If the energy of an electron in the first Boh | vedclass

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(C) The energy of an electron in the $n^{th}$ orbit of a hydrogen-like atom is given by the formula: $E_n = -2.18 	imes 10^{-18} 	imes \frac{Z^2}{n^

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$-0.545 	imes 10^{-18} 	ext{ J}$

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(C) The energy of an electron in the $n^{th}$ orbit of a hydrogen-like atom is given by the formula: $E_n = -2.18 	imes 10^{-18} 	imes \frac{Z^2}{n^2} 	ext{ J}$.For the $H$-atom, the atomic number $Z = 1$.For the first orbit $(n = 1)$, $E_1 = -2.18 	imes 10^{-18} 	imes \frac{1^2}{1^2} = -2.18 	imes 10^{-18} 	ext{ J}$.For the second orbit $(n = 2)$, $E_2 = -2.18 	imes 10^{-18} 	imes \frac{1^2}{2^2} = -2.18 	imes 10^{-18} 	imes \frac{1}{4} 	ext{ J}$.$E_2 = -0.545 	imes 10^{-18} 	ext{ J}$.

If the energy of an electron in the first Bohr orbit of the $H$-atom is $-2.18 \times 10^{-18} \text{ J}$, then the energy of the electron in the second orbit will be:

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