The energy of electron in first orbit of ${\rm{H}}{{\rm{e}}^ + }$ is $\left( {{R_{\rm{H}}} = - 871.6 \times {{10}^{ - 20}}{\rm{\;J}}} \right).$ The energy of electron in the first orbit of H is:

$ - 217.9 \times {10^{ - 20}}\;{\rm{J}}$

$ - 871.6 \times {10^{ - 20}}\;{\rm{J}}$

$ - 435.8 \times {10^{ - 20}}\;{\rm{J}}$

$ - 108.9 \times {10^{ - 20}}\;{\rm{J}}$

NEET UG CHEMISTRY MCQ: STRUCTURE OF ATOM

1 Hard

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Application +4 | -1

The energy of electron in first orbit of

\mathrm{H}{\mathrm{e}^ + }

\left( {{R_\mathrm{H}} = - 871.6 \times {{10}^{ - 20}}\mathrm{\;J}} \right).

The energy of electron in the first orbit of H is:

View answer and explanation

Correct option: C

- 217.9 \times {10^{ - 20}}\;\mathrm{J}

Option C (

- 217.9 \times {10^{ - 20}}\;\mathrm{J}

) is correct because the energy of an electron is proportional to

Z^2

, where Z is the atomic number.

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