Question 40 Arrange the various regions of the electromagnetic spectrum in the correct order, in order of increasing energy. O A. Ultraviolet < visible < infrared < microwave < radio B. Infrared < ultraviolet < visible < microwave < radio C. Microwave < infrared < visible < ultraviolet < radio D. Radio < microwave < infrared < visible < ultraviolet

Question 40 Arrange the various regions of the electromagnetic spectrum in the correct order, in order of increasing energy. O A. Ultraviolet < visible < infrared < microwave < radio B. Infrared < ultraviolet < visible < microwave < radio C. Microwave < infrared < visible < ultraviolet < radio D. Radio < microwave < infrared < visible < ultraviolet

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter5: Electron Configurations And The Periodic Table

Section: Chapter Questions

Problem 13QRT

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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?
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.)
Ozone absorbs energy with a frequency of 1.291015 s1. (a) What is the wavelength (in nm) of the absorption? (b) In what spectral range does the absorption occur? (c) What is the energy absorbed by one photon?
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?
The most prominent line in the spectrum of mercury is at 253.652 nm. Other lines are located at 365.015 nm, 404.656 nm, 435.833 nm, and 101.975 nm. (a) which of these lines represents the most energetic light? (b) what is the frequency of the most prominent line? What is the energy of one photon with this wavelength? (c) Are any of these lines found in the spectrum of mercury shown in figure 6.6? What color or colors are these lines?
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.
Estimate the probability of finding an electron which is excited into the 2s orbital of the H atom, looking in a cubical box of volume 0.751036m3 centered at the nucleus. Then estimate the probability of finding the electron if you move the volume searched to a distance of 105.8 pm from the nucleus in the positive z direction. (Note that since these volumes are small, it does not matter whether the volume searched is cubical or spherical.)
How does probability fit into the description of the atom?
Sketch the major features (number of peaks and relative intensities for the peaks) of the expected photoelectron spectrum for atoms of nitrogen.
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6.105 When we say that the existence of atomic spectra tells us that atoms have specific energy levels, are we using deductive or inductive reasoning?
What is the difference between an atom’s ground state and an excited state?