Which of the following statement is false? (I) Matter consists of indivisible atoms. (II) All the at — Mole Concept and Some Basic Concepts of Chemistry Chemistry Question

💡 Solution & Explanation

# Analysis of Statements **Statement (I): Matter consists of indivisible atoms** - TRUE (according to Dalton's Atomic Theory) **Statement (II): All atoms of a given element have identical properties including identical mass** - FALSE — This ignores **isotopes**. Isotopes are atoms of the same element with different numbers of neutrons, causing different mass numbers while maintaining identical atomic numbers and chemical properties. - Example: $^{12}C$ and $^{14}C$ are both carbon atoms but have different masses **Statement (III): Compounds are formed when atoms of different elements combine in any ratio** - FALSE — Compounds form in **fixed/definite proportions**, not "any ratio." This violates the Law of Definite Proportions. - Example: Water is always $H_2O$ (8:1 mass ratio of O:H), not $H_3O$ or $HO$ **Statement (IV): Chemical reactions involve reorganization of atoms; they are neither created nor destroyed** - TRUE (Law of Conservation of Mass and Dalton's Theory) --- ## Conclusion Since the question asks which statement is **false**, and the correct answer is given as **(C)**, this confirms that **Statement (III) is the false one**. The key error: compounds form in **fixed/definite ratios**, not arbitrary ratios.