* Empirical Formula: The simplest whole-number ratio of atoms in a compound. It tells you the relative proportions of elements but not the actual number of atoms.
* Molecular Formula: The actual number of atoms of each element in a molecule.
Here's a breakdown:
* Case 1: Molecular formula is the same as the empirical formula.
* Example: Water (H₂O). Both the empirical and molecular formulas are H₂O.
* Case 2: Molecular formula has a higher number of atoms.
* Example: Glucose (C₆H₁₂O₆). Its empirical formula is CH₂O, but the molecular formula shows the actual number of atoms.
* Case 3: Molecular formula has a lower number of atoms.
* This is impossible because the molecular formula represents the actual number of atoms in a molecule. It cannot be smaller than the empirical formula, which represents the simplest ratio.
In summary:
* The molecular formula will always be the same as or a multiple of the empirical formula.
* It's only when the molecular formula is a multiple of the empirical formula that the number of atoms in the molecular formula is greater.
