1. Light’s Wave Nature

2. Wave Nature of Light
Electromagnetic radiation is a form of energy that exhibits wavelike behavior as it travels through space.
Examples: sunlight, microwaves, x-rays radio and television waves

3. Characteristics of Waves
Wavelength (λ – lambda) – the shortest distance between the same points on a wave; usually measure in meters, centimeters, or nanometers
Frequency (f)– the number of waves that pass a given point per second; 1 Hertz equals 1 wave per second (1/s or s-1)
Amplitude is a waves height from origin to crest

4. Speed of Light
All electromagnetic waves travel at the speed of light in a vacuum and this value is a very important constant
c = x 108 meters per second (m/s)
The speed of light is related to wavelength and frequency by the following equation:
c = wavelength x frequency or
c = λ f

5. Using the Equation c = λ f
Looking at the equation, you can see that wavelength and frequency are inversely related, so as one increases the other decreases and vice versa.

6. Light and the Visible Spectrum
Sunlight or white light is made up of a continuous range of wavelengths and frequencies.
Passing sunlight through a prism show you all the color of the visible spectrum
When passing through a prism, the short wavelengths bend more than the long ones, resulting in the sequence of colors
ROY G BIV (red, orange, yellow, green, blue, indigo, violet)

7. Electromagnetic Spectrum
Includes all forms of electromagnetic radiation, with the only difference being wavelength and frequency

9. Calculations
Because all electromagnetic radiation travels at the same speed (speed of light), we can use the formula c = λ f to calculate wavelength and frequency any wave. Remember c = speed of light!

11. Quantum? So how does that relate to energy levels in an atom?
A quantum is the minimum amount of energy that can be gained or lost by an atom; so matter can gain or lose energy only in small, specific amounts.
So how does that relate to energy levels in an atom?

12. Ground State vs. Excited State
The ground state of an electron is the lowest energy level possible for that electron. It’s comfortable there. By adding energy, like heat or light, electrons can be exited and move up to a new energy level – they would then be in an “excited state”.
This “excited state” is very uncomfortable for the electron, it wants to be back home in its ground state energy level, so it loses the energy it gained (the quantized amount) and begins to drop back down to its lowest energy level (kind of like stepping down a ladder).
Sometimes the energy it loses can be seen as colors of light because the frequency of the energy is in the “visible light” range.”

13. Photons
A photon is a particle of electromagnetic radiation (like visible light) with no mass that carries a quantum of energy. So basically, it’s a package of electromagnetic radiation with a set amount of energy.
Photons can travel at different wavelengths and frequencies, so we interpret that as different colors of light. (remember, visible light can have different wavelengths and frequencies that we see as different colors!)

14. Bohr’s Model

15. We can use this equation to relate the amount of quantum energy to the actual frequency of the radiation.
E = hf
E is the quantum energy or a photon’s energy, h is Planck’s constant (6.626 x J · s), f is the frequency

16. Practice 1. What is the energy for the following type of radiation?
6.32 x 1020 s-1
2. Use the Electromagnetic Spectrum to determine the type of radiation described in problem #1.