The energy of electron of H atom is, `E_n = -(2.18xx10^-18)/n^2`J. How amount of energy is required to remove the electron from n = 2 orbit? What is the value of longest wave length of light required to remove this electron?

Energy of an electron in the n-th orbit of H-atom, E_(n)=(-2.17xx10^(-11))/(n^(2))erg . How much energy is required to remove the electron from its second orbit? Also calculate the wavelength of the light used for this process?

The electron energy is hydrogen atom is given by E"(n)=(-2.18xx10^(-18)) J . Calculate the energy required to remove an electron completely from the n=2 orbit. What is the longest wavelength of light in cm that can be used to cause this transition?

Calculate the minimum amount of energy requried to remove the electron from a hydrogen atom in its ground state.

If the binding energy of the electron in a hydrogen atom is 13.6 eV, what will be the energy required to remove the electron from the first excited state of Li^(++) ?

Energy required for the electron excitation in Li^(2+) from the first to the Bohr orbit is

The ionisation enthalpy of hydrogen atom is 1.312xx10^(6)J*mol^(-1) . The energy required to excited the electron in the atom from n=1 to n=2 is-

How much enerrgy is needed to ionise a H-atom if the electron occupies n=5 orbit? Compare your answer with the ionisation enthalpy of H-atom (energy required to remove the electron from n=1 orbit).

The electron energy in hydrogen atom is given by E=21.7XX10^-12/n^2 erg. What is the longest wavelength (in cm)of light that can be used to cause this transition?

According to Bohr's theory, energy of electron in n-th orbit of H-atom, E_(n)=-(21.76xx10^(-19))/(n^(2))J . Find the longest wavelength of radiation required to remove one electron from the 3rd orbit of He^(+) ion.

Calculate the energy required for promotion of electrons from the 1st to 5th Bohr orbit of all the atoms present in 1 mole of H-atoms.