Question 3 Which of the following statements is true about the visible electromagnatic radiation? O it is only a small portion of the entire electromagnetic spectrum and it includes the colors commonly observed its wavelengths range from 400 nm to nearly 800 nm. the mixture of all visible electromagnetoc radiation is observed as white light. O UV and IR are common examples of visible electromagnetic radiation

Question 3 Which of the following statements is true about the visible electromagnatic radiation? O it is only a small portion of the entire electromagnetic spectrum and it includes the colors commonly observed its wavelengths range from 400 nm to nearly 800 nm. the mixture of all visible electromagnetoc radiation is observed as white light. O UV and IR are common examples of visible electromagnetic radiation

Organic Chemistry

9th Edition

ISBN:9781305080485

Author:John E. McMurry

Publisher:John E. McMurry

Chapter12: Structure Determination: Mass Spectrometry And Infrared Spectroscopy

Section12.5: Spectroscopy And The Electromagnetic Spectrum

Problem 6P

See similar textbooks

Similar questions

When a tube containing hydrogen atoms is energized by passing several thousand volts of electricity into the tube, the hydrogen emits light than when passed through a prism, resolves into the "bright line" spectrum shown in Fig. 11.10. Why do hydrogen atoms emit bright lines of specific wavelengths rather than a continuous spectrum?
In two-photon ionization spectroscopy, the combined energies carried by two different photons are used to remove an electron from an atom or molecule. In such an experiment, a K atom in the gas phase is to be ionized by two different light beams, one of which has a 650-nm wavelength. What is the maximum wavelength for the second beam that will cause two-photon ionization?
What type of relationship (direct or inverse) e xists between wavelength, frequency, and photon energy? What does a photon energy unit of a joule equal?
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.
Sketch the major features (number of peaks and relative intensities for the peaks) of the expected photoelectron spectrum for atoms of nitrogen.
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.)
The colors of the visible spectrum and the wavelengths corresponding to the colors are given in Figure 5.2. (a) Which colors of light involve photons with less energy per photon than yellow light? (b) Which color of visible light has photons of greater energy, green or violet? (c) Which color of light has the greater frequency, blue or green?
The Doppler effect is one of the sources of the line broadening in atomic absorption spectroscopy. Atoms moving toward the light source encounter higher-frequency radiation than atoms moving away from the source. The difference in wavelength experienced by an atom moving at speed v (compared to one atrest) is / = v/c , where c is the velocity of light. Estimate the line width (in nanometers) of the lithiumline at 670.776(6707.76 Å) when the absorbing atoms are at a temperature of (a) 2000 K and (b) 3120 K.The average speed of an atom is given by v=8kT/m , where k is Boltzmann’s constant, Tis the absolute temperature, and m is its mass.
The figure below represents part of the emission spectrum for a one-electron ion in lhe gas phase. All the lines result from electronic transitions from excited states to the n = 3 state. (See Exercise 160.) a. What electronic transitions correspond to lines A and B? b. If the wavelength of line B is 142.5 nm, calculate the wavelength of line A.
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.
Traffic signals are often now made of LEDs (light-emitting diodes). Amber and green ones are pictured here. (a) The light from an amber signal has a wave-length of 595 nm, and that from a green signal has a wavelength of 500 nm. Which has the higher frequency? (b) Calculate the frequency of amber light.