In Bohr's atomic model, the energy of the ele | vedclass

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(B) The energy of an electron in the $n^{th}$ orbit of a hydrogen-like atom is given by the formula: $E_n = -13.6 	imes \frac{Z^2}{n^2} 	ext{ eV}$.F

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$16E/9$

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(B) The energy of an electron in the $n^{th}$ orbit of a hydrogen-like atom is given by the formula: $E_n = -13.6 	imes \frac{Z^2}{n^2} 	ext{ eV}$.For the second orbit of a hydrogen atom $(Z=1, n=2)$: $E = -13.6 	imes \frac{1^2}{2^2} = -13.6 	imes \frac{1}{4} 	ext{ eV}$.Thus, $-13.6 	ext{ eV} = 4E$.For the third orbit of a helium atom $(Z=2, n=3)$: $E' = -13.6 	imes \frac{2^2}{3^2} = -13.6 	imes \frac{4}{9} 	ext{ eV}$.Substituting $-13.6 = 4E$ into the equation for $E'$:$E' = (4E) 	imes \frac{4}{9} = \frac{16E}{9}$.

In Bohr's atomic model, the energy of the electron is $E$ in the second orbit of a hydrogen atom. The energy of the electron in the third orbit of a helium atom $(Z = 2)$ will be:

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