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Atoms: The Greek Idea

Explore the historical development of the concept of matter from the Greek idea of atoms by Leucippus and Democritus to modern theories such as the Law of Conservation of Mass by Lavoisier, the Law of Definite Proportions by Proust, and the Atomic Theory of Matter by John Dalton. Discover how the Periodic Table by Dmitri Mendeleev revolutionized our understanding of chemical elements. Learn about isotopes, molecules, and advancements in atom observation technology.

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Atoms: The Greek Idea

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  1. ~384 B.C.E., Aristotle: All matter is composed of four elements and all matter is continuous, not atomistic. Atoms: The Greek Idea

  2. ~ 450 B.C.E., Leucippus and Democritus Atomos: The point at which matter can no longer be subdivided. Atoms: The Greek Idea

  3. Early 1700s Lavoisier Law of Conservation of Mass:During a chemical change, matter is neither created nor destroyed. Lavoisier: The Law of Conservation of Mass

  4. Lavoisier: The Law of Conservation of Mass

  5. Proust: The Law of Definite Proportions 1799, Proust Law of Definite Proportions:A compound always contains the same elements in certain definite proportions.

  6. Proust: The Law of Definite Proportions Regardless of the source, copper carbonate always has the same composition.

  7. Proust: The Law of Definite Proportions The Berzelius experiment illustrates the Law of Definite Proportions.

  8. John Dalton and the Atomic Theory of Matter 1803, John Dalton Law of Multiple Proportions:Elements may combine in more than one set of proportions, with each set corresponding to a different compound.

  9. John Dalton and the Atomic Theory of Matter

  10. John Dalton and the Atomic Theory of Matter • All matter is composed of extremely small particles called atoms. • All atoms of a given element are alike and differ from the atoms of any other element. • Compounds are formed when atoms of different elements combine in fixed proportions. • A chemical reaction involves the rearrangement of atoms.

  11. Isotopes Much of John Dalton’s atomic theory has been modified. For example, John Dalton assumed that all atoms of an element are alike. He did not understand the existence of isotopes. Isotopes are atoms of the same element with different relative masses.

  12. Out of Chaos: The Periodic Table 1869, Dmitri Mendeleev Mendeleev arranged the elements in order of increasing atomic mass. He left gaps for yet undiscovered elements. He also predicted the properties of those elements. When those elements were eventually discovered, many of his predictions were found to be accurate.

  13. Out of Chaos: The Periodic Table

  14. Out of Chaos: The Periodic Table

  15. Atoms: Real and Relevant Atoms are a very real concept. It is even possible to observe computer-enhanced images of atoms.

  16. Leucippus Revisited: Molecules Moleculesare groups of atoms chemically bonded together. A molecule of water is composed of two atoms of hydrogen (H) bonded to an atom of oxygen (O). H2O

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