27. Refer to the handout "Reference Absorption Spectra."Which gases produced this spectrum?A. ironB. boronC. sulfurD. titanium

Option A: This option is incorrect because the spectrum shown does not match the known absorption…

Answered: 27. Refer to the handout "Reference…

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter5: Electrons In The Atom

Section: Chapter Questions

Problem 61A: What is the difference between an atom’s ground state and an excited state?

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Similar questions

When metallic sodium is dissolved in liquid sodium chloride, electrons are released into the liquid. These dissolved electrons absorb light with a wavelength near 800 nm. Suppose we treat the positive ions surrounding an electron crudely as defining a three-dimensional cubic box of edge L, and we assume that the absorbed light excites the electron from its ground state to the first excited state. Calculate the edge length L in this simple model.
Suppose an atom in an excited state can return to the ground state in two steps. It first falls to an intermediate state, emitting radiation of wavelength 1 , and then to the ground state, emitting radiation of wavelength 2 . The same atom can also return to the ground state in one step, with the emission of radiation of wavelength . How are 1,2, and related? How are the frequencies of the three radiations related?
The power output of a laser is measured by its wattage, that is, the number of joules of energy it radiates per second (1W=1Js1) . A 10-W laser produces a beam of green light with a wavelength of 520 nm (5.2107m) . (a) Calculate the energy carried by each photon. (b) Calculate the number of photons emitted by the laser per second.
Quantum mechanics predicts that the energy of the ground state of the H atom is 13.6eV . Insight into the magnitude of this quantity is gained by considering several methods by which it can be measured. (a) Calculate the longest wavelength of light that will ionize H atoms in their ground state. (b) Assume the atom is ionized by collision with an electron that transfers all its kinetic energy to the atom in the ionization process. Calculate the speed of the electron before the collision. Express your answer in meters per second (ms1) and miles per hour (milesh1) . (c) Calculate the temperature required to ionize a H atom in its ground state by thermal excitation. (Hint: Recall the criterion for thermal excitation of an oscillator in Planck’s theory of blackbody radiation is that hvkBT .)
Consider the transition from the energy levels n=2 to n=5. (a) What is the wavelength associated with this transition? (b) In what spectral region does the transition occur? (c) Is energy absorbed?
The following is an energy-level diagram for electronic transitions in the Bohr hydrogen atom. 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.
For the Li atom, the energy difference between the ground state and the first excited state, in which the outermost electron is in a 2p orbital, is 2.961019J . In the Li2+ ion, the energy difference between the 2s and 2p levels is less than 0.00002 of this value. Explain this observation.
Consider the representations of the p and d atomic orbitals in Figs. 2-15 and 2- 17. What do the + and signs indicate?
Write an acceptable electron configuration for these atoms, including ml and ms values. a Li b N c Ne d Sc
Using Table 5.2, write down the mathematical expression for the 2px wave function for an electronically excited H atom. Estimate the probability of finding the 2px electron if you look in a cubical box of volume of 0.8(pm)3 centered at a distance of 0.5001010m in the =/2 , =0 direction. Does this probability change as you change ? At what angles is the probability of finding the electron smallest and at what angles is the probability the largest? (Note that =2 is the same location as =0 , so don’t double count.)
What evidence do we have that energy levels in an atom are quantized? State and explain the evidence.
Section 11.6 uses a "firefly" analogy to illustrate how the wave mechanical modal for the atom differs from Bohr’s. model. Explain this analogy.

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27. Refer to the handout "Reference Absorption Spectra." Which gases produced this spectrum? A. iron B. boron C. sulfur D. titanium