Calculate the frequency of the light emitted when an electron Jumps form n=3 to n =1 [R = `1096789 cm^-1`]

Calculate the frequency nad wave length of the energy emitted when the electron jumps from 4th orbit to 1st orbit of a H-atom.

Calculate the wavalength of radiation emitted when electron in a hydrogen atom jumps from n=oo to n=1 .

Total number of spectral lines emitted when an electron jumps from n=5 to n=1 in hydrogen atom is

What will be the wavelength of the light emitted due to a transition of electron from n = 3 orbit to n = 2 orbit in hydrogen atom? Given: the Rydberg constant for hydrogen atom is R_(H) = 1.09 xx 10^(7) m^(-1) .

What will be the wavelength of the light emitted due to a transition of electron from n=3 orbit to n=2 orbit in hydrogen atom ? Given : in the Rydbeg constant for hydrogen atom is R_H=1.09xx10^(7) m^(-1) .

The ionization energy of hydrogen atom in the ground state is 1312 kJ "mol"^(-1) . Calculate the wavelength of radiation emitted when the electron in hydrogen atom makes a transition from n = 2 state to n = 1 state (Planck’s constant, h = 6.626 xx 10^(-34) Js , velocity of light, c = 3 xx 10^8 m s^(-1) , Avogadro’s constant, N_A = 6.0237 xx 10^23 "mol"^(-1) ).

Using Bohr's postulates, derive the expression for the frequency of radiation emitted when electron in hydrogen atom undrgoes transition from higher energy state (quantum number n_i ) to the lower state ( n_f ). When electron in hydrogen atom jumps from energy state n_i=4 to n_f=3,2,1 , identify the spectral series to which the emission lines belong.

The threshold frequency, v_(0) for a metal is 7.0xx10^(14)s^(-1) . Calculate the kinetic energy of an electron emitted, when radiation of frequency v=1.2xx10^(15)s^(-1) , strikes this metal.