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What is the wavelength of light emitted ...

What is the wavelength of light emitted when the electron in a hydrogen atom undergoes transition from an energy level with n = 5 to an energy level with n = 3 ?

Text Solution

Verified by Experts

Formulae :
`barv=(1)/(lamda)=R[(1)/(n_(1)^(2))-(1)/(n_(2)^(2))]`
`=1,09,677[(1)/(3^(2))-(1)/(5^(2))]`
`=1,09,677[(25-9)/(9xx25)]`
`lamda=(1)/(barv)=(1)/(7799.25)=(1.2821xx10^(-4))cm`
`=12821Å`
`R=1,09,677cm^(-1)`
`n_(1)=3`
`n_(2)=3`
`n_(2)=5`
`barv=7799.25cm^(-1)`
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Knowledge Check

  • An electron in a hydrogen atom undergoes a transition from a higher energy level to a lower energy level. The incorrect statement of the following is .

    A
    Kinetic energy of the electron increases
    B
    Velocity of the electron increases
    C
    Angular momentum of the electron remains constant
    D
    Wavelength of de - Broglie wave associated with the motion of electron decreases.

  • The speed of the electron in a hydrogen atom in the n = 3 level is

    A
    `6.2 xx 10^(5) ms^(-1)`
    B
    `3.7 xx 10^(5) ms^(-1)`
    C
    `7.3 xx 10^(5) m^(-1)`
    D
    `1.6 xx 10^(5) ms^(-1)`

  • The frequency of light emitted, when the electron makes transition from the level of principle quantum number n = 2 to the level with n = 1 is (Take, the ionization energy of hydrogen to be 13.6eV andh =4xx 10 ^(-15) eV -s )

    A
    `2.55xx10^(15)Hz`
    B
    `1.7xx10^(15)Hz`
    C
    `3.4xx10^(15)Hz`
    D
    `5.1xx10^(15)Hz`

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