In a series of experiments, a chemist prepared three different compounds that contain only iodine and fluorine and determined the mass of each element in each compound: Compound Mass of Iodine (g) Mass of Fluorine (g) 1 4.75 3.56 2 7.64 3.43 3 9.41 9.86 (b) How do the numbers in part (a) support the atomic theory?

Key Concepts

Atomic Theory

Atomic theory posits that matter is composed of discrete units called atoms, which combine in specific ratios to form compounds. This theory explains the behavior of elements and compounds, including their mass relationships. In the context of the question, the varying masses of iodine and fluorine in the compounds illustrate how different combinations of atoms can yield distinct substances, supporting the idea that atoms combine in fixed proportions.

Law of Definite Proportions

The Law of Definite Proportions states that a chemical compound always contains its component elements in fixed ratio by mass, regardless of the sample size or source. This principle is crucial for understanding the data presented in the question, as the mass ratios of iodine to fluorine in each compound should reflect consistent proportions, reinforcing the atomic theory and the concept of fixed composition in compounds.

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It allows chemists to predict the amounts of substances consumed and produced in a given reaction. In this question, stoichiometric calculations can be applied to analyze the mass data of iodine and fluorine, demonstrating how the ratios of these elements in the compounds align with the principles of atomic theory and the law of definite proportions.