Chemistry · Bohr model of a hydrogen atom: its postulates, derivation of the relations for the energy of the electron and radii of the different orbits, limitations of Bohr's model
The energy of an electron in the first Bohr orbit is -13.6 ev then find the ener
The energy of an electron in the first Bohr orbit is -13.6 ev then find the energy of \( H e^{+} \) in the same Bohr orbit.
- A. 27.2 ev
- B. -27.2 ev
- C. 54.4 ev
- D. - 54.4 ev
Step-by-step solution
For hydrogen-like ions, the energy of an electron in the nth Bohr orbit is E = -13.6 * Z^2 / n^2 eV. For He⁺ (Z=2) in the first orbit (n=1), E = -13.6 * 4 / 1 = -54.4 eV.
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