Horizons: Exploring the Universe (MindTap Course List)
14th Edition
ISBN: 9781305960961
Author: Michael A. Seeds, Dana Backman
Publisher: Cengage Learning
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Chapter 6, Problem 1LTL
To determine
The part of the spectrum emitted when an electron in a helium atom makes the same transition.
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Calculate the energy of the first 4 photons emitted in the balmer series of the hydrogen spectrum. The Balmer series corresponds to nf=2 and the first 4 photons are the lowest energy transitions from higher energy levels. These 4 photons all hvae a wavelength in the visible spectrum.
Chapter 6 Solutions
Horizons: Exploring the Universe (MindTap Course List)
Ch. 6 - Prob. 1RQCh. 6 - Prob. 2RQCh. 6 - Prob. 3RQCh. 6 - Prob. 4RQCh. 6 - Prob. 5RQCh. 6 - Prob. 6RQCh. 6 - Prob. 7RQCh. 6 - Prob. 8RQCh. 6 - Prob. 9RQCh. 6 - Prob. 10RQ
Ch. 6 - Prob. 11RQCh. 6 - How Do We Know? How is the world you see around...Ch. 6 - Prob. 1DQCh. 6 - Prob. 2DQCh. 6 - Prob. 1PCh. 6 - Prob. 2PCh. 6 - Prob. 3PCh. 6 - Prob. 4PCh. 6 - If one star has a temperature of 6000 K and...Ch. 6 - Prob. 6PCh. 6 - Prob. 7PCh. 6 - Prob. 8PCh. 6 - Prob. 1LTLCh. 6 - Prob. 2LTLCh. 6 - Prob. 3LTLCh. 6 - Prob. 4LTL
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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, physics and related others by exploring similar questions and additional content below.Similar questions
- Choose the correct statements concerning the elec- tromagnetic spectrum given off by stars. (Give ALL correct answers, i.e., B, AC, BCD...)A) If we see a blue star and a red star in a nearby star cluster, we know the red star is hotter.B) Blue photons are more energetic than red photons.C) Hot stars are much brighter than cool stars of the same size and distance from the Earth.D) Blue photons (blue light) have a longer wavelength than red photons.E) A hot star will be more red in color than a cooler star. F) All stars are the same color as our Sun.arrow_forwardStar X has lines of ionized helium in its spectrum, and star Y has bands of titanium oxide. Which is hotter? Why? The spectrum of star Z shows lines of ionized helium and also molecular bands of titanium oxide. What is strange about this spectrum? Can you suggest an explanation?arrow_forwardThe electron in a hydrogen atom makes a transition from the n = 4 state to the n = 2 state, as indicated in the image. (Figure 1) Determine the linear momentum of the photon emitted as a result of this transition. Figure Momentum of atom Electron jump > p = ΜΕ ΑΣΦ Submit Request Answer Part B ? kg. m/s Using your result to part A, find the recoil speed of the hydrogen atom, assuming it was at rest before the photon was emitted. v = ΜΕ ΑΣΦ Submit Request Answer Provide Feedback 1 of 1 Momentum of photon ? cm/s Next >arrow_forward
- answer for 3arrow_forwardSuppose we detect red photons at 656 nm emitted by electrons dropping from the n = 3 to the n = 2 orbital in hydrogen. The hydrogen is in an interstellar cloud at 5000k. If the cloud were heted to 10000 K, what would be the wavelength of the photons emitted by the transition? a) 328 nm b) 656 nm c) 1312 nm d) 658 nm e) 654 nmarrow_forwardPlease solve accurate. Thanksarrow_forward
- a) To which object corresponds this spectrum to? b) What is the source of radiation for each of the two humps? c) Why does the hump on the right hand side peak at higher wavelength than the hump on the left? [Specifically, what does this tell you about the temperature for each object that the light originates from?]arrow_forwardBriefly explain why the intensities of rotational spectral lines increase with increasing J and pass through a maximum before tailing off as J becomes large.arrow_forwardConsider a hydrogen atom is in its second excited state. Part (a) What is the shortest wavelength photon it can emit? Give your answer in nanometers. Part (b) What is the longest wavelength photon it can emit? Give your answer in nanometers.arrow_forward
- n = 5 n = 4 3. Refer to the illustration on the right. In a set of experiments on a hypothetical one-electron atom, you measure the wavelengths of the photons emitted from transitions ending in the ground state (n=1). You also observe that it takes 15 eV to ionize this atom. (a) What is the energy of the atom in each of the levels (i.e. n=1, n=2, n=3, n=4, n=5)? (b) If an electron made a transition from the n=4 to the n=2 level, what wavelength of light n = 3 n = 2 would it emit? n = 1 A = 73.86 nm A = 75.63 nm A=79.76 nm A = 94.54 nmarrow_forwardHow does one go about question b?arrow_forwardWhat is the photon frequency (Terahertz) needed to move an electron in a hydrogen atom from a lower energy level n; = 1 to a higher energy level nf = 5? (keep 3 decimal places)arrow_forward
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