Final answer:
Empirical formulas represent the simplest whole-number ratio of elements in a compound, which may be derived from its molecular formula by dividing the subscripts by the greatest common divisor. The molecular formula of a substance may or may not be the same as its empirical formula, but it is always a multiple of it. To convert an empirical formula into a molecular formula, the molar mass of the compound is required.
Step-by-step explanation:
The subject of this question is to match each molecular formula to the corresponding empirical formula and to discuss related concepts.
Empirical formulas represent the simplest whole-number ratio of elements in a compound. For example, a molecule's molecular formula may be more complex, such as C4H8O2, but the empirical formula might be reduced to C2H4O by dividing each subscripts by the greatest common divisor, in this case, 2.
It's important to note that C6H12O6 is not the empirical formula for glucose because its simplest whole-number ratio is CH2O. Molecular formulas are exact representations of the molecules in a substance, while empirical formulas are a simplified representation showing the ratio of elements. Notably, the molecular formula is always a whole-number multiple of the empirical formula.
A compound's molecular formula can be the same as its empirical formula if the compound's simplest ratio of elements happens to match the actual number of atoms in the molecule. For instance, water (H2O) and benzene (C6H6) have molecular formulas that are also their empirical formulas.
To determine a molecular formula from an empirical formula, one must know the molar mass of the compound. This information, combined with the molar mass of the empirical formula, allows for the calculation of the molecular formula by finding the ratio between the two molar masses.