Empirical Formula Class Notes Introduction:There are several ways of showing the formula of a compound:Displayed or Structural formula: Shows all atoms and bonds between themCondensed formula: Show the atoms and which elements are bonded to each but does not show the bondsMolecular formula: Shows only the atoms present in a compoundEmpirical formula: Minimum ratio of the elements in a molecular formula. It is a simplification of the molecular formula. Empirical Formula is the minimum whole ratio between the atoms in a molecule expressed in Moles.Having the % composition as data or the amount of each element in grams in the compound, it is easy to work out the empirical formula: Steps to calculate the empirical formula: Find the number of grams of each element, present in the compound. Convert the mass of each element to moles using the molar mass from the periodic table. (mass /Ar in grams = # of moles)Divide each mole value by the smallest number of moles calculated in 2 to get whole number ratios. Example 1:Calculate the empirical formula for a compound that has 19.60g of Iron and 5.60 g of Oxygen19.60 g Fe ÷ 56 g Fe/mol = 0.35 /0.35 = 1 ==> Fe15.60 g O ÷ 16 g O/mol = 0.35 / 0.35 = 1 ==> O1 Empirical Formula: FeO Example 2:Calculate the empirical formula for a compound that has 69.94% of Iron and 30.06% of Oxygen.69.94 g Fe ÷ 56 g Fe/mol = 1.24893 / 1.24893 = 1 30.06 g O ÷ 16 g O/mol = 1.87875 / 1.24893 = 1.5 we cannot round numbers that can be expressed by a fraction. In this case, we need to multiply BOTH NUMBERS by two to get two WHOLE NUMBERSFe = 1 x 2 = 2O = 1.5 x 2 = 3 Videos on how to calculate the empirical and molecular formulas