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Electromagnetic Spectrum

Electromagnetic Radiation Spectrum Diagram

Electromagnetic spectrum radiation diagram and entire distribution chart represent the number of radiation spectra (frequency and wavelength) formed by the electrical field and magnetic field in quantum physics or chemistry. Each type of electromagnetic emission spectrum radiation like radio waves, ultraviolet (UV), infrared (IR), and visible rays travel at the speed of light in a vacuum with a wide range of frequencies, wavelengths, and photon energies. Electromagnetic rays (Quanta or photon ) in science can describe the two characteristics of radiation spectra, particle properties (mass, momentum, and velocity) and wave properties (energy, frequency, and wavelength) of the light spectrum. The various portions in the electromagnetic spectrum chart contain different types of names according to behavior and applications of radiation spectra like emission, transmission, absorption.

Wavelengths of the Electromagnetic Spectrum

The shortest and longest wavelength of the electromagnetic spectrum radiation diagram define the distance between two consecutive series of lines and express in si units like meters, millimeters, micrometers, or nanometers.

Electromagnetic Waves Ultraviolet, Visible and IR Radiation Spectrum Frequency Wavelength Diagram

In addition to the wavelength scale, the frequency scale also uses to derive the electromagnetic spectrum for learning chemistry and physics. The frequency of the spectrum is defined as the number of complete cycles per second (cps), also name as Hertz according to the name of German physicist H.R Hertz.

Wavelength Frequency and Energy

The definition of wavelength and frequency in the electromagnetic spectrum suggest that the wavelength are inversely proportional to frequency, or ν ∝ 1/λ; or, ν = c/λ, where c = velocity of light = 3 × 1010 cm sec-1. de Broglie wavelength relation provides a common equation between the frequency wavelength and electromagnetic energy in spectroscopy. Therefore, energy (E) = hν = hc/λ, where h = Plank constant. According to the de Broglie facts, when the frequency of the bands is very high or the wavelength of the bands is very short, the electromagnetic energy of the emission spectrum is also very high. For example, x- rays are more energetic than visible light in science.

Electromagnetic Spectrum Chart

The classification chart of the electromagnetic radiation flows from cosmic rays to the microwave regions but the visible spectrum flows from the wavelength 400 nm to 750 nm or violet to red color. The below table includes different types of electromagnetic region with frequency and wavelength of emission or absorption spectra.

Region Wavelength (λ) Frequency
(ν)
Cosmic rays 5 × 10-5 nm
Gamma rays 10-3 – 15 nm
x-rays 0.01 – 15 nm
Far UV 15 – 200 nm 666,667 to 50,000 cm-1
Near UV 200 – 400 nm 50,000 to 20,000 cm-1
Visible 400 – 800 nm 25,000 to 12,500 cm-1
Near IR 0.8 – 2.5 μ 15,500 to 4000 cm-1
Vibrational IR 2.5 – 25 μ 4,000 to 400 cm-1
Far IR 0.025 – 0.5 nm 400 to 200 cm-1
Microwave 0.05 – 300 nm 200 to 0.033 cm-1

Different types of spectrum examples on the above wavelength or frequency chart show that the visible region of spectra contains very small parts of the entire electromagnetic rays. Therefore, the waves of the visible region slightly higher than IR radiation and slightly lower than the ultraviolet spectrum.

Energy and Wavelength of Spectrum

The energy and wavelength of spectrum radiation are different for different substances (atom or molecules). When the electromagnetic energy of the system does not match, then the light is not absorbed by the substances or atoms. The electromagnetic radiation in science uses widely to explain the most important physical or chemical properties and structure of inorganic and organic compounds or chemical elements present in the periodic table. Therefore, the electromagnetic model in spectroscopy widely uses in the field of science (chemistry, physics, biology, medicine, environmental analysis) in everyday life.

The ultraviolet or visible light brings the electrons from lower atomic energy levels to higher energy to forms the atomic spectrum with a definite frequency and wavelength. In Infrared (IR) spectroscopy, the vibrational movements of the molecules change to form vibrational excitation among the molecules. In science, the microwave spectroscopy changes the rotational movement of the chemical bond in the molecule to form NMR-spectrum in the region of electromagnetic radiation.