➗Empirical formula vs Molecular formula🧮
Chemical formulas come in two forms. One gives the simplest ratio, the other gives the true number of atoms.
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➗Empirical formula
- ✓Shows the simplest whole-number ratio
- ✓Reduced to lowest terms
- ✓Found from percentage composition
- ✓Same for related compounds
- ✓Example: CH for benzene
🧮Molecular formula
- ✓Shows the actual number of atoms
- ✓A whole-number multiple of the empirical
- ✓Found using the molar mass
- ✓Unique to the specific compound
- ✓Example: C6H6 for benzene
Verdict
The empirical formula gives the simplest ratio; the molecular formula gives the real count. Multiply the empirical formula by a whole number, found from molar mass, to get the molecular one.
Frequently asked
How do I get the molecular formula?+
Find the empirical formula, then multiply it by molar mass divided by empirical mass.
Can they be the same?+
Yes. For water, both the empirical and molecular formula are H2O.
What does the empirical formula come from?+
It is calculated from the percentage composition by mass of each element.
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