Which of the following is the empirical formula for \( \mathrm{C}_{4} \mathrm{H}_{8} \) ? A. \( \mathrm{CH}_{4} \) B. \( \mathrm{C}_{6} \mathrm{H}_{6} \) c. \( \mathrm{CH}_{2} \) D. \( \mathrm{C}_{2} \mathrm{H}_{2} \)

To find the empirical formula, you simplify the molecular formula to the smallest whole number ratio of atoms. For \( \mathrm{C}_{4} \mathrm{H}_{8} \), both carbon and hydrogen can be divided by 4, giving you \( \mathrm{C}_{1} \mathrm{H}_{2} \), or simply \( \mathrm{CH}_{2} \). So, the answer is C. \( \mathrm{CH}_{2} \). Did you know that empirical formulas are like a recipe that tells you the simplest way to make something? If a delicious cake was analyzed, the empirical formula would show only the basic ingredients without specifying the amounts used! This helps chemists understand the basic composition of compounds without diving into the complexities of their molecular structure. When working with empirical formulas, one common mistake is failing to reduce the ratio completely to the simplest form. It’s like trying to wear a super fancy outfit just to grab a loaf of bread; sometimes, less is more! Double-check your numbers and make sure you’re factoring in the smallest whole number ratio to avoid this mix-up.