This energy diagram shows the allowed energy levels of an electron in a certain atom or molecule: D energy Use this diagram to complete the table below. Which is the ground state? (pick one) e How many excited states are there? How many lines are in the absorption line spectrum? Which transition causes the absorption line at the shortest wavelength? Which transition causes the absorption line at the longest wavelength?

This energy diagram shows the allowed energy levels of an electron in a certain atom or molecule: D energy Use this diagram to complete the table below. Which is the ground state? (pick one) e How many excited states are there? How many lines are in the absorption line spectrum? Which transition causes the absorption line at the shortest wavelength? Which transition causes the absorption line at the longest wavelength?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter6: Electronic Structure And The Periodic Table

Section: Chapter Questions

Problem 63QAP: A carbon dioxide laser produces radiation of wavelength 10.6 micrometers (1micrometer=106meter)....

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Consider the following transitions 1. n=3 to n=1 2. n=2 to n=33. n=4 to n=34. n=3 to n=5(a) For which of the transitions is energy absorbed? (b) For which of the transitions is energy emitted? (c) Which transitions involve the ground state? (d) Which transition absorbs the most energy? (e) Which transition emits the most energy?
A carbon dioxide laser produces radiation of wavelength 10.6 micrometers (1micrometer=106meter). laser produces about one joule of energy per pulse, how many photons are produced per pulse? (c) Which transitions involve the ground state? (d) Which transition absorbs the most energy? (e) Which transition emits the most energy?
6.103 Atomic absorption spectroscopy is based on the atomic spectra of the elements being studied. It can be used to determine the impurities in a metal sample. If an element is present, light at the appropriate wavelength is absorbed. You are working with a metal stamping company and the rolled steel you use to form panels for automobile doors is failing at an alarming rate. There is some chance that the problem is unacceptably high levels of manganese in the steel. Given that the atomic spectrum of manganese has three lines near 403 nm, how could you use a spectrometer to determine the amount of manganese in the steel?
Using a simple particle-in-a-box model for the multiple bonding in 1,2-butadiene (see Example 4.7) and the n=2 wave function for the weakest bound electron, calculate the probability of finding the electron in an 0.1 interval centered midway between the two inner carbon atoms (that is, the center is at x=2.11 , so this interval is from x1=2.06 to x2=2.16 ). Then calculate the probability of finding the electron in an 0.1 interval centered midway between an end carbon atom and the carbon atom that is double-bonded to it in the Lewis dot structure. (You may calculate the appropriate integrals or estimate the relevant areas under the curve graphically.) Then recalculate the probabilities by approximating the integral as |( x 0)|2x , where x0 is evaluated in the middle of the range from x1 to x2 . Finally, explain why you can’t approximate the integral needed for Problem 37(a) in this way.
How many nodal planes exist for a 5d orbital? (a) 0 (b) 1 (c) 2 (d) 3
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.)
6.9 If a string of decorative lights includes bulbs with wave-lengths of 480, 580, and 700 mm, what are the frequencies of the lights? Use Figure 6.6 to determine which colors are in the set.
Consider a hydrogen atom in the ground state. What is the energy of its electron? ?= Now consider an excited‑state hydrogen atom. What is the energy of the electron in the ?=3n=3 level? ?3=
For each of the following electron configurations determine whether it is ground state, excited state or impossible. a. 1s22s32p1 b. 1s22s2 c. 1s22s2 d. 1s22s22p54f1 e. 1s22p2 f. 1s22s2 g. 2p63s13d1 h. 1s11p1
Which of these transitions do you expect to release the lowest energy photon? I II III
Consider the He atom with its two electrons. What are the possible excited states (i.e. terms) of He with one electron having n=1 and the other n=2. Explain
1-Which of the following molecules or ions is not polar? a.SO2 b.O3 c.S3 d.H2O e.I3− 2-Which of the following electron configurations represents an excited state? a.[Kr]4d105s25p1 b.[Ar]3d104s24p6 c.[Ne]3s23p5 d.[Ne]3s23p64s2 e.[Kr]4d105s15p1 3-What is the Aufbau ground state electron configuration for phosphorous? a.1s22s22p63s23p64s24p1 b.[Ne]3s13p4 c.[Ar]4s24p3 d.[Ne]3s23p3 e.1s22s22p63s23p5