Given that in H-atom the transitioin energy for `n=1` to n=2 is 10.2eV, the energy for the same transition in `Be^(3+)` is

It the 1st ionisation energy of H atom is 13.6 eV, then the 2nd ionisation energy of the atom is-

If the 1st ionisation energy of H atom is 13.6 eV then the 2nd ionisation energy of He atom is

(1) Show that the sum of energies for the transition from n=3 to n=2 and from n=2 to n=1 is equal to the energy of transition from n=3 to n=1 in case of an H-atom. (2) Are wavelength and frequencies of the emitted spectrum also additive as their energies?

The ionisation energy of H atom is x kJ. The energy required for the electron to jump from n=2 to n=3 will be

The ionization energy of H atom is x kJ. The energy required for the electron to jump from n = 2 to n = 3 will be:

The ionization energy of H atom is x kJ. The energy required for the electron to jump from n = 2 to n = 3 will be:

The ionization energy of the hydrogen atom is 13.6eV. The potential energy of the electron in n=2 state of hydrogen atom is

If an electron undergoes transition from n = 2 to n =1 in Li^(2+) ion , the energy of photon radiated will be best given by

If the principal quantum number of an energy state be n , the energy of a hydrogen atom, E= -(13.6)/(n^2)eV . Due to transition of electron from n=3 to n=2 level, what will be the energy of the photon emitted ?

At what temperature the transitional kinetic energy of atomic hydrogen equal that for n_2 =1 to n_2 =2 transition.