Question:medium
In hydrogen atom, an electron is transferred from an orbit of radius $1.3225$ nm to another orbit of radius $0.2116$ nm. What is the energy (in J) of emitted radiation? (Rydberg constant $R_H \approx 1.097 \times 10^7 \text{ m}^{-1}$)
In hydrogen atom, an electron is transferred from an orbit of radius $1.3225$ nm to another orbit of radius $0.2116$ nm. What is the energy (in J) of emitted radiation? (Rydberg constant $R_H \approx 1.097 \times 10^7 \text{ m}^{-1}$)
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The radius of the $n^{th}$ orbit in a hydrogen atom is $r_n = n^2 a_0$. For an electron transition, the energy of the emitted/absorbed photon is $E = 13.6 \left|\frac{1}{n_f^2} - \frac{1}{n_i^2}\right| \text{ eV}$. To convert to Joules, multiply by $1.602 \times 10^{-19} \text{ J/eV}$.
Updated On: Mar 30, 2026
- $1.635\times 10^{-18}$
- $3.027\times 10^{-19}$
- $4.087\times 10^{-19}$
- $0.4578\times 10^{-18}$
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The Correct Option is D
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