(D) The energy of an electron in the $n^{th}$ Bohr orbit of a hydrogen-like species is given by the formula: $E_n = -13.6 \times \frac{Z^2}{n^2} \ eV$

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(D) The energy of an electron in the $n^{th}$ Bohr orbit of a hydrogen-like species is given by the formula: $E_n = -13.6 \times \frac{Z^2}{n^2} \ eV$. For the first Bohr orbit of $He^{+}$,we have $n = 1$ and the atomic number $Z = 2$. Substituting these values into the formula: $E_1 = -13.6 \times \frac{2^2}{1^2} \ eV = -13.6 \times 4 \ eV = -54.4 \ eV$.

Class 11 Chemistry Structure of Atom Atomic models and Planck's quantum theory

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The energy of an electron in the first Bohr orbit of the hydrogen atom is $-13.6 \ eV$. Calculate the energy of an electron in the first Bohr orbit of $He^{+}$ in $eV$.

A
$27.2$
B
$-27.2$
C
$54.4$
D
$-54.4$

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Structure of Atom

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Atomic models and Planck's quantum theory

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The energy of an electron in the first Bohr orbit of the hydrogen atom is $-13.6 \ eV$. Calculate the energy of an electron in the first Bohr orbit of $He^{+}$ in $eV$.

Similar Questions

If the ionization energy of a hydrogen atom is $E$,then the ionization energy of $Li^{2+}$ will be ............ $E$.

Which electron transition in a hydrogen atom requires the largest amount of energy?

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For the $H$ spectrum,the limiting line in the $Balmer$ series has a frequency of ...... $(R_\infty = 3.29 \times 10^{15} \text{ cycles/s})$

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