When a hydrogen atom makes the transition from the second excited state to the ground state (at -13.6 eV) the energy of the photon emitted is:
Correct answer: D. 12.1 eV
- A. 0
- B. 9.1 eV
- C. 1.5 eV
- D. 12.1 eV
Explanation
2nd excited means 3rd energy level (n = 3). Ground state is −13.6 eV.Energy of emitted photon = E_initial − E_final= (−1.51 eV) − (−13.6 eV)= 13.6 − 1.51≈ 12.1 eVSo the photon carries about 12.1 eV of energy.
Report an error
The more specific you are, the faster it gets fixed. A source beats an opinion.
Prefer email? [email protected]
About Atomic Spectra
Atoms emit or absorb light at specific wavelengths because electrons occupy quantized energy levels and change levels by absorbing or releasing photons. The topic covers emission and absorption spectra, spectral series, hydrogen’s line spectrum, energy-level transitions, and the relation between wavelength, frequency and photon energy.
Practise Atomic Spectra
356 free Atomic Spectra MCQs from Physics, each with the correct answer and an explanation. Unlimited attempts, no account needed.
Discussion
Stuck on an option, or know a faster way to get there? Ask or explain it here.
No comments yet. Be the first to explain this one.
Exams that ask Physics questions like this
Physics is on 16 papers prepared for on TestUstad, and all of them draw the same bank, so this question is worth knowing for every one of them.
More Atomic Spectra questions
The diagram shows the graphs of the stopping potential as a function of the frequency of the incident light for photoelectric experiments performed on three different materials. Rank the materials according to the values of their work functions, from least to greatest.
The longest wavelength radiations in Paschen series have wavelength equal to:
In Balmer series the shortest wavelength radiations have wavelength equal to:
The maximum wavelength in the Brackett series is given by:
If wave number is RH/9, the corresponding series is:
The radiations of which spectral series are more energetic than others?