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Why Do Elements Have More Than One Spectral Line: Exploring The Quantum Phenomenon

Spectroscopy - How Can Every Atom Have Unique Spectral Lines? - Chemistry  Stack Exchange

Why Do Elements Have More Than One Spectral Line: Exploring The Quantum Phenomenon

Emission And Absorption Line Spectra – A Level Physics

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Why Does Each Element Have More Than One Coloured Line?

An absorption spectrum, as seen in the context of individual elements, often exhibits multiple colored lines. This phenomenon occurs because when ground state electrons within atoms absorb energy in the form of light, they can become excited to various energy states, each requiring a distinct amount of energy. Consequently, these different energy transitions result in the presence of multiple absorption lines in the spectrum. In essence, an absorption spectrum provides a visual representation of the unique energy levels an atom’s electrons can reach when they absorb photons of specific energies.

What Causes More Spectral Lines?

The number of spectral lines in an atom is influenced by the behavior of electrons around the nucleus. Electrons spend varying durations of time near the nucleus based on their angular momentum. This indicates that the energy of an electron is generally determined by its principal quantum number (n) and azimuthal quantum number (ℓ). As ℓ can range from 0 to n-1, atoms with higher complexity exhibit a greater abundance of spectral lines. This relationship was elucidated on November 21, 2018.

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Spectroscopy - How Can Every Atom Have Unique Spectral Lines? - Chemistry  Stack Exchange
Spectroscopy – How Can Every Atom Have Unique Spectral Lines? – Chemistry Stack Exchange
Hydrogen Spectral Series - Wikipedia
Hydrogen Spectral Series – Wikipedia
Periodic Table - Wikipedia
Periodic Table – Wikipedia
Chapter 5 Spectral Lines Of Hydrogen Atom | Ppt
Chapter 5 Spectral Lines Of Hydrogen Atom | Ppt
17.3.2 Emission Spectrum – Xmphysics
17.3.2 Emission Spectrum – Xmphysics

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Emission and Absorption Line Spectra - A Level Physics
Emission and Absorption Line Spectra – A Level Physics

Different elements have different spectra because they have different numbers of protons, and different numbers and arrangements of electrons. The differences in spectra reflect the differences in the amount of energy that the atoms absorb or give off when their electrons move between energy levels.This type of spectrum is called an absorption spectrum. For atoms of a particular element, there are usually more than one absorption line present because a ground state electron can be excited to different excited energy states by absorbing different amounts of energy (in the form of light).Since electron spend different amounts of time near the nucleus depending on their angular momentum, this means that the energy of an electron is, in generally, a function of n and ℓ. Since ℓ ranges from 0 to n−1, this means that more complicated atoms have lots more spectral lines.

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