chem 112

• A redox reaction will occur only if the atom being oxidized is listed above the atom being reduced.
• Molecular/covalent compounds (no metals) use prefixes.
• Compounds containing a metal that only has one common oxidation state are simple to name and the chemical formula of these compounds is determined using the relative charges of the ions and remembering that the complex must be net neutral (have an overall charge of 0).
• Compounds containing a metal that can take a variety of oxidation states are named using a roman numeral to indicate the oxidation state of the metal.
• For ionic compounds containing polyatomic ions, you will need to know the names, charges, and formulas of the ions.
• The type of intramolecular bonding (ionic, polar covalent, nonpolar covalent) can be determined based on the electronegativity differences between bonded atoms in CH E M 112.
• Nonpolar covalent bonds have a bond order of 0, polar covalent bonds have a bond order of 0.4 – 2.0, ionic bonds have a bond order greater than 2.0.
• The solubility of a substance is the amount of that substance that can be dissolved in a given quantity of solvent at a given temperature.
• The atom that loses electrons in a redox reaction is oxidized, and the atom that gains electrons is reduced.
• Oxidation states can generally be determined by applying the following trends in order: the oxidation state of a free atom is 0, monoatomic ions are assigned an oxidation state of their own charge, the sum of the oxidation states in a compound is equal to the net charge, alkali and alkaline earth metals are always +1 and +2, respectively, fluorine atoms are always assigned an oxidation state of -1, hydrogen atoms in compounds are often assigned an oxidation state of +1, oxygen atoms in compounds are often assigned an oxidation state of -2, elements in groups 17, 16, and 15 are often -1, -2, o
• Oxidation-reduction reactions, also known as redox reactions, occur when electrons are transferred from one reactant to another.
• Two compounds react in a double replacement reaction to form two new compounds.
• The compound containing the atom that is oxidized in a redox reaction is called the reducing agent, and the compound containing the atom that is reduced is called the oxidizing agent.
• The solubility rules for ionic compounds in water are applied in order: alkali metal salts and ammonium salts (NH4+) are soluble, nitrate (NO3-), acetate (CH3CO2-), and perchlorate (ClO4-) salts are soluble, most halides are soluble (except with Ag+, Pb2+, and Hg2+), most sulfates (SO42-) are soluble (except with Ag+, Pb2+, Hg2+, Ba2+, and Ca2+), most carbonates (CO32-), chromates (CrO42-), sulfides, oxides, phosphates (PO42-), and hydroxides are insoluble.
• Atoms in periods 3 and higher may have extended valence shells.
• In a titration, a precisely measured volume of a solution of known concentration is added to a precisely measured volume of a solution of unknown concentration.
• Titration calculations use stoichiometry and mole:mole ratios to determine either the concentration of the unknown solution or the volume of an acid/base required to neutralize a solution.
• In stoichiometry, it is the relative number of reactants and products that is important.
• The percent yield of a reaction is the quantity of product formed as a percentage of the theoretical quantity of that product that should form.
• The mole:mole ratio is used in conversion between substances.
• For reactions in solution, calculations involving Molarity (M) are needed.
• To determine the limiting reactant, calculate the moles of one product that will form if each reactant is completely consumed.
• Acids and bases react in a neutralization reaction to form water and a salt.
• If the quantity of two or more reactants are provided, determine which reactant is limiting.
• The strong acids are: hydrochloric acid, hydrobromic acid, hydroiodic acid, nitric acid, perchloric acid, and sulfuric acid.
• The limiting reactant is the one that runs out first.
• Strong acids completely dissociate in solution, making them strong electrolytes.
• Molarity describes the concentration of a substance in moles of solute per liter of solution.
• Strong bases are the alkali metal hydroxides (LiOH, NaOH, KOH, RbOH, and CsOH), the alkaline-earth metal hydroxides (Ca(OH)2, Sr(OH)2, and Ba(OH)2), and TlOH.
• The dilution equation is: M 1 V 1 = M 2 V 2.