Polyatomic Ions, Vocab for ch. 1-11, 20
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Accuracy | The closeness of a measurement to the true value of the quantity that is being measured
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Anion | An ion with a negative net charge
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Cation | An ion with a positive net charge
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Chemical Formula | An expression showing the chemical composition of a compound in terms f the symbols for the atoms of the elements involved
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Chemical Properties | Any property of a substance that cannot be without converting the substance into some other substance
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Chemistry | The science that studies the properties of substances and how substances react with one another
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Compounds | Substances composed of two or more elements chemically united in fixed proportions
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Empirical Formula | An expression using chemical symbols to show the types of elements in a substance and the simplest ratios of the different kinds of atoms
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Energy | The capacity to do work or produce change
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Extensive Property | A property that depends on how much matter is being considered
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Hypothesis | A tentative explaination for a set of observations
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Intensive Property | A property that does not depend on how much matter is being considered
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Law | A concise verbal or mathematical statement of a relationship between phenomena that is always the same under the same conditions
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Law of Conservation of Energy | The total quantity of energy in the universe is constant
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Law of Conservation of Mass | Matter can be neither created nor destroyed
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Limiting Reagent | The reactant used up first in a reaction
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Matter | Anything that occupies space and possesses mass
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Mole | The amount of substance that contains as many entities (atoms, molecules, or other particles) as there are exactly atoms in exactly 12 grams of the carbon-12 isotope
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Molecular Formula | An expression showing the exact number of atoms of each element in a molecule
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Molecule | An aggregate of at least two atoms helt together by special forces
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I - | Iodide
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Fl - | Fluoride
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Br - | Bromide
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MoO4 2- | Molybdate
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MnO4 - | Permangante
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WO4 - | Tungstate
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Se 2- | Selenide
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ClO4 - | Perchlorate
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ClO3 - | Chlorate
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ClO2 - | Chlorite
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ClO - | Hypochlorite
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Cl - | Chloride
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CrO4 2- | Chromate
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Cr2O7 2- | Dichrimate
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CO3 2- | Carbonate
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HCO3 - | Bicarbonate
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C2H3O2 - | Acetate
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C2O4 2- | Oxalate
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CN - | Cyanide
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SCN - | Thiocynate
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O2 2- | Peroxide
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O 2- | Oxide
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OH - | Hydroxide
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H - | Hydride
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NO2 - | Nitrite
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NO3 - | Nitrate
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N 3- | Nitride
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NH2 - | Amide
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PO4 3- | Phosphate
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HPO4 2- | Hydrogen Phosphate
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H2PO4 - | Dihydrogen Phosphate
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HSO3 - | Bisulfite
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SO4 2- | Sulfate
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SO3 2- | Sulfite
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S2O3 2- | Thiosulfate
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S4O6 2- | Tetrathionate
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S 2- | Sulfide
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HSO4 - | Bisulfate
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Area of High Electron Density | Area of an atom or ion at which either a lone pair, single, double, or triple bond is located.
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Atomic Mass | The mass of an atom in atomic mass units.
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Atomic Number (Z) | The number of protons in the nucleus of an atom.
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Atomic Radius | One-half the distance between the nuclei in two adjacent atoms of the same element in a metal. For elements that exist as diatomic units (e.g. oxygen), the atomic radius is one-half the distance between the nuclei of two atoms in a particular molecule.
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Aufbau Principle | As protons are added one by one to the nucleus to build up the elements, electrons similarly are added to the atomic orbitals.
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Coordinate Covalent Bond | A bond in which the pair of electrons is supplied by one of the two bonded atoms.
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Covalent Bond | A bond in which two electrons are shared by two atoms.
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Covalent Compounds | Compounds containing only covalent bonds.
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Dipole-dipole Forces | Forces that act between polar molecules.
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Dipole Moment | The product of charge and distance between the charges in a molecule.
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Electron Affinity | The negative of the energy change that takes place when an electron is accepted by an atom (or an ion) in the gaseous state.
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Electronegativity | The ability of an atom to attract electrons toward itself in a chemical bond.
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Formal Charge | The electrical charge difference between the number of valence electrons in an isolated atom and the number of electrons assigned to that atom in a Lewis structure.
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Hund's Rule | The most stable arrangement of electrons in atomic subshells is the one with the greatest number of parallel spins.
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Hybrid Orbitals | Atomic orbitals obtained when two or more nonequivalent orbitals of the same atom combine before covalent bond formation.
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Aldehydes | Compounds with a carbonyl functional group and the general formula RCH0,in which R is an H atom, an alkyl, or an aromatic hydrocarbon group.
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Alcohol | An organic compound containing the hydroxyl group (- OH)
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Alkanes | Hydrocarbons having the general formula CnH2n+2, in which n=1, 2...
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Alkenes | Hydrocarbons containing one or more carbon-carbon double bonds. They hace the general formula CnH2n, in which n=2, 3,...
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Alkynes | Hydrocarbons that contain one or more carbon-carbon triple bands. They have the general formula CnH2n-2, in whcih n=2, 3,...
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Amines | Organic bases that have the functional group (-NR2), in which R may be H, an alkyl group, or an aromatic hydrocarbon group.
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Aromatic hydrocarbon | A hydrocarbon that contains one or more benzene rings.
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Bronsted base | A substance capable of accepting a proton in a reaction.
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Carboxylic acids | Acids that contain the carboxyl group (-COOH).
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Chelating agent | A substance that forms complex ions with metal ions in solution.
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Chiral | Compounds or ions that are not superimposable with their mirror images.
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Combination reaction | A reaction in which two or more substances combine to form a single product.
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Concentration of a solution | The amount of solute present in a given quantity of solution.
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Coordination number | In coordination compounds, it is defined as the number of donor atoms surrounding the central metal atom in a complex.
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Decomposition reaction | The breakdown of a compound into two or more components.
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Displacement reaction | A reaction in which an atom or an ion in a compound is replaced by an atom of another element.
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Donor atom | The atom of a ligand that is bonded directly to the metal atom.
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Electrolyte | A substance that, when dissolved in water, results in a solution that can conduct electricity.
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End point | Occurs in a titration when the indicator changes color.
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Enantiomers | Compounds and their nonsuperimposable mirror images.
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Equivalenve point | The point at which an acid is completely reacted with or neutralized by a base.
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Esters | Compounds that have the ceneral formula RCOOR', in which R can be H or an alkyl group or an aromatic hydrocarbon and R' is an alkyl group or an aromatic hydrocarbon.
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Ether | An organic compound containint the R-O-R' linkage, in which R and R' are alkyl and/or aromatic hydrocarbons.
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Geometric isomers | Compounds with the same type and number of atoms and the same chemical bonds but different spatial arrangements; such isomers cannot be interconverted without breaking a chemical bond.
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Hydrocarbons | Compounds made up of only carbon and hydrogen.
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Ionic equation | An equation that shows dissolved ionic compounds in terms of their free ions.
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Ketones | Compounds with a carbonyl functional group and the general formula RR'CO, in which R and R' are alkyl and/or aromati c hydrocarbon groups.
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Lewis acid | A substance that can accept a pair of electrons.
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Lewis base | A substance that can donate a pair of electrons.
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Ligand | A molecule or an ion that is bonded to the metal ion in a complex ion.
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Metathesis reaction | A reaction that involves the exchange or parts between compounds.
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Molarity | The number of moles of solute in one liter of solution.
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Molecular equations | Equations in which the formulas of the compounds are written as though all species existed as molecules or whole units.
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Net ionic equation | An equation that includes only the ionic species that actually take part in the reaction.
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Spectator ions | Ions that are not involved in the overall reaction.
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Nonelectrolytes | A substance that, when dissolved in water, gives a solution that is not electrically conducting.
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Oxidation number | The number of charges an atom would have in a molecule if electrons were transferred completely in the direction indicated by the difference in electronegativity.
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pH | The negative logarithm of the hydrogen ion concentration in a aqueous solution.
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Polymer | A molecular compound distinguished by a high molar mass and made up of many repeating units.
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Racemic mixture | An equimolar mixture of two enantioners.
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Redox reaction | A reaction in which there is either a transfer of electrons or a change in the oxidation numbers of the substances taking part in the reaction.
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Resonance | The use of two or more Lewis structures to represent a particular molecule.
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Saturated hydrocarbon | Hydrocarbons that contain only single covalent bonds.
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Solute | The substance present in the smaller amount in a solution.
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Solvent | The substance present in larger amount in a solution.
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Structural isomers | Molecules that have the same molecular formula but different structures.
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Titration | The gradual addition of a solution of accurately known concentration to another solution of unknown concentration until the chemical reaction between the two solutions is complete.
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Unsaturated hydrocarbons | A solution that contains less solute than it has the capacity to dissolve.
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Heat | The thermal energy that can be transferred from an object at one temperature to an object at another temperature.
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Energy | The capacity to do work or cause change.
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Internal energy | The sum pf potential and kinetic energy of a system; the internal energy of a chemical system depends on 1) the number of particles, 2) the type of particles, and 3) the temperature.
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Kinetic energy | Energy due to the motion of an object.
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Potential energy | Energy stored in an object because of the relative positions or orientations of its components.
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Endothermic | Any reaction or process that results in an addition of heat to the system; indicated by +q.
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Exothermic | Any reaction or process that results in a loss of heat from the system; indicated by -q.
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Thermodynamics | the science of heat (energy) transfer.
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Thermal equilibrium | The system and the surroundings are equal in temperature; heat transfer occurs until thermal equilibrium is established.
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System | The object under study; generally the reactants.
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Surroundings | Everything outside the system.
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Law of Conservation of Energy | Energy is conserved.
q surroundings = -q system
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Heat capacity (C) | The amount of heat required to raise the temperature of a given quantity of substance by one degree Celcius.
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Specific heat capacity | calculated as [heat lost of gained by substance, J] / [mass, g] x [T change, K]
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First law of thermodynamics | The change in energy is equal to the heat transferred plus the work done by the system.
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Melting | The phase change from a solid to a liquid.
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Freezing | The phase change from a liquid to a solid.
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Deposition | The process in which vapor molecules are converted directly to the solid phase.
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Sublimation | The process in which molecules go directly from the solid phase into the vapor phase.
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Evaporation | The phase change from a liquid to a gas.
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Condensation | The phase change from a gas to a liquid.
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State function | The properties of a system that depend only on the state of the system.
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Standard state temperature | 298.15 K
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Standard state pressure | 1.0000 atm
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Standard states matter | Any solid is a pure solid; any liquid is a pure liquid; and gas is at 1.00 atm of pressure.
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Enthalpy | A thermodynamic quantity used to describe heat changes taking place at constant pressure.
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Hess's law | When reactants are converted to products, the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps.
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Thermochemical equation | An equation that shows both the mass and enthalpy relations.
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Enthalpy of formation | The enthalpy for the reaction in which one mole of a substance is formed from its constituent elements.
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