EBK PHYSICS FOR SCIENTISTS & ENGINEERS
5th Edition
ISBN: 9780134296074
Author: GIANCOLI
Publisher: VST
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Chapter 39, Problem 5Q
To determine
The reason for the excited hydrogen and excited helium atoms to have very different
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Excited hydrogen and excited helium atoms both radiatelight as they jump down to the n=1,l=0 ,ml=0 state.Why do the two elements have very different emission spectra?
1) An electron is sitting in the -9eV energy level of the atom shown here. Which of the following photons would raise the electron up to the -2.5eV energy level?
163 nm
191 nm
248 nm
216 nm
The first five energy levels of the hydrogen atom are at n = 1, − 13.6 eV; n = 2, − 3.4 eV;n = 3, − 1.51 eV; n = 4, − 0.85 eV; n = 5, − 0.54 eV. A hydrogen discharge lamp givesan infrared spectrum that includes a sharp line at a wavelength of 4 µm, coming from electronsexcited by the discharge to a higher level, and then jump down to a lower level. Determine theenergy lost by these electrons, and identify the higher and lower levels involved.
Chapter 39 Solutions
EBK PHYSICS FOR SCIENTISTS & ENGINEERS
Ch. 39 - Prob. 2QCh. 39 - Prob. 3QCh. 39 - Prob. 4QCh. 39 - Prob. 5QCh. 39 - Prob. 6QCh. 39 - Prob. 7QCh. 39 - On what factors does the periodicity of the...Ch. 39 - Prob. 9PCh. 39 - Prob. 10PCh. 39 - Prob. 11P
Ch. 39 - Prob. 12PCh. 39 - Prob. 13PCh. 39 - Prob. 14PCh. 39 - Prob. 15PCh. 39 - Prob. 16PCh. 39 - Prob. 17PCh. 39 - Prob. 18PCh. 39 - Prob. 19PCh. 39 - Prob. 20PCh. 39 - Prob. 21PCh. 39 - Prob. 22PCh. 39 - Prob. 23PCh. 39 - Prob. 24PCh. 39 - Prob. 25PCh. 39 - Prob. 26PCh. 39 - Prob. 27PCh. 39 - Prob. 34PCh. 39 - Prob. 35PCh. 39 - Prob. 36PCh. 39 - Prob. 37PCh. 39 - Prob. 40PCh. 39 - Prob. 41PCh. 39 - Prob. 42PCh. 39 - Prob. 43PCh. 39 - Prob. 44PCh. 39 - Prob. 45PCh. 39 - Prob. 46P
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- Check Your Understanding When an election in a hydrogen atom is in the first excited state, what prediction does the Bohr model give about its orbital speed and kinetic energy? What is the magnitude of its orbital angular momentum?arrow_forwardWhat, if any, constraints does a value of m = 1 place on the other quantum numbers for an electron in an atom?arrow_forwardWhat are the possible values of m for an electron in the n = 4 state?arrow_forward
- 0arrow_forwardThe 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).arrow_forwardWhich of the following transitions in a hydrogen atom produces high frequency photons: n = 2 to n = 1 n =1 to n = ∞ n = ∞ to n =1n = 3 ton = 1 9:42 صarrow_forward
- How does the distance between adjacent orbits in a hydrogen atom vary with increasing values of the orbital number n? What should take place for a hydrogen atom to emit longest possible wavelength in Balmer series? Explain.arrow_forwardA hydrogen atom is in the ground state. It absorbs energy and makes نقطة واحدة a transition to the n = 3 excited state. The atom returns to the ground state by emitting two photons. What are their ?wavelengths None of these O 5.66x10^-7 m and 2.12x10^-7 m O 6.65×10^-7 m and 2.21×10^-7 m 6.56×10^-7 m and 1.22×10^-7 m Oarrow_forward- - - The first five energy levels of the hydrogen atom are at n 1, 13.6 eV; n = 2, 3.4 eV; n = 3, 1.51 eV; n = 4, -0.85 eV; n = 5, -0.54 eV. A hydrogen discharge lamp gives an infrared spectrum that includes a sharp line at a wavelength of 4 μm, coming from electrons excited by the discharge to a higher level, and then jump down to a lower level. Determine the energy lost by these electrons, and identify the higher and lower levels involved.arrow_forward
- 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.arrow_forwardWhat wavelength of light is emitted by a hydrogen atom in which an electron makes a transition from the n = 8 to the n = 5 state? Enter this wavelength expressed in nanometers. 1 nm = 1 x 10-9 m Assume the Bohr model.arrow_forwardIdentify the line with the smallest energy in the Balmer series. What is the energy of the emitted photon? Using the Bohr atom model for hydrogen, identify (by their quantum numbers) the electronic states that are involved in this transition (3p): Lyman Balmer Paschen +91.2 nm 121.6 nm + 364.7 nm +656.5 nm 820.6 nm + 1876.0 nmarrow_forward
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