The angular momentum of the electron in a Boh'r orbit of hydrogen atom is `4.2178xx10^(-34)kg*m^(2)*s^(-1)`. Calculate the wavelength of the spectral line when the electrton falls from this level to the next lower level

The angular momentum of an electron in a Bohr's orbit of hydrogen atom is 3.1655xx10^(-34)kg*m^(2)*s^(-1) . Calculate the wavelength of the spectral line emitted when an electron falls from this level to the next lower level.

The angular momentum of an electron present in a Bohr orbit is 3.1655xx10^(-34)kg*m^(2)*s^(-1) . What will be the wavelength of the spectral line produced when the electron jumps to the adjacent orbit with lowest radius?

The angular momentum of an electron in a Bohr's orbit of He+ is 3.1652xx10^-34 kg-m^2/sec what is the wavenumber in terms of Rydberg constant of the spectral line emitted when an electrons falls from this level to the first excited state [h= 6.626xx10^-34 Js]

if the velocity of the electron in Bohr's first orbit is 2.19xx10^(6)m*s^(-1) , calculate the de Broglie wavelength associated with it.

An electron in a Bohr orbit of hydrogen atom in quantum level n_2 has an angular momentum of 4.2176xx10^-34 kgm^2s^-1 . If this electron drops from this level to the next lower level, find the wavelength of this spectral line.

An electron is in the third orbit of a hydrogen atom. If h =6.6 xx10^(-34) J *s , its orbital angular momentum is

Angular momentum of an electron in an orbit hydrogen atom is 4.2xx10^(-34) J*s . What is the energy of that electron in that orbit? Given mass of an electron = 9.1xx10^(-31)kg ,e=1.6xx10^(-19)C,1eV=1.6xx10^(-19) erg .

Calculate the wavelength of an electron moving with a velocity of 2.05xx10^(7)m*s^(-1) .

Name the series of spectral lines obtained, when electrons from various energy levels jump to the first orbit in hydrogen.

The orbital angular momentum of the earth with respect to the sun divided by the mass of the earth is 4.4xx10^(15)m^2*s^(-1) . Determine the area enclosed by the orbit of the earth.