The energy of $\mathrm{e}^{-}$ in first orbit of $\mathrm{He}^{+}$ is $-871.6 \times 10^{-20} \mathrm{~J}$.…

The energy of $\mathrm{e}^{-}$ in first orbit of $\mathrm{He}^{+}$ is $-871.6 \times 10^{-20} \mathrm{~J}$. The energy of $\mathrm{e}^{-}$ in first orbit of $\mathrm{H}$ is:
  1. $-871.6 \times 10^{-20}$
  2. $-435.8 \times 10^{-20} \mathrm{~J}$
  3. $-217.9 \times 10^{-20} \mathrm{~J}$
  4. $-108.9 \times 10^{-20}$

Solution

$\mathrm{E}_{1} \mathrm{He}^{+}=\mathrm{E}_{1} \mathrm{H} \times \mathrm{Z}^{2}$
$\therefore-871.6 \times 10^{-20}=\mathrm{E}_{1 \mathrm{H}} \times 4$
$\therefore \mathrm{E}_{1_{\mathrm{H}}}=-217.9 \times 10^{-20} \mathrm{~J}$ .

Asked in: JEE-TOPICTESTS-CHEMISTRY

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