1. Light and Energy Chemistry I

2. Classical description of light Light is an electromagnetic wave. Light consists of elementary particles called photons. A photon is a little packet of energy which can carry electromagnetic radiation.

3. Wave Nature of Light Electromagnetic (EM) Spectrum: (page 120 in textbook) list of all forms of radiation. Radiation is a form of energy that exhibits wavelike behavior as it travels through space.

4. Light as a Wave Wavelength (λ) Frequency (v) Amplitude All light travels at the same speed (3 x 10 8 m/s, symbol = c) Frequency and wavelength are inversely proportional C = ( λ )(v)

5. Visible Light Visible light is a very small part of the EM spectrum and can be separated into a continuous spectrum we call a rainbow. Red light has the lowest frequency and least energy. Violet light has the highest frequency and most amount of energy.

6. Spectral Lines make up a bright line spectrum Spectral lines are produced by colored light passing through a prism. The prism breaks down the colored light into specific colors that make up the colored light we see.

7. Electromagnetic Spectrum

8. Type of WaveWavelength Radio Waves1 m – 1 km Microwaves1 cm Infra-red0.01 mm Visible400-700 nm Ultraviolet100 nm X-Ray1 nm Gamma Ray0.01 nm

9. Electromagnetic Spectrum RabbitsRadio MeetMicrowave InInInfra-red VeryVisible UnusualUltraviolet eXpensiveX-Rays GardensGamma

10. Calculations Find the wavelength of blue light if its frequency is known to be 6.4 x 10 14 /s? (any number per second is also a unit of frequency). The answer is 4.7 x 10 -7 m Substitute into your equation: 3.0 x 10 8 m/s = * 6.4 x 10 14 /s

11. Light as a Particle The energy of a photon can also be calculated. E=hv says that the energy of a photon is related to its’ frequency. h is Planck’s constant (named for Max Planck) h = 6.626 x 10 -34 Js

12. Light as a Particle c=λν speed of light = wavelength times frequency E=hv energy = Planck’s constant times frequency E=hc/λ We can combine the two equations as well to find the energy, if only the wavelength is known.

13. Calculations

14. What is the energy of x- radiation with a 1 x 10 -6 m wavelength? E=hvand c=λvso E=hc/λ E=(6.626 x 10 -34 Js)(3x10 8 m/s)/(1x10 -6 m) E=1.99 x 10 -19 J

15. Electrons move between levels of energy When an atom aborbs heat or electricity, its electrons move to a higher level of energy. This is called the excited state. The original level of energy is called the ground state.

16. Excited state electron = unstable electron Electrons in an excited state are unstable and quickly fall back to ground state. This causes a release of energy in the form of light. The color of light emitted depends upon the falling distance of the electron. If the falling distance was large, much energy is released.

17. Falling distance is related to energy released If the falling distance is small, then little energy is released.

18. Questions 1. What is the difference between continuous and bright line spectrum? How are each produced? 2. What lead to the development of the Bohr model? 3. What are spectral lines?

19. Questions 4. What is the relationship between frequency and wavelength? 5. What is the difference between ground and excited state electrons? 6. How is light produced? 7. Why is light of different color? 8. What color is high frequency light? Low frequency?

20. Questions