The energy of the electron in the first orbit of He+ 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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-435.8 X 10^-20J

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-217.9 X 10^-20 J

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-108.9 X 10^-20 J

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Solution

The correct option is C
-217.9 X 10^-20 J

$E_{1 H e^{+}} = E_{1 H} \times z^{2}$

$- 871.6 \times 10^{- 20} = E_{1 H} \times 4$

$E_{1 H} = - 217.9 \times 10^{- 20} J$

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Similar questions

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

- 871.6 \times 10^{- 20} J

- 871.6 \times 10^{- 20} J

{H e}^{+}

- 871.6 \times 10^{- 20} J

{H e}^{+}

- 871.6 \times 10^{- 20} J

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