1. Day 5 12-9 2. High frequency = _____ energy and ______ wavelength High Short

2. h a

3. 1. Amplitude affects __________. 2. Shorter wavelengths = ______ frequencies higher brightness Quantum Theory

4. What did scientists observe that led them to view light as quantized? Quantum Theory

5. How is energy related to frequency? Frequency to wavelength? And so energy to wavelength? Quantum Theory

6. 2. Who demonstrated photons can move electrons? Compton AHHHH!

7. TODAY - Planck’s term quantum and Einstein’s term photon are used interchangeably. …Scientists also believe that light has properties of both waves and particles. Quantum Theory … - Dual nature of light Periods 3 & 6

8. The relationship between frequency , wavelength ( ), and color to the energy of light:  , Color: red = low E, violet = high E E  : many photon punches E  : big gaps between consecutive photons.

9. Color: red = low E, violet = high E each color has its own energy color = type of light

10. The Effects of Different Photons: Microwaves: can’t feel Infrared: feel with skin, warms or burns. Visible light: see with eyes, heats when absorbed. Ultraviolet: can’t feel or see, affects cells – freckles, tan, burn, cataracts.

11. X-rays: can’t feel or see, pass through body, but absorbed by bones and dense matter. Gamma rays: can’t see or feel, affects cells, causes mutations in cells and molecules. The Effects of Different Photons: Ultraviolet: can’t feel or see, affects cells – freckles, tan, burn, cataracts.

12. Day 6 12-12 2. Low energy = _____ fequency and ______ wavelength Low Long

13. h a

14. 1. Amplitude affects __________. 2. Shorter wavelengths = ______ frequencies higher brightness Quantum Theory

15. Radiant Energy = The dual nature of light? Sun or electromagnetic radiation Light can act as a particle OR a wave

16. Quick Talk Radiant energy Wavelength Compton Quantized Bohr Electron Light Dual nature Proton Amplitude Electromagnetic radiation

17. Neils Bohr (bright) line spectrumH Tried to explain why each element has its own unique (bright) line spectrum. He studied H. specific energy levels orbitshell nucleus Using previous discoveries- Bohr hypothesized that an atom’s electrons are located in specific energy levels. Each energy level, aka orbit or shell is a set distance from the atom’s nucleus. …

18. jumpfall energy between … Electrons jump or fall from one energy level to another, while simultaneously gaining or losing energy. Electrons are not permitted to stop between energy levels. Neils Bohr orbitshell nucleus … Each energy level, aka orbit or shell. Is a set distance from the atom’s nucleus. …

19. Bohr’s Hypothesis In the line spectrum of an atom, Bohr saw specific colors.In the line spectrum of an atom, Bohr saw specific colors. Each specific color has a specific energy.Each specific color has a specific energy. That specific amount of energy is related to a specific distance from the nucleus.That specific amount of energy is related to a specific distance from the nucleus.

20. Review section 5.3 AND complete #s 19, 20, 22, and 23 on page 148