Atomic Spectra

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What is Atomic Spectra?

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The atomic spectra are defined as the spectrum of frequencies of electromagnetic radiation emitted or absorbed during transitions of electrons between energy levels within an atom. Each element has a characteristic spectrum through which it can easily be recognized. In an atom, electrons have discrete and some specific energies. There are more energy states in a tom than there are electrons. When an electron transitions from one energy level to another, it emits light or photon with a specific wavelength. When an electron gets excited from one energy level to another, it emits or absorbs light of a specific wavelength.

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Characteristics of Atomic Spectrum

The characteristics of the atomic spectrum are observed as:

  1. The atomic spectrum should be a pure line spectrum.

  2. The atomic spectrum should be the emission band spectrum. 

  3. The atomic spectrum should be an absorption line spectrum.

  4. The atomic spectrum should be the absorption band spectrum.

Atomic Spectrum Overview

In any given set of conditions like pressure, temperature, etc., the collection of all these specific wavelengths is what constitutes the atomic spectrum. Hence, atomic spectra are the spectra of atoms. Below we will be looking at atomic spectra more in detail along with the Rydberg formula and the spectral series of the hydrogen atom. There are three types of atomic spectra: emission spectra, absorption spectra, and continuous spectra.

Rydberg Formula

In atomic physics, Rydberg's formula calculates the wavelength of a spectral line in many chemical elements. The formula was primarily presented as a generalization of the Balmer series for all atomic transitions of hydrogen. It is a unit of energy defined in terms of the ground-state energy of an electron in the Bohr model for the hydrogen atom, in cgs, where is the electron mass, e is the charge on the electron, is h-bar, Z is the atomic number, and n is the principal quantum number for a given electron state. It becomes easy to calculate the spectral lines by the Rydberg formula. Following is the formula:

\[\frac{1}{\lambda} = RZ^{2} (\frac{1}{n'^{2}} - \frac{1}{n^{2}})\]

In the above formula R is the Rydberg constant (1.09737*107 m-1),

Z is the atomic number,

n is the upper energy level,

n' is the lower energy level, and

λ is the wavelength of light.

Spectral series of single-electron atoms such as hydrogen has Z = 1.

Atomic Spectroscopy

Atomic spectroscopy studies the electromagnetic radiation absorbed or emitted by the atoms. There are three types of atomic spectroscopy:

  • Atomic Emission Spectroscopy: This includes the transfer of energy from the ground state to an excited state. The electronic transition can be discussed in atomic emission.

  • Atomic Absorption Spectroscopy: Absorption to be taken place, there should be an identical energy difference between the lower and higher energy levels. The atomic absorption spectroscopy principle uses the fact that generating free electrons in an atomizer can absorb radiation at specific frequencies. It quantifies the absorption of ground-state atoms in the gaseous state.

  • Atomic Fluorescence Spectroscopy: This is a combination of atomic emission and atomic absorption, as it involves radiation of both excitation and de-excitation as well.

Uses of Atomic Spectroscopy

  • It is used to identify the spectral lines of materials used in metallurgy.

  • It is used in pharmaceutical industries to find the traces of materials used.

  • It can be used to study multidimensional elements.

  • It is used as a tool for studying the structures of atoms and molecules.

  • It provides a precise analytical method for finding the constituents in a material having unknown chemical composition.

  • Atomic spectroscopy is used in occupational and environmental monitoring. 

Solved Examples

Question: An electron excites in an atom to the fourth orbit, so when it jumps back to the energy levels, a spectrum is formed. A total number of spectra is formed. What would be the total number of spectral lines in this spectrum?

Answer: An electron excites in an atom to the fourth orbit, n=4.

The total number of spectral lines in the spectrum is,

\[\frac{n(n - 1)}{2} = \frac{4(4 - 1)}{2} = \frac{4\times 3}{2} = 6\]

Fun Facts

When atoms get excited, they emit certain specific wavelengths that correspond to different colors. The emitted light can be noted as a series of colored lines with dark spaces in between, this colored lines series is called a line of atomic spectra. A unique set of spectral lines is produced through each element. Rainbow is an example of a continuous spectrum.

FAQ (Frequently Asked Questions)

Question 1: Why is the Bright Line Spectrum Used for?

Answer: A bright-line spectrum is a dark line in a continuous and uniform spectrum, following from emission or absorption of light in a narrow frequency range, compared with the nearby frequencies. Spectral lines are usually used to identify atoms and molecules. These fingerprints can be contrasted to the previously kept account of atoms and molecules' fingerprints. So, they are used to identify the atomic and molecular components of stars and planets, which would otherwise be impossible. The bright spectrum is produced by the electrons in the element's atoms jumping to lower energy states after being bumped upward by a collision with another atom.

Question 2: Which Colour has the Most Energy and Why?

Answer: Violet waves carry the most because violet waves have the shortest wavelength of the visible light spectrum. Waves having a short wavelength contain the most energy. Red waves have a relatively long wavelength in the 700 nm range, and violet waves are much shorter-roughly half that. Violet is the shortest visible wavelength band for which a single violet photon has more energy than a single photon of red light. However, this does not mean that a violet flashlight beam is more powerful than a red beam. It just means that there are twice as many photons in the red light if they have the same power.