The angular momentum of an electron in Bohr's orbit of H-atom is `3.02 xx10^(-34) kgm^2s^-1`. Calculate the wavelength of the spectral line emitted when the electron jumps from this level to the next lower level.

The angular momentum of an electron in a Bohr's orbit of He^(+) is 3.1652xx10^(-34) kg- m^(2) /sec. What is the wave number in terms of Rydberg constant (R ) of the sepectral line emitted when an electron falls from this level to the first excited state.l [ Use h =6.626xx10^9-34) Js]

If the velocity of the electron in Bohr's first orbit is 2. 19 xx 10 ^(5) ms ^(-1). Calculate the de-Broglie wavelength associated with it .

Calculate the wavelength associated with an electron moving with a velocity of 10^(3) m s^(-1).

The mass of an electron is 9.1 xx 10 ^(-31) kg . If its K. E. is 3. 0 xx 10 ^(-25) J, calculate its wavelength.

The electron in given Bohr orbit has a total energy of -3.4 eV.Calculate its wavelength of the light eitted ,if an electron makes a transition to the ground state.(Ground state energy = -13.6 eV).

If the velocity of electron in bohr's is 3.5(10*6)ms-1, calculate the de broglie wavelength associated with it.

Calculate the de-Broglie wavelength for electron moving with speed of 6 xx 10^5 m s^(-1) .

The radius of 2nd Bohr's orbit of an electron in H - atom is 2.12 overset @A .Calculate th radius of 3 rd orbit of the same atom.

A difference of 2.3 eV separates two energy levels in an atom. What is the frequency of radiation emitted when the atom make a transition from the upper level to the lower level?