Molecular Formula Chemistry Example 1

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easy

Explain the difference between an empirical formula and a molecular formula. Give an example where they differ.

1
The empirical formula shows the simplest whole-number ratio of atoms (e.g., $\text{CH}_2\text{O}$ ).
2
The molecular formula shows the actual number of atoms in one molecule (e.g., $\text{C}_6\text{H}_{12}\text{O}_6$ for glucose).
3
The molecular formula is always a whole-number multiple of the empirical formula: $\text{C}_6\text{H}_{12}\text{O}_6 = (\text{CH}_2\text{O})_6$ .

Answer

\text{Empirical: CH}_2\text{O. Molecular: C}_6\text{H}_{12}\text{O}_6\text{ (×6 multiple)}

Some compounds have the same empirical and molecular formula (e.g., water is both

\text{H}_2\text{O}

). Others differ — acetic acid (

\text{C}_2\text{H}_4\text{O}_2

) and glucose (

\text{C}_6\text{H}_{12}\text{O}_6

) share the same empirical formula

\text{CH}_2\text{O}

but are completely different compounds.

About Molecular Formula

The chemical formula showing the actual number of atoms of each element in one molecule of a compound, as opposed to the empirical formula which.

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