Using Bohr's formula for energy quantisation, determine (i) the largest wavelength in Balmer series of hydrogen atom spectrum and (ii) the excitation energy of `n = 3` level of `He^(+)` ion. Given `R = 1.097 xx 10^(7) m^(-1)`

Using Bohr's formula for energy quantization, determine (i) the longest wavelength in Lymann series of hydrogen atom spectrum. (ii) the excitation energy of the n=3 level of He^(+) atom. (iii) the ionization potential of the ground state of Li^(++) atom.

Assuming Bohr's atomic model find (a)largest wavelength in Balmer series, (b)the excitation energy of n=3 level of He^+ atom.

What is maximum wavelength of line of Balmer series of Hydrogen spectrum (R=1.09 xx10^(7)m^(-1) ):

Find the two longest wavelength ("in" Å) emitted when hydrogen atom make transition and the spectrum lines lie in the visible regain (R = 1.097 xx 10^(7) m^(-1))

Calculate longest wavelength of Paschen series. Given R=1.097xx10^(7)m^(-1) .

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

Calculate the shortest wavelength of light emitted in the Paschen series of hydrogen spectrum. Which part of the electromagnetic spectrum, does it belong ? ( Given : Rydberg constant , R = 1.1 xx 10^(7)m^(-1)

Taking Rydberg's constant R_(H) = 1.097 xx 10^(7)m first and second wavelength of Balmer series in hydrogen spectrum is

Determine the smallest wavelength in Lyman series among first four spectral lines in of hydrogen atom using Bohr's formula of energy quantisation .