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

- 871.6 X 10^-20J

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- 435 X 10^-20J

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- 217.9 X 10^-20J

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- 108.9 XS 10^-20J

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Solution

The correct option is C - 217.9 X 10^-20J
$E_{H e^{+}} = E_{H} \times \frac{z^{2}}{n^{2}}$
$E_{H} = - 871.6 \times 10^{- 20} \times \frac{1^{2}}{4}$
$= - 217.9 \times 10^{- 20} J$

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

The correct option is C - 217.9 X 10-20JEHe+=EH×z2n2 EH=−871.6×10−20×124 =−217.9×10−20 J

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

The correct option is C - 217.9 X 10^-20J
$E_{H e^{+}} = E_{H} \times \frac{z^{2}}{n^{2}}$
$E_{H} = - 871.6 \times 10^{- 20} \times \frac{1^{2}}{4}$
$= - 217.9 \times 10^{- 20} J$