Which electronic transition in a hydrogen atom, starting from the orbit n=7, will produce infrared light of wavelength 2170 nm?
`(Given: R_(H)=1.09677xx10^(7)M^(-1))`

In a hydrogen atom, an electron jumps from third orbit to the first orbit. Find out the frequency and wavelength of the spectral line. Given R=1.097xx 10^(7) m^(-1)

In a hydrogen atom, an electron jumps from the third orbit to the first orbit. Find out the frequency and wavelength of the spectral line. (R_(H)=1.09678xx10^(7)m^(-1)) .

Find the quantum of the excited state of electrons in He^(+) ion which on transition to first excited state emit photons of wavelengths 108.5 nm . (R_(H)=1.09678xx10^(7) m^(-1))

Find the quantum of the excited state of electrons in He^(+) ion which on transition to first excited state emit photons of wavelengths 108.5 nm . (R_(H)=1.09678xx10^(7) m^(-1))

What is the energy difference and the frequancy and the wavelength of light emitted when the electron in a hydrogen atom undergoes transition from the energy level n = 4 to the energy n = 3 given that the value of Rydberg constant is 1.0974 xx 10^(7)m^(-1) ?

What is the energy difference and the frequency of light emitted when the electron in a hydrogen atom undergoes transition from the energy level n = 4 to the energy n = 3 given that the value of Rydberg constant is 1.0974 xx 10^(7)m^(-1) ?

If an electron transits from n = 7 to n = 1 in a hydrogen atom then the maximum number of spectral lines that can form will be?