Compare the energy (in joules) carried by an X-ray pho- ton (wavelength A = 0.20 nm) with that carried by an AM radio wave photon (A = 200 m). Calculate the 1.00 mol of each type of photon. What effect do you expect each type of radiation to have for inducing chemi- cal reactions in the substances through which it passes? energy of

Compare the energy (in joules) carried by an X-ray pho- ton (wavelength A = 0.20 nm) with that carried by an AM radio wave photon (A = 200 m). Calculate the 1.00 mol of each type of photon. What effect do you expect each type of radiation to have for inducing chemi- cal reactions in the substances through which it passes? energy of

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter4: Introduction To Quantum Mechanics

Section: Chapter Questions

Problem 48AP: Compare the energy (in joules) carried by an X-ray photon (wavelength=0.20nm) with that carried by...

See similar textbooks

Similar questions

Photobromination of cinnamic acid to dibromocinnamic acid was carried out in blue light of wavelength 440nm at 35degree celsius using light intensity of 1.5 *10 power -3 joule per second. An exposure of 20 minutes produces a decrease of 0.075 millimoles of bromine. The solution absorb 80% of light passing through it. Calculate the quantum yield of the reaction.
Covalent bonds in a molecule absorb radiation in the IR re-gion and vibrate at characteristic frequencies.(a) The C—O bond absorbs radiation of wavelength 9.6 μm.What frequency (in s⁻¹) corresponds to that wavelength?(b) The H—Cl bond has a frequency of vibration of 8.652x10^13Hz. What wavelength (in μm) corresponds to that frequency?
2.9 Vibrations in crystals. (a) Calculate the average vibrational energy per mole for Si at 400 K to within the limits of the Einstein theory. Let VẸ = 12 x 1012 s-1, (b) If each atom carried three quanta of vibrational energy, how much vibrational energy would the crystal contain?
Ozone (O3) in the stratosphere absorbs the harmful radiation from the sun by undergoing decomposition: O3->O+O2. (A) Calculare the delta H degrees for this process. (B) Calculate the maximum wavelength of photons in (nm) that possesses the energy to cause the decomposition of ozone photochemically.
Item 11 11 of 13 > I Review I Constants I Periodic Table Part A Note on the left that the color is deep pink in the interior of each lobe but fades to pale pink at the edges. What does this change in color represent? The intensity of the color indicates that Pz Px Py the interactions between electrons and the nucleus are greater at the interior of the lobes than on the edges. (a) (b) The p orbitals. (a) Electron-density distribution of a 2p orbital. (b) Contour representations of the three p orbitals. The subscript on the orbital label indicates the axis along which the orbital lies. The intensity of the color indicates that the probability of finding the electron is greater at the interior of the lobes than on the edges. The intensity of the color indicates that the interactions between electrons and the nucleus are greater on the edges of the lobes than at the interior. The intensity of the color indicates that the probability of finding the electron is greater on the edges of the…
9. Determine (a) the energy, in joules per photon, of radiation of frequency 7.39 X 1015 s1; |(b) the energy, in kilojoules per mole, of radiation of frequency 1.97 x 1014's-1.
Calculate the frequency of green light with a wavelength of 517 nm. A/ Paragraph B I Ev O 80 :
Covalent bonds in a molecule absorb radiation in the IR region and vibrate at characteristic frequencies. (a) The C---O bond absorbs radiation of wavelength 9.6 mm. What frequency (in s-1) corresponds to that wavelength? (b) The H---Cl bond has a frequency of vibration of 8.652x1013 Hz. What wavelength (in mm) corresponds to that frequency?
Match each statement with one or more of the following: flame AA, flame photometry, atomic fluorescence, ICP, graphite furnace AA, and spark emission. (a) The technique that uses a partially ionized stream of argon gas called a plasma - (b) The technique in which a light source is used to excite atoms, the emission from which is then measured - (c) The three techniques that require light to be directed at the atomized ions - (d) The technique that utilizes a solid sample - (e) The four techniques that measure some form of light emission by excited atoms present in an atomizer - (f) The absorption technique in which the atoms are in the path of the light for a relatively short time - (g) The technique in which the emitting source may reach a temperature of 6000 K -
(a) Calculate the wavelength of a photon with an energy equivalent to that of an O=O bond ( 120 kcal/mol) (b) In what region of the electromagnetic spectrum does this wavelength fall? (c) If you wanted photons with energy greater than the O=O bond, would you want longer or shorter wavelengths than that which you just calculated?
In a typical fireworks device, the heat of the reaction betweena strong oxidizing agent, such as KClO₄, and an organic com-pound excites certain salts, which emit specific colors. Stron-tium salts have an intense emission at 641 nm, and barium saltshave one at 493 nm. (a) What colors do these emissions pro-duce? (b) What is the energy (in kJ) of these emissions for 5.00 g each of the chloride salts of Sr and Ba? (Assume that allthe heat released is converted to light emitted.)
Questions lesbucional sinine52 1. List the elements tested in the flame test in order of increasing energy of the light emitted (based on the general color of the flame).