Domanda del libro di testo
(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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Ch.18 - Chemistry of the Environment
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Capitolo 18, Problema 16
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?
Guida verificata passo dopo passo1
Step 1: Understand the concept of bond dissociation energy, which is the energy required to break a bond in a molecule. Here, we have two different C-Cl bonds with different dissociation energies: 339 kJ/mol for CF3Cl and 293 kJ/mol for CCl4.
Step 2: Convert the bond dissociation energies from kJ/mol to energy per photon. Use the formula: Energy per photon (J) = (Bond dissociation energy (kJ/mol) * 1000 J/kJ) / Avogadro's number (6.022 x 10^23 mol^-1).
Step 3: Calculate the frequency of the photon required to break the bond using the energy per photon. Use the formula: Frequency (ν) = Energy per photon (J) / Planck's constant (6.626 x 10^-34 J·s).
Step 4: Convert the frequency to wavelength using the speed of light. Use the formula: Wavelength (λ) = Speed of light (c, approximately 3.00 x 10^8 m/s) / Frequency (ν).
Step 5: Determine the range of wavelengths that can break the C-Cl bond in one molecule but not the other by comparing the wavelengths calculated for CF3Cl and CCl4.
Concetti chiave
Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.
Bond Dissociation Energy
Bond dissociation energy (BDE) is the energy required to break a bond in a molecule, resulting in the formation of separate atoms or radicals. It is a crucial factor in determining the stability of a molecule; higher BDE indicates a stronger bond. In the context of the question, the differing BDEs of C-Cl bonds in CF3Cl and CCl4 suggest that different amounts of energy (and thus different photon wavelengths) are needed to break these bonds.
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Percorso guidato
01:50
Bond Energy
Photon Energy and Wavelength
The energy of a photon is inversely related to its wavelength, described by the equation E = hc/λ, where E is energy, h is Planck's constant, c is the speed of light, and λ is the wavelength. To cause bond rupture, the energy of the photon must match or exceed the bond dissociation energy. Therefore, the range of wavelengths that can cause C-Cl bond rupture in CF3Cl and CCl4 can be calculated based on their respective BDEs.
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Percorso guidato
01:40Photon Energy Formulas
Energy Threshold for Bond Rupture
The energy threshold for bond rupture is the minimum energy required to break a specific bond in a molecule. In this scenario, the C-Cl bond in CF3Cl has a higher energy threshold (339 kJ/mol) compared to CCl4 (293 kJ/mol). This difference means that photons with energies corresponding to wavelengths shorter than those calculated from these BDEs will be able to break the C-Cl bond in CF3Cl but not in CCl4, establishing a range of wavelengths for each molecule.
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Percorso guidato
01:50Bond Energy
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