[" Calculate the energy of the second stationary "],[" state of hydrogen atom."],[" (Given: Rydberg constant "R=2.18times10^(-)]

Calculate the longest and shortest wavelength in the Balmer series of hydrogen atom. Given Rydberg constant = 1.0987xx10^7m^-1 .

(a) Using Bohr's postulates, derive the expression for the total energy of the electron in the stationary states of the hydrogen atom. (b) Using Rydberg formula, calculate the wavelengths of the spectral lines of the first member of the Lyman series and of the Balmer series.

The energy of an electron in an excited hydrogen atom is -3.4 eV . Calculate the angular momentum of the electron according to Bohr's theory. (Given Rydberg's constant R=1.09737 xx 10^-7 m^-1, h=6.626176 xx 10^-34 Js, c=3 xx 10^8 ms^-1) .

Calculate the ionisation energy of the hyddrogen atom. How much energy will be required to ionise 1 mole of hydrogen atoms? Given, that the Rydberg constant is 1.0974xx10^(7)m^(-1) .

Calculate the energy of an electron in the second Bohr's orbit of an excited hydrogen atom the energy of electron in the first Bohr orbit is -2.18 xx 10^(-11) erg

Calculate the energy of an electron in the second Bohr's orbit of an excited hydrogen atom the energy of electron in the first Bohr orbit is -2.18 xx 10^(-11) erg

The wavelength (in cm) of second line in the Lyman series of hydrogen atomic spectrum is (Rydberg constant =" R cm"^(-1) )