Chemistry Sheds Light on Our Lives Unit 4 Atoms and Light

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Presentation transcript:

Chemistry Sheds Light on Our Lives Unit 4 Atoms and Light Glow in the Dark Chemistry Sheds Light on Our Lives Unit 4 Atoms and Light

Glow in the Dark 4.1 Development of Atomic Theory 4.2 Atomic Structure 4.3 Electron Structure 4.4 Periodic Table 4.5 Periodicity 4.6 Light 4.7 Light and Matter

4.1 & 4.2 Atomic Theory and Atomic Structure Objectives Determine the location, charge, and relative mass of protons, neutrons, electrons. Use symbols in writing isotope notation. Identify isotopes using mass number and atomic number and determine the number of protons, neutrons and electrons. Differentiate actual atomic mass of an element from the mass number of an isotope Calculate average atomic mass from % abundances of an isotope

Atomic Structure Timeline On Wednesday’s quiz, you will be expected to… 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 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 Billiard Ball Model atom is a uniform, solid sphere

John Dalton Dalton’s Atomic Theory All matter is made of tiny particles “atoms” Atoms cannot be created, divided, destroyed or changed into other types of atoms Atoms of the same element have identical properties Atoms of different elements have different properties Atoms of different elements combine in whole-number ratios to form compounds Chemical changes join, separate or rearrange atoms in compounds

Henri Becquerel (1896)‏ Discovered radioactivity Three types: 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

Cathode Ray Tubes A cathode ray is a ray of light traveling in a vacuum (no other particles inside) The ray travels from one metal plate to another as the plates are connected to electricity Cathode ray Metal plate (cathode) releases stream Metal plate (anode) to which stream travels

Cathode Ray Tubes & Charge In the late 1800’s, JJ Thomson put charged plates outside the tube Negatively charged plate - + Ray is deflected away from negative plate and towards positive plate Positively charged plate It made no difference what type of metal he used in the tube—all material produced this stream that curved towards the positive charge

J. J. Thomson (1903)‏ Plum-pudding Model Chocolate Cookie Model positive sphere (pudding) with negative electrons (plums) dispersed throughout Chocolate Cookie Model Dough is positive area and chips are negative electrons

Robert Millikan (1909) Discovered the charge of an electron Balanced the downward gravitational force and the upward electrical and buoyant forces of charged oil droplets suspended between two metal plates. Discovered the charge of an electron

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

Ernest Rutherford (1911)‏

Ernest Rutherford (1911)‏ Nuclear Model dense, positive nucleus Mainly empty space filled with electrons

Niels Bohr (1913)‏ Bright-Line Spectrum Energy Levels Planetary Model tried to explain presence of specific colors in hydrogen’s spectrum Energy Levels He stated that 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 areas Electron cloud model orbital: region around the nucleus where e- are likely to be found

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

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

Make a chart like the one below and fill it in to help you study for your quiz. Scientist Experiment Discoveries New model described New model drawing Dalton (1809) Other’s data 6 postulates (two were later proven incorrect) Billiard Ball Model Thomson (1903) Millikan (1909) Rutherford (1911) Bohr (1913) Bright-Line Spectrum Schrödinger (1926) N/A Chadwick (1932)