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Q.

The energy of the electron in the first orbit of He⁺ is -871.6x10^-20 J . The energy of the electron in the first orbit of hydrogen would be

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a

${−871.6×10}^{- 20} J$

b

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

c

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

d

$- 108 .9 \times 10^{- 20} J$

answer is C.

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Detailed Solution

$E_{1 {He}^{+}} = E_{1 H} \times z^{2}$
$- 871 .6 \times 10^{- 20} = E_{1 H} \times 4$
$E_{1 H} = - 217 .9 \times 10^{- 20} J$

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The energy of the electron in the first orbit of He+ is -871.6x10-20 J . The energy of the electron in the first orbit of hydrogen would be