The ionization energy of a singly ionized hel | vedclass

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(A) For a hydrogen-like species,the total energy of an electron in the $n^{th}$ orbit is given by $E_n = -13.6 	imes \frac{Z^2}{n^2} \ eV$. For $He^+

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Kinetic energy of the first orbit

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(A) For a hydrogen-like species,the total energy of an electron in the $n^{th}$ orbit is given by $E_n = -13.6 	imes \frac{Z^2}{n^2} \ eV$. For $He^+$,$Z = 2$ and for the ground state,$n = 1$. Thus,$E_1 = -13.6 	imes \frac{2^2}{1^2} = -54.4 \ eV$. The ionization energy $(IE)$ is the energy required to remove the electron,which is $-E_1 = 54.4 \ eV$. According to Bohr's model,the kinetic energy $(KE)$ of an electron in the $n^{th}$ orbit is equal to the magnitude of its total energy $(|E_n|)$. Therefore,$IE = |E_1| = KE_1$.

The ionization energy of a singly ionized helium ion $(He^+)$ is equal to:

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