Atomic Structure Timeline Use the following information to complete the lecture handout. On your Atomic Structure Timeline quiz, you will be expected to… draw the atomic models match scientists to their experiments and discoveries place the models in chronological order

Democritus (400 B.C.) Proposed that matter was composed of tiny indivisible particles called atoms 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 Billiard Ball Model based his theory on others’ experimental data Scientists used the way elements form compounds Billiard Ball Model atom is a 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.

J. J. Thomson (1904) Cathode Ray Tube Experiments Discovered Electrons beam of negative particles Discovered Electrons negative particles within the atom Plum-pudding Model

J. J. Thomson (1903) Plum-pudding Model Using the cathode ray tube experiment, he used a beam to discover negative particles: electrons. 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 Contained two parts: the nucleus in the center which is surrounded by electrons on the outside. Nuclear Model

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

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

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

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

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

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