Atomic Structure Timeline Read Around the Room. Democritus (400 B.C.) Proposed that matter was composed of tiny indivisible particles Not based on experimental.

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Presentation transcript:

Atomic Structure Timeline Read Around the Room

Democritus (400 B.C.) Proposed that matter was composed of tiny indivisible particles Not based on experimental data Greek: atomos

Alchemy (next 2000 years) Mixture of science and mysticism. Lab procedures were developed, but alchemists did not perform controlled experiments like true scientists.

John Dalton (1807) British Schoolteacher – based his theory on others’ experimental data Ball Model – atom is a tiny, uniform, solid sphere

John Dalton Dalton’s Four Postulates 1.Elements are composed of small indivisible particles called atoms. 2.Atoms of the same element are identical. Atoms of different elements are different. 3.Atoms of different elements combine together in simple proportions to create a compound. 4.In a chemical reaction, atoms are rearranged, but not changed.

Henri Becquerel (1896) Discovered radioactivity – spontaneous emission of radiation from the nucleus Three types: – alpha (  ) - positive – beta (  ) - negative – gamma (  ) - neutral

J. J. Thomson (1903) Cathode Ray Tube Experiments – beam of negative particles Discovered Electrons – negative particles within the atom Plum-pudding Model

J. J. Thomson (1903) Plum-pudding Model – positive sphere (pudding) with negative electrons (plums) dispersed throughout

Ernest Rutherford (1911) Gold Foil Experiment Discovered the nucleus – dense, positive charge in the center of the atom Nuclear Model

Rutherford’s Apparatus beam of alpha particles radioactive substance gold foil circular ZnS - coated fluorescent screen Dorin, Demmin, Gabel, Chemistry The Study of Matter, 3 rd Edition, 1990, page 120 Rutherford received the 1908 Nobel Prize in Chemistry for his pioneering work in nuclear chemistry.1908 Nobel Prize in Chemistry

Ernest Rutherford (1911) Nuclear Model – dense, positive nucleus surrounded by negative electrons

Niels Bohr (1913) Bright-Line Spectrum – tried to explain presence of specific colors in hydrogen’s spectrum Energy Levels – electrons can only exist in specific energy states Planetary Model

Niels Bohr (1913) Planetary Model – electrons move in circular orbits within specific energy levels Bright-line spectrum

Erwin Schrödinger (1926) Quantum mechanics – electrons can only exist in specified energy states Electron cloud model – orbital: region around the nucleus where e - are likely to be found

Erwin Schrödinger (1926) Electron Cloud Model (orbital) dots represent probability of finding an e - not actual electrons

James Chadwick (1932) Discovered neutrons – neutral particles in the nucleus of an atom Joliot-Curie Experiments – based his theory on their experimental evidence

James Chadwick (1932) Neutron Model revision of Rutherford’s Nuclear Model