1. Law of Conservation of Mass: During a chemical reaction, the total mass of the products is always equal to the total mass of the reactants. This principle established that matter cannot be created or destroyed during chemical changes.
2. Law of Definite Proportions: When elements combine to form compounds, they do so in fixed and definite proportions by mass. The ratio of the masses of the elements in a compound is constant regardless of the amount of the compound.
3. Law of Multiple Proportions: When two elements form more than one compound, the masses of one element that combine with a fixed mass of the other element are in simple, whole-number ratios.
4. Atomic Structure: All matter is made up of tiny particles called atoms. Atoms are the fundamental building blocks of matter and are indivisible by chemical means.
5. Indestructibility of Atoms: Atoms cannot be created or destroyed during chemical reactions. They can only be rearranged to form different substances.
6. Homogeneity of Atoms: All atoms of a given element are identical in terms of their mass, size, and other fundamental properties.
7. Heterogeneity of Compounds: Compounds are formed when atoms of different elements combine. The atoms in a compound are held together by chemical forces.
Dalton's atomic theory revolutionized the understanding of the nature of matter and laid the groundwork for modern chemistry.
