The energy of an electron in the first orbit of $H e^{+}$ is $- 871.6 \times 10^{- 20} J$ . The energy of the electron in the first orbit of hydrogen would be:

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Solution

$E_{n} = - 2.18 \times (z^{2} / n^{2}) J$
for $H e^{+}$ atom z value is 2
and energy for H atom of first orbit $= - 2.18 \times 10^{- 18} J$
this value is also calculated by energy of an electron in the first orbit of $H e^{+}$ dividing by $2^{2}$ or 4.
$E_{1}$ H atom $= - 871.6 \times 10^{- 20} J / 4 = - 2.18 \times 10^{- 18} J$

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The energy of an electron in the first orbit of He+ is −871.6×10−20J. The energy of the electron in the first orbit of hydrogen would be:

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