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The following is an energy-level diagram for electronic transitions in the Bohr hydrogen atom.
REFER IMAGE
a. Explain why the energy levels get closer together as they increase. Provide
mathematical support for this.
b. Verify that the colors given in the diagram are correct. Provide mathematical support.
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- 25. According to the image below answering all the questions. Each transition is labeled with a letter (A,B, etc) near its arrowhead. Each transition can be radiative, non-radiative, or both. (A) Select the arrow(s) that correspond to electronic excitation. (B) Select the arrow(s) that correspond to vibrational excitation. (C) Select the arrow(s) that correspond to IR absorption. (D) Select the arrow(s) that correspond to UV-visible absorption. (E) Select the arrow(s) that correspond to emission of a UV-visible photon. (F) Select the arrow(s) that correspond to thermal relaxation (non-radiative). (G) Select the arrow(s) that correspond to a chemical reaction (e.g. fragmentation). (H) Select the arrow(s) that correspond to intersystem crossing. All choosing options are the same as indicated below. -A -B -C -D -F -G -HIR Absorption takes into account a. The energy transitions between orbitals b. The energy transition from molecules in rotation motion c. The energy transition from molecules in translational motion d. Energy is absorbed in the substance being probedPlease explain and give the correct answer
- please help as soon as possibleThe energy levels for a Bohr atom are shown below. Use this diagram to solve problems 7 and 8. 0 eV -2.5 eV -4.0 eV -7.0 eV -12.5 eV 7. What amount of energy is needed for an electron to jump from n = 1 to n = 4? 8. What is the wavelength of the photon needed to make this happen? Is it emission or absorption?Which of these expressions would yield the wavelength of light in meters emitted when an electron drops from orbit n = 3 to n = 2 in a Bohr hydrogen atom? Given h = 4.14 x 10-15 eVs and c = 3.00 x 108 m/s. a. 1.89/hxc b. hc/1.89 c. 1.89 x h x c d. (1.51 + 3.4)/hc e. hc/3.4
- 1. Enumerate the microstates of p3. Determine the MS and ML values for each microstate. 2. On a table of possible MS and ML values, tally the microstates in no. 1 for a particular combination of MS and ML 3. Based on the table in no. 2, determine the atomic term symbols for the allowed atomic states of p3 resulting from the coupling of orbital and spin angular momentums. 4. Arrange the term symbols in no. 3 according to increasing energy.2. Consider the states of hydrogen atom given by (n, l, m) where n a. What is the maximum value of l? If L² is measured what is the maximum possible value that can be obtained? b. What is the maximum value of L₂?As shown a few energy levels of the mercury atom. One valence electron is always in the 6s state; the other electron changes states. Make a table showing all of the allowed transitions in the emission spectrum. For each transition, indicatea. The wavelength, in nm.b. Whether the transition is in the infrared, the visible, or the ultraviolet spectral region.c. Whether or not the transition would be observed in the mercury absorption spectrum.