Hydrogen spectrum

Introduction

As you may be aware that electrons in an atom or a molecule consume energy, get excited and jump to a higher energy level from a lower energy level, and then emit radiation when they return to their initial states. This phenomenon accounts for the emission spectrum through hydrogen as well, known as the hydrogen emission spectrum. Excited state: When an atom absorbs some amount of a quantum of energy, it is said to be in an excited state relative to its ground state. After that, when an atom in an excited state returns to the ground state, it emits light. For example, the red light of neon signs is due to neon atoms which have been first sent to an excited state by an electrical discharge. When light from excited atoms is viewed by a spectroscope, images of the slit can be clearly seen along the scale of the instrument as a series of colored lines. The definite wavelengths have a corresponding color, and the series of lines is known as a line spectrum.

Body

As most of the universe is made of hydrogen, the spectrum of hydrogen is particularly important in astronomy. The process of absorption in hydrogen gives rise to the series, which are sequences of lines corresponding to atomic transitions, each ending or beginning with the same atomic state in hydrogen. Thus, for example, the Lyman series involves transitions starting (for absorption) or ending (for emission) with the first excited state of hydrogen, while the Lyman series involves transitions that start or end from the ground state of the hydrogen atom.

Hydrogen spectrum wavelength

As we studied earlier when any hydrogen atom absorbs a photon, it causes the electron to experience some transition to a higher energy level, for example, n = 1,  n = 2. When a photon is emitted from a hydrogen atom, the electron undergoes a transition from a higher energy level to a lower one, for example, n = 3, n = 2. During the transition from a higher energy level to a lower energy level, the transmission of light occurs. The spectrum is caused by the quantized energy levels of the atoms, to comprise wavelengths that reflect the differences in these energy levels. For example, the line at 486 nm corresponds to the transition, n = 4  n = 2. Wave number  v can be find out by following formula v = RH(1/n₁² – 1/n₂² ) Here RH is Rydberg constant n₁  and n₂ are principle quantum number of two energy levels.

Lyman series:

This series was discovered by Theodore Lyman. This series is a hydrogen spectral series of transitions, resulting in the wavelengths in the ultraviolet region and emission lines of the hydrogen atom as an electron goes from n ≥ 2 to n = 1, where n represents the quantum number. The transitions are named on the basis of Greek letters: Lyman-alpha is called when transition takes from  n = 2 to n = 1 Lyman-beta,  n = 3 to n = 1 Lyman-gamma, n = 4 to n = 1 RH(1/1² – 1/n₂² ).

Balmer series

The Balmer series is a series of spectral emission lines of hydrogen that result from electron transitions from higher energy levels down to the energy level with principal quantum number 2. Out of all the transitions, there are four transitions that are visible in the optical waveband, which are empirically given by the Balmer formula: RH(1/2² – 1/n₂² ).

Paschen series

When an electron jumps from any higher orbit, i.e., if n₁= 3 and n₂= 4,5,6…, the series obtained is called the Paschen series. Discovered by German physicist Friedrich Paschen in 1908, all the Paschen lines lie in the infrared region. This series of lines overlaps with the lines of the Brackett series, i.e., the shortest line of the Brackett series has a wavelength that is equal to that of the Paschen series. Most of the subsequent series overlap. It is given by: RH(1/3² – 1/n₂² ). It lies in the infrared region.

Brackett series

When an electron jumps from any higher orbit to the fourth orbit, i.e., n₁= 4 and n₂= 5,6,7, the series obtained is called the Brackett series. Named after the American physicist Frederick Sumner Brackett who first observed the spectral lines in 1922, the spectral lines of the Brackett series lie in the far-infrared band. It is given by: RH(1/4² – 1/n₂² ). It lies in the infrared series.

Pfund  series

When an electron jumps from any higher orbit to the fifth orbit, i.e., n₁= 5 and n₂= 6,7,8, the series thus obtained is called the Pfund series. Experimentally discovered in 1924 by August Herman Pfund, it is given by: RH(1/5² – 1/n₂² ). It lies in the infrared region.

Conclusion

The explanation of the hydrogen spectrum prepared by Niels Bohr was a brilliant achievement for modern quantum theory. It greatly stimulated progress. Bohr was awarded the Nobel Prize in 1992 for excellent work in Physics. Following are the wavelength equations for different series:

• For Lyman series : RH(1/1² – 1/n₂² ).
• For Balmer series : RH(1/2² – 1/n₂² ).
• For  Paschen series : RH(1/3² – 1/n₂² )
• For Brackett series : RH(1/4² – 1/n₂² )
• For  Pfund series : RH(1/5² – 1/n₂² )