7.14 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 µm. What frequency (in s) corresponds to that wavelength? (b) The H-CI bond has a frequency of vibration of 8.652x10 Hz. What wavelength (in um) corresponds to that frequency?
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- The bond energy of O2 is 498 kJ / mol. What is the maximum wavelength of the photonthat has enough energy to break the O=O bond of oxygen?If the energy of the H2, covalent bond is –4.48 eV, what wavelength of light is needed to break that molecule apart? In what part of the electromagnetic spectrum does this light lie?The energy required to break one mole of fluorine-fluorine bonds in F2 is 155 kJ/mol. What is the longest wavelength of light capable of breaking a single F-F bond?
- The energy required to break one mole of hydrogen-hydrogen bonds in H2 is 436 kJ. What is the longest wavelength of light with sufficient energy to break a single hydrogen-hydrogen bond?The experimentally determinded Bi-Cl bond distance in bismuth trichloride is 2.48Å . Given the tablulated value of 0.99Å for the atomic radius of Cl, predict the atomic radius of Bi?The stratospheric ozone 1O32 layer helps to protect usfrom harmful ultraviolet radiation. It does so by absorbingultraviolet light and falling apart into an O2 molecule and anoxygen atom, a process known as photodissociation.O31g2¡O21g2 + O1g2Use the data in Appendix C to calculate the enthalpy changefor this reaction. What is the maximum wavelength a photoncan have if it is to possess sufficient energy to cause thisdissociation? In what portion of the spectrum does thiswavelength occur?
- What is the energy of infrared radiation in kilojoules/mol with λ= 1.46×10−6 mm? ultraviolet light with λ= 261 nm? X rays with λ = 5.34 nm?Sunscreen contains compounds that absorb ultraviolet light. Whensunscreen is applied to skin, it prevents ultraviolet light from reachingthe skin. The graph that follows shows the absorbance of light as afunction of wavelength for two different compounds (2-EHMC andTDSA) common in sunscreen. Absorbance is a measure of theamount of light absorbed by the compound—the higher theabsorbance, the more light is absorbed. Study the graph and answerthe questions below.a. Calculate the energy of a photon at the maximumabsorption of TDSA.b. Calculate the energy of a photon at the maximum absorption of 2-EHMC.c. Which compound absorbs more energy at its maximum absorption?d. Why do you think sunscreens commonly contain both of these compounds and not just one of them?e. Assuming that sunlight produces 3.066 ? 1022 ?? ?ℎ??????2?and that the skin absorbs one-half of thesephotons (and reflects the other half), calculate the total UV energy absorbed over 0.42 m2of skin thatis exposed to sunlight for…(a) Draw the Lewis structure for hydrogen peroxide, H2O2.(b) What is the weakest bond in hydrogen peroxide? (c) Hydrogenperoxide is sold commercially as an aqueous solution inbrown bottles to protect it from light. Calculate the longestwavelength of light that has sufficient energy to break theweakest bond in hydrogen peroxide.
- A bond vibration has a frequency of 8.52x1013 Hz. a. What is the energy associated with this transition?b. What is the wavelength of this transition, in microns?By using photons of specific wavelengths, chemists can dissociate gaseous HI to produce H atoms with certain speeds. When HI dissociates, the H atoms move away rapidly, whereas the heavier I atoms move more slowly. (a) What is the longest wavelength (in nm) that can dissociate a molecule of HI? (b) If a photon of 254 nm is used, what is the excess energy (in J) over that neededfor dissociation? (c) If this excess energy is carried away by the H atom as kinetic energy, what is its speed (in m/s)?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?