# draw a labelled energy level diagram of hydrogen atom and its various spectral series

### Mohammed

Guys, does anyone know the answer?

get draw a labelled energy level diagram of hydrogen atom and its various spectral series from screen.

## Draw a neat labelled energy level diagram and explain the different series of spectral lines for hydrogen atom.

Click here👆to get an answer to your question ✍️ Draw a neat labelled energy level diagram and explain the different series of spectral lines for hydrogen atom.

Question

## Draw a neat labelled energy level diagram and explain the different series of spectral lines for hydrogen atom.

Hard Open in App

Updated on : 2022-09-05

Solution Verified by Toppr

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.

λ 1 =R( 1 2 1 − n 2 1 ) 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.

λ 1 =R( 2 2 1 − n 2 1 ) 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.

λ 1 =R( 3 2 1 − n 2 1 ) 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.

λ 1 =R( 4 2 1 − n 2 1 ) 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.

λ 1 =R( 5 2 1 − n 2 1 ) Where n=6,7

Solve any question of Atoms with:-

Patterns of problems

>

Was this answer helpful?

61 3

## Draw a neat labeled energy level diagram and explain the different series of spectral lines for the hydrogen atom.

Draw a neat labeled energy level diagram and explain the different series of spectral lines for the hydrogen atom.. Ans: Hint: The electrons are transited from higher energy level to the lower energy levels. This causes the spectral lines of differen...

## Draw a neat labeled energy level diagram and explain the different series of spectral lines for the hydrogen atom.

Last updated date: 18th Mar 2023

• Total views: 264.3k • Views today: 5.44k Answer Verified 264.3k+ views

**Hint:**The electrons are transited from higher energy level to the lower energy levels. This causes the spectral lines of different wavelengths. The single electron orbiting around the nucleus of the hydrogen atom is explained by the Bohr model of the atom.

**Complete step by step answer:**

The energy level diagram of the hydrogen atom is given below.

When the electron transits from a higher energy level to a lower energy level photon is emitted. The energy of the photon is the difference in the energy of the states. The photon will emit with a frequency corresponding to the energy difference of the final and initial energy states. The energy of each state remains the same. Hence the emitted photon will always have the same frequency always.

The spectral lines are classified into series. The expression connecting the wavelength and the difference between the energy levels is described by the Rydberg formula.

1 λ = Z 2 R( 1 n 2 f − 1 n 2 i ) 1λ=Z2R(1nf2−1ni2) . Where λ λ is the wavelength, Z Z

is the atomic number,

R R

is the Rydberg constant,

n f nf

is the principal quantum number of the final state, and

n i ni

is the principal quantum number of the initial state.

The spectral lines including the transition of the electron to

n=1 n=1

energy state from the higher energy levels are called Lyman series. That is

n f =1 nf=1 and n i >1 ni>1 .

The spectral lines including the transition of the electron to

n=2 n=2

energy state from the higher energy levels are called Balmer series. That is

n f =2 nf=2 and n i >2 ni>2 .

The spectral lines including the transition of the electron to

n=3 n=3

energy state from the higher energy levels are called Paschen series. That is

n f =3 nf=3 and n i >3 ni>3 .

The spectral lines including the transition of the electron to

n=4 n=4

energy state from the higher energy levels are called Brackett series. That is

n f =4 nf=4 and n i >4 ni>4 .

The spectral lines including the transition of the electron to

n=5 n=5

energy state from the higher energy levels are called Pfund series. That is

n f =5 nf=5 and n i >5 ni>5 .

**Note:**

The wavelength will be higher for the transitions between adjacent energy levels. The Balmer series have wavelengths similar to the visible light. Hence they are visible. And the Paschen lies in the infrared region.

## Draw a Neat and Labelled Energy Level Diagram and Explain Balmer Series and Brackett Series of Spectral Lines for Hydrogen Atom.

Draw a Neat and Labelled Energy Level Diagram and Explain Balmer Series and Brackett Series of Spectral Lines for Hydrogen Atom.

Advertisement Remove all ads Ads by

Draw a neat and labelled energy level diagram and explain Balmer series and Brackett series of spectral lines for the hydrogen atom.

Advertisement Remove all ads

### SOLUTION

Balmer series: The spectral lines of this series corresponds to the transition of an electron from some higher energy state to 2nd orbit. For Balmer series, p = 2 and n = 3, 4, 5. The wave numbers and the wavelengths of spectral lines constituting the Balmer series are given by.

v¯ =1λ =R(122-1n2)

This series lies in the visible region.

**Bracket series**: The spectral lines of this series corresponds to the transition of an electron from a higher energy state to the 4th orbit.

For this series, p = 4 and n = 5, 6, 7, ....

The wave numbers and the wavelengths of the spectral lines constituting the Bracket series are given by

v¯=1λ=R(142-1n2)

These series lie in the near infrared region of the spectrum.

Concept: Hydrogen Spectrum

Is there an error in this question or solution?

2017-2018 (March) Q 8.2 Q 8.1

### APPEARS IN

2017-2018 (March) (with solutions)

VIDEO TUTORIALSQ 8.2 | 7 marks VIEW ALL [2] view

Video Tutorials For All Subjects

Hydrogen Spectrum video tutorial 00:21:31 Hydrogen Spectrum video tutorial 00:11:11

Guys, does anyone know the answer?