Respuesta :
The emission spectrum for hydrogen gas are red, blue-green, blue-violet and violet so I believe the absorption spectrum would be the same and these are given off when a glass that has hydrogen gas is passed through with an electric current at low pressure and it gives off blue light which when passed through a prism is broken down into the above light colors.
Dark lines are observed in the absorption spectrum of hydrogen atom.
Further explanation:
Electronic transition:
An electronic transition is a process that occurs when an electron undergoes emission or absorption from one energy level to another energy level.
When an electron undergoes a transition from lower energy level to the higher energy level then it requires energy to complete the process. This transition is an absorption process.
When an electron undergoes a transition from higher energy level to lower energy level then it emits energy to complete the process. This transition is an emission process.
A hydrogen atom has one proton and one electron. This single electron will be present in specific energy level. The atomic number of hydrogen atom is 1 so it has only one shell and every orbital in this shell have the same energy. The range of energy levels starts from n =1 and can reach up to infinity.
The formula to calculate the energy levels for hydrogen is as follows:
[tex]{E_n}=-\frac{{{R_H}}}{{{n^2}}}[/tex] ...... (1)
Here,
[tex]{E_n}[/tex] is the energy of the nth orbital.
n is the principal quantum number.
[tex]{R_H}[/tex] is the Rydberg constant.
The energy that is associated with the transitions is the energy difference between the two levels in which the transition takes place.
The formula to calculate the difference between two energy levels of the hydrogen atom is,
[tex]\Delta E={R_{\text{H}}}\left({\frac{1}{{{{\left({{{\text{n}}_{\text{i}}}} \right)}^2}}}-\frac{1}{{{{\left({{{\text{n}}_{\text{f}}}}\right)}^2}}}}\right)[/tex]
Where,
[tex]\Delta E[/tex] is the energy difference between two energy levels.
[tex]{R_{\text{H}}}[/tex] is a Rydberg constant.
[tex]{{\text{n}}_{\text{i}}}[/tex] is the initial energy level of transition.
[tex]{{\text{n}}_{\text{f}}}[/tex] is the final energy level of transition.
The gaseous hydrogen molecule dissociates when electric discharge through it. The lines that are produced due to the emission from [tex]{{\text{n}}_{\text{i}}}[/tex] equal to 2 appear in the emission spectrum.
The emission spectrum of hydrogen shows 4 lines. One line is in the higher range that is [tex]656\;{\text{nm}}[/tex] and the other three lines in the range of [tex]400 - 500\;{\text{nm}}[/tex] .
Since hydrogen is present in the first shell, it will always absorb some amount of energy to reach the higher levels. So absorption spectrum is observed in hydrogen atom. Absorbed photons show black lines. The absorbed photons show black lines in the spectrum. In such photons, energies of particular wavelengths are absorbed, but these are not visible and therefore absorption spectrum is just the opposite of emission spectrum.
Learn more:
1. Component of John Dalton’s atomic theory: https://brainly.com/question/2357175
2. Basis of investigation for the scientists: https://brainly.com/question/158048
Answer details:
Grade: Senior School
Subject: Chemistry
Chapter: Atomic structure
Keywords: transition, hydrogen atom, Rydberg constant, absorption spectrum, electronic transition, initial energy level, final energy level, RH, ni, nf, energy difference between two levels.
