Explore blog

The relationship between energy, wavelength and frequency of light is indirectly related. The higher the wavelength range, the lower the frequency and the lower the energy. This description fits with the color red. The wavelength is long, with a lot of space in between the crests and troughs. The photon energy is low, it ranges from 269 to 318 Joules. Light emission demonstrates electron transition by releasing the color the energy change corresponds to. If an electron moves from a high energy state to a lower energy state, it will likely give off a higher frequency color, like violet or blue, given the amount of energy it is releasing to move that electron closer to the nucleus.  Say an electron moved from energy level 6 to energy level 2. Since it would lose alot of energy because it moved much closer to the nucleus, it would give off a high frequency with a high photon energy, such as violet, which has a short wavelength of 380 to 440 nm. Say it was the other way around, and the electron was moving from a lower, or ground, state, to a higher, or excited, state. The electron would absorb the color light corresponding to its wavelength because the electron has to gain energy to overcome the forces of attraction with the protons in the nucleus. Light can be used to measure the electron transition of electrons simply by observing the color given off and relating it to its wavelength, frequency and energy.

 

sources: http://en.wikipedia.org/wiki/Light