test 2

• excess reactant remaining = starting amount of excess reactant - excess reactant consumed
• percent yield = (actual yield / theoretical yield) * 100
• in liquid solutions, the solvent is the substance present in the greatest amount
• molecular compounds are typically non-electrolytes
• strong electrolytes ionize completely when dissolved in water and solutions with them conduct electricity strongly
• weak electrolytes ionize minimally when dissolved in water and solutions with them conduct electricity minimally
• molarity (M) = moles (solute) / liters (solution)
• molarity is a temperature dependent quantity
• dilution equation: (initial molarity)(initial volume (L)) = (final molarity)(final volume (L))
• when we dilute a solution, the amount of solute does not change and the amount of solvent increases
• when doing a net ionic equation, if all reactants and products are soluble, then we say there is no reaction, and thus no net ionic equation
• strong acids and bases completely ionize in a solution
• weak acids and bases partially ionize in a solution
• strong acids: HCl (hydrochloric acid), HBr (hydrobromic acid), HI (hydroiodic acid), HClO4 (perchloric acid), HNO3 (nitric acid), and H2SO4 (sulfuric acid)
• weak acids include carboxylic acids and oxyacids
• strong bases include group 1 and 2 metal hydroxides
• weak bases usually include an NH group
• alcohols and alkanes are non electrolytes while carboxylic acids are weak electrolytes
• carbonate and phosphate are insoluble; exceptions = alkali metal ions and ammonium ions
• when an acid and base react, they neutralize each other then form a salt and water
• atoms in their elemental forms have an oxidation state of zero
• monoatomic ions have the same oxidation state as their charge
• halogens have a -1 oxidation state except when combined with fluorine or oxygen
• oxygen has a -2 oxidation state; exception = H2O2 (-1)
• hydrogen has a +1 oxidation state
• oxidation = losing electrons = more positive charge
• reduction = gaining electrons = more negative charge
• in precipitation reactions, the specator ions in the aqueous product have the same concentration as they did before the reaction took place
• boyles law: pressure and volume have are inversely proportional
• charles law: volume and temperature are directly proportional
• avogadro's law: volume and moles of gas are directly proportional
• according to boyles law, as pressure increases volume decreases
• according to charles law, as temperature increases volume increases
• according to avogadros law, as moles increases volume increases
• ionic compounds are strong electrolytes