9/23/2012. Democritus 400 B.C. Greek philosopher Proposed that all materials are made from atoms. Coined Greek word atmos, meaning indivisible.
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1 Mr. Sudbury Atoms are too small to see with your eyes. Atoms are too small to see with the most powerful microscopes. Scientist use models to explain atoms. A scientific model is an representation containing the essential structure on a smaller scale used to explain or show examples. An explanation of how phenomena occur or how events and data are related. Modern Model of an Atom: Atoms are single particles of an element. Elements are a pure substances that cannot be broken down any further by ordinary chemical means (changes). Elements combine to form compounds which have different physical and chemical properties then the elements that make them up. How did we get to the modern model of an atom? Democritus 400 B.C. Greek philosopher Proposed that all materials are made from atoms. Coined Greek word atmos, meaning indivisible. John Dalton English Scientist from 1800s. Offered proof that atoms exist. Published first detailed atomic theory in All matter is composed of extremely small particles called atoms. 2. Atoms of a given element are identical in size, mass, and other properties; Atoms of different elements differ in size, mass, and other properties. 3. Atoms cannot be subdivided, created, or destroyed. 4. Atoms of different elements combine in simple whole-number ratios to form chemical compounds. 5. In chemical reactions, atoms are combined, separated, or rearranged. (Atoms are not created or destroyed) 1
2 Law of conservation of mass Mass is neither created or destroyed during ordinary chemical reactions or physical changes. Law of Definite Proportions The fact the a chemical compound contains the same elements in exactly the same proportions by mass regardless of the size of the sample or source of the compound. Law of Multiple Proportions If two or more different compounds are composed of the same two elements, then the ratio of the masses of the second element combine with a certain mass of the first element is always a ratio of small whole numbers. In a chemical reaction: Reactants Products The mass of the reactants before a chemical equation is always equal to the mass of the products after a chemical reaction. CaCl 2 + Na 2 SO 4 CaSO 4 + NaCl So the mass of all the reactants must equal the mass of all the products. H 2 O 2
3 English Physicist 1897 Used a cathode ray tube to discover the electron. Proposed atoms were spheres covered in electrons. Revealed that electrons had a very large charge relative to its mass. Deflected towards positive plate = negative charge. Called the plum pudding model. American Chemist Published paper in 1913 after determining the mass and charge of an electron. Important to prove that electrons were ~2000 less mass then Protons. But the charge was opposite but as strong as protons. Atomic sized droplets of oil were attracted to a negative charge. British Physicist Discovered atomic nucleus in Discovered Proton in Gold foil experiment 3
4 Lead block Uranium Fluorescent Screen Gold Foil What he expected Because He thought the mass was evenly distributed in the atom Since he thought the mass was evenly distributed in the atom 4
5 What he got + Atom is mostly empty. Small dense, positive piece at center. Alpha particles are deflected by it if they get close to the nucleus. How he explained it + Volume of nucleus is very small compared to the total volume of the atom. If an atom was the size of a football field, the nucleus would be the size of a marble. Nucleus is positive because it repelled positive particles. Positive nucleus and mostly empty space 5
6 Danish physicist Hypothesized in 1913 that the electrons travel in fixed orbits around the nucleus. Like planets orbiting the sun. Discovered neutron in 1913 Student of Rutherford Accounted for additional mass of nucleus by hypothesizing about neutrons in nucleus. Additional mass with no charge. French scientist 1924 Hypothesized that electrons do not follow orbits (Bohr) but move randomly in energy levels. 6
7 German Scientist Heisenberg Uncertainty Principle. You can know where an electron is or how fast it is moving, but you can t know both simultaneously. Democritus Called them atmos. (400 B.C) John Dalton (1808) Published atomic theory. L of Cons. Of Mass Indef. & def. proportions JJ Thompson (1897) Discovered the Electron. Earnest Rutherford Discovered Nucleus (1911) Discovered Proton (1919) Robert Millikan (1913) Mass and Charge of Electron. Niels Bohr (1913) Electrons travel in orbits. James Chadwick (1913) Discovered Neutron Louis debroglie (1924) Electrons travel randomly in energy levels. Werner Heisenberg Heisenberg Uncertainty Principle (1927) 7
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