The structural formulas of the compounds n-butane and isobutane are shown below. (b) Determine the empirical formula of each.

Verified step by step guidance

1. Identify the molecular formula of isopentane by counting the number of carbon (C) and hydrogen (H) atoms in the structure.
2. Identify the molecular formula of hexane by counting the number of carbon (C) and hydrogen (H) atoms in the structure.
3. Determine the empirical formula of isopentane by finding the simplest whole number ratio of the atoms in its molecular formula.
4. Determine the empirical formula of hexane by finding the simplest whole number ratio of the atoms in its molecular formula.
5. Compare the empirical formulas of isopentane and hexane to see if they are the same or different.

Key Concepts

Empirical Formula

The empirical formula of a compound represents the simplest whole-number ratio of the elements present in that compound. It is derived from the molecular formula by dividing the subscripts of each element by their greatest common divisor. For example, the empirical formula for C6H12 is CH2, indicating that for every carbon atom, there are two hydrogen atoms.

Structural Formulas

Structural formulas depict the arrangement of atoms within a molecule, showing how the atoms are bonded to each other. They provide insight into the molecular geometry and can help identify isomers, which are compounds with the same molecular formula but different structural arrangements. Understanding structural formulas is crucial for determining the empirical formula accurately.

Isomers

Isomers are compounds that share the same molecular formula but differ in the arrangement of atoms, leading to different properties. For instance, n-butane and isobutane are structural isomers, meaning they have the same molecular formula (C4H10) but different structural formulas. Recognizing isomers is essential when calculating empirical formulas, as it affects the interpretation of the molecular structure.