What is the energy difference and the frequancy and the wavelength of light emitted when the electron in a hydrogen atom undergoes transition from the energy level `n = 4` to the energy `n = 3` given that the value of Rydberg constant is `1.0974 xx 10^(7)m^(-1)`?

Answer

A, B, D

Explanation

`Delta E = Rhc [(1)/(n_(1)^(2)) - (1)/(n_(2)^(2))]`
`= (1.0974 xx 10^(7))(6.626 xx 10^(-34))(3 xx 10^8)[(1)/(9) -(1)/(16)]`
`= 1.06 xx 10^(-19) J`
`v = (Delta E )/(h) = (1.06 xx 10^(-19) J)/(6.262 xx 10^(-34)J s) = 1.60 xx 10^(14) s^(-1)`
`lambda = (c )/(v) = (3 xx 10^(8) m s^(-1))/(1.60 xx 10^(14) s^(-1)) = 1.875 xx 10^(6) m`