Home
Class 11
CHEMISTRY
The wavelength of the radiation emitted ...

The wavelength of the radiation emitted when in a H atom electron falls from infinity to stationary state 1, would be (Rydberg constant = `1.097 xx 10^7 m^(-1`)

A

406 nm

B

192nm

C

91nm

D

`9.1 xx 10^(-8)` nm

Text Solution

Verified by Experts

The correct Answer is:
C
Promotional Banner

Similar Questions

Explore conceptually related problems

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) ).

The frequency of radiation emitted when the electron falls from n=4 to n=1 in a hydrogen atom will be (given ionisation energy of H=2.18xx10^(18)J"atom"^(-1) and h=6.625xx10^(-25)Js )

when a certain energy is applied to an hydrogen atom, an electron jumps from n =1 to n = 3 state. Find (i) the energy absorbed by the electron. (ii) wavelength of radiation emitted when the electron jump back to its initial state. ( Energy of electron in first orbit = - 13.6 eV , Planck's constant = 6.6225 xx10^(-34) Js, Charge on electron = 1.6 xx10^(-19) C, speed of light in vacuum = 3xx10^(8)ms^(-1)

Calculate the wave number of the spectral line when electron jumps from the seond Bohr orbit to the ground state. R = 1.097xx 10^(7) m^(-1)

The wave number of the shortest wavelength of absorption specturm of H-atom is (Rydberg constant =109700cm^(-1) )