January 10th 2015 Chemistry Video Notes Chapter 2 Formulas Names and Masses of Compounds Binary Ionic Compounds Normal balance them Transition Metals these are the ones that have roman numerals next to them Study tables 2 3 2 4 2 5 2 6 prefixes Polyatomic Ions just like simple ionics Cation first then anion Polyatomic must be in parenthesis only if there is more than 1 eg Ca NO3 2 Hydrates are ionic compounds having a humber of water molecules associated with each formula unit prefix hydrate Only use prefixes Di or Mono when Oxoanions Families of 2 Whichever has more ate Less ite Ex Sulfate so4 2 and sulfite so3 2 phosphate and phosphite Nitrate and nitrite 4 in a family Pre and suffixes Most oxygen per ate One less than most ate Two less oxygen atoms ite One with three less hypo ite Ex 4 Chlorine oxoanions ClO4 is perchlorate ClO3 is chlorate ClO2 is chlorite ClO is hypochlorite Acids Two kinds Binary acids hydrogen plus one more atom Oxoacids oxoanions with enough hydrogen ions to make them neutral Binary acids Hydro anion nonmetal root suffix ic word acid Oxoacid names much like oxoanions Anion ate becomes ic suffix in acid Anion ite suffix becomes an ous suffix in acid Oxoanion prefixes hypo and per are retained Ex BrO4 is perbromate so HBrO4 is perbromic acid Binary Covalent Compounds element with lower group number first Second element changes suffix to ide First element when 2 atoms has prefix Second element always does Exception oxygen and halogen halogen comes first Straight chain Alkanes Hydrocarbons simplest type of organic compound Methane CH4 Ethane C2H6 Propane C3H8 Butane C4H10 Pentane C5H12 Number of Carbons times 2 plus two Molecular mass sum of atomic masses Mixtures Aqueous Solutions are mixtures in water