Concept explainers
The transition that results in the spectral lines.
Answer to Problem 65P
The transition from
Explanation of Solution
Given data:
The given values of the wavelength
Formula:
The expression to determine the energy
The expression to determine the wavelength of the
The expression for the energy difference
Calculation:
The expression for the energy difference
The wavelength of the
Solve further as,
From above the table for the values of the final energy state for different values of the initial energy state is shown in Table 1
The required table is shown in Table 1
Table 1
From above table it is clear that the transition is produced from state
The state of transition when the for wavelength of
From above the table for the values of the final energy state for different values of the initial energy state is shown in Table 2
The required table is shown in Table 2
Table 2
From above table it is clear that the transition is produced from state
The state of transition when the for wavelength of
From above the table for the values of the final energy state for different values of the initial energy state is shown in Table 3
The required table is shown in Table 3
Table 3
From above table it is clear that the transition is produced from state
Conclusion:
Therefore, the transition from
Want to see more full solutions like this?
Chapter 36 Solutions
Physics for Scientists and Engineers, Vol. 3
- For an electron in a hydrogen atom in the n=2 state, compute: (a) the angular momentum; (b) the kinetic energy; (c) the potential energy; and (d) the total energy.arrow_forwardMeasurements indicate that an atom remains in an excited state for an average time of 50.0 ns before making a transition to the ground state with the simultaneous emission of a 2.1-eV photon. (a) Estimate the uncertainty in the frequency of the photon. (b) What fraction of the photon's average frequency is this?arrow_forwardA researcher observes hydrogen emitting photons of energy 1.89 eV. What are the quantum numbers of the two states involved in the transition that emits these photons?arrow_forward
- Consider only the transitions involving the first four energy levels for a hydrogen atom:a. How many emissions are possible for an electron in the n = 4 level as it goes tothe ground state?b. Which electronic transition is the lowest energy?c. Which electronic transition corresponds to the shortest wavelength emissionarrow_forwardA collection of atoms has 20% of the sample in a state 7.60 eV above the ground state. If these emit coherent radiation, what is the wavelength of the laser light produced in nanometers? (c = 3.00 × 108 m/s, h = 6.626 × 10-34 J ∙ s, 1 eV = 1.60 × 10-19 J) Give your answer as a whole number.arrow_forwardA photon with a wavelength of 410 nm has energy Ephoton = 3.0 eV. Do you expect to see a spectral line with λ = 410 nm in the emission spectrum of the atom represented by this energy-level diagram? If so, what transition or transitions will emit it? Do you expect to see a spectral line with λ = 410 nm in the absorption spectrum? If so, what transition or transitions will absorb it?arrow_forward
- Light of wavelength 121.6 nm is emitted by a hydrogen atom. What are the (a) higher quantum number and (b) lower quantum number of the transition producing this emission? (c) What is the name of the series that includes the transition?arrow_forwardConsider only transitions involving the n = 1 through n = 4 energy levels for the hydrogen atom (see Figures 6.7 and 6.10). (a) How many emission lines are possible, considering only the four quantum levels? (b) Photons of the lowest enerrgy are emitted in a transition from the level with n = _ _ _ _ to a level with n = _ _ _ _ (c) The emission line having the shortest wavelength corresponds to a transition from the level with n = _ _ _ _ to the level with n =arrow_forwardDetermine the wavelength if the electron is excited n=2 for Helium (Z=2).( E=(-13.6ev)Z2/n2 and 1/mu=1/hc(En-En-1)arrow_forward
- A hypothetical atom has two energy levels, with a transition wavelength between them of 580 nm. In a particular sample at 300 K, 4.0 * 10^20 such atoms are in the state of lower energy. (a) How many atoms are in the upper state, assuming conditions of thermal equilibrium? (b) Suppose, instead, that 3.0*10^20 of these atoms are “pumped” into the upper state by an external process, with 1.0 * 10^20 atoms remaining in the lower state. What is the maxi-mum energy that could be released by the atoms in a single laser pulse if each atom jumps once between those two states (either via absorption or via stimulated emission)?arrow_forwardThe longest wavelength line of the Balmer Series for hydrogen occurs at 656.3 nm corresponding to the transition from n2 = 3 to n1 = 2. Determine the value for the Rydberg constant for hydrogen using these values.arrow_forwardWhat is the energy of the photon that, when absorbed by a hydrogen atom, could cause an electronic transition from the n = 2 state to the n = 5 state? Answer in units of eV.arrow_forward
- Principles of Physics: A Calculus-Based TextPhysicsISBN:9781133104261Author:Raymond A. Serway, John W. JewettPublisher:Cengage LearningGlencoe Physics: Principles and Problems, Student...PhysicsISBN:9780078807213Author:Paul W. ZitzewitzPublisher:Glencoe/McGraw-HillModern PhysicsPhysicsISBN:9781111794378Author:Raymond A. Serway, Clement J. Moses, Curt A. MoyerPublisher:Cengage Learning
- University Physics Volume 3PhysicsISBN:9781938168185Author:William Moebs, Jeff SannyPublisher:OpenStaxCollege PhysicsPhysicsISBN:9781305952300Author:Raymond A. Serway, Chris VuillePublisher:Cengage LearningCollege PhysicsPhysicsISBN:9781285737027Author:Raymond A. Serway, Chris VuillePublisher:Cengage Learning