I.  Symbols and Elements
    A.  Names of Elements
        Planets:               People:                 Places:
         Mercury             Curium                 Europium
         Uranium            Einsteinium         Francium
         Plutonium         Mendelevium        Americium
                                   Lawrencium          Berkelium
                                                                 Californium
    B.  Symbols for Elements
         1.  chemical symbol:  short-hand representation of an element
         2.  J.J. Bezerlius:  Swedish chemist given credit for creating the modern
                                     symbols for elements.
         3.  Use first letter of elements name.  For two elements with the same first
              letter, the second letter or another important letter is added.  In some
              cases, the Latin name is used.

             Ex.  S - Sulfur        Se - Selenium    Sr - Strontium    Na - Sodium (Latin for
                                                                                                   Natrium)

        4.  Scientists in both the U.S. and Russia claim the discovery of elements 104
            and 105.  They couldn't decide on a name; therefore, the IUPAC
            (International Union of Pure and Applied Chemistry) adopted a system for
            naming the rest of the elements.

    C.  Use of Symbols
        1.     ³²₁₆S    32 - mass #    16 - atomic #

        2.  Ion:  a charged atom
            a.  positive ion - loses electrons
            b.  negative ion - gains electrons
    D.  Chemical Formulas
          1.  combination of symbols that represents the composition of a compound
          2.  shows 2 things:
               a.  elements present
               b.  # of atoms of each element
 
 

    E.  Oxidation Number
        1.  monotomic ion:  single atom takes a charge
                                      ex.  Cl^-, O^-2
        2.  oxidaton number:  charge on a monotomic ion
        3.  polyatomic ion:  ion made of more than one atom
                                    ex.  CO₃^-2, SO₄^-2, OH^{-
        4.  2 types of compounds
             a.  ionic compounds:  composed of ions; metal and non-metal
                                              ex. NaCl
             b.  molecular compounds:  neutral atoms formed from molecules;
                                                     non-metal and non-metal}
                                                     ex.  H₂O
                        -- diatomic molecules:  made of two atoms of the same element;
                                                          always found in nature as diatomic
 

     5.  Writing Formulas for Ionic Compounds

          ex.  Ca⁺²   Br^-      use subscripts to make the overall charge zero
                CaBr₂

                 _Al⁺³   SO₄^-2  =   Al₂(SO₄)₃

                       Mg⁺²    O^-2    =   MgO

II.  Nomenclature (Rules for Naming)
     A.  Naming Compounds
          1.  Binary Inorganic Compounds - contain only two elements
               a.  write the name of the element having the + charge
               b.  add the name of the negative element
               c.  name of the negative element must be modified to end in -ide
 

            2.  Naming Binary Molecular Compounds
              -- use prefix and end in -ide
 

              Examples:
 
 

    3.  Naming Compounds with Polyatomic Ions
        -- Name the element and end with negative ion name
 
 

  4.  Naming Organic Compounds
 
 

                    ex.  CH₄  -  methane
                          C₂H₆  -  ethane
                          C₅H₁₂ -  pentane

III.  Molecular and Empirical Formulas
       1.  molecular:  formulas for compounds that exist as molecules
                             ex.  H₂O₂  hydrogen peroxide
       2.  empircal:  simplest formula
                           ex.  H₂O₂ ---  HO
                                 C₆H₁₂O₆ --- CH₂O
       3.  coefficients:  used to represent the # of molecules or formula units of a
                                substance.
                                a.  molecules -- molecular compounds
                                b.  formula units -- ionic compounds