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Exploring Bohr Atom Energy Levels & Electromagnetic Spectrum

Learn about Bohr atom, energy calculations, electron orbits, absorption vs. emission, electromagnetic spectrum properties, wave energy calculations, and frequency-wave relationship through interactive practice and video review.

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Exploring Bohr Atom Energy Levels & Electromagnetic Spectrum

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  1. The Bohr Atom

  2. Essential Question • How can properties of a wave be used in energy calculations?

  3. The Bohr atom • Protons and neutrons are located in the nucleus • Electrons orbit the nucleus • Also called the “Planetary model” because it is similar to the solar system

  4. Energy levels “N” • Electrons occupy differing orbits based on energy levels • Quantized: Can only have certain energy levels • As you move away from the nucleus, levels increase in energy • Number per level=2n2

  5. Lets practice • Nitrogen: • How many electrons? • How many in the first energy level? • How many in the second energy level? • Draw the picture

  6. You try • Calcium (Ca): • How many total electrons? • How many in the first energy level? • How many in the second energy level? • Third? • Draw the picture

  7. Try these! • Phosphorus: • Carbon: • Nitrogen:

  8. How are nitrogen and carbon similar? How are they different? • How are nitrogen and phosphorus similar? How are they different?

  9. Diagram of Absorption vs. Emission

  10. Absorption vs. Emission • Absorption • If energy is added, electrons can become excited and jump to higher energy levels. • They can move multiple energy levels • Emission: • Electrons are not stable in their excited state • Want to emit energy to return to their original state • Do this by emitting a photon (packet of light). • The color given off depends how many energy levels the electrons fall.

  11. When electrons absorb or emit energy, they act as a wave

  12. Electromagnetic Spectrum

  13. Essential Question • How can the properties of waves be used in energy calculations?

  14. What do you already know about the electromagnetic spectrum?? • Based on the video, write down something you already know about the electromagnetic spectrum. We will turn and talk, then do a whip around. • https://www.youtube.com/watch?v=P_PVz8HrrCI

  15. Video • In the video, write down something about each type of radiation. http://www.youtube.com/watch?v=P_PVz8HrrCI • Gamma • X-rays • UV • visible • Infrared • Microwaves • Radio

  16. Visible Light Spectrum

  17. FREQUENCY, WAVELENGTH, ENERGY Frequency Relationship

  18. How to convert between the two • C= λ · ν • c= speed of light (3.00 x 108 m/s) • λ = wavelength (m) • ν = frequency (Hertz: Hz) • 1.0 nm = 1 x 10-9 m • Let’s Practice! C ν λ

  19. Why is this important • Allows us to calculate the amount of energy released. • h= Planck’s Constant (6.63 x 10-34 J · s)

  20. REVIEW OF EQ: How can the properties of waves be used in energy calculations? • Without looking, put the following in order from longest wavelength, to shortest wavelength. • X-ray Microwave Radio Wave • Infrared Visible Gamma • Circle the one with the highest frequency? • Put a smiley face over the one with the most amount of energy

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