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

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

CBSE | Chemistry | Class 11 | NCERT | Structure of Atom

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

The expression for the ionization energy is given by,

$E_{n} =\frac{-(2.18\times 10^{-18})Z^{2}}{n^{2}}$

Where Z denotes the atomic number and n is the principal quantum number

For the ionization from $n_{t}=5 to n_{2} =\infty$ ,

$\Delta E=E_{\infty }-E_{5 }$ = $[(\frac{-(2.18\times 10^{-18}\, J)(1)^{2}}{(\infty )^{2}})-(\frac{-(2.18\times 10^{-18}\, J)(1)^{2}}{(5 )^{2}})]$ = $0.0872\times 10^{-18}\, J$

$\Delta E=8.72\times 10^{-20}\, J$

Therefore, the required energy for the ionization of hydrogen from n = 5 to n = ∞ = Energy required for n1 = 1 to n = ∞, is $8.72\times 10^{-20}\, m \Delta E=E_{\infty }-E_{5 }$