Which statements are inconsistent with Dalton's atomic theory as it was originally stated? Why? a. All carbon atoms are identical. b. An oxygen atom combines with 1.5 hydrogen atoms to form a water molecule. c. Two oxygen atoms combine with a carbon atom to form a carbon dioxide molecule. d. The formation of a compound often involves the destruction of one or more atoms.

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1. 1. Dalton's atomic theory has several key points: atoms of a given element are identical in size, mass, and other properties; atoms cannot be subdivided, created, or destroyed; atoms of different elements combine in simple whole-number ratios to form chemical compounds; and in chemical reactions, atoms are combined, separated, or rearranged.
2. 2. Statement a: 'All carbon atoms are identical.' This statement is consistent with Dalton's atomic theory, which states that all atoms of a given element are identical in their physical and chemical properties.
3. 3. Statement b: 'An oxygen atom combines with 1.5 hydrogen atoms to form a water molecule.' This statement is inconsistent with Dalton's atomic theory. According to the theory, atoms combine in simple whole-number ratios to form compounds. The ratio of 1.5 is not a whole number, so this statement contradicts the theory.
4. 4. Statement c: 'Two oxygen atoms combine with a carbon atom to form a carbon dioxide molecule.' This statement is consistent with Dalton's atomic theory. It describes atoms combining in a simple whole-number ratio to form a compound, which is one of the key points of the theory.
5. 5. Statement d: 'The formation of a compound often involves the destruction of one or more atoms.' This statement is inconsistent with Dalton's atomic theory. According to the theory, atoms cannot be created or destroyed in chemical reactions, they are simply rearranged. Therefore, the idea of atoms being destroyed during the formation of a compound contradicts the theory.

Key Concepts

Dalton's Atomic Theory

Dalton's atomic theory, proposed in the early 19th century, states that matter is composed of indivisible atoms, each element consists of identical atoms, and chemical reactions involve the rearrangement of these atoms. This theory laid the groundwork for modern chemistry by introducing the idea that atoms combine in fixed ratios to form compounds.

Law of Conservation of Mass

The law of conservation of mass states that mass is neither created nor destroyed in a chemical reaction. This principle implies that the total mass of reactants must equal the total mass of products, which contradicts the idea of atoms being destroyed during the formation of compounds, as suggested in option d.

Stoichiometry and Atomic Ratios

Stoichiometry involves the calculation of reactants and products in chemical reactions based on the conservation of mass and the fixed ratios of atoms. According to Dalton's theory, atoms combine in whole number ratios, making the statement about an oxygen atom combining with 1.5 hydrogen atoms inconsistent with the theory, as it suggests a fractional atom ratio.