Atomic Spectra

An atom has a range of readily absorbed and emitted characteristic frequencies of electromagnetic radiation. An electron can hop from one fixed orbital to another: if the orbital it jumps to has higher energy, it must absorb a photon of a particular frequency; if the orbital it jumps to has lower energy, it must emit a photon of a specific frequency. The energy difference between the orbitals determines the frequency. The development of quantum mechanics hinged on the explanation of this phenomenon. Each chemical element’s atomic spectrum is distinct, and it is substantially responsible for matter’s colour.

During transitions between different energy levels within an atom, an electron produces or absorbs a spectrum of electromagnetic radiation. When an electron is excited from one energy level to the next, it emits or absorbs light of a specific wavelength. The atomic spectra of atoms are a collection of all these wavelengths of the atom in a specific range of parameters, such as pressure, temperature, etc. Emission spectra, absorption spectra, and continuous spectra are the three types of atomic spectra.

Characteristic Spectrum of radiation :

Characteristic radiation may be a style of energy emission relevant for X-ray production. This energy emission happens when a fast-moving electron collides with a K-shell electron. The electron within the K-shell is ejected (provided the incident electron’s energy is larger than the separation energy of the K-shell electron), abandoning a ‘hole’ with an emission of one x-ray photon, sometimes called a characteristic photon, with energy equal to the energy state difference between the outer and inner shell electron involved within the transition.

As critical the continual spectrum of bremsstrahlung radiation, characteristic radiation is represented by a spectrum. As each element encompasses a specific arrangement of electrons at discrete energy, it is appreciated that the radiation produced from such interactions is ‘characteristic’ of the element involved.

Electron transitions from the L-shell to the K-shell, for example, yield x-ray photons with energies of 57.98 and 59.32 keV in a tungsten target. The Pauli exclusion principle asserts that no two half-integer spin particles (such as electrons) in an atom may occupy the same energy state simultaneously; thus, the K-shell represents two different energy states, the L-shell eight, and so on.

Absorption spectrum :

We know that light is radiation composed of several frequencies of radiation. A normal light features a large range of wavelengths with respective frequencies. Electromagnetic waves can travel in an exceeding vacuum at the speed of sunshine. Electromagnetic waves are further classified as portions, and ultraviolet rays and visual light are examples. Microwaves, actinic radiation, ultraviolet radiation, X-rays, and gamma-rays are kinds of radiation included within the Spectrum.

When the white light is responded to a medium, they get split consistent with their respective frequencies and wavelengths. The interaction of electromagnetic waves with matter causes the molecules and atoms present in a very large area to absorb energy and reach the next energy level. This higher energy level is unstable, and hence they need to emit energy within the kind of radiation to return to their original states. This process generates emission spectra and absorption spectra.

Spectral series : 

The simplest approach to grasp the concept of spectral series is to look at the hydrogen atom. It is the most basic atom with which we may examine the spectral series. A beam of light must be directed into the slit to examine these spectrum series. When the photos are subjected to a spectroscope, each component of this beam of light may generate a different image, which can appear as a spectral series.

These spectral series resemble parallel lines of equal length and speed. If the wavelength of spectral lines is higher and the spacing is greater, the lines appear to be separated, and the wavelength of light can influence these spacings. Conversely, as the wavelength decreases, the lines become closer and appear next to one another. The distance between the lines was also recorded if the shortest wavelength was recorded. This is referred to as the “series limit.” We can tell if the volume is high or low by looking at this series limit.

Characteristics of Atomic Spectra :

Atomic spectra have a variety of features, including:

• A pure line spectrum should be used for the atomic spectra.
• It should be a spectrum with emission bands.
• It should be a spectrum with absorption lines.
• It should also be the spectrum of the absorption band.

Conclusion :

The atomic spectra are the spectrum of frequencies of radiation emitted or absorbed during transitions of electrons between energy levels within an atom. As an electron moves between different energy levels within an atom, its spectrum of electromagnetic waves is released or absorbed. An electron emits or absorbs light of a selected wavelength because it jumps from one energy state to the following.