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Chemistry
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28 Oct 2017

73. Ultraviolet radiation and radiation of shorter wavelengths can damage biological molecules because these kinds of radiation carry enough energy to break bonds within the molecules. A typical carbon-carbon bond requires 348 kJ/mol to break. What is the longest wavelength of radiation with enough ener gy to break carbon-carbon bonds?

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Related questions

The dissociation energy of a carbon–bromine bond is typically about 210 kJ/mol. (a) What is the maximum wavelength of photons that can cause C–Br bond dissociation? (b) Which kind of electromagnetic radiation—ultraviolet, visible, or infrared—does the wavelength you calculated in part (a) correspond to?

One type of sunburn occurs on exposure to UV light of wavelength in the vicinity of 325 nm. (a) What is the energy of a photon of this wavelength? (b) What is the energy of a mole of these photons? (c) How many photons are in a 1.00 mJ burst of this radiation? (d) These UV photons can break chemical bonds in your skin to cause sunburn—a form of radiation damage. If the 325-nm radiation provides exactly the energy to break an average chemical bond in the skin, estimate the average energy of these bonds in kJ/mol.

b) 1 mole of photons has Avogadro’s number of photons. Energy of 1 mole of photons is:

c) Number of photons in 1 mJ of radiation is calculated by dividing total energy with the energy of one photon:

d) Average energy of chemical bonds (in human skin equals the energy of photons with 325 nm wavelength, which is already calculated to be 3.68×10­5 J/mol which is 368 kJ/mol.

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