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Moseley's Law

the ground st...

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the ground state energy of hydrogen atom is -13.6 eV.If anelectron makes a tramnstion from an level of -1.51ev to-3.4eV calculate the wavelenght of spectral line emitted and name the seriesof hydrogen spectrum to ehich it belongs

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Q. The ground state energy of hydrogen atom is -13.6 eV. If an electron makes a transition from an energy level -1.51 eV to -3.4 eV, calculate the wavelength of the spectral line emitted and name the series of hydrogen spectrum to which it belongs.

Q. The ground state energy of hydrogen atom is

- 13.6 e V

. If an electron make a transition from an energy level

- 0.85 e V

- 1.51 e V

, calculate the wavelength of the spectral line emitted. To which series of hydrogen spectrum does this wavelength belong?

Q. The ground state energy of hydrogen atom is

- 13.6 e V

. If an electron makes a transition from an energy level

- 0.85 e V

- 3.4 e V

, calculate the wavelength of the spectral line emitted. To which series of hydrogen spectrum does the wavelength belong? (

R = 1.097 \times 10^{7} m^{- 1}

Q. Using Bohr's postulates, derive the expression for the frequency of radiation emitted when an electron in a hydrogen atom undergoes transition from a higher energy state (quantum number

n_{i}

) to a lower state,

(n_{f})

.
When an electron in a hydrogen atom jumps from energy state

n_{i} = 4

n_{f} = 3, 2, 1,

identify the spectral series to which the emission lines belong.

Q. The transition of an electron in hydrogen atom from fourth to first energy state emits a spectral line which falls in :

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