A hydrogen atom in an excited state emits a photon of wavelength 95 nm. What are the initial and final states of the hydrogen atom?
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A: we know.energy emitted by photon:E=hcλ=E4-E2
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Q: A line of the Lyman series(nf=1) of the spectrum of hydrogen has a wavelength of 95nm. What was the…
A: Wavelength of spectrum λ = 95 nm lower state nf= 1 we have to find out upper state ni
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Q: A hydrogen atom in its n = 9 state is ionized by absorbing a 109 nm photon. If all the excess energy…
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Q: A hydrogen atom emits a photon of wavelength 486 nm. From what energy orbit to what lower energy…
A: Given, Wavelength = 486nm. ninitial =? nfinal =?
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Q: A hydrogen atom in its n = 4 state is ionized by absorbing a 268 nm photon. If all the excess energy…
A: Given that the wavelength of the photon is 268 nm. So, the energy obtained by absorbing a photon is…
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Q: A hydrogen atom in an n=2 state absorbs a photon.What wavelength photons might be emitted by the…
A: Let's proceed with the calculations:1. \( \lambda_1 = \frac{{100 \times 3^2}}{{3^2 - 2^2}} =…
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Q: The energy of a photon (hydrogen) emitted in a transition from the n = 3 to the n = 2 state is
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A: Given, Potential energy of electron proton in an atom, U = 15.4 eV 1 eV = 1.6×10-19 C
Q: In state n=1, the energy of the hydrogen atom is -13.58eV. What is its energy in state n=2?
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Q: An electron is in an f state. Can it undergo a quantum jump to an s state? A p state? A d state?…
A: To determine: Whether an electron in f-state can undergo a quantum jump to s-state, p-state, d-state…
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- What wavelength of light is emitted by a hydrogen atom in which an electron makes a transition from the n = 7 to the n = 4 state? Enter this wavelength expressed in nanometers. 1nm = 1 x 10-9m. Assume the Bohr model.The energy difference between the 1st excited state (n = 2) and the 2nd excited state (n = 3) in the hydrogen atom is 1.9 eV, what is the wavelength of the emission line resulting from the electron transitions between those two levels? Give your answer in units of nanometers (nm).Chapter 39, Problem 044 A hydrogen atom in a state having a binding energy (the energy required to remove an electron) of -1.51 eV makes a transition to a state with an excitation energy (the difference between the energy of the state and that of the ground state) of 10.200 eV. (a) What is the energy of the photon emitted as a result of the transition? What are the (b) higher quantum number and (c) lower quantum number of the transition producing this emission? Use -13.60 eV as the binding energy of an electron in the ground state. (a) Number Units (b) Number Units (c) Number Units
- The L series of the characteristic x-ray spectrum of tungsten contains wavelengths of 0.1099 nm and 0.1282 nm. The L-shell ionization energy is 11.544 keV. Which x-ray wavelength corresponds to an N → L transition? Determine the ionization energies of the M and N shells: If the incident electrons were accelerated through a 40.00 keV potential difference before striking the target, find the shortest wavelength of the emitted radiation:An electron in a hydrogen atom is excited from the ground state to the n = 3 state. True or false?a) The wavelength of light emitted when the electron drops from n=3 to n = 1 is longer than that from n = 3 to n = 2.A 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?