The angular momentum of electron in a Bohr's orbit of H atom is `4.2178 xx 10^(-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 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.

Bohr.s theory explains that when Hydrogen-like particles are excited, their electrons are shifted higher energy orbits. As such a state of atom is not stable, electrons return to lower energy orbits releasing quantum of energy. Thus different spectral lines are formed. The wave number of spectral line is given by bar(v) = (2pi^(2)me^(4)z^(2))/(c h^(3))[(1)/(n_(1)^(2)-(1)/(n_(2)^(2)))] The angular momentum of an electron in a Bohr.s orbit of H-atom is 4.2178 xx 10^(-34) kg m^(2) sec^(-1) . What is the wave number of the spectral line emitted when electron falls from this level to the next lower level

The angular momentum of an electron in Bohr's orbit of H-atom is 3.02 xx 10^(-34) kg m^2 s^(-1) . Calculate the wavelength of the spectral line emitted when the electron jumps this level to the next lower level.

The orbital angular momentum of electron in 4s orbital of H atom is ……….

The orbital angular momentum of electron in 4s orbital of H atom is ……….