What is the Difference Between Empirical and Molecular Formulas?
🆚 Go to Comparative Table 🆚The main difference between empirical and molecular formulas lies in the ratio of atoms in a compound. Here is a comparison of the two types of formulas:
Empirical Formula:
- Represents the simplest whole-number ratio of atoms in a compound.
- Found from mass percentages of elements in a compound.
- Used to determine the actual elemental composition of a compound.
- Can be found through combustion or composition analysis.
Molecular Formula:
- Shows the actual number of each type of atom in a molecule.
- Found using the empirical formula and the molecular weight of the compound.
- Represents the actual elemental composition of a compound.
- The molecular formula is a multiple of the empirical formula, although sometimes the empirical formula is multiplied by "1", making the two formulas the same.
For example, the empirical formula for glucose is CH₂O, while its molecular formula is C₆H₁₂O₆. The molecular formula is a multiple of the empirical formula, which is simplified to represent the simplest whole-number ratio of the elements in the compound.
Comparative Table: Empirical vs Molecular Formulas
Here is a table comparing the differences between empirical and molecular formulas:
Property | Empirical Formula | Molecular Formula |
---|---|---|
Definition | The simplest whole-number ratio of elements in a compound. | The actual ratio of elements in a compound. |
Determination | Found from mass percentages of elements in a compound. | Found using the empirical formula and the molar mass of the compound. |
Subscripts | Always the smallest whole-number ratio of atoms or ions. | Shows exactly how many atoms are present in a molecule. |
Relationship | The molecular formula can be an integer multiple of the empirical formula. | - |
For example, consider the compound glucose. It has a molecular formula of C6H12O6 and an empirical formula of CH2O. The molecular formula shows the actual number of atoms of each element present in a molecule, while the empirical formula represents the simplest whole-number ratio of atoms.
- Molecular Formula vs Structural Formula
- Formula Weight vs Molecular Weight
- Formula Unit Mass vs Molecular Mass
- Formula Mass vs Molar Mass
- Molecular Equation vs Ionic Equation
- Chemical Symbol vs Chemical Formula
- Ionic vs Molecular Compounds
- Molar Mass vs Molecular Mass
- Molecules vs Compounds
- Atomic vs Molecular Elements
- Ionic vs Molecular Solids
- Exact Mass vs Molecular Weight
- Molecular Geometry vs Electron Geometry
- Conceptual vs Empirical
- Atomic Spectroscopy vs Molecular Spectroscopy
- Mass vs Molar Mass
- Atomic Mass vs Molecular Weight
- Molecule vs Mixture
- Element vs Molecule