To which orbit the electron in the hydrogen atom (ground state) will jump of absorbing `2.044xx10^(-18)J` of energy.

The electron energy of hydrogen atom in the ground state works out to be - 2.18 xx 10^(-18) J per atom. Calculate what will happen to the position of the electron in this atom if an energy of 1.938 xx 10^(-18) J is supplied to the each hydrogen atom.

What is the energy in joules, requried to shift the electron of the hydrogen atom from the first Bohr orbit to the fifth Borh orbit and what is the wavelength of the light emitted when the electron returns to the ground state? The ground state electron energy is -2.18xx10^(-11) erg.

What is the energy in joules required to shift the electron of a hydrogen atom from first Bohr orbit to fifth Bohr orbit and what is the wavelength of the light emitted when the electron returns to the ground state?the ground state electron energy is -2.18x10^(-11) erg.

Total energy of an electron in a ground state of hydrogen atom will be—

What is the electron velocity in the second orbit of hydrogen atom ?

The total energy of an electron in the ground state , of hydrogen atom is

Calculate the wave length in.angsfrom of the photon emitted when an electron returns to 2nd orbit from third orbit in the hydrogen atom. Given ionisation energy of hydrogen = 2.17 xx 10^(-11) erg /atom , h = 6.62 xx 10^(-27) erg sec.

Energy of electron is given by E=-2.178xx10^(-18)((Z^(2))/(n^(2))) J. Wavelength of light required to excited an electron in an hydrogen atom from level n=1 to n=2 will be (h=6.62xx10^(-34)J*s and c=3.0xx10^(8)m*s^(-1)) -

Find the wavelength (in angstrom) of the photon emitted when an electron jumps from the second Bohr orbit to the first bohr orbit of hydrogen atom. Ionisation potential of hydrogen atom in its ground energy state =2.17xx10^(-11) erg *"atom"^(-1)

The radius of the orbit of an electron in the ground state of hydrogen atom is a_0 . Then