Provide an example of an empirical and molecular formula.

An empirical formula is the simplest whole number ratio of atoms in a compound, while a molecular formula shows the actual number of atoms of each element in a molecule.

For example, glucose has the empirical formula CH2O, as the ratio of carbon, hydrogen, and oxygen atoms is 1:2:1. However, the molecular formula of glucose is C6H12O6, as there are six carbon, twelve hydrogen, and six oxygen atoms in each molecule.

Another example is ethene, which has the empirical formula CH2, as there is one carbon and two hydrogen atoms. However, the molecular formula of ethene is C2H4, as there are two carbon and four hydrogen atoms in each molecule.

Empirical and molecular formulas are important in determining the composition of compounds and their properties. They can also be used to calculate the molar mass of a compound, which is useful in stoichiometry calculations.

In summary, the empirical formula is the simplest whole number ratio of atoms in a compound, while the molecular formula shows the actual number of atoms of each element in a molecule. Understanding these formulas is essential in chemistry and can be used to determine the composition and properties of compounds.