Draw a neat labelled energy level diagram and explain the different series of spectral lines for hydrogen atom.
The energy level diagram of the hydrogen atom is shown in the
figure above depicting different series line.
There are four series namely
1. Lyman Series (U.V.)
2 Blamer Series (visible)
3. Psachen Series (infrared)
4. Brackett Series (infrared)
5. Pfund Series (infrared)
n=principle quantum number whose values ranges from 1−∞
n=1represents the ground energy level
n=∞is the highest energy level.
1.
Lyman Series (U.V.)
In this series the transition occur from n>1 to the first orbit that isn=1. This represents the Lyman Series of
the Hydrogen atom.
It is mainly observed in the ultraviolet
region of the EM wave.
1λ=R(112−1n2)
Wheren=2,3
This is further divided into sublevels as α−lymanfor n=2 and so on.
2 Blamer
Series (visible)
In this series the transition occur from n>2to the second orbit that isn=2. This represents the Balmer Series
of the Hydrogen atom.
It is mainly observed in the Visible region
of the EM wave.
1λ=R(122−1n2)
Where, n=3,4
This is further divided into sublevels as α−Balmerfor n=3and so on.
3.
Psachen Series (infrared)
In this series the transition occur from n>3 to the second orbit that isn=3. This represents the Paschen Series
of the Hydrogen atom.
It is mainly observed in the Infrared region
of the EM wave.
1λ=R(132−1n2)
Where n=4,5,6
4. Brackett Series (infrared)
In this series the transition occur from n>4 to the second orbit that isn=4. This represents the Bracket Series
of the Hydrogen atom.
It is mainly observed in the Infrared region
of the EM wave.
1λ=R(142−1n2)
Where n=5,6,
5.
Pfund Series (infrared)
In this series the transition occur fromn>5to the second orbit that isn=5. This represents the Bracket Series
of the Hydrogen atom.
It is mainly observed in the Infrared region
of the EM wave.
1λ=R(152−1n2)
Where n=6,7
The energy level diagram of the hydrogen atom is shown in the figure above depicting different series line.
There are four series namely
1. Lyman Series (U.V.)
2 Blamer Series (visible)
3. Psachen Series (infrared)
4. Brackett Series (infrared)
5. Pfund Series (infrared)
n=principle quantum number whose values ranges from 1−∞
n=1represents the ground energy level
n=∞is the highest energy level.
1. Lyman Series (U.V.)
In this series the transition occur from n>1 to the first orbit that isn=1. This represents the Lyman Series of the Hydrogen atom.
It is mainly observed in the ultraviolet region of the EM wave.
1λ=R(112−1n2)
Wheren=2,3
This is further divided into sublevels as α−lymanfor n=2 and so on.
2 Blamer Series (visible)
In this series the transition occur from n>2to the second orbit that isn=2. This represents the Balmer Series of the Hydrogen atom.
It is mainly observed in the Visible region of the EM wave.
1λ=R(122−1n2)
Where, n=3,4
This is further divided into sublevels as α−Balmerfor n=3and so on.
3. Psachen Series (infrared)
In this series the transition occur from n>3 to the second orbit that isn=3. This represents the Paschen Series of the Hydrogen atom.
It is mainly observed in the Infrared region of the EM wave.
1λ=R(132−1n2)
Where n=4,5,6
4. Brackett Series (infrared)
In this series the transition occur from n>4 to the second orbit that isn=4. This represents the Bracket Series of the Hydrogen atom.
It is mainly observed in the Infrared region of the EM wave.
1λ=R(142−1n2)
Where n=5,6,
5. Pfund Series (infrared)
In this series the transition occur fromn>5to the second orbit that isn=5. This represents the Bracket Series of the Hydrogen atom.
It is mainly observed in the Infrared region of the EM wave.
1λ=R(152−1n2)
Where n=6,7
