic energy in a nuclear reaction.

FatSolid triester of glycerol and (mostly) saturated fatty acids.

Fatty AcidsAn aliphatic acid; many can obtained from animal fats.

FerromagnetismThe ability of a substance to become permanently magnetized by exposure to an externalmagnetic field.

Film badgeA small patch of photographic film worn on clothing to detect and measure accumulated incidentionizing radiation.

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

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Flash PointThe temperature at which a liquid will yield enough flamable vapour to ignite. There are variousrecognized industrial testing methods; therefore the method used must be stated.

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

Fossil FuelsSubstances consisting largely of hydrocarbons, derived from decay of organic materials undergeological conditions of high pressure and temperature (metamorphism) include coal, petroleum,natural gas, peat and oil shale.

Frasch ProcessMethod 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.

First Law of ThermodynamicsThe total amount of energy in the universe is constant (also known as the Law of Conservationof Energy) energy is neither created nor destroyed in ordinary chemical reactions and physicalchanges.

FlotationMethod by which hydrophobic (water-repelling) particles of an ore are separated fromhydrophilic (water-attracting) particles of a metallurgical pretreatment process.

FluidsSubstances that flow freely; gases and liquids.

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

FoamColloidal suspension of a gas in a liquid.

Forbidden ZoneA relatively large energy separation between an insulator's highest filled electron energy bandand the next higher energy vacant band. Beginning in the fourth energy level, a set of sevendegenerate orbitals per energy level, higher in energy than s, p, and d orbitals of the same energylevel.

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

FormulaCombination of symbols that indicates the chemical composition of a substance.

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

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Formula WeightThe mass of one formula unit of a substance in atomic mass units.

Fractional DistillationThe process in which a fractioning column is used in distillation apparatus to separatecomponents of a liquid mixture that have different boiling points.

Fractional PrecipitationRemoval of some ions from solution by precipitation while leaving other ions with similarproperties in solution.

Free Energy, Gibbs Free EnergyThe thermodynamic state function of a system that indicates the amount of energy available forthe system to do useful work at constant T and P.

Free Energy ChangeThe indicator of spontaneity of a process at constnt T and P. If delta-G is negative, the process isspontaneous.

Free RadicalA highly reactive chemical species carrying no charge and having a single unpaired electron inan orbital.

Freezing Point DepressionThe decrease in the freezing point of a solvent caused by the presence of a solute.

FrequencyThe number of repeating corresponding points on a wave that pass a given observation point perunit time.

Fuel CellsVoltaic cells in which the reactants (usually gases) are supplied continuously.A voltaic cell that converts the chemical energy of a fuel and an oxidizing agent directly intoelectriacl energy on a continuous basis.

Functional GroupA group of atoms that represents a potential reaction site in an organic compound.

GGamma RayHigh energy electromagnetic radiation.A highly penetrating type of nuclear radiation similar to x-ray radiation, except that it comesfrom within the nucleus of an atom and has a higher energy. Energy wise, very similar to cosmicray except that cosmic rays originate from outer space.

GalvanizingPlacing a thin layer of zinc on a ferrous material to protect the underlying surface fromcorrosion.

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

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Geiger counterA gas filled tube which discharges electriaclly when ionizing radiation passes through it.

GelColloidal suspension of a solid dispersed in a liquid; a semirigid solid.

Gem-dimethyl groupTwo methyl groups of the same carbon atom.

Geometrical IsomersCompounds with different arrangements of groups on either side of a bond with restrictedrotation, such as a double bond or a single bond in a ring; for example cis-trans isomers ofcertain alkenes.Stereoisomers that are not mirror images of each other; also known as position isomers.

Graham's LawThe rates of effusion of gases are inversely proportional to the square roots of their molecularweights or densities.

Greenhouse EffectTrapping of heat at the surface of the earth by carbon dioxide and water vapour in theatmosphere.

Ground StateThe lowest energy state or most stable state of an atom, molecule or ion.

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

HHaber ProcessA process for the catalyzed industrial production of ammonia from N2 and H2 at hightemperature and pressure.

Half-CellCompartment in which the oxidation or reduction half-reaction occurs in a voltaic cell.

Half-LifeThe time required for half of a reactant to be converted into product(s).The time required for half of a given sample to undergo radioactive decay.

Half-ReactionEither the oxidation part or the reduction part of a redox reaction.

HalogensGroup VIIA elements: F, Cl, Br, I

Hard WaterWater containing Fe3+, Ca2+, and Mg2+ ions, which forms precipates with soap.

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HeatA form of energy that flows between two samples of matter because of their differences intemperature.

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

Heat of CondensationThe amount of heat that must be removed from one gram of a vapor at it's condensation point tocondense the vapour with no change in temperature.

Heat of CrystallizationThe amount of heat that must be removed from one gram of a liquid at its freezing point to freezeit with no change in temperature.

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

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

Heat of VaporizationThe amount of heat required to vaporize one gram of a liquid at its boiling point with no changein temperature. Usually expressed in J/g. The molar heat of vaporization is the amount of heatrequired to vaporize one mole of liquid at its boiling point with no change in temperature andusually expressed ion kJ/mol.

Heavy WaterWater containing deuterium, a heavy isotope of hydrogen.

Heisenberg Uncertainty PrincipleIt is impossible to determine accurately both the momentum and position of an electronsimultaneously.

Henry's LawThe pressure of the gas above a solution is proportional to the concentration of the gas in thesolution.

Hess' Law of Heat SummationThe enthalpy change for a reaction is the same whether it occurs in one step or a series of steps.

Heterocyclic AmineAmine in which the nitrogen is part of a ring.

Heterogeneous CatalystA catalyst that exists in a different phase (solid, liquid or gas) from the reactants; a contactcatalyst.

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Heterogeneous EquilibriaEquilibria involving species in more than one phase.

Heterogeneous MixtureA mixture that does not have uniform composition and properties throughout.

HeteronuclearConsisting of different elements.

High Spin ComplexCrystal field designation for an outer orbital complex; all t2g and eg orbitals are singly occupiedbefore any pairing occurs.

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

Homogeneous EquilibriaEquilibria involving only one species in a single phase. For example, all gases, all liquids or allsolids.

Homogeneous MixtureA mixture which has uniform composition and properties throughout.

Homologous SeriesA series of compounds in which each member differs from the next by a specific number andkind of atoms.

HomonuclearConsisting of only one element.

Hund's RuleAll orbitals of a given sublevel must be occupied by single electrons before pairing begins (seeAufbau Principle)

HybridizationMixing a set of atomic orbitals to form a new set of atomic orbitals with the same total electroncapacity and with properties and energies intermediate between those of the originalunhybridized orbitals.

HydrateA solid compound that contains a definite percentage of bound water.

Hydrate IsomersIsomers of crystalline complexes that differ in whether water is present inside or outside thecoordination sphere

HydrationReaction of a substance with water.

Hydration EnergyThe energy change accompanying the hydration of a mole of gase and ions.

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HydrideA binary compound of hydrogen.

HydrocarbonsCompounds that contain only carbon and hydrogen.

Hydrogen BondA fairly strong dipole-dipole interaction (but still considerably weaker than the covalent or ionicbonds) between molecules containing hydrogen directly bonded to a small, highlyelectronegative atom, such as N, O, or F.

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

Hydrogen-Oxygen Fuel CellFuel cell in which hydrogen is the fuel (reducing agent) and oxygen is the oxidizing agent.

HydrolysisThe reaction of a substance with water or its ions.

Hydrolysis ConstantAn equilibrium constant for a hydrolysis reaction.

HydrometerA device used to measure the densities of liquids and solutions.

Hydrophilic ColloidsColloidal particles that repel water molecules.

Inner Orbital ComplexValence bond designation for a complex in which the metal ion utilizes d orbitals for one shellinside the outermost occupied shell in its hybridization.

IIsomersDifferent substances that have the same formula.

Ionization IsomersIsomers that result from the interchange of ions inside and outside the coordination sphere.

Inert s-pair EffectCharacteristic of the post-transition minerals; tendency of the outermost s electrons to remainnonionized or un shared in compounds.

Insoluble CompoundA very slightly soluble compound.

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

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Ionization ConstantEquilibrium constant for the ionization of a weak electrolyte.

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

Inhibitory CatalystAn inhibitor, a catalyst that decreases the rate of reaction.

Integrated Rate EquationAn equation giving the concentration of a reactant remaining after a specified time; has differentmathematical form for different orders of reactants.

IoniztionThe breaking up of a compound into separate ions.

Ideal SolutionA solution that obeys Raoult's Law exactly.

InsulatorPoor electric and heat conductor.

Intermolecular ForcesForces between individual particles (atoms, molecules, ions) of a substance.

IsomorphousRefers to crystals having the same atomic arrangement.

Ideal GasA hypothetical gas that obeys exactly all postulates of the kinetic-molecular theory.

Ideal Gas LawThe product of pressure and the volume of an ideal gas is directly proportional to the number ofmoles of the gas and the absolute temperature.

IonizationIn aqueous solution, the process in which a molecular compound reacts with water and formsions.

Ionic BondingChemical bonding resulting from the transfer of one or more electrons from one atom or a groupof atoms to another.

Ionic CompundsCompounds containing predominantly ionic bonding.

Ionic GeometryThe arrangement of atoms (not lone pairs of electrons) about the central atom of a polyatomicion.

IsoelectricHaving the same electronic configurations

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Ionization EnergyThe minimum amount of energy required to remove the most loosely held electron of an isolatedgaseous atom or ion.

IsotopesTwo or more forms of atoms of the same element with different masses; atoms containing thesame number of protons but different numbers of neutrons.

IonAn atom or a group of atoms that carries an electric charge.

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

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

KetoneCompound in which a carbonyl group is bound to two alkyl or two aryl groups, or to one alkyland one aryl group.

Kinetic EnergyEnergy that matter processes by virtue of its motion.

Kinetic-molecular TheoryA theory, that attempts to explain macroscopic observations on gases in microscopicobservations on gases in microscopic observations on gases in microscopic or molecular terms.

LLanthanidesElements 58 to 71 (after lanthanum)

Lanthanide ContractionA decrease in the radii of the elements following the lanthanides compared to what would beexpected if there were no f-transition metals.

Law of Combining Volumes (Gay-Lussac's Law)At constant temperature and pressure, the volumes of reacting gases ( and any gaseous products)can be expressed as ratios of small whole numbers;

Law of Conservation of EnergyEnergy cannot be created or destroyed; it may be changed from one form to another.

Law of Conservation of MatterThere is no detectable change in the quantity of matter during an ordinary chemical reaction.

Law of Conservation of Matter and EnergyThe total amount of matter and energy available in the universe is fixed.

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Law of Definite Proportions (Law of Constant Composition)Different samples of a pure compound always contain the same elements in the same proportionsby mass.

Law of Partial Pressures (Dalton's Law)The total pressure exerted by a mixature of gases is the sum of the partial pressures of theindividual gases.

Lead Storage BatterySecondary voltaic cell used in most automobiles.

Leclanche CellA common type of dry cell.

Le Chatelier's PrincipleStates that a system at equilibrium, or striving to attain equilibrium, responds in such a way as tocounteract any stress placed upon it.If a stress (change of conditions) is applied to a system at equilibrium, the system shifts in thedirection that reduces stress.

Leveling EffectEffect by which all acids stronger than the acid that is characteristic of the solvent react withsolvent to produce that acid; similar statement applies to bases. The strongest acid (base) that canexist in a given solvent is the acid (base) characteristic of the solvent.

LevorotatoryRefers to an optically active substance that rotates the plane of plane polarized lightcounterclockwise; also called levo.

Lewis AcidAny species that can accept a share in an electron pair.

Lewis BaseAny species that can make available a share in an electron pair.

Lewis Dot Formula (Electron Dot Formula)Representation of a molecule, ion or formula unit by showing atomic symbols and only outershell electrons

LigandA Lewis base in a coordination compound.

Limiting ReactantSubstance that stoichiometrically limits the amount of product(s) that can be formed.

Linear AcceleratorA device used for accelerating charged particles along a straight line path.

Line SpectrumAn atomic emission or absorption spectrum.

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Linkage IsomersIsomers in which a particular ligand bonds to a metal ion through different donor atoms.

Liquid AerosolColloidal suspension of liquid in gas.

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

Lone PairPair of electrons residing on one atom and not shared by other atoms; unshared pair.

Low Spin ComplexCrystal field designation for an inner orbital complex; contains electrons paired t2g orbitalsbefore eg orbitals are occupied in octahedral complexes.

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

ManometerA two-armed barometer.

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

Mass Action ExpressionFor 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 balancedchemical 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. Atequilibrium the mass action expression is equal to K;

Mass DeficiencyThe amount of matter that would be converted into energy if an atom were formed fromconstituent particles.

Mass NumberThe sum of the numbers of protons and neutrons in an atom; an integer.

Mass SpectrometerAn instrument that measures the charge-to-mass ratio of charged particles.

MatterAnything that has mass and occupies space.

MechanismThe sequence of steps by which reactants are converted into products.

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Melting PointThe temperature at which liquid and solid coexist in equilibrium; also the freezing point.

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

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

Metallic BondingBonding within metals due to the electrical attraction of positively charges metal ions for mobileelectrons that belong to the crystal as a whole.

Metallic ConductionConduction of electrical current through a metal or along a metallic surface.

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

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

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

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

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

MixtureA sample of matter composed of two or more substances, each of which retains its identity andproperties.

ModeratorA substance such as hydrogen, deuterium, oxygen or paraffin capable of slowing fast nuetronsupon collision.

MolalityConcentration expressed as number of moles of solute per kilogram of solvent.

MolarityNumber of moles of solute per litre of solution.

Molar SolubilityNumber of moles of a solute that dissolve to produce a litre of saturated solution.

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Molecular EquationEquation for a chemical reaction in which all formulas are written as if all substances existed asmolecules; only complete formulas are used.

Molecular FormulaFormula that indicates the actual number of atoms present in a molecule of a molecularsubstance.

Molecular GeometryThe arrangement of atoms (not lone pairs of electrons) around a central atom of a molecule orpolyatomic ion.

Molecular OrbitalAn orbit resulting from overlap and mixing of atomic orbitals on different atoms. An MObelongs to the molecule as a whole.

Molecular Orbital TheoryA theory of chemical bonding based upon the postulated existence of molecular orbitals.

Molecular WeightThe mass of one molecule of a nonionic substance in atomic mass units.

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

Mole FractionThe number of moles of a component of a mixture divided by the total number of moles in themixture.

Monoprotic AcidAcid that can form only one hydronium ion per molecule; may be strong or weak.Acid that contains one ionizable hydrogen atom per formula unit.

Mother NuclideNuclide that undergoes nuclear decay.

NNative StateRefers to the occurrence of an element in an uncombined or free state in nature.

Natural RadioactivitySpontaneous decomposition of an atom.

Nernst EquationCorrects standard electrode potentials for nonstandard conditions.

Net Ionic EquationEquation that results from canceling spectator ions and eliminating brackets from a total ionicequation.

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

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NeutronA neutral subatomic particle having a mass of 1.0087 amu.

Nickel-cadmium cell (Nicad battery)A dry cell in which the anode is Cd, the cathode is NiO2, and the electrolyte is basic.

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

Nitrogen CycleThe complex series of reactions by which nitrogen is slowly but continually recycled in theatmosphere, lithosphere and hydrosphere.

Noble Gases (Rare Gases)Elements of the periodic Group 0; also called rare gases; formerly called inert gases, He,Ne,Ar,Kr, Xe, Rn.

Nodal PlaneA region in which the probability of finding an electron is zero.

Nonbonding OrbitalA molecular orbital derived only from an atomic orbital of one atom; lends neither stability norinstability to a molecule or ion when populated with electrons.

NonelectrolyteA substance whose aqueous solutions do not conduct electricity.

Nonpolar BondCovalent bond in which electron density is symmetrically distributed

Nuclear Binding EnergyEnergy equivalent of the mass deficiency; energy released in the formation of an atom from thesubatomic particles.

Nuclear FissionThe process in which a heavy nucleus splits into nuclei of intermediate masses and one or moreprotons are emitted.

Nuclear ReactionInvolves a change in the composition of a nucleus and can evolve or absorb an extraordinarilylarge amount of energy

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

NucleonsParticles comprising the nucleus; protons and neutrons.

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NucleusThe very small, very dense, positively charged center of an atom containing protons andneutrons, as well as other subatomic particles.

NuclidesRefers to different atomic forms of all elements in contrast to isotopes, which refer only todifferent atomic forms of a single element.

Nuclide SymbolSymbol for an atom A/Z E, in which E is the symbol of an element, Z is its atomic number, andA is its mass number.

OOctahedralA term used to describe molecules and polyatomic ions that have one atom in the center and sixatoms at the corners of a octahedron.

Octane NumberA number that indicates how smoothly a gasoline burns.

Octet RuleMany representative elements attain at least a share of eight electrons in their valence shellswhen they form molecular or ionic compounds; there are some limitations.

OilLiquid triester of glycerol and unsaturated fatty acids.

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

Optical ActivityThe rotation of plane polarized light by one of a pair of optical isomers.

Optical IsomersStereoisomers that differ only by being nonsuperimposable mirror images of each other, likeright and left hands, also called enantiomers.

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

Organic ChemistryThe chemistry of substances that contain carbon-hydrogen bonds.

OsmosisThe process by which solvent molecules pass through a semipermable membrane from a dilutesolution into a more concentrated solution.

Osmotic PressureThe hydrostatic pressure produced on the surface of a semipermable membrane by osmosis.

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Ostwald ProcessA process for the industrial production of nitrogen oxide and nitric acid from ammonia andoxygen.

Outer Orbital ComplexValence bond designation for a complex in which the metal ion utilizes d orbitals in theoutermost (occupied) shell in hybridization.

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

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

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

Oxidation-reduction ReactionsReactions in which oxidation and reduction occur; also called redox reactions.

OxideA binary compound of oxygen.

Oxidizing AgentThe substance that oxidizes another substance and is reduced.

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

Pairing EnergyEnergy required to pair two electrons in the same orbital.

ParamagnetismAttraction toward a magnetic field, stronger than diamagnetism, but still weak compared toferromagnetism.

Partial PressureThe pressure exerted by one gas in a mixture of gases.

Particulate MatterFine divided solid particles suspended in polluted air.

Pauli Exclusion PrincipleNo two electrons in the same atom may have identical sets of four quantum numbers.

Percentage IonizationThe percentage of the weak electrolyte that ionizes in a solution of given concentration.

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Percent by Mass100% times the actual yield divided by theoretical yield.

Percent CompositionThe mass percent of each element in a compound.

Percent PurityThe percent of a specified compound or element in an impure sample.

PeriodThe elements in a horizontal row of the periodic table.

PeriodicityRegular periodic variations of properties of elements with atomic number (and position in theperiodic table).

Periodic LawThe properties of the elements are periodic functions of their atomic numbers.

Periodic TableAn arrangement of elements in order of increasing atomic numbers that also emphasizesperiodicity.

PeroxideA compound containing oxygen in the -1 oxidation state. Metal peroxides contain the peroxideion, O2

2- pH Negative logarithm of the concentration (mol/L) of the H3O+[H+] ion; scale iscommonly used over a range 0 to 14.

Phase DiagramDiagram that shows equilibrium temperature-pressure relationships for different phases of asubstance.

PhenolHydrocarbon derivative containing an [OH-] group bound to an aromatic raing.

Photochemical OxidantsPhotochemically produced oxidizing agents capable of causing damage to plants and animals.

Photochemical SmogA brownish smog occurring in urban areas receiving large amounts of sunlight; caused byphotochemical (light-induced) reactions among nitrogen oxides, hydrocarbons and othercomponents of polluted air that produce photochemical oxidants.

Photoelectric EffectEmission of an electron from the surface of a metal caused by impinging electromagneticradiation of certain minimum energy; current increases with increasing intensity of radiation.

PhotonA packet of light or electromagnetic radiation; also called quantum of light

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Physical ChangeA change in which a substance changes from one physical state to another but no substanceswith different composition are formed. Example Gas to Liquid - Solid.

PlasmaA physical state of matter which exists at extremely high temperatures in which all molecules aredissociated and most atoms are ionized.

Polar BondCovalent bond in which there is an unsymmetrical distribution of electron density.

PolarimeterA device used to measure optical activity.

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

PolydentateRefers to ligands with more than one donor atom.

PolyeneA compound that contains more than one double bond per molecule.

PolymerizationThe combination of many small molecules to form large molecules.

PolymerA large molecule consisting of chains or rings of linked monomer units, usually characterized byhigh melting and boiling points.

PolymorphousRefers to substances that crystallize in more than one crystalline arrangement.

Polyprotic AcidAn Acid that can form two or more hydronium ions per molecule; often a least one step ofionization is weak.

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

Potential EnergyEnergy that matter possesses by virtue of its position, condition or composition.

PrecipitateAn insoluble solid formed by mixing in solution the constituent ions of a slightly solublesolution.

Primary StandardA substance of a known high degree of purity that undergoes one invariable reaction with theother reactant of interest.

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Primary Voltaic CellsVoltaic cells that cannot be recharged; no further chemical reaction is possible once the reactantsare consumed.

ProtonA subatomic particle having a mass of 1.0073 amu and a charge of +1, found in thew nuclei ofatoms.

PseudobinaryIonic CompoundsCompounds that contain more than two elements but are named like binary compounds.

QQuantum MechanicsMathematical method of treating particles on the basis of quantum theory, which assumes thatenergy (of small particles) is not infinitely divisible.

Quantum NumbersNumbers that describe the energies of electrons in atoms; derived from quantum mechanicaltreatment.

RRadiationHigh energy particles or rays emitted during the nuclear decay processes.

RadicalAn atom or group of atoms that contains one or more unpaired electrons (usually very reactivespecies)

Radioactive DatingMethod of dating ancient objects by determining the ratio of amounts of mother and daughternuclides present in an object and relating the ratio to the objects age via half-life calculations.

Radioactive TracerA small amount of radioisotope replacing a nonradioactive isotope of the element in a compoundwhose path (for example, in the body) or whose decomposition products are to be monitored bydetection of radioctivity; also called a radioactive label.

RadioactivityThe spontaneous disintegration of atomic nuclei.

Raoult's LawThe vapor pressure of a solvent in an ideal solution decreases as its mole fraction decreases.

Rate-determining StepThe slowest step in a mechanism; the step that determines the overall rate of reaction.

Rate-law ExpressionEquation relating the rate of a reaction to the concentrations of the reactants and the specific rateof the constant.

Rate of ReactionChange in the concentration of a reactant or product per unit time.

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ReactantsSubstances consumed in a chemical reaction.

Reaction QuotientThe mass action expression under any set of conditions (not necessarily equlibrium); itsmagnitude relative to K determines the direction in which the reaction must occur to establishequilibrium.

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

Reaction StoichiometryDescription of the quantitative relationships among substances as they participate in chemicalreactions.

Reducing AgentThe substance that reduces another substance and is oxidized.

ResonanceThe 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.

Reverse OsmosisForcing solvent molecules to flow through a semipermable membrane from a concentatedsolution into a dilute solution by the application of greater hydrostatic pressure on concentratedside than the osmotic pressure opposing it.

Reversible ReactionReactions that do not go to completion and occur in both the forward and reverse direction.

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

SaponificationHydrolysis of esters in the presence of strong soluable bases.

Saturated HydrocarbonsHydrocarbons that contain only single bonds. They are also called alkanes or paraffinhydrocarbons.

Saturated SolutionSolution in which no more solute will dissolve.

Second Law of ThermodynamicsThe universe tends toward a state of greater diorder in spontaneous processes.

Secondary Standarda solution that has been titrated against a primary standard. A standard solution is a secondarystandard.

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Secondary Voltaic CellsVoltaic cells that can be recharged; original reactanats can be regenerated be reversing thedirection of the current flow.

SemiconductorA substance that does not conduct electricity at low temperatures but does so at highertemperatures.

Semipermable MembraneA thin partition between two solutions through which certain molecules can pass but otherscannot.

Shielding EffectElectrons in filled sets of s , p orbitals between the nucleus and outer shell electrons shield theouter shell electrons somewhat from the effect of protons in the nucleus; also called screeningeffect.

Sigma BondsBonds resulting from the head-on overlap of atomic orbitals, in which the region of electronsharing is along and (cylindrically) symmetrical to the imaginary line connecting the bondedatoms.

Sigma OrbitalMolecular orbital resulting from head-on overlap of two atomic orbitals.

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

Single BondCovalent bond resulting from the sharing of two electrons (one pair) between two atoms.

Solubility Product ConstantEquilibrium constant that applies to the dissolution of a slightly soluble compound.

Solubility Product PrincipleThe solubility product constant expression for a slightly soluble compound is the product of theconcentrations of the constituent ions, each raised to the power that corresponds to the number ofions in one formula unit.

SoluteThe dispersed (dissolved) phase of a solution.

SolutionHomogeneous mixture of two or more substances.

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

SolventThe dispersing medium of a solution.

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

S OrbitalA spherically symmetrical atomic orbital; one per energy level.

Specific GravityThe ratio of the density of a substance to the density of water.

Specific HeatThe amount of heat required to raise the temperature of one gram of substance one degreeCelsius.

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

Spectator IonsIons in a solution that do not participate in a chemical reaction.

Spectral LineAny of a number of lines corresponding to definite wavelengths of an atomic emission orabsorption spectrum; represents the energy difference between two energy levels.

Spectrochemical SeriesArrangement of ligands in order of increasing ligand field strength.

SpectrumDisplay of component wavelengths (colours) of electromagnetic radiation.

Square PlanarA term used to describe molecules and polyatomic ions that have one atom in the center and fouratoms at the corners of a square.

Square Planar ComplexComplex in which the metal is in the center of a square plane, with ligand donor atoms at each ofthe four corners

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

Standard Electrode PotentialBy convention , potential, Eo, of a half-reaction as a reduction relative to the standard hydrogenelectrode when all species are present at unit activity.

Standard EntropyThe absolute entropy of a substance in its standard state at 298 K.

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Standard Molar Enthalphy of FormationThe amount of heat absorbed in the formation of one mole of a substance in a specified statefrom its elements in their standard states.

Standard Molar VolumeThe volume occupied by one mole of an ideal gas under standard conditions; 22.4liters.

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

StereoisomersIsomers that differ only in the way that atoms are oriented in space; consist of geometrical andoptical isomers.

StoichiometryDescription of the quantitative relationships among elements and compounds as they undergochemical changes.

Strong ElectrolyteA substance that conducts electricity well in a dilute aqueous solution.

Strong Field LigandLigand that exerts a strong crystal or ligand electrical field and generally forms low spincomplexes with metal ions when possible.

Structural IsomersCompounds that contain the same number of the same kinds of atoms in different geometricarrangements.

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

SubstanceAny kind of matter all specimens of which have the same chemical composition and physicalproperties.

Substitution ReactionA reaction in which an atom or a group of atoms is replaced by another atom or group of atoms.

Supercooled LiquidsLiquids that, when cooled, apparently solidify but actually continue to flow very slowly underthe influence of gravity.

Supercritical FluidA substance at temperature above its critical temperature.

Supersaturated SolutionA solution that contains a higher than saturation concentration of solute; slight disturbance orseeding causes crystallization of excess solute.

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SuspensionA heterogeneous mixture in which solute-like particles settle out of solvent-like phase some timeafter their introduction.

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

Ternary AcidA ternary compound containing H, O, and another element, often a nonmetal.

Ternary CompoundA compound consisting of three elements; may be ionic or covalent.

TetrahedralA term used to describe molecules and polyatomic ions that have one atom in center and fouratoms at the corners of a tetrahedron.

Theoretical YieldMaximum amount of a specified product that could be obtained from specified amounts ofreactants, assuming complete consumption of limiting reactant according to only one reactionand complete recovery of product. (Compare with Actual Yield)

Thermal CrackingDecomposition by heating a substance in the presence of a catalyst and in the absence of air.

ThermodynamicsThe study of the energy transfers accompanying physical and chemical processes.

Thermonuclear EnergyEnergy from nuclear fusion reactions.

Third Law of ThermodynamicsThe entropy of a hypothetical pure, perfect, crystalline sustance at absolute zero temperature iszero.

TitrationA Procedure in which one solution is added to another solution until the chemical reactionbetween the two solutes is complete; the concentration of one solution is known and that of theother is unknown.

Total Ionic EquationEquation for a chemical reaction written to show the predominant form of all species in aqueoussolution or in contact with water.

Transition State TheoryTheory of reaction rates that states that reactants pass through high-energy transition statesbefore forming products.

Tyndall EffectThe scattering of light by colloidal particles.

46

UUnsaturated HydrocarbonsHydrocarbons that contain double or triple carbon-carbon bonds.

VValence Bond TheoryAssumes that covalent bonds are formed when atomic orbitals on different atoms overlap and theelectrons are shared.

Valence ElectronsOutermost electrons of atoms; usually those involved in bonding.

Valence Shell Electron Pair Repulsion TheoryAssumes that electron pairs are arranged around the central element of a molecule or polyatomicion so that there is maximum separation (and minimum repulsion) among regions of highelectron density.

van der Waals' EquationAn equation of state that extends the ideal gas law to real gases by inclusion of two empiricallydetermined parameters, which are different for different gases.

VaporA gas formed by boiling or evaporating a liquid.

Vapor PressureThe particle pressure of a vapor at the surface of its parent liquid.

VoltagePotential difference between two electrodes; a measure of the chemical potential for a redoxreaction to occur.

Voltaic CellsElectrochemical cells in which spontaneous chemical reactions produce electricity; also calledgalvanic cells.

WWater EquivalentThe amount of water that would absorb the same amount of heat as the calorimeter per degreetemperature increase.

Weak ElectrolyteA substance that conducts electricity poorly in a dilute aqueous solution.

Weak Field LigandA Ligand that exerts a weak crystal or ligand field and ge- nerally forms high spin complexeswith metals.

ZZone RefiningA method of purifying a bar of metal by passing it through an induction heater; this causesimpurties to move along a melted portion.

47

Products: A series

Compound Formula

Aluminum arsenide AlAsAluminum bromide AlBr3

Aluminum bromide, hexahydrate AlBr3·6H2OAluminum chloride AlCl3

Aluminum chloride, hexahydrate AlCl3·6H2OAluminum iodide AlI3

Aluminum oxide Al2O3

Aluminum phosphate AlPO4

Aluminum selenate Al2(SeO4)3

Aluminum selenite Al2(SeO3)3

Aluminum tellurate Al2(TeO4)3

Aluminum tellurite Al2(TeO3)3

Aluminum titanate Al2(TiO3)3

Ammonium dihydrogen arsenate (NH4)H2AsO4

Antimony (III) bromide SbBr3

Antimony (III) chloride SbCl3

Antimony (V) chloride SbCl5

Antimony (III) iodide SbI3

Antimony (III) oxide Sb2O3

Antimony (V) oxide Sb2O5

Antimony (III) phosphate SbPO4

Antimony (III) selenide Sb2Se3

Antimony (V) selenide Sb2Se5

Antimony (III) sulfide Sb2S3

Antimony (III) tellluride Sb2Te3

Arsenic (III) bromide AsBr3

Arsenic (III) chloride AsCl3

Arsenic (III) iodide AsI3

Arsenic (III) oxide As2O3

Arsenic (V) oxide As2O5

Arsenic (V) oxide, hydrate As2O5·H2OArsenic (III) selenide As2Se3

Arsenic (V) selenide As2Se5

Arsenic (II) sulfide AsSArsenic (III) sulfide As2S3

Arsenic (V) sulfide As2S5

Arsenic (III) telluride As2Te3

Arsenic (V) telluride As2Te3

B seriesBarium aluminate Ba(AlO2)2

Barium arsenate Ba(AsO4)2

Barium bromate, dihydrate Ba(BrO3)2·2H2OBarium bromate, monohydrate Ba(BrO3)2·H2OBarium bromide BaBr2

48

Barium chromate BaCrO4

Barium iodide BaI2

Barium molybdate BaMoO4

Barium metaniobate BaNb2O6

Barium Oxide BaOBarium orthophosphate Ba3(PO4)2

Barium selenate BaSeO4

Barium selenite BaSeO3

Barium metasilicate BaSiO3

Barium tellurate, trihydrate BaTeO4·3H2OBarium tellurite BaTeO3

Barium thiocyanate, monohydrate Ba(SCN)2·H2OBarium metatitanate BaTiO3

Barium orthotungstate BaWO4

Barium pyrovanadate Ba2V2O7

Bismuth (III) acetate Bi(C2H3O2)3

Bismuth (III) orthoborate BiBO3

Bismuth (III) bromide BiBr3

Bismuth (III) chloride BiCl3

Bismuth (III) iodide BiI3

Bismuth (III) molybdate Bi2(MoO4)3

Bismuth (III) nitrate, pentahydrate Bi(NO3)3·5H2OBismuth (III) oxide Bi2O3

Bismuth (III) oxychloride BiOClBismuth (III) oxyiodide BiOIBismuth (III) orthophosphate BiPO4

Bismuth (III) selenide Bi2Se3

Bismuth (III) sulfide Bi2S3

Bismuth (III) telluride Bi2Te3

Bismuth (III) orthotungstste Bi2(WO4)3

Bismuth (III) metavanadate Bi(VO3)3

Boron (III) arsenate BAsO4

Boron (III) bromide BBr3

Boron (III) oxide B2O3

Boron (III) orthophosphate BPO4

Boron (III) phosphide BP

C seriesCadmium arsenide Cd3As2

Cadmium bromide CdBr2

Cadmium bromide, dihydrateCdBr2·2H2OCadmium bromide, tetrahydrate CdBr2·4H2OCadmium cabonate CdCO3

Cadmium perchorate, hydrate Cd(ClO4)2·H2OCadmium chloride CdCl2

Cadmium chloride, dihemihydrate CdCl2·2H2OCadmium fluoride CdF2

Cadmium formate, dihydrate Cd(CHO2)2·2H2OCadmium hyroxide Cd(OH)2

Cadmium iodide CdI

49

Cadmium molybdate CdMoO4

Cadmium pyroniobate Cd2Nb2O7

Cadmium nitrate, tetrahydrate Cd(NO3)2·4H2OCadmium oxalate CdC2O4

Cadmium oxide CdOCadmium orthophosphate Cd3(PO4)2

Cadmium selenate, dihydrate CdSeO4·2H2OCadmium selenide CdSeCadmium selenite CdSeO3

Cadmium sulfide CdSCadmium sulfite CdSO3

Cadmium metatantalate Cd(TaO3)2

Cadmium tellurate CdTeO4

Cadmium telluride CdTeCadmium orthotungstate CdWO4

Cadmium metazirconate CdZrO3

Calcium bromide CaBr2

Calcium bromide, dihydrate CaBr2·2H2OCalcium bromide, hexahydrate CaBr2·6H2OCalcium fluoride CaF2

Calcium molybdate CaMoO4

Calcium metaniobate Ca(NbO3)2

Calcium orthophosphate, dihydrate CaHPO4·2H2OCalcium selenate CaSeO4

Calcium selenite CaSeO3

Calcium metasilicate CaSiO3

Calcium orthosilicate Ca2SiO4

Calcium tellurate CaTeO4

Calcium tellurite CaTeO3

Calcium thiocyanate, trihydrate Ca(SCN)2·3H2OCalcium metatitanate CaTiO3

Calcium orthotungstate CaWO4

Calcium metavanadate Ca(VO3)2

Calcium orthovanadate Ca(VO4)2

Calcium sulfate, whiskers crystal CaSO4

Cesium acetate CsC2H3O2

Cesium bromate CsBrO3

Cesium bromide CsBrCesium tribromide CsBr3

Cesium carbonate Cs2CO3

Cesium chlorate CsClO3

Cesium chloride CsClCesium chromate Cs2CrO4

Cesium dichromate Cs2Cr2O7

Cesium iodide CsICesium triiodide CsI3

Cesium molybdate Cs2MoO4

Cesium metaniobate CsNbO3

Cesium nitrate CsNO3

Cesium oxalate Cs2C2O4

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Cesium orthophosphate Cs3PO4

Cesium dihydrogen orthophosphate CsH2PO4

Cesium hydrogen orthophosphate Cs2HPO4

Cesium selenate CsSeO4

Cesium metasilicate Cs2SiO3

Cesium sulfate Cs2SO4

Cesium sulfite Cs2SO3

Cesium metatantalate CsTaO3

Cesium tellurate Cs2TeO4

Cesium thiocyanate CsSCNCesium metatitanate Cs2TiO3

Cesium orthotungstate Cs2WO4

Cesium orthovanadate Cs3VO4

Chromium (II) antimonide Cr3Sb2

Chromium (III) antimonide CrSbChromium (II) arsenide Cr3As2

Chromium (III) arsenide CrAsChromium (III) bromide, hexahydrate CrBr3·6H2OChromium (II) chloride CrCl2

Chromium (III) chloride CrCl3

Chromium (III) oxalate, hexahydrate Cr2(C2O4)3·6H2OChromium (III) oxide Cr2O3

Chromium (VI) oxychloride CrO2Cl2

Chromium (III) selenide Cr2Se3

Chromium (III) silicide Cr3Si2

Chromium (III) tellurate Cr2(TeO4)3

Chromium (III) telluride Cr2Te3

Chromium (III) orthovanadate CrVO4

Cobalt (II) bromide CoBr2

Cobalt (II) chloride CoCl2

Cobalt (II) fluoride, dihydrate CoF2·2H2OCobalt (II) fluoride, hydrate CoF2·H2OCobalt (II) fluosilicate, hexahydrate CoSiF6·6H2OCobalt (II) iodate, hexahydrate Co(IO3)2·6H2OCobalt (II) iodide CoI2

Cobalt (II) iron (II) oxide CoFe2O4

Cobalt (II) nitrate, hexahydrate Co(NO3)2·6H2OCobalt (II) oxalate, dihydrate CoC2O4·2H2OCobalt (II) oxide CoOCobalt (II) selenide CoSeCobalt (II) selenite CoSeO3

Cobalt (II) orthosilicate Co2SiO4

Cobalt (II) orthotungstate CoWO4

Copper (I) antimonide Cu3SbCopper (I) arsenide Cu3AsCopper (II) bromate, hexahydrate Cu(BrO3)2·6H2OCopper (I) bromide CuBrCopper (II) bromide CuBr2

Copper (II) chlorate, hexahydrate Cu(ClO3)·6H2O

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Copper (I) chloride CuClCopper (II) chloride CuCl2

Copper (II) hydroxide Cu(OH)2

Copper (II) iodate Cu(IO3)2

Copper (I) iodide CuICopper (II) iron (II) oxide CuFe2O4

Copper (II) orthomolybdate CuMoO4

Copper (II) orthoniobate Cu(NbO3)2

Copper (II) nitrate, trihydrate Cu(NO3)2·3H2OCopper (II) oxide CuOCopper (I) phosphide Cu3PCopper (II) selenate, pentahydrate CuSeO4·5H2OCopper (I) selenide Cu2SeCopper (II) selenide CuSeCopper (II) selenite, dihydrate CuSeO3·2H2OCopper (II) metasilicate CuSiO3

Copper (II) sulfate, pentahydrate CuSO4·5H2OCopper (I) sulfide Cu2SCopper (I) telluride Cu2TeCopper (II) telluride CuTeCopper (II) tellurite CuTeO3

Copper (I) thiocyanate CuSCNCopper (II) metatitanate CuTiO3

Copper (II) orthotungstate CuWO4

Copper (II) metavanadate Cu(VO3)2

F seriesFremy's salt (Potassium nitrosodisulfonate) (KSO3)2NO

G seriesGallium (III) acetate Ga(C2H3O2)3

Gallium (III) antimonide GaSbGallium (III) orthoarsenate GaAsO4

Gallium (III) arsenide GaAsGallium (II) bromide GaBr2

Gallium (III) bromide GaBr3

Gallium (II) chloride GaCl2

Gallium (III) chloride GaCl3

Gallium (III) hydroxide Ga(OH)3

Gallium (II) iodide GaI2

Gallium (III) iodide GaI3

Gallium (III) nitride GaNGallium (III) oxide Ga2O3

Gallium (III) orthophosphate GaPO4

Gallium (III) sulfate, octadecahydrate Ga2(SO4)3·18H2OGallium (III) sulfide Ga2S3

Gallium (II) telluride GaTeGallium (III) telluride Ga2Te3

Germanium (IV) bromide GeBr4

Germanium (II) iodide GeI2

Germanium (IV) iodide GeI4

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H seriesHafnium (IV) acetate, basic HfOH(C2H3O2)3

Hafnium (IV) bromide HfBr4

Hafnium (IV) oxychloride, octahydrate HfOCl2·8H2OHafnium (IV) fluoride HfF4

Hafnium (IV) sulfate Hf(SO4)2

I seriesIndium (III) antimonide InSbIndium (III) arsenide InAsIndium (I) bromide InBrIndium (III) bromide InBr3

Indium (III) bromodiiodide InBrI2

Indium (III) dibromoiodide InBr2IIndium (I) chloride InClIndium (II) chloride InCl2

Indium (III) chloride InCl3

Indium (III) chloride, tetrahydrate InCl3·4H2OIndium (III) hydroxide In(OH)3

Indium (III) iodate In(IO3)3

Indium (I) iodide InIIndium (II) iodide InI2

Indium (III) iodide InI3

Indium (III) nitrate, tetrahemihydrate In(NO3)3·4H2OIndium (III) oxide In2O3

Indium (III) orthophosphate InPO4

Indium (III) phosphide InPIndium (III) selenide In2Se3

Indium (III) sulfate, hydrate In2(SO4)3·xH2OIndium (II) sulfide InSIndium (III) sulfide In2S3

Indium (II) telluride InTeIndium (III) telluride In2Te3

Iodine (I) bromide IBrIodine (III) bromide IBr3

Iodine (I) cholride IClIodine (III) chloride ICl3

Iron (II) bromide FeBr2

Iron (III) bromide FeBr3

Iron (III) bromide, hexahydrate FeBr3·6H2OIron (III) chloride FeCl3

Iron (II) fluoride, tetrahydrate FeF2·4H2OIron (II) iodide FeI2

Iron (II) iodide, tetrahydrate FeI2·4H2OIron (II) orthomolybdate FeMoO4

Iron (II) oxide FeOIron (II) iron (III) oxide Fe3O4

Iron (III) oxide Fe2O3

Iron (III) phosphide FePIron(di) phosphide Fe2P

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Iron(tri) phosphide Fe3PIron (II) selenide FeSeIron (II) sulfide FeSIron sulfide, iron rich FeSIron (II) telluride FeTeIron (II) metatitanate FeTiO3

Iron (II) orthotungstate FeWO4

Iron (III) orthotungstate Fe2(WO4)3

Iron (III) orthovanadate FeVO4

Iron (II) metazirconate FeZrO3

L seriesLithium tetraborate, pentahydrate Li2B4O7·5H2OLithium bromate LiBrO3

Lithium bromide LiBrLithium bromide, dihydrate LiBr·2H2OLithium chromate Li2CrO4

Lithium chromate, dihydrate Li2CrO4·2H2OLithium cyanide LiCNLithium dichromate Li2Cr2O7

Lithium ethoxide LiC2H5OLithium iodate LiIO3

Lithium orthomolybdate Li2MoO4

Lithium metaniobate Li2NbO3

Lithium nitrate LiNO3

Lithium nitrate, hydrate LiNO3·xH2OLithium selenate Li2SeO4

Lithium selenite Li2SeO3

Lithium metasilicate Li2SiO3

Lithium orthosilicate Li2SiO3

Lithium hydrogen sulfate LiHSO4

Lithium metatantalate LiTaO3

Lithium tellurate Li2TeO4

Lithium tellurite Li2TeO3

Lithium metatitanate Li2TiO3

Lithium orthotungstate Li2WO4

Lithium metavanadate, dihydrate LiVO3·2H2OLithium metazirconate Li2ZrO3

M seriesMagnesium aluminate Mg(AlO2)2

Magnesium arsenide Mg3As2

Magnesium bismuthide Mg3Bi2

Magnesium chlorate, hydrate Mg(ClO3)2·H2OMagnesium chloride MgCl2

Magnesium chromate, pentahydrate MgCrO4·5H2OMagnesium iodide MgI2

Magnesium molybdate MgMoO4

Magnesium nitrate, hexahydrate Mg(NO3)2·6H2OMagnesium oxide MgOMagnesium phosphide Mg3P2

Magnesium pyrophosphate Mg2P2O7

54

Magnesium selenate MgSeO4

Magnesium selenide MgSeMagnesium selenite MgSeO3

Magnesium metasilicate MgSiO3

Magnesium sulfide MgSMagnesium metatitanate MgTiO3

Magnesium tungstate MgWO4

Magnesium metavanadate Mg(VO3)2

Magnesiun orthovanadate Mg3(VO4)2

Manganese (II) antimonide Mn3Sb2

Manganese (II) arsenide Mn3As2

Manganese (III) arsenide MnAsManganese (III) bisuthide MnBiManganese (II) bromide MnBr2

Manganese (II) bromide, tetrahydrate MnBr2·4H2OManganese (II) carbonate MnCO3

Manganese (II) chloride MnCl2

Manganese (II) formate, dihydrate Mn(CHO2)2·2H2OManganese (II) fluoride MnF2

Manganese (II) iodide MnI2

Manganese (II) orthomolybdate MnMoO4

Manganese (II) nitrate, tetrahydrate Mn(NO3)2·4H2OManganese (II) oxide MnOManganese (II) manganese (III) oxide Mn2O4

Manganese (III) oxide Mn2O3

Manganese (II) phosphide Mn3P2

Manganese (II) telluride MnTeManganese (II) metazirconate MnZrO3

Mercury (II) acetate Hg(C2H3O2)2

Mercury (II) ammonium thiocyanate (NH4)2Hg(SCN)4

Mercury (II) orthoarsenate Hg3(AsO4)2

Mercury (II) benzoate, hydrate Hg(C7H5O2)2·xH2OMercury (II) bromate, dihydrate Hg(BrO3)2·2H2OMercury (I) bromide Hg2Br2

Mercury (II) bromide HgBr2

Mercury (I) perchlorate, tetrahydrate HgClO4·4H2OMercury (II) perchlorate, trihydrate Hg(ClO4)2·3H2OMercury (II) chloride HgCl2

Mercury (II) iodate Hg(IO3)2

Mercury (II) iodide HgI2

Mercury (II) nitrate, hydrate Hg(NO3)2·xH2OMercury (II) selenide HgSeMercury (II) selenite HgSeO3

Mercury (II) sulfide HgSMercury (II) telluride HgTeMercury (II) tellurite HgTeO3

Mercury (II) thiocyanate Hg(SCN)2

Mercury (II) tungstate HgWO4

Molybdenum (II) bromide MoBr2

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Molybdenum (III) bromide MoBr3

Molybdenum (II) chloride MoCl2

Molybdenum (III) chloride MoCl3

Molybdenum (V) chloride MoCl5

Molybdenum (IV) oxide MoO2

N seriesNickel (II) antmonide Ni3Sb2

Nickel (III) arsenide NiAsNickel (II) bromide NiBr2

Nickel (II) bromide, trihydrate NiBr2·3H2ONickel (II) bromide, hexahydrate NiBr2·6H2ONickel (II) chloride NiCl2

Nickel (II) hydroxide Ni(OH)2

Nickel (II) iodide NiI2

Nickel (II) iron (III) oxide NiFe2O4

Nickel (II) orthomolybdate NiMoO4

Nickel (II) nitrate, hexahydrate Ni(NO3)2·6H2ONickel (II) oxalate, dihydrate NiC2O4·2H2ONickel (II) oxide NiONickel (II) orthophosphate Ni3(PO4)2

Nickel (II) hypophophite, hexahydrate Ni(H2PO)2·6H2ONickel (II) selenide NiSeNickel (II) orthosilicate Ni2SiO4

Nickel sulfide NiS2

Nickel (II) sulfide NiSNickel (II) metatitanate NiTiO3

Nickel (II) orthotungstate NiWO4

Nickel (II) metavanadate Ni(VO3)2

Niobium (V) bromide NbBr5

Niobium (III) chloride NbCl3

Niobium (V) chloride NbCl5

Niobium (V) iodide NbI5

Niobium (III) oxide Nb2O3

P seriesPhosphorus (II) iodide P2I4

Phosphorus (V) nitride P3N5

Phosphorus (III) selenide P2Se3

Phosphorus (V) selenide P2Se5

Phosphorus (III) sulfide P2S3

Phosphorus (III) telluride P2Te3

Potassium ethoxide KC2H5OPotassium fluostannate, hydrate K2SnF4·xH2OPotassium orthomolybdate K2MoO4

Potassium nitrosodisulfonate(Fremys salt) (KSO3)2NOPotassium selenate K2SeO4

Potassium selenite K2SeO3

Potassium selenocyanate KSeCNPotassium tantalate KTaO3

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Potassium tellurate K2TeO4

Potassium tellurite K2TeO3

Potassium thiomolybdate K2MoS4

Potassium metatitanate K2TiO3

Potassium orthovanadate K2VO4

Potassium metazirconate K2ZrO3

R seriesRare Earth (RE) Compounds La, Ce, Pr, Nd, Sm, Tm, Yb and Lu.

RE (III) acetate, hydrate RE(C2H3O2)3·xH2ORE (IV) aluminate REAl2O3

RE (III) hydrogen arsenate, hydrate RE(HAsO4)3·xH2ORE (III) benzoate, trihydrate RE(C7H5O2)3·3H2ORE (III) bromate, hydrate RE(BrO3)3·xH2ORE (III) bromide REBr3

RE (III) bromide, hydrate REBr3·xH2ORE (III) chlorate, hydrate RE(ClO3)3·xH2ORE (III) chloride RECl3

RE (III) chloride, hydrate RECl3·xH2ORE (III) chromate, hydrate RE2(CrO4)3·xH2ORE (III) orhtomolybdate RE2(MoO4)3

RE (III) metaniobate RE(NbO3)3

RE (III) nitrate, hydrate RE(NO3)3·xH2ORE (III) oxalate, hydrate RE2(C2O4)3·xH2ORE (III) orthophosphate REPO4

RE (III) selenate, hydrate RE(SeO4)3·xH2ORE (III) selenite RE(SeO3)3

RE (IV) orhtosilicate RESiO4

RE (III) sulfate, hydrate RE2(SO4)3·xH2ORE (III) metatantalate RE(TaO3)3

RE (III) tellurate RE2(TeO4)3

RE (III) tellurite RE2(TeO3)3

RE (IV) metatitanate RE2(TiO3)3

RE (III) orthotungstate RE2(WO4)3

RE (III) orhtovanadate REVO4

RE (III) metazirconate RE2(ZrO3)3

Rubidium actate RbC2H3O2

Rubidium aluminum sulfate, dodecahydrate RbAl(SO4)2·12H2ORubidium bromide RbBrRubidium perclorate RbClO4

Rubidium chloride RbClRubidium chromate Rb2CrO4

Rubidium citrate, monohydrate Rb3C6H5O7·H2ORubidium fluoride RbFRubidium nitrate RbNO3

Rubidium oxalate Rb2C2O4

Rubidium orthophosphate Rb2PO4

Rubidium selenate Rb2SeO4

Rubidium selenite Rb2SeO3

57

S seriesSelenic acid, 40% H2SeO4

Selenium (IV) bromide SeBr4

Selenium (I) chloride SeClSelenium (IV) chloride SeCl4

Selenium (IV) oxide SeO2

Selenium (IV) oxychloride SeOCl2

Selenium (IV) telluride SeTe

Silicon (IV) acetate Si(C2H3O2)4

Silicon (IV) bromide SiBr4

Silicon (IV) chloride SiCl4

Silicon (IV) iodide SiI4

Silicon (IV) oxide SiO2

Silver (I) antimony (III) selenide AgSbSe2

Silver (I) antimony (III) sulfide AgSbS2

Silver (I) antimony (III) telluride AgSbTe2

Silver (I) arsenic (III) selenide AgAsSe2

Silver (I) arsenic (III) sulfide AgAsS2

Silver (I) arsenic (III) telluride AgAsTe2

Silver (I) bismuth (III) selenide AgBiSe2

Silver (I) bismuth (III) sulfide AgBiS2

Silver (I) bismuth (III) telluride AgBiTe2

Silver (I) bromide AgBrSilver (I) chloride AgClSilver (I) iodide AgISilver (I) oxide Ag2OSilver (I) selenide Ag2SeSilver (I) telluride Ag2TeSilver (I) orthotungstate Ag2WO4

Silver (I) metavanadate AgVO3

Silver (I) metazirconate Ag2ZrO3

Sodium metaarsenite NaAsO2

Sodium metaniobate NaNbO3

Sodium metaniobate, heptahydrate NaNbO3·7H2OSodium selenate Na2SeO4

Sodium selenite NaSeO3

Sodium monosulfide Na2SSodium tetrasulfide Na2S4

Sodium metatantalate NaTaO3

Sodium tellurate Na2TeO4

Sodium tellurite Na2TeO3

Sodium thiomolybdate Na2MoS4

Sodium metatitanate Na2TiO3

Sodium metavanadate NaVO3

Sodium orthovanadate Na3VO4

Sodium pyrovanadate Na4V2O7

Sodium zincate Na2ZnO2

Sodium metazirconate Na2ZrO3

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Strontium bromide SrBr2

Strontium bromide, hexahydrate SrBr2·6H2OStrontium iodide SrI2

Strontium iodide, hexahydrate SrI2·6H2OStrontium permanganate Sr(MnO4)2

Strontium orthomolybdate SrMoO4

Strontium metaniobate Sr(NbO3)2

Strontium selenate SrSeO4

Strontium selenite SrSeO3

Strontium tellurate SrTeO4

Strontium tellurite SrTeO3

Strontium metatitanate SrTiO3

Sulfur (II) bromide S2Br2

T seriesTantalum (III) bromide TaBr3

Tantalum (V) bromide TaBr5

Tantalum (V) chloride TaCl5

Tantalum (V) iodide TaI5

Telluric acid H6TeO6

Tellurous acid H2TeO3

Tellurium (II) bromide TeBr2

Tellurium (IV) bromide TeBr4

Tellurium (II) chloride TeCl2

Tellurium (IV) chloride TeCl4

Tellurium (II) iodide TeI2

Tellurium (IV) iodide TeI4

Tellurium (IV) oxide TeO2

Thallium (I) acetate TlC2H3O2

Thallium (I) arsenide Tl3AsThallium (I) bromide TlBrThallium (III) bromide TlBr3

Thallium (I) chloride TlClThallium (III) chloride TlCl3

Thallium (I) formate Tl(CHO2)Thallium (I) fluoride TlFThallium (I) hydroxide TlOHThallium (I) iodide TlIThallium (III) iodide TlI3

Thallium (I) malonate Tl(C3H3O4)Thallium (I) orthomolybdate Tl2MoO4

Thallium (I) nitrate TlNO3

Thallium (I) selenite Tl2SeO3

Thallium (I) tellurite Tl2TeO3

Thallium (I) orthotungstate Tl2WO4

Tin (IV) antimonide Sn3Sb4

Tin (II) bromide SnBr2

Tin (IV) bromide SnBr4

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Tin (IV) bromotrichloride SnBrCl3

Tin (IV) dibromodichloride SnBr2Cl2

Tin (IV) tribromochloride SnBr3ClTin (II) chloride SnCl2

Tin (IV) chloride SnCl4

Tin (IV) dichlorodiiodide SnCl2I2

Tin (IV) chromate Sn(CrO4)2

Tin (IV) iodide SnI4

Tin (IV) oxide SnO2

Tin (II) selenide SnSeTin (IV) selenide SnSe2

Tin (IV) sulfate, dihydrate Sn(SO4)2·2H2OTin (II) telluride SnTeTin (IV) telluride SnTe4

Tin (II) metavanadate Sn(VO3)2

Titanic acid H2TiO3

Titanium (IV) bromide TiBr4

Titanium (IV) bromotrichloride TiBrCl3

Titanium (IV) tribromochloride TiBr3ClTitanium (IV) dichlorodiiodide TiCl2I2

Titanium (IV) trichloroiodide TiCl3ITitanium (IV) iodide TiI4

Titanium (IV) oxynitrate, hydrate TiO(NO3)2·xH2O

V seriesVanadium (II) bromide VBr2

Vanadium (III) bromide VBr3

Vanadium (II) chloride VCl2

Vanadium (III) chloride VCl3

Vanadium (III) chloride, hexahydrate VCl3·6H2OVanadium (III) oxide V2O3

Z seriesZinc (II) aluminate Zn(AlO2)2

Zinc (II) antimonide Zn3Sb2

Zinc (II) arsenide Zn3As2

Zinc (II) bromide ZnBr2

Zinc (II) chlorate Zn(ClO3)2

Zinc (II) chloride ZnCl2

Zinc (II) hydroxide Zn(OH)2

Zinc (II) iron (III) oxide ZnFe2O4

Zinc (II) iodate, dihydrate Zn(IO3)2·2H2OZinc (II) iodide ZnI2

Zinc (II) orthomolybdate ZnMoO4

Zinc (II) metaniobate Zn(NbO3)2

Zinc (II) oxide ZnOZinc (II) selenate, pentahydrate ZnSeO4·5H2OZinc (II) selenite ZnSeO3

Zinc (II) stannate ZnSnO3

Zinc (II) metatantalate Zn(TaO3)2

Zinc (II) tellurate ZnTeO4

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Zinc (II) tellurite ZnTeO3

Zinc (II) metatitanate ZnTiO3

Zinc (II) orthotungstate ZnWO4

Zinc (II) metavanadate Zn(VO3)2

Zinc (II) metazirconate ZnZrO3

Zirconium (IV) bromide ZrBr4

Zirconium (IV) iodide ZrI4

Zirconium (IV) phosphate Zr3(PO4)4