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Ans. The emission spectrum of hydrogen is a series of coloured lines produced when hydrogen gas is excited and then emits light as it returns to its ground state. Each line in the spectrum corresponds to a specific wavelength of light associated with the energy transitions of hydrogen atoms.
Q.2 : What is a line spectrum?
Ans. A line spectrum is a pattern of distinct lines or bands of light produced when an element emits or absorbs energy. Each line in the spectrum corresponds to a specific wavelength of light associated with a particular energy transition within the atom or molecule.
Q.3 : What is the Balmer series in the hydrogen spectrum?
Ans. The Balmer series is a specific set of spectral lines observed in the visible region of the hydrogen spectrum. These lines are produced when hydrogen atoms transition from higher energy levels to the second energy level (n = 2). The Balmer series includes several prominent lines, such as H-alpha, H-beta, H-gamma, and so on, each corresponding to a specific wavelength of light.
Emission And Line Spectrum Of Hydrogen, Spectra Lines, Important Topics For JEE 2025
Spectrum of Hydrogen : spectrum of hydrogen consists of distinct spectral lines resulting from electron transitions between energy levels. These lines, including the Lyman, Balmer, and Paschen series, provide critical insights into quantum mechanics, atomic structure, and have applications in spectroscopy, astronomy, and understanding fundamental physical constants.
Shrivastav 4 Jun, 2024
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Emission and Line Spectrum of Hydrogen :
Hey there, young scientists! Have you ever wondered what makes up the colourful lights we see in fireworks or neon signs? Or why do certain elements emit specific colours of light when heated or excited? Well, get ready to uncover the mysteries of hydrogen– the simplest and most abundant element in the universe – and its fascinating emission and line spectrum. In this article, we'll embark on an illuminating journey to understand how hydrogen atoms emit light and produce unique spectral lines, all explained in simple terms just for you.
Emission Spectrum of Hydrogen
Let's start by unravelling the concept of the emission spectrum. Imagine you have a special flashlight that shines light through a prism. When you shine the light through the prism, it breaks up into a rainbow of colours – just like a rainbow in the sky after it rains! This rainbow of colors is called a spectrum. Now, if we're talking about the emission spectrum, it means we're looking at the specific colours of light emitted by a substance when it's excited or heated.
In the case of hydrogen, when we heat it or run an electric current through it, the hydrogen atoms get excited and emit light. But here's the cool part – the light emitted by hydrogen isn't just a random mishmash of colours. Instead, it produces a series of distinct lines of light at specific wavelengths, creating what we call an emission spectrum.
Line Spectrum of Hydrogen
Line Spectrum of Hydrogen :
Line spectrum of hydrogen is observed due to excitation or de-exicitation of electron from one stationary orbit to another stationary orbit.
Let electron make transition from
n
2
to
n
1
(
n
2
>
n
1
) in a H-like sample
Energy of emitted photon =
Wavelength of emitted photon
Wave number,
R = Rydberg constant = 1.09678 × 10
7
m
–1
Series
Discovered by
Regions
n
2
n
1
Lyman
Lyman
U.V. region
n
2
= 2, 3, 4…
n
1
= 1
Balmer
Balmer
Visible region
n
2
= 3, 4, 5…
n
1
= 2
Paschen
Paschen
Infra red (I.R.)
n
2
= 4, 5, 6…
n
1
= 3
Brackett
Brackett
I.R. region
n
2
= 5, 6, 7…
n
1
= 4
Pfund
Pfund
I.R. region
n
2
= 6, 7, 8…
n
1
= 5
Humphery
Humphery
Far I.R. region
n
2
= 7, 8, 9…
n
1
= 6
Spectra Lines of Hydrogen Atom
Lyman series
It is first spectral series of H.
It was found to be in
ultraviolet region
by Lyman in 1898.
For it value of n
1
= 1 and n
2
= 2, 3, 4 where ‘n
1
’ is ground state and ‘n
2
’ is called excited state of electron present in a H-atom.
where n
2
> 1 always.
The wavelength of marginal line (i.e. n
2
= ∞) =
for all series. So for lyman series
I
st
line of lyman series
=
2 → 1
II
nd
line of lyman series = 3 → 1
Last line of lyman series = ∞ → 1
[10.2 eV ≤ (ΔE)
lyman
≤ 13.6eV]
Balmer series
It is the second series of H-spectrum.
It was found to be in
visible region
by Balmer in 1892.
For it value of n
1
= 2 and n
2
= 3, 4, 5, …
The wavelength of marginal line of Balmer series =
where n
2
> 2 always.
1.9 ≤ (ΔE)
balmer
≤ 3.4 eV.
Paschen series
It is the third series of H - spectrum.
It was found to be in
infrared region
by Paschen.
For it value of n
1
= 3 and n
2
= 4, 5, 6……..
The wavelength of marginal line of Paschen series =
where n
2
> 3 always.
Brackett series
It is fourth series of H - spectrum.
It was found to be in
infrared region
by Brackett.
For it value of n
1
= 4 and n
2
= 5, 6, 7 …
The wavelength of marginal line of brackett series =
where n
2
> 4 always.
Pfund series
It is fifth series of H - spectrum.
It was found to be in
infrared region
by Pfund.
For it value of n
1
= 5 and n
2
= 6, 7, 8……. where n
1
is ground state and n
2
is excited state.
The wavelength of marginal line of Pfund series =
∙
where n
2
> 5 always.
Humphry series
It is the sixth series of H-spectrum.
It was found to be in
infrared region
by Humphry.
For it value of n
1
= 6 and n
2
= 7, 8, 9
The wavelength of marginal line of Humphry series =
∙
where n
2
> 6.
Solved Example Of Spectrum of Hydrogen
1.
In the spectrum of He
+
ion the wavelength of
line of Balamer series is
x
Å. What is the wavelength of
line of Brackett series.
Sol.:
2.
A sample of He
+
ions in ground state absorbs the radiation of
x
Å. Subsequently, The sample emit radiation of 6 different wavelength. Calculate the value of
x
.
Sol.:
3.
In a hydrogen spectrum if electron moves from 6
th
to 2
nd
by transition in multi steps then find out the number of lines in spectrum.
Sol.:
Total number of lines = 4 + 3 + 2 + 1 + 0 = 10
Total number of lines =
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