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Unit 4: Atomic and Nuclear Structure Electromagnetic Spectrum

Unit 4: Atomic and Nuclear Structure Electromagnetic Spectrum. Unit 4: Atomic and Nuclear Structure Electromagnetic Spectrum. History of Atomic Theory:. 1. Greek philosophers. 2. Daltons Atomic Theory. 3. JJ Thompson and the “plum pudding model”. 4. Rutherford and the gold foil experiment.

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Unit 4: Atomic and Nuclear Structure Electromagnetic Spectrum

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  1. Unit 4: Atomic and Nuclear Structure Electromagnetic Spectrum

  2. Unit 4: Atomic and Nuclear Structure Electromagnetic Spectrum History of Atomic Theory: 1. Greek philosophers 2. Daltons Atomic Theory 3. JJ Thompson and the “plum pudding model” 4. Rutherford and the gold foil experiment 5. Niels Bohr and the planetary model 6. Quantum mechanical model - later

  3. Unit 4: Atomic and Nuclear Structure Electromagnetic Spectrum Electromagnetic Radiation: All forms of radiation can be described in terms of an oscillating electrical and magnetic field. (waves!) Wavelength and frequency What visible color has highest frequency? Lowest? Microwaves in the US operate at a frequency of 2.45 GHz. What is the wavelength of this radiation? Energy In summation: Low energy waves = ________ frequency and _________ wavelenghts.

  4. Unit 4: Atomic and Nuclear Structure Electromagnetic Spectrum Quantization and Planck’s Equation: Planck found a relationship between energy and the frequency of electromagnetic radiation. Planck’s Equation So what does it mean??? As frequency increases … Only certain energies are allowed; energy is quantized !!!

  5. Unit 4: Atomic and Nuclear Structure Electromagnetic Spectrum ? ? The Photoelectric Effect: When light bombards certain materials, electrons are emitted from the material. Einstein said that light must be made of particles in order to do this!!! The quantized energy values from Planck are describing these particles called … Equation connection

  6. Unit 4: Atomic and Nuclear Structure Electromagnetic Spectrum Applying Planck, Einstein and Light … A CD player emits a red light with a wavelength of 685 nm. How much energy does 1 photon of this light have? For 1 mole of photons? Energy

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