EBK PHYSICS FOR SCIENTISTS & ENGINEERS
5th Edition
ISBN: 9780134296074
Author: GIANCOLI
Publisher: VST
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An electron in a hydrogen atom makes a transition from the n=1 state to the n=3 state
(1eV= 1.6 x10^-19 J and h = 6.63 x 10^-34 J s= 4.136 x 10^-15 Ev/hz c =3.0 x10^8 m/s)
what is the energy of the photon absorbed in transition and what is the frequency of the absorbed photon energy?
An electron in a hydrogen atom makes a transition from the fifth excited state to n = 2.What are the frequency and wavelength of the emitted photon? (h = 4.136 x 10 -15 eV/Hz = 6.63 x 10 -34 J.s, c = 3.0 x 10 8 m/s, 1eV = 1.6 x 10 -19 J)
A mercury atom emits light at many wavelengths, two of which are at (1) 404.7 nm and (2) 435.8 nm . Both of these transitions are
to the same final state. Determine the energy of each emitted wavelength (in J).
A
E1 = 7.908 x 10-19 J and E2 = 6.558 x10-19 J
E1 = 4.628 x 10-19 J and E2 = 4.968 x10-19 J
E1 = 5.908 x 10-19 J and E2 = 5.558 x10-19J
E1 = 4.908 x 10-19 J and E2 = 4.558 x10-19 J
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- In the Hydrogen atom, an electron gains energy and moves from n=2 of energy -3.39 eV to n=3 of energy -1.51 eV. It is unstable and returns from n=3 to n=2. Calculate the frequency and the wavelength of the emitted photon. E = hf and h = 6.63 x 10-34arrow_forwardWhat are the (a) energy, (b) magnitude of the momentum, and (c) wavelength of the photon emitted when a hydrogen atom undergoes a transition from a state with n = 4 to a state with n = 2? (a) Number 2.55 Units eV (b) Number 1.3617 Units kg-m/s or N-s (c) Number 4.865976353 Units This answer has no unitsarrow_forwardUse the table to determine the energy in eV of the photon emitted when an electron jumps down from the n = 2 orbit to the n = 1 orbit of a hydrogen atom. Allowed Values of the Hydrogen Electron's Radius and Energy for Low Values of n n rn En 1 0.053 nm −13.60 eV 2 0.212 nm −3.40 eV 3 0.477 nm −1.51 eV 4 0.848 nm −0.85 eV eVarrow_forward
- A hydrogen atom emits a photon as it makes a transition from the n = 4 state to the n = 3 state. The energies of these two states are –0.9 eV and –1.5 eV, respectively.(a) What is the energy of the photon?(b) What is its frequency?arrow_forwardA hydrogen atom is initially in the n = 6 state. It drops to the n = 2 state, emitting a photon in the process. (a) What is the energy (in ev) of the emitted photon? 3.022 ev (b) What is the frequency (in Hz) of the emitted photon? 7.293e14 v Hz (c) What is the wavelength (in um) of the emitted photon? 41.14 umarrow_forwardUse the table to determine the energy in eV of the photon emitted when an electron jumps down from the n = 3 orbit to the n = 2 orbit of a hydrogen atom. Allowed Values of the Hydrogen Electron's Radius and Energy for Low Values of n n rn En 1 0.053 nm −13.60 eV 2 0.212 nm −3.40 eV 3 0.477 nm −1.51 eV 4 0.848 nm −0.85 eVarrow_forward
- A photon is absorbed by a hydrogen atom in the ground state. n=3 n=2 n=1 n=7 n=6 n=s n=4 n n 11=3 n=2 n=1 + E = 0 Es=-0.544 eV E4-0.850 eV E3 = -1.51 eV E2 = -3.40 eV E1-13.6 eV Ground state If the electron is boosted from to the n = 2, what was the energy of the photon? Give your answer in electron volts (eV). evarrow_forwardUse the table to determine the energy in eV of the photon absorbed when an electron jumps up from the n = 1 orbit to the n = 3 orbit of a hydrogen atom. Allowed Values of the Hydrogen Electron's Radius and Energy for Low Values of n n rn En 1 0.053 nm −13.60 eV 2 0.212 nm −3.40 eV 3 0.477 nm −1.51 eV 4 0.848 nm −0.85 eVarrow_forwardFigure below shows the energy levels of a hydrogen atom. Which transition produces radiation of wavelength 436 nm? (Given: Electron charge, e-1.602x10 19 C) n=00 O ev -0.54 ev n=5 n=4 -0.85 ev -1.51 eV n= 3 -3.39 ev n=1 -13.58 eV On=3 to n = 2 On=4 to n = 2 On=4to n = 1 On=5 to n- 2 Submit Answerarrow_forward
- b. An electron and a photon has the same wavelength of 0.21 nm. Calculate the momentum and energy (in eV) of the electron and the photon. (Given c =3.00x108 m s-1, h =6.63 x 1034 J s, me=9.11 x 10-31 kg, mp=1.67 x 1027 kg and e=1.60x1019 C)arrow_forwardA hydrogen atom emits a photon that has momentum 6.977 × 10-27 kg·m/s. This photon is emitted because the electron in the atom falls from a higher energy level into the n = 1 level. What is the quantum number of the level from which the electron falls? Use values of h = 6.626 × 10-34 J·s, c = 2.998 × 108 m/s, and e = 1.602 × 10-19 C.arrow_forwardA potential well has 4 energy levels as given here: Energy of the state (eV) 13 12 9 4 Suppose that there are three electrons in the well, and that the system is in the first excited state. If the system emits a photon, what energy could the photon have? O (a) 3 eV Ⓒ (b) 5 eV O (c) 4 eV O (d) 8 eV (e) 9 eV x X 0%arrow_forward
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