# Why does electromagnetic radiation in the ultraviolet region represent a larger energy transition than does radiation in the infrared region?

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Jun 20, 2016

The energy associated to a photon is given by the equation

$E = h \setminus \nu$

where $E$ is the energy, $h$ is the Planck's constant and $\setminus \nu$ is the frequency of the photon.

The electromagnetic radiation is composed by photons at a certain frequency. The ultraviolet radiation has a frequency that can range from $800$ till $30000$ THz.
The infrared radiation has a frequency that can range from $0.3$ till $430$ THz.

Then, because the Energy is proportional to the frequency, the infrared light has an energy that is lower than the ultraviolet radiation.

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