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
Given that in the H-atom the transition energy for to Rydberg states in . The en
Given that in the H-atom the transition energy for \( n=1 \) to \( n=2, \) Rydberg states in \( 10.2 \mathrm{eV} \). The energy for the same transition in \( B e^{3+} \) is:
- A. 20.4 ev
- B. 163.2 eV
- C. 30.6 ev
- D. 40.8 ev
Step-by-step solution
For hydrogen-like ions, transition energy scales with Z^2. Since Be^3+ has Z=4, the energy is 4^2 = 16 times that of hydrogen: 10.2 eV × 16 = 163.2 eV.
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