var nc = 20, fc = new Array(nc); fc[0] = {t:"Actual Yield",d:"The amount of product obtained from a chemical reaction, which is often less than the theoretical yield."}; fc[1] = {t:"Avogadro’s Number (NA)",d:"The number of carbon atoms in exactly 12 grams of the carbon-12 isotope; NA = 6.022 × 1023. It is the number of particles in one mole."}; fc[2] = {t:"Chemical Equation",d:"Notation in which chemical formulas express the identities and their coefficients express the quantities of substances involved in a chemical reaction; a description of the identities and quantities of reactants (substances consumed during a chemical reaction) and products (substances formed)."}; fc[3] = {t:"Combination Reaction",d:"A reaction in which two (or more) substances combine to form one product."}; fc[4] = {t:"Combustion Analysis",d:"A laboratory procedure for determining the composition of a substance by burning it completely in oxygen to produce known compounds whose masses are used to determine the composition of the original material."}; fc[5] = {t:"Combustion Reaction",d:"A reaction between oxygen and another element or compound that produces heat."}; fc[6] = {t:"Formula Mass",d:"The mass in atomic mass units of one formula unit of an ionic compound."}; fc[7] = {t:"Hydrocarbons",d:"A class of organic compounds containing molecular compounds composed of only hydrogen and carbon."}; fc[8] = {t:"Hydrolysis",d:"The reaction of water with another material. The hydrolysis of nonmetal oxides produces acids."}; fc[9] = {t:"Law of Conservation of Mass",d:"The sum of the masses of the reactants in a chemical reaction is equal to the sum of the masses of the products."}; fc[10] = {t:"Limiting Reactant",d:"A reactant that is consumed completely in a chemical reaction. The amount of product formed depends on the amount of the limiting reactant available."}; fc[11] = {t:"Mass Spectrum",d:"A graph of the data from a mass spectrometer, where m/z ratios of the deflected particles are plotted against the number of particles with a particular mass. Because the charge on the ions typically is 1+, m/z = m/1 = m, and the mass of the particle may be read directly from the m/z axis."}; fc[12] = {t:"Molar Mass (M)",d:"The mass of 1 mole of a substance. The molar mass of an element in grams per mole is numerically equal to that element’s average atomic mass in atomic mass units."}; fc[13] = {t:"Mole (mol)",d:"An amount of material (atoms, ions, or molecules) that contains Avogadro’s number (NA = 6.022 × 1023) of particles."}; fc[14] = {t:"Molecular Ion (M+)",d:"An ion formed in a mass spectrometer when a molecule loses an electron after being bombarded with high-energy electrons. The molecular ion has a charge of 1+ and has essentially the same molecular mass as the molecule from which it came."}; fc[15] = {t:"Molecular Mass",d:"The mass of one molecule of a molecular compound."}; fc[16] = {t:"Percent Composition",d:"The composition of a compound expressed in terms of the percentage by mass of each element in the compound."}; fc[17] = {t:"Percent Yield",d:"The ratio, expressed as a percentage, of the actual yield of a chemical reaction to the theoretical yield."}; fc[18] = {t:"Stoichiometry",d:"The quantitative relation between the reactants and products in a chemical reaction."}; fc[19] = {t:"Theoretical Yield",d:"The maximum amount of product possible in a chemical reaction for given quantities of reactants; also known as stoichiometric yield."};