Textbook Question
The dissociation energy of a carbon-bromine bond is typically about 276 kJ/mol. (a) What is the maximum wavelength of photons that can cause C-Br bond dissociation?
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Ch.18 - Chemistry of the Environment
Chapter 18, Problem 19a
(a) Distinguish between photodissociation and photoionization.
Verified step by step guidance1
Understand the concept of photodissociation: Photodissociation is a process where a molecule absorbs a photon and breaks into smaller fragments. This typically involves the breaking of chemical bonds within the molecule due to the energy provided by the absorbed light.
Understand the concept of photoionization: Photoionization occurs when a molecule or atom absorbs a photon with enough energy to eject an electron, resulting in the formation of a positively charged ion.
Compare the energy requirements: Photodissociation generally requires less energy compared to photoionization, as breaking a bond often requires less energy than removing an electron from an atom or molecule.
Identify the outcomes: In photodissociation, the outcome is the formation of smaller molecular fragments, whereas in photoionization, the outcome is the formation of ions due to the loss of electrons.
Consider the applications and implications: Photodissociation is important in atmospheric chemistry and the breakdown of pollutants, while photoionization is crucial in processes like mass spectrometry and the study of ionization energies.
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Related Practice
Textbook Question
The dissociation energy of a carbon-bromine bond is typically about 276 kJ/mol. (b) Which kind of electromagnetic radiation—ultraviolet, visible, or infrared—does the wavelength you calculated in part (a) correspond to?
Open Question
In CF3Cl, the C-Cl bond dissociation energy is 339 kJ/mol. In CCl4, the C-Cl bond dissociation energy is 293 kJ/mol. What is the range of wavelengths of photons that can cause C-Cl bond rupture in one molecule but not in the other?
Textbook Question
(b) Use the energy requirements of these two pro- cesses to explain why photodissociation of oxygen is more important than photoionization of oxygen at altitudes below about 90 km.
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Textbook Question
The wavelength at which the O2 molecule most strongly absorbs light is approximately 145 nm. (a) In which region of the electromagnetic spectrum does this light fall?
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Textbook Question
The wavelength at which the O2 molecule most strongly absorbs light is approximately 145 nm. (b) Would a photon whose wavelength is 145 nm have enough energy to photodissociate O2 whose bond energy is 495 kJ/mol? Would it have enough energy to photoionize O2?