9. Quantum Mechanics
Bohr Equation
08:10
Practice this topic
- Multiple Choice
What is the wavelength of a photon (in nm) absorbed during a transition from the n = 2 to n = 5 state in the hydrogen atom?
2648views7rank2comments - Multiple Choice
Determine the end (final) value of n in a hydrogen atom transition, if the electron starts in n = 5 and the atom releases a photon of light with an energy of 4.5738 × 10-19 J.
3150views1rank1comments - Multiple Choice
An electron releases energy as it moves from the 6th shell to the 3rd shell. If it releases 4.25 x 109 kJ of energy at a wavelength of 915.7 nm, how many photons were released in the process?
1975views2rank4comments - Textbook Question
Consider the three electronic transitions in a hydrogen atom shown here, labeled A, B, and C. (c) Calculate the wavelength of the photon emitted for each transition. Do any of these transitions lead to the emission of visible light? If so which one(s)?
Calculate the wavelength of the photon emitted for transition B.
968views - Textbook Question
Consider the three electronic transitions in a hydrogen atom shown here, labeled A, B, and C. (b) Calculate the energy of the photon emitted for each transition.
Calculate the energy of the photon emitted for transition C.
413views - Textbook QuestionCalculate the wavelength in nm of the light emitted when an electron makes a transition from an orbital in n = 5 to an orbital in n = 2 in the hydrogen atom. (LO 5.8)(a) 2.31 * 10-3 nm (b) 4.34 * 10-2 nm (c) 231 nm(d) 434 nm4435views
- Textbook Question
The visible emission lines observed by Balmer all involved nf = 2. (b) Calculate the wavelengths of the first three lines in the Balmer series—those for which ni = 3, 4, and 5—and identify these lines in the emission spectrum shown in Figure 6.11.
1281views - Multiple ChoiceUsing the Bohr equation, calculate the wavelength (in nm) for the electron transition from n=4 to n=1 in the Lyman series.662views