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

Answer 1

The equation provides the energy associated with a photon.

#E=h\nu#

where #E# is the energy, #h# is the Planck's constant and #\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.

Hence, the energy of infrared light is less than that of ultraviolet radiation since energy is proportionate to frequency.

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Answer 2

Piper Hoffman

Compared to radiation in the infrared region, electromagnetic radiation in the ultraviolet region has a higher frequency and a shorter wavelength, which results in larger energy transitions.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.