Molecular Formula Notes
Molecular Formula Notes
An ionic compound’s formula unit is usually the empirical formula, but a covalent or molecular compound’s formula does not necessarily indicate the actual numbers of atoms present in each molecule.
Steps:
• First, you calculate up the compound’s molar mass from the periodic table.
• Then, you divide the mass they give you in the problem by the molar mass you calculated in the first step
• Finally, you multiply the subscripts in the given formula by the number you calculated in the second step
Examples:
1) The empirical formula of a compound of phosphorus and oxygen is found to be P2O5. Experimentation shows that the molar mass of this compound is 284g/mol. What is the molecular formula?
P2O5=142g 284g=2 Molecular formula is P4O10 because you
142g multiply P2O5 by 2.
2) Determine the molecular formula of a compound with an empirical formula of NH2 and a formula mass of 48g/mol.
NH2=16g 48g=3 Molecular formula is N3H6 because you
16g multiply NH2 by 3.
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