9. Absorption spectra for molecules are more complex than atomic spectra because: C (a) Molecular species have side reactions C (b) Atomic species do not absorb light C (c) The number of energy states of molecules is enormous when compared with the number of energy states for isolated atoms. 10 absorption / emission of light by a molecule and describe the processes in terms of energy levels. How this information can be used for obtaining analytical information on an analyte of interest? Explain the phenomenon of

9. Absorption spectra for molecules are more complex than atomic spectra because: C (a) Molecular species have side reactions C (b) Atomic species do not absorb light C (c) The number of energy states of molecules is enormous when compared with the number of energy states for isolated atoms. 10 absorption / emission of light by a molecule and describe the processes in terms of energy levels. How this information can be used for obtaining analytical information on an analyte of interest? Explain the phenomenon of

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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How many photons are produced in a laser pulse of 0.360 J at 481 nm
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The relationship between photons of light at various energies and wavelengths is Given by E=hv , c=v(wavelength) Therefore, when a photon of energy at wavelength of 275 nm is compared with photons of energy at wavelength of 390 nm and higher we have a decrease in the energy and its dissociation energy that would attack polymeric or chemical bonds of various structures. Therefore, the higher the wavelength the lower the frequency or higher wavelengths have less energy than lower wavelengths 275nm is far greater energy than 390nm or higher. Given we have established light is composed of photons and high energy gamma radiation are also photons but of higher energy does the math for photochemistry given above apply to higher sources of photon energy from gamma and other sources of radiation? If so why or why not. If there is a relationship what equations exist to compare and predict equivalence of standard electromagnetic model wavelength for actinic and visible and IR radiations to more…
Part A1: Do you notice any pattern in the color of the light used to detect absorbance (preset) and the color of the solution? If so, describe the pattern. What happened to the transmittance when the wavelength being detected was changed to approximately the same color as the solution? Try to come up with an explanation for this. How does the percent transmittance of the preset wavelength compare to the percent transmittance when looking at the transmittance over the entire visible spectrum? What happened to the transmittance when the width of the sample was changed? Explain why this makes sense. Explain why there was an upper maximum on the concentrations for each solution. What would happen to the absorbance or percent transmittance of a sample above that concentration? If you needed to measure the exact concentration of a solution whose concentration is above that limit, is there anything you can do?
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