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:
- A$-2.18 \times 10^{-18} \text{ J}$
- B$-4.36 \times 10^{-18} \text{ J}$
- C$-0.545 \times 10^{-18} \text{ J}$
- D$-0.273 \times 10^{-18} \text{ J}$
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