text: # Molecular Formula
  
  Molecular Formula - represent the actual numbers of atoms of the different elements in one molecule of a compound. An example is Ca(NO3)2
  
  Ca = Ca (only one Ca) , (1*2)N = 2N (two nitrogens) , (3*2)O = 6O (six oxygens)
  
  It is not written CaN2O6  but Ca(NO3)2  - why is that?
  That is because there is more information in Ca(NO3)2 than CaN2O6. By the molecular formula we can see that Ca(NO3)2 contain two NO3 - groups. Other groups used in a typical moelcular formula: NO2 (nitrite) , SO4 (sulfate) , SO3  (sulfite) , OH (hydroxyl)...
  
  Determination of the molecular formula by the empirical formula and mass percent composition
  
  Example: A combustion analysis gives the following mass %:  H= 9.15%    C = 54.53%   O = 36.32% . Determine the molecular formula knowing that : molecular mass = 132.16 , empirical formula = C2H4O
  
  Solution
  
  Assume a 100 gram sample which will convert the given percentages to gram amounts
  
  (9.15 gram H)/(1 gram/mole) = 9.15 moles
  
  (54.53 gram C)/(12 gram/mole) = 4.54 moles
  
  (36.32 gram O)/(16 gram/mole) = 2.27 moles
  
  Determination of the simplest moles ratio:
  
  Divide each of the moles figures by the lowest of the three (in this case 2.27).
  
  2.27 moles O /2.27 =1     ,    9.15 moles H/2.27 = 4      ,     4.54 moles C/2.27 = 2
  
  2*12.0 + 4*1.0 + 1*16.0 = 44
  
  Calculating the common factor:
  
  The common factor defines the ratio (molecular formula)/(empirical formula):
  
  132.16/ 44  =  3
  
  Determination of the molecular formula :
  
  The solution: Multiply C2H4O  by the common factor --> C(2*3)H(4*3)O(1*3)  =  C6H12O3
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