## Energy Levels and Color of light

$c=\lambda v$

Nikki Razal 1L
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### Energy Levels and Color of light

just to clarify, what is the relationship between the color of light emitted and the energy level an electron jumps to?

RobertXu_2J
Posts: 104
Joined: Fri Aug 30, 2019 12:17 am

### Re: Energy Levels and Color of light

Color of light is decided by the wavelength of the light. If the electron loses energy and releases that energy as a photon, the wavelength of the photon decides the color of the light i think.

AprilPaz
Posts: 51
Joined: Wed Sep 18, 2019 12:18 am

### Re: Energy Levels and Color of light

When light is emitted, an electron goes from high orbit to low orbit and the electron is absorbed when going from low orbit to high orbit. The difference of energy between two orbitals determines the energy and frequency of light emitted. Thus, different frequencies equate to different wavelengths, which in turn means different colors of light are produced.

Sydney Pell 2E
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Joined: Wed Sep 11, 2019 12:17 am

### Re: Energy Levels and Color of light

It depends on which levels the electron is jumping to and from. This will determine the amount of excess energy which will then determine the wavelength of light emitted. The color of the light depends on its wavelength.

Sometimes, the light emitted will not be in the visible spectrum and so it will not have color. If more energy is released, the electromagnetic radiation emitted will be in the ultraviolet spectrum, while if less energy is released, it will be in the infrared category.

DLee_1L
Posts: 103
Joined: Sat Aug 17, 2019 12:17 am

### Re: Energy Levels and Color of light

Also, the electron must be jumping from an energy level of n=>3 to n=2 to emit any visible light. The higher the initial energy level, the shorter the wavelength with the shortest being purple and longest being red.