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    Wavelength of the transition

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    A hydrogen-like ion has a nucleus of charge +Ze and a single electron outside this nucleus. The energy levels of these ions are -ZsquaredRH/n2 (where Z = atomic number). Calculate the wavelength of the transition from n=3 to n=2 for He+, a hydrogen-like ion. In what region of the spectrum does this emission occur?

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    https://brainmass.com/physics/bohr-theory/wavelength-transition-17638

    Solution Preview

    E= h c R (Z ^2) / (n^2)

    h= Planck's constant= 6.6261x 10 ^(- 34) J s
    c=speed of light=3 x 10 ^ 8 m/s
    R=Rydberg constant= 1.09678 x 10 ^ 7 (m^ -1)

    hcR= 2.18021E-18 Joules
    This can also be ...

    Solution Summary

    This solution provides a calculation of wavelength of transition from n=3 to n=2 for He+, a hydrogen-like ion.

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