What is the wavelength of light emitted when the electron in a hydrogen atom undergoes transition from an energy level with n = 4 to an energy level with n = 2?
According to Balmer formula
Wave no = RH [1/n12 – 1/n22]
Here n1 = 2 , n2 = 4, RH = 109678
Putting these values in the equation we get
Wave number =109678(1/22 - ¼2) = 109678 x 3/16
Also λ = 1/ wave number
Therefore λ = 16 / 109678 x 3 = 486 nm
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How answer obtained ?
All thing are ok fools
Good but we can obtain the value by energy formula....Or not.Rh value explain please....
What is the colour
Calculations are incorrect
Why the value of rh is taken as 109678
Why rh is 109678
unit is cm or nm
Why RH value is taken as 109678?
How there comes 10 on last line and where is 3 ???