JEE MAIN - Physics (2002 - No. 21)
If $$13.6$$ $$eV$$ energy is required to ionize the hydrogen atom, then the energy required to remove an electron from $$n=2$$ is
$$10.2$$ $$eV$$
$$0$$ $$eV$$
$$3.4$$ $$eV$$
$$6.8$$ $$eV.$$
Explanation
KEY CONCEPT :
The energy of nth orbit of hydrogen is given by
$${E_n} = {{13.6} \over {{n^2}}}eV/$$ atom
For $$n=2,$$ $${E_n} = {{ - 13.6} \over 4} = - 3.4eV$$
Therefore the energy required to remove electron from
$$n = 2$$ is $$+3.4eV.$$
The energy of nth orbit of hydrogen is given by
$${E_n} = {{13.6} \over {{n^2}}}eV/$$ atom
For $$n=2,$$ $${E_n} = {{ - 13.6} \over 4} = - 3.4eV$$
Therefore the energy required to remove electron from
$$n = 2$$ is $$+3.4eV.$$
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