Here's a breakdown:
* Empirical formula: Shows the simplest ratio of atoms in a compound.
* Molecular formula: Shows the actual number of each type of atom in a molecule.
Example:
* Glucose (C6H12O6) and Acetic acid (C2H4O2) both have the same empirical formula: CH2O.
* Glucose has a molecular formula of C6H12O6, meaning it contains six carbon atoms, twelve hydrogen atoms, and six oxygen atoms.
* Acetic acid has a molecular formula of C2H4O2, meaning it contains two carbon atoms, four hydrogen atoms, and two oxygen atoms.
Why does this happen?
Covalent compounds can form different arrangements of the same atoms, resulting in different structures and properties. These different arrangements can lead to different molecular formulas but the same empirical formula.
In summary:
The empirical formula only provides a simplified view of the compound's composition. It doesn't show the actual number of atoms in a molecule, which is necessary to differentiate between different covalent compounds with the same empirical formula.
