what is the wavelength of light emitted when the electron in a hydrogen atom undergoes transition from an energy level with n=4 to and energy level with n=2 ?
`{:((e),n=3, l=3,m_(1)=-3,m_(s)=+1//2), ((f), n=3, l=1, m_(1)=0, m_(s)=+1//2):}`

What is the wavelength of light emitted when the electron in a hydrogen atom undergoes transition from the energy level with n=4 to the energy level with n=1 ?

Calculate the wavelength of radiation emited when an electron in a hydrogen atom makes a transition from an energy level with n = 3 to a level with n= 2

What is the wavelength of light emitted when the electron of a hydrogen atom undergoes a transition from an energy level with n= 4 to an energy level with n = 2 ? .What is the colour corresponding to this wavelength ?

What is the wavelength of light emitted when the electron in a hydrogen atom undergoes transition from the energy level with n = 4 to the energy level with n = 1 ? In which region of the electromagnetic spectrum does this radiation fall ?

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) ?

Arrange the electrons represented by the following sets of quantum numbers in decreasing order of energy. (i) n=4, l=0, m_(l)=0, s=+1//2 , (ii) n=3, l=1, m_(l)=1, s=-1//2 (iii) n=3, l=2, m_(l)=0, s=+1//2 , (iv) n=3, l=0, m_(l)=0, s=-1//2

The quantum numbers of six electrons are given below. Arrange them in order of increasing energies. If any of these combination(s) has/have the same energy lists: 1. n=4 , l=2 , m_(i) =-2, m_(s) =-1//2 2. n=3 , l=2 , m_(l) =1 , m_(s) =+1//2 3. n=4 , l=2 ,m_(l)=-2, m_(s) =-1//2 4. n=3 , l= 2, m_(i) =-1 , m_(s) = +1//2 5. n=3 , l=1 , m_(l) =-1 , m_(s) = +1//2 6. n=4 , l= 1 , m_(l) =0 , m_(s) =+1//2