1. Wave & Particle Nature of Light EQ: How can an atom be a "particle" and a "wave" at the same time?

2. Quantum Concept Why do heated objects emit only certain frequencies of light? Temperature of an object is a measure of the average kinetic energy of its particles As an object gets hotter, it possess a greater amount of energy and emits different colors of light Different colors are due to different frequencies and wavelengths

3. Ground vs. Excited States of e - Ground State: Lowest energy e - configuration ◦Shown on Periodic Table ◦Innermost energy level fills first, then work outward Ground State vs. Excited State

4. Excited State: e - can move to a higher energy level without filling the lower energy level first ◦Do this by absorbing energy Excited e - fall back to ground state by releasing energy Ground State vs. Excited State

5. The SVP Universal Cosmology A Rosetta Stone for the New Science Paradigm photon Photon: Massless particle that carries a quantum of engergy.

6. Diagram Elements give off different colors depending on the amount of energy released (how far the e - falls)

7. Neon – Ground vs. Excited State

8. Quantum Concept German physicist Max Planck established that matter gains or loses energy in small amounts called quantum Quantum is the minimum amount of energy that can be gained or lost by an atom. Planck’s mathematical equation for his findings is E quantum = hv

9. Quantum Concept E photon = hv E quantum = Energy h = Planck’s constant (6.626 x 10 -34 J s) v = Frequency *Note: Joule (J) is the unit of energy

10. We also need to know……… c = λv c = Speed of light (3.00 x 10 8 m/s) λ = Wavelength (shortest distance between equivalent points on a wave) ν = Frequency (# of waves that pass a given point per second)

11. We also need to know………

13. E photon = hv What can we determine from these equations? As energy of a photon increases, the frequency increases and the wavelength decreases c = λv v= c / λ

14. Example: A photon is emitted from an atom with an energy of 5.10 x 10 -20 J. What is the wavelength of the photon using correct significant figures? E photon = hv c = λv v = E photon / h v = 5.10 x 10 -20 J / 6.626 x 10 -34 J s v = 7.69695 x 10 13 s -1 λ = c / v λ = 3.00 x 10 8 m/s / 7.69695 x 10 13 s -1 λ = 3.89764 x 10 -6 m = 3.90 x 10 -6 m

15. Solve & use correct number of sig. figs. (Rally Coach) 1. Ultraviolet radiation has a frequency of 6.8 × 10 15 s -1. Calculate the energy, in joules, of the photon. 2. Find the energy, in joules, of microwave radiation with a frequency of 7.91 × 10 10 s -1. 3. A sodium vapor lamp emits light photons with a wavelength of 5.89 × 10 -7 m. What is the energy of these photons? 4. One of the electron transitions in a hydrogen atom produces infrared light with a wavelength of 7.464 × 10 -6 m. What amount of energy causes this transition? 4.5 x 10 -18 J 5.24 x 10 -23 J 3.37 x 10 -19 J 2.663 x 10 -20 J

16. Solve & use correct number of sig. figs. 1.Find the energy in kJ for an x-ray photon with a frequency of 2.4 × 10 18 s -1. (1 kJ = 1000 J) 2. A ruby laser produces red light that has a wavelength of 500 nm. Calculate its energy in joules. (1m = 1 000 000 000 nm) 3. What is the frequency of UV light that has an energy of 2.39 × 10 -18 J? 4. What is the wavelength and frequency of photons with an energy of 1.4 × 10 -21 J?

17. E photon = hvc = λv E quantum = Energy h = Planck’s constant (6.626 x 10 -34 J s) v = Frequency *Note: Joule (J) is the unit of energy c = Speed of light (3.00 x 10 8 m/s) λ = Wavelength ν = Frequency