Hydrogen Spectrum

Chemistry Level 2

A series of lines in the spectrum of atomic Hydrogen lies at wavelength range 656.46 nano meters ........... 410.29 nano meters (these are the two extreme values).What will be the wavelength of the next line in the series? Give your answer in nano meters.

Given : Rydberg Constant is $1.095 \times 10^{7} m^{-1}$

397 320 300 353

1 solution

Adhiraj Mandal
Oct 1, 2014

The visible spectrum lies in the range $4 \times 10^{-7}$ meters to $7.5 \times 10^{-7}$ meters.The given wavelengths fall in this range and hence are visible.Therefore this ranger fall in the Balmer Series (the only visible series).Therefore we get n1=2 and for the wavelength 410.29 nano meter n2=6.(Where transition of electron is from n1 to n2).Therefore the wavelength corresponds to transition from n1=2 to n2=7.Solving we get the wavelength of the next line is 397 nano meters.

@Adhiraj Mandal, Balmer series is the name given to a series of spectral emission lines of the Hydrogen atom that result from the electron transitions from higher energy level with principal quantum number 6 down to the energy level with principal quantum number 2. There are four transitions that are visible in the optical waveband that are empirically given by Balmer formula with maximum $n_2=6$ and not $n_2=7$ .

Winod DHAMNEKAR - 1 year, 4 months ago

Hydrogen Spectrum

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