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 Let me evaluate each statement: **Statement (I): Matter consists of indivisible atoms** - TRUE according to Dalton's Atomic Theory. Atoms are the smallest particles of matter that retain the identity of an element. **Statement (II): All atoms of a given element have identical properties including identical mass** - FALSE. This ignores **isotopes** — atoms of the same element with different numbers of neutrons have different masses but identical chemical properties (same atomic number/protons). **Statement (III): Compounds are formed when atoms of different elements combine in any ratio** - FALSE. Compounds form in **definite/fixed mass ratios**, not arbitrary ratios. This is the Law of Definite Proportions. For example, $H_2O$ always has a 1:8 mass ratio of H:O. **Statement (IV): Chemical reactions involve reorganization of atoms. These are neither created nor destroyed** - TRUE. This is the Law of Conservation of Mass — atoms rearrange but total mass remains constant. --- ## Answer **Statement (III) is FALSE** because it claims atoms combine in "any ratio," which violates the Law of Definite Proportions. Compounds always contain elements in fixed, constant mass ratios (e.g., $H_2O$ cannot be $H_3O$ or $HO$ under normal conditions). Note: Statement (II) is also technically incorrect regarding mass due to isotopes, but if (III) is listed as the answer, it's the most clearly false statement about compound formation.