Question

The second line in Paschen series corresponds to an electronic transition between which Bohr orbit in hydrogen? ​

Answer 1

Second Line of Paschen Series :

Always remember the following informations:

• In case of Paschen Series, the electron will always descend from a higher orbit to a lower orbit with Principal Quantum Number = 3.

• That means the lower orbit will be n = 3.

Now, the first line in Paschen Series corresponds from n = 4 to n = 3 , with the highest wavelength of electromagnetic radiation.

So, second line in Paschen Series will be from:

• n = 5 to n = 3.

$\star$ Hope It Helps.

Answer 2

The second line in Paschen series corresponds to an electronic transition between following Bohr orbit in hydrogen:

• Paschen series in the hydrogen spectrum is belongs to 3 line which is its ground energy level , or n1 = 3 where n is corresponds to the principal quantum number.

• When electron comes from high energy to low energy level at the ground state of n=3 then paschen series will be observed . It lies in the range of IR region.

• Electron always descends from high orbit to the low orbit . Here the lower orbit is 3 .

• So, the first line in Paschen series corresponds to n2=4 to n1= 3 i.e from 4—> 3.

• We have to find the 2nd series which corresponds to n2=5 to n1= 3 i.e from 5—> 3.

• So, the second line in Paschen series corresponds to an electronic transition between n2=5 to n1= 3 i.e from 5—> 3 Bohr orbit in hydrogen.