Atomic Spectra Last Updated : 11 Apr, 2025 Comments Improve Suggest changes Like Article Like Report Atomic Spectra is the spectrum of radiation of electromagnetic waves produced due to the transition of an electron from one energy level to another level within an atom. Atoms have an equal number of negative and positive charges. Atoms were described as spherical clouds of positive charges with embedded electrons in Thomson's concept. In Rutherford's model, one tiny nucleus carries the majority of the atom's mass, as well as its positive charges, and the electrons orbit it.Every element's atoms have their own unique spectra and are stable. The spectrum is made up of line spectrums, which are parallel lines that are isolated. In this article, we will learn atomic spectra, its definition, and more in detail.Table of Content Postulates of Bohr Atomic ModelWhat is Atomic Spectra?Atomic SpectroscopySpectral SeriesPostulates of Bohr Atomic ModelThe foundations of quantum mechanics were laid by Niels Bohr, and they are as follows:The electrons in the hydrogen atom spin around in stable orbits, generating no radiant energy.The angular momentum in stationary orbits is a multiple of the equation h / 2,π and L = n h / 2π, where n is known as the quantum number.The electron changes from a non-radiating orbit to a lower-energy orbit. When this occurs, a photon with the same energy as the difference between the final and beginning states is emitted. hv= Ei Ef is used to calculate frequency (v).What is Atomic Spectra?An electron's spectrum of electromagnetic radiation is released or absorbed as it moves between different energy levels within an atom. When an electron moves from one energy level to the next, it emits or absorbs light of a given wavelength. The atomic spectra of atoms are the collection of all these unique wavelengths of the atom in a certain set of variables such as pressure, temperature, and so on. Emission spectra, absorption spectra, and continuous spectra are the three forms of atomic spectra.The Rydberg formula clearly divides the atomic hydrogen emission spectrum into a number of spectral lines with wavelengths. Atomic transitions between different energy levels cause the observable spectral lines in the hydrogen emission spectrum. In astronomical spectroscopy, spectral series are very important.Atomic SpectroscopyThe study of the electromagnetic radiation received or emitted by atoms is known as atomic spectroscopy. There are three different forms of atomic spectroscopy:The transfer of energy from the ground state to an excited state is the subject of atomic emission spectroscopy. Atomic emission can explain the electronic transition.Atomic absorption spectroscopy: For absorption to occur, the lower and higher energy levels must have equivalent energy differences. The notion that free electrons created in an atomizer can absorb radiation at a given frequency is used in the atomic absorption spectroscopy principle. The absorption of ground-state atoms in the gaseous state is measured.Atomic fluorescence spectroscopy combines atomic emission and atomic absorption since it uses both excitation and de-excitation radiation.Uses of Atomic SpectroscopyIt is used to identify the spectral lines of metallurgical materials.It is utilised in the pharmaceutical industry to detect traces of materials that have been used.It can be used to investigate elements with multiple dimensions.Spectral SeriesA spectral series is a collection of wavelengths arranged in a logical order. Light, or any electromagnetic radiation released by energised atoms, has this property.Because the hydrogen atom is the most basic atomic system found in nature, it produces the most basic series. When a slit allows a beam of light or other radiation to enter the device, each component of the light or radiation forms an image of the source. When resolved under the spectroscope, these images can be seen. The photos will be in the shape of parallel lines with consistent spacing positioned next to each other. When moving from a higher to a lower wavelength side, the lines will be farther apart on the higher wavelength side and eventually closed. The shortest wavelength has the fewest separated spectral lines, which is referred to as the series limit.Line spectrum of the hydrogen atomA hydrogen atom is made up of several line spectrum series, including:Pfund SeriesBrackett SeriesPaschen SeriesBalmer SeriesLyman SeriesSpectral Series FormationBohr's atomic model models and well explains the set of energy levels/states that each atom encloses. Quantum numbers (n=1, 2, 3, 4, 5, 6,.....) are used to name energy states. A photon of energy nh – nl is released when electrons jump from higher energy states (nh) to lower energy ones (nl). Because the energy related to each state is fixed, the difference between them is also fixed, resulting in a transition between similar energy states producing the same energy photon.The electron transition to a lower energy state divides the spectral series into equivalent series. Within the series, the Greek alphabets are utilised to separate the spectral lines of corresponding energy. Hydrogen has the following spectral series:Lyman series (nl=1) The series was discovered by Theodore Lyman between 1906 and 1914. As a result, it bears his name. When electrons transition from higher energy states (nh=2, 3, 4, 5, 6,...) to nl=1 energy states, according to Bohr's model, the Lyman series appears. The Lyman series' wavelengths are all in the Ultraviolet band. For a list of wavelengths related to spectral lines, see the table below:Energy level (n) Wavelength (in nm) in vacuum∞91.175693.78594.974497.2563102.572121.57Balmer series (nl=2) Johann Balmer was the first to discover the series in 1885. As a result, the series is named after him. The Balmer series emerges when electrons go from higher energy levels (nh=3,4,5,6,7,...) to a lower energy state (nl=2). The wavelengths of the Balmer series are all visible in the electromagnetic spectrum (400 nm to 740 nm). The H-Alpha line of the Balmer series, which is also a part of the solar spectrum, is used in astronomy to identify hydrogen. See the table below for a list of wavelengths associated with spectral lines.Energy level (n)Wavelength (in nm) in air∞364.67397.06410.25434.04486.13656.3Paschen series (nl=3) In 1908, a German physicist named Friedrich Paschen was the first to notice the series. As a result, the series is named after him. The Paschen series develops when electrons migrate from higher energy levels (nh=4, 5, 6, 7, 8, ...) to lower energy states (nl=3). All of the wavelengths in the Paschen series are in the infrared portion of the electromagnetic spectrum. The Brackett series, which has the smallest wavelength, overlaps with the Paschen series. This series overlaps with all subsequent ones. See the table below for a list of wavelengths associated with spectral lines.Energy level (n)Wavelength (in nm) in air∞820.48 954.671005610945128241875Brackett series (nl=4) In the year 1922, an American physicist named Friedrich Sumner Brackett spotted the series for the first time. As a result, the series is named after him. The Brackett series develops when electrons move from higher energy levels (nh=5, 6, 7, 8, 9 ...) to lower energy states (nl=4). The wavelengths of the Brackett series are all in the infrared region of the electromagnetic spectrum. See the table below for a list of wavelengths associated with spectral lines.Energy level (n)Wavelength (in nm) in air∞14589181781944721666262554051Pfund series (nl=5) In 1924, August Harman Pfund became aware of the series for the first time. As a result, the series is named after him. The Pfund series emerges when an electron transitions from a higher energy state (nh=6, 7, 8, 9,10, ...) to a lower energy level (nl=5). The wavelengths of the Pfund series are all in the infrared region of the electromagnetic spectrum. See the table below for a list of wavelengths associated with spectral lines.Energy level (n)Wavelength (in nm) in vacuum∞227910303993297837417465467460Humphreys series (nl=6) In 1953, an American physicist called Curtis J Humphreys spotted the series for the first time, and the series is named after him. The Humphreys series develops when electrons migrate from higher energy levels (nh=7, 8, 9, 10, 11...) to a lower energy state (nl=6). The wavelengths of the Humphreys series are all in the infrared region of the electromagnetic spectrum. For a list of wavelengths linked with spectral lines, see the table below.Energy level (n)Wavelength (in μm) in vacuum∞3.282114.673105.12995.90887.503712.37Also, CheckBohr's Model of AtomElectromagnetic Spectrum Comment More infoAdvertise with us Next Article Atomic Spectra S snehabhosale1715 Follow Improve Article Tags : School Learning Physics Class 12 Physics-Class-12 Atomic and Nuclear Physics +1 More Similar Reads CBSE Class 12 Physics Notes 2023-24 CBSE Class 12 Physics Notes are an essential part of the study material for any student wanting to pursue a career in engineering or a related field. Physics is the subject that helps us understand our surroundings using simple and complex concepts combined. Class 12 physics introduces us to a lot o 10 min read Chapter 1 - ELECTRIC CHARGES AND FIELDSElectric Charge and Electric FieldElectric Field is the region around a charge in which another charge experiences an attractive or repulsive force. 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Bar 9 min read Gauss's LawGauss's law is defined as the total flux out of the closed surface is equal to the flux enclosed by the surface divided by the permittivity. The Gauss Law, which analyses electric charge, a surface, and the issue of electric flux, is analyzed. Let us learn more about the law and how it functions so 15+ min read Magnetization and Magnetic IntensityWe've all had fun with magnets as kids. Some of us are now even playing with them! What makes them magnetic though? Why aren't there magnetic fields in all materials and substances? Have you ever given it any thought? The subjects of magnetization and magnetic intensity will be covered in this chapt 6 min read CHAPTER 6 - ELECTROMAGNETIC INDUCTIONExperiments of Faraday and HenryFor a long time, electricity and magnetism were thought to be separate and unrelated phenomena. 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Circuits in everyday life consist of resistances, capacitors, and inductance. Capacitors are the devices that accumula 6 min read Series LCR CircuitsIn contrast to direct current (DC), which travels solely in one direction, Alternating Current (AC) is an electric current that occasionally reverses direction and alters its magnitude constantly over time. Alternating current is the type of electricity that is delivered to companies and homes, and 8 min read Power Factor in AC circuitThe power factor is determined by the cosine of the phase angle between voltage and current. In AC circuits, the phase angle between voltage and current is aligned, or in other words, zero. But, practically there exists some phase difference between voltage and current. The value of the power factor 8 min read TransformerA transformer is the simplest device that is used to transfer electrical energy from one alternating-current circuit to another circuit or multiple circuits, through the process of electromagnetic induction. A transformer works on the principle of electromagnetic induction to step up or step down th 15+ min read CHAPTER 8 - ELECTROMAGNETIC WAVESDisplacement CurrentDisplacement current is the current that is produced by the rate of change of the electric displacement field. It differs from the normal current that is produced by the motion of the electric charge. Displacement current is the quantity explained in Maxwell's Equation. It is measured in Ampere. Dis 12 min read Electromagnetic WavesA wave is a propagating dynamic disturbance (change from equilibrium) of one or more quantities that is commonly described by a wave equation in physics, mathematics, and related subjects. 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