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The energy of n^(th) orbit is given by ...

The energy of `n^(th)` orbit is given by
`E_(n) = ( -Rhc)/(n^(2))`
When electron jumpsfrom one orbit to another orbit then wavelength associated with the radiation is given by
`(1)/(lambda) = RZ^(2)((1)/(n_(1)^(2)) - (1)/ (n_(2)^(2)))`
When electron of 1.0 gm atom of Hydrogen undergoes transition giving the spectral line of lowest energy is visible region of its atomic spectra, the wavelength of radiation is

A

`6489Å`

B

`3640Å`

C

`5000Å`

D

`4312Å`

Text Solution

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The correct Answer is:
A
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Knowledge Check

  • The energy of n^(th) orbit is given by E_(n) = ( -Rhc)/(n^(2)) When electron jumpsfrom one orbit to another orbit then wavelength associated with the radiation is given by (1)/(lambda) = RZ^(2)((1)/(n_(1)^(2)) - (1)/ (n_(2)^(2))) The series that belongs to visible region is

    A
    Lyman Series
    B
    Balmer Series
    C
    Pfund Series
    D
    Humphrey Series

  • The energy of n^(th) orbit is given by E_(n) = ( -Rhc)/(n^(2)) When electron jumps from one orbit to another orbit then wavelength associated with the radiation is given by (1)/(lambda) = RZ^(2)((1)/(n_(1)^(2)) - (1)/ (n_(2)^(2))) The ratio of wavelength H_(alpha) of Lyman Series and H_(alpha) of Pfund Series is

    A
    `54.7 :1`
    B
    `0.0183 :1`
    C
    `61.4 :1`
    D
    `0.0163 :1`

  • When an electron jumps from n_(1) th orbit to n_(2) th orbit, the energy radiated is given by

    A
    `h v = E_(1)//E_(2)`
    B
    `h v = E_(2)//E_(1)`
    C
    `h v = E_(1) - E_(2)`
    D
    `h v = E_(2) - E_(1)`