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Atomic Theory

Explore the history of the atom, from the Early Greeks' belief in tiny particles to John Dalton's Atomic Theory. Learn about the fundamental principles of atomic structure that govern the composition of matter. Discover how Dalton's theory still resonates today, with insights into isotopes, laws of conservation, definite composition, and multiple proportions.

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Atomic Theory

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  1. Atomic Theory

  2. History of Atom • Early Greeks believed that matter consisted of tiny particles – they called the “atoms”

  3. John Dalton • English school teacher in 1800’s • Proposed atomic theory

  4. Dalton’s Atomic Theory • All matter is composed of tiny particles called atoms • Atoms of a given element have the same size, mass, and physical properties • Atoms cannot be subdivided, created, or destroyed

  5. Atoms can combine in simple, whole-number ratios to form compounds • In chemical reactions, atoms can combine, separate, or rearrange

  6. Dalton’s Theory Today • Dalton’s theory still holds true today with a few exceptions • Atoms can be subdivided in nuclear reactions • Atoms of he same element can have different masses – they are called Isotopes

  7. Law of Conservation of Mass • Matter and its mass cannot be created or destroyed

  8. Law of Definite Composition • In a compound, the ratio of atoms is always the same • For example: water (H2O) always has a mass ratio of 1:8 • In water there is always 1 gram of water for 8 grams of oxygen

  9. Law of Multiple Proportions • Two or more different compounds are composed of the same 2 elements, they are whole number ratios of each other

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