JEE MAIN - Physics (2018 - 15th April Morning Slot - No. 9)
The energy required to remove the electron from a singly ionized Helium atom is $$2.2$$ times the energies required to remove an electron from Helium atom. The total energy required to ionize the Helium atom completely is :
$$20$$ $$eV$$
$$34$$ $$eV$$
$$79$$ $$eV$$
$$109$$ $$eV$$
Explanation
Energy required to remove e$$-$$ from singly ionized Helium atom
E1 = $${{13.6{z^2}} \over {{n^2}}}$$ = $${{13.6 \times {2^2}} \over {{1^2}}}$$ = 54.4 eV.
Let, E2 = energy required to remove e$$-$$from He $$-$$ atom
$$\therefore\,\,\,\,$$ According to q vertion.
E1 = 2.2 E2
$$\therefore\,\,\,\,$$ E2 = $${{54.4} \over {2.2}}$$ = 24.72 eV
$$\therefore\,\,\,\,$$ Total energy required to ionize Helium atom completely
= (54.4 + 24.72) eV
= 79.12 eV
E1 = $${{13.6{z^2}} \over {{n^2}}}$$ = $${{13.6 \times {2^2}} \over {{1^2}}}$$ = 54.4 eV.
Let, E2 = energy required to remove e$$-$$from He $$-$$ atom
$$\therefore\,\,\,\,$$ According to q vertion.
E1 = 2.2 E2
$$\therefore\,\,\,\,$$ E2 = $${{54.4} \over {2.2}}$$ = 24.72 eV
$$\therefore\,\,\,\,$$ Total energy required to ionize Helium atom completely
= (54.4 + 24.72) eV
= 79.12 eV
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