What distinguishes an empirical formula from a molecular formula?

The distinction between an empirical formula and a molecular formula lies primarily in what they represent. An empirical formula is defined as the simplest whole-number ratio of the different types of atoms in a compound. It does not provide information about the actual number of atoms in a molecule but rather simplifies the representation to reflect the relative proportions of each element.

For instance, if a compound contains carbon and hydrogen with a molecular formula of C6H12, the empirical formula would be CH2, indicating that for every carbon atom, there are two hydrogen atoms. This simplification is valuable in understanding the basic composition of compounds, especially when comparing different substances.

In contrast, a molecular formula provides the actual numbers of each type of atom present in a molecule, conveying more detailed information than what is provided by the empirical formula. Therefore, the essence of the empirical formula's role is to summarize the composition of a compound in the simplest terms, highlighting the underlying ratio of elements.