What is the wavelength of light emitted when the electron in a hydrogen atom undergoes transmission from n=4 to n=2? (`R_(H) = 109677 cm^(-1)`)

What is the energy in joules required to shift the electron of the hydrogen atom from the first Bohr orbit to the fifth Bohr orbit and what is the wavelength of the light emitted when the electron returns to the ground state? The ground state electron energy is -2.18xx10^(-11) ergs. (1erg=10^(-7)J)

What is the maximum number of emission lines when the excited electron of a hydrogen atom in n = 6 drops to the ground state?

Energy of an electron is given by, E=-2.178 xx10^(-18) 4 ((Z^(2))/(n^(2))) J. Wavelength of light required to excite an electron in hydrogen atom from level n = 1 to n = 2 will be: (h = 6.62 xx 10^(-34) J s and c = 3 xx 10^(8) ms^(-1))

Find the maximum number of emission lines, when the excited electron of hydrogen atom in n = 6, drops to the ground state (n = 1)

Calculate the energy of radiation emitted for the electronic transition from infinity to ground state for hydrogen atom. Given c = 3xx10^(8)" ms"^(-1), R_(H) = 1.09678 xx 10^(7) m^(-1), h = 6.6256 xx 10^(-34)" J s"^(-1)

Based on the equation Delta E=-(2.0xx10^(-18)J) ((1)/(n_(2)^(2))-(1)/(n_(1)^(2))) the wavelength of the light that must be absorbed to excite hydrogen electron from level n=1 to level n=2 will be (Given : h=6.625xx10^(-34) J s, c=3xx10^(8) ms^(-1) )