How is the molecular formula different from the empirical formula?

The distinction between the molecular formula and the empirical formula lies in what they represent regarding the composition of a chemical compound. The molecular formula provides specific information about the actual number of each type of atom present in a molecule of a substance. For example, if a compound has the molecular formula C6H12O6, it indicates that there are 6 carbon atoms, 12 hydrogen atoms, and 6 oxygen atoms in each molecule.

In contrast, the empirical formula expresses the simplest whole-number ratio of the types of atoms in a compound, which for glucose would be CH2O, reflecting the ratio of carbon to hydrogen to oxygen without indicating the actual count of atoms in the molecule.

This means that while the molecular formula provides a complete picture of the structure and composition of a molecule, the empirical formula provides a simplified version based on the ratio of elements. Thus, the statement about the molecular formula showing the number of each type of atom in a molecule accurately captures its role in chemical representation. In the context of chemical formulas, understanding this difference is crucial for various applications in chemistry, including stoichiometry, synthesis, and characterization of compounds.