learnbin.net nav logo

More results...

Generic selectors
Exact matches only
Search in title
Search in content
Post Type Selectors

Spectroscopy and Spectrometry

What is spectroscopy?

Simply, spectroscopy explains the interaction between electromagnetic radiation (Ultraviolet, visible light, infrared and etc.) and matter.

Spectroscopy is the studying of the interactions between matter and electromagnetic radiation and studying of absorbance characteristics and behavior of matter when matter interacted with electromagnetic radiation. In spectroscopic methods, samples (molecules/ matter) are exposed to a beam of electromagnetic radiation to obtain a spectrum.   

Electromagnetic wave
Figure 01: Electromagnetic wave

Spectroscopic methods can be used to identify molecules, their active groups, their structures, arrangements of the active groups, etc.

Common spectroscopic methods

  1. UV – Visible spectroscopy
  2. IR spectroscopy
  3. Raman spectroscopy
  4. Fluorescence spectroscopy
  5. Atomic absorption and emission spectroscopy
  6. Nuclear magnetic resonance spectroscopy (NMR spectroscopy)
    • Photon NMR (H-NMR)
    • Carbon NMR (13C NMR)

The concepts and principles of these spectroscopic methods will be discussed more deeply in separate articles.

Types of spectroscopy

Considering the kind of method used to get the spectrum, spectroscopy can be categorized into three types.

01. Absorption spectroscopy

In absorption spectroscopic methods, the amount of radiation that was absorbed by the sample was used to determine the spectrum. For this, the instrument measures the intensity of the EM radiation before and after it interacted with the sample. Using this amount of absorption can be calculated.

Examples of absorption spectroscopic methods

  • Infrared spectroscopy
  • NMR spectroscopy (Photon NMR, Carbon NMR)
  • UV visible spectroscopy
  • Atomic absorption spectroscopy (AAS)

02. Emission spectroscopy

Emission spectroscopic methods use electromagnetic radiations that were emitted by the sample to obtain the spectrum.

Examples of emission spectroscopic methods

  • Atomic emission spectroscopy (AES)
  • Fluorescence spectroscopy                     

03. Scattering spectroscopy

When EM radiation passthrough molecules, a fraction of EM radiation scatter in a different direction due to vibrations of the molecules. This scattered EM beam has a different wavelength than the incident beam. This difference in wavelength depends on the structure of the molecule.       

Examples of scattering spectroscopic methods

  • Raman spectroscopy 

What is spectrometry?

Determination of the nature of a material (molecule, substance, compound) using a quantitative measurement of an observable property like the amount of emitted light, the rate/ speed of the ions that move through a channel or medium, mass-to-charge ratio, can be identified as spectrometry.

Most of the time molecules are bombarded with high-energy electron (electric) beams to break them into ions. So high-energy electron beam is used to get the spectrum in spectrometric methods instead of electromagnetic radiation like in spectroscopic methods.

 Examples for spectrometry

  • Mass spectrometry

Difference between spectroscopy and spectrometry

Spectroscopic methods use electromagnetic radiation to obtain a spectrum from a sample while spectrometric methods use energy sources like high-energy electric beams to obtain a spectrum from a sample. This is a key difference between spectroscopy and spectrometry.

Also, spectroscopy is a non-destructive method that means the radiation (energy) source won’t destroy (affect) the sample. But spectrometry is a destructive method because it involves breaking samples/molecules into ions/ fragments using high energy sources.

What happens when a molecule has interacted with electromagnetic radiation?

Different ranges of EM radiations interacted differently with the same molecule. So, the different wavelengths of EM radiations show different interactions in the molecules. That is because EM radiations that have high wavelengths, give low energy to a molecule. Also, EM radiations have lower wavelengths, giving higher energy to a molecule. That is why molecules show different behavior when they are subjected to different wavelengths of EM radiation.

Electromagnetic Spectrum
Figure 02: Electromagnetic Spectrum

E = hC/λ

E = energy

h = plank’s constant

C = Speed of light (Speed of electromagnetic radiation)

λ = Wavelength

It can be seen that energy is inversely proportional to the wavelength of radiation.  

When electromagnetic radiation provides energy to a molecule (hits a molecule), the molecule has the ability to

  1. Reflect
  2. Absorb and emit
  3. Transmit those radiations.

When electrons present in a molecule or an atom absorbs energy from electromagnetic radiations, electrons are excited to the excited state (high energy) from the ground state (low energy).

Jablonski diagram
Figure 03: Jablonski diagram

After that, those excited electrons have emitted that energy as electromagnetic radiation and fall back to the ground state.                  

When the above phenomenon happens because molecules interacted with electromagnetic radiation, that will cause some changes in the molecules. Some of those changes are causing rotational and vibrational motions in the molecules, causing lamination, and breaking bonds in the molecules.

For example, microwaves cause rotation in molecules. IR radiation cause vibrational motions in molecules. Visible light and UV could cause luminance and fluorescence in molecules. Also, UV radiation and X-ray could cause breaking bonds due to high energy.

This table shows different kinds of interactions that can be observed when molecules/ atoms are subjected to different EM radiation wavelengths.

Type of EM radiationType of spectroscopyWavelength rangeType of quantum transition
Gamma radiationGamma-ray emissionLess than 0.01nm (1*10-11m)Nuclear level transition
X-rayX-ray emission, absorption, diffraction fluorescence0.01nm - 10nm (1*10-11m - 10*10-9m)Inner electrons
Ultraviolet radiationVacuum UV absorption10nm – 180nm (1*10-8m – 18*10-8m)Bonding electrons
Visible light and Ultraviolet radiationUV- Visible absorption and emission spectroscopy180nm – 780nm (18*10-8m – 78*10-8m)Bonding electrons
Infrared radiationInfrared spectroscopy780nm - 300µm (7.8*10-7m – 3*10-4m)Rotational and transitional energy levels
 Raman spectroscopy Rotational and transitional energy levels
MicrowavesMicrowave absorption0.75mm – 3.75mm (7.5*10-4m – 3.75*10-3m)Rotation of the molecules
Radio wavesElectron spin resonance (ESR)3cm (3*10-2m)Spin of electrons
 Nuclear magnetic resonance (NMR)0.6m – 10mSpin of nuclei

Buy me a coffee

References and Attributes

Khan Academy - Spectroscopy
Hollas, J., 2004. Modern spectroscopy. New York: J. Wiley.
Pavia, D., 2015. Introduction to spectroscopy. Stamford


The cover image was created using Image by OpenClipart-Vectors from Pixabay
Figure 01: DECHAMMAKL, CC BY-SA 4.0, via Wikimedia Commons
Figure 02: Philip Ronan, Gringer, CC BY-SA 3.0, via Wikimedia Commons

Express your thoughts below!

Leave a Reply

Your email address will not be published. Required fields are marked *

One Comment

© 2024 learnbin.net. All rights reserved.
linkedin facebook pinterest youtube rss twitter instagram facebook-blank rss-blank linkedin-blank pinterest youtube twitter instagram