The energy required to remove the electron from a singly ionized Helium atom is $2.2$ times the energy…
The energy required to remove the electron from a singly ionized Helium atom is $2.2$ times the energy required to remove an electron from Helium atom. The total energy required to ionize the Helium atom completely is:
$20 \mathrm{eV}$
$79 \mathrm{eV}$
$109 \mathrm{eV}$
$34 \mathrm{eV}$
Solution
Energy required to remove $\mathrm{e}^{-}$from singly ionized helium atom $=\frac{(13.6) Z^2}{1^2}=54.4 \mathrm{eV}$ $(\because \mathrm{Z}=2)$ Energy required to remove $\mathrm{e}^{-}$from helium atom $=x \mathrm{eV}$
According to question, $54.4 \mathrm{eV}=2.2 \mathrm{x} \Rightarrow \mathrm{x}$ $=24.73 \mathrm{eV}$
Therefore, energy required to ionize helium atom $=(54.4+24.73) \mathrm{eV}=79.12 \mathrm{eV}$