Understanding Empirical and Molecular Formulas

A molecular formula shows the actual number of atoms of each element in a molecule. For example, $$C_6H_{12}O_6$$ is the molecular formula for glucose.

An empirical formula represents the simplest whole-number ratio of atoms of each element in a compound. For example, the empirical formula for glucose ( $$C_6H_{12}O_6$$ ) is $$CH_2O$$ .

To find the empirical formula, divide the subscripts in the molecular formula by their greatest common divisor. For example, for $$C_8H_{18}$$ , divide by 2 to get $$C_4H_9$$ .

The molecular formula is always a multiple of the empirical formula. For example, if the empirical formula is $$CH_2$$ , the molecular formula could be $$C_2H_4$$ or $$C_4H_8$$ .

No, the empirical formula is not always the same as the molecular formula. They can differ, especially in larger molecules.

The empirical formula is $$CH_2$$ .

The empirical formula is $$C_2H_5$$ .

$$C_6H_{12}O_6$$ is an example of a molecular formula.

$$CH_2O$$ is an example of an empirical formula.

False. The molecular formula is always a multiple of the empirical formula.