(B) The energy of an orbit in a hydrogen-like species is given by the formula: $E_n = -13.6 \times \frac{Z^2}{n^2} \, eV$. For $He^{+}$,the atomic num

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(B) The energy of an orbit in a hydrogen-like species is given by the formula: $E_n = -13.6 \times \frac{Z^2}{n^2} \, eV$. For $He^{+}$,the atomic number $Z = 2$. For the first orbit $(n = 1)$: $E_1 = -13.6 \times \frac{2^2}{1^2} = -13.6 \times 4 = -54.4 \, eV$. For the second orbit $(n = 2)$: $E_2 = -13.6 \times \frac{2^2}{2^2} = -13.6 \times \frac{4}{4} = -13.6 \, eV$.

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

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If the energy of the first orbit of $He^{+}$ is $-54.4 \, eV$,then the energy of the second orbit will be ............. $eV$.

A
$-54.4$
B
$-13.6$
C
$-27.2$
D
$+27.2$

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Structure of Atom

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If the energy of the first orbit of $He^{+}$ is $-54.4 \, eV$,then the energy of the second orbit will be ............. $eV$.

Similar Questions

Calculate the energy associated with the second orbit of $Li^{+}$ and find its radius.

In which one of the following pairs of experimental observations and phenomena does the experimental observation correctly account for the phenomenon?

What is the ratio of the wave number of the first line (lowest energy line) of the Balmer series of the $H$ atomic spectrum to the first line of its Brackett series?

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