History of the Atomic Theory. Law of Definite Proportions A given compound contains the same elements in exactly the same proportions by mass, regardless.

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Presentation transcript:

History of the Atomic Theory

Law of Definite Proportions A given compound contains the same elements in exactly the same proportions by mass, regardless of the size of the sample or the source of the compound e.g. NaCl always contains 39.34% by mass of sodium and 60.66% by mass of Chlorine

Law of Conservation of Mass  The mass of the products of a reaction equals the mass of the reactants  e.g. 32 mass units of sulfur and 32 mass units of oxygen react to form 64 mass units of sulfur dioxide

Law of Multiple Proportions  The mass ratio for one of the elements that combines with a fixed mass of another element can be expressed in small whole numbers  e.g. 2 grams of hydrogen combine with 16 grams of oxygen to form water, but 2 grams of hydrogen combine with 32 grams of oxygen to form hydrogen peroxide 16:32 = 1:2 16:32 = 1:2

John Dalton

John Dalton’s Billiard Ball Model Category/categoryID/77.cfm?STLCMPID=1798&engine=adwords!1994&keyword = %28billiard+ball%29&match_type=

Dalton’s Atomic Theory  1. All matter is made of indivisible and indestructible atoms.  2. All atoms of a given element are identical in their physical and chemical properties.  3. Atoms of different elements differ in their physical and chemical properties.  4. Atoms of different elements combine in simple whole-number ratios to form compounds.  5. Chemical reactions consist of the combination, separation, or rearrangement of atoms.

J. J. Thomson

Plum Pudding model

Ernest Rutherford

Rutherford’s Gold Foil Experiment

Niels Bohr

James Chadwick

Model of the Atom Model of the Atom

Louis deBroglie and Erwin Schrodinger

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