wiz-icon
MyQuestionIcon
MyQuestionIcon
1
You visited us 1 times! Enjoying our articles? Unlock Full Access!
Question

Calculate the wavelength of 1st and 2nd line in the Paschen series.


Open in App
Solution

Step 1: Given

Step 1: Formula used

The wave number of the Paschen series is given by,
1λ=R132-1n2

λ=wavelength

R=Rydberg constant

n=orbit number

The value of the rydberg constant is R=1.1×107m-1

Step 2: Determine the wavelength of the Paschen series

In the hydrogen spectrum, various lines can be seen in the spectrum due to the change in the wavelength of the photons emitted from the atom.

This is called the Paschen series when the electron jumps from a higher orbit to the third orbit and reaches a line in the spectrum.

The first line in the Paschen series is the line when the electron jumps from the 4th to the 3 rd.

The second line of the orbit and the Passhen series is the line found when the electron jumps from the 5th orbit to 3rd orbit.

Currently, the wavenumber of the Paschen series is given by the following equation,

1λ=R132-1n2

So, putting the value for first-line n=4 we have,
1λ1=R132-142

1λ1=1.1×107132-142
Upon simplifying we have,
λ1=1447×1.1×10-7

λ1=1870nm
Now, putting the value for the second line n=5 we have,
1λ2=1.1×107132-152

λ2=1258nm
Hence, the wavelength of the first lines of the Paschen series is 1870nm and the wavelength for the second lines is 1258nm.


flag
Suggest Corrections
thumbs-up
18
Join BYJU'S Learning Program
similar_icon
Related Videos
thumbnail
lock
Bohr's Derivations
CHEMISTRY
Watch in App
Join BYJU'S Learning Program
CrossIcon