Question

Many chemical reactions that occur in the atmosphere and stratosphere involve free radicals. Free radical formation occurs when a photon of light is absorbed and the energy of the radiation being absorbed causes a chemical bond in the compound to break. Which of the following bonds requires the most energy (and the most energetic radiation) to be broken? (a) The oxygen-oxygen bond in \(\mathrm{O}_{2}\) (b) The chlorine-carbon bond in \(\mathrm{CCl}_{2} \mathrm{F}_{2}\) (c) The oxygen-oxygen bond in \(\mathrm{O}_{3}\)

Short answer

The oxygen-oxygen bond in \(\mathrm{O}_2\) requires the most energy to break.

Step-by-step solution

Understanding Bond Energy

Bond energy is the amount of energy required to break one mole of a bond in a molecule in the gas phase. The higher the bond energy, the stronger the bond.

Evaluate Bond Energy in O2

The oxygen-oxygen bond in dioxygen (\(\mathrm{O}_2\)) is a double bond with a high bond energy of approximately 498 kJ/mol. This strong bond requires a significant amount of energy to break.

Evaluate Bond Energy in CCl2F2

The chlorine-carbon bond in dichlorodifluoromethane (\(\mathrm{CCl}_2\mathrm{F}_2\)) has a bond energy estimated around 330 kJ/mol, which is less than that of the \(\mathrm{O_2}\) bond.

Evaluate Bond Energy in O3

The oxygen-oxygen bond in ozone (\(\mathrm{O}_3\)) is a weaker single bond compared to \(\mathrm{O_2}\), with a bond energy of about 146 kJ/mol in ozone.

Comparing Bond Energies

By comparing the bond energies, we see that \(\mathrm{O}_2\) has the highest bond energy at approximately 498 kJ/mol, followed by \(\mathrm{CCl}_2\mathrm{F}_2\), and then \(\mathrm{O}_3\).

Key concepts

Free Radicals

Free radicals are atoms or molecules containing unpaired electrons, making them highly reactive. In the realm of chemistry, these unpaired electrons are like tiny agitators that push the radical towards reactions. This reactivity is why free radicals play a significant role in atmospheric reactions.
- Free radicals are often formed through the breaking of chemical bonds by absorbing energy from light or heat. - The reactivity of free radicals can lead to chain reactions, particularly in the atmosphere, where they may attack and modify stable molecules such as ozone. - Over time, these radicals can contribute to significant environmental processes, affecting the creation and decomposition of compounds in the atmosphere.
Understanding how free radicals work is crucial for comprehending broader processes in atmospheric chemistry.

Atmospheric Chemistry

Atmospheric chemistry involves studying the chemical composition of the atmosphere and the reactions and interactions that occur here. It's a unique field since the atmosphere is vast and continuously changing.
- One of the key focuses is on how pollutants are formed and how they are removed from the atmosphere. - Reactions in the atmosphere often involve free radicals and can affect phenomena such as the greenhouse effect, acid rain, and ozone depletion. - The breakdown of chemicals by free radicals in the atmosphere is a critical aspect of maintaining and altering atmospheric balance.
Knowledge of these processes helps us understand air quality, climate change, and protection of the ozone layer.

Photodissociation

Photodissociation is a process where a chemical bond is broken due to the absorption of light energy. This absorption typically happens in the ultraviolet or visible light regions and plays a significant role in atmospheric chemistry.
- When molecules absorb light, their chemical bonds can gain enough energy to break, leading to the formation of free radicals.- For example, ozone (\(\mathrm{O}_{3}\)) in the atmosphere can undergo photodissociation to produce oxygen gas and individual oxygen radicals.- These reactions are vital as they initiate chains of chemical reactions that govern the composition and behavior of the atmosphere.
The balance between formation and breakdown through photodissociation is vital for the stability of the atmospheric composition.

Chemical Bonds

Chemical bonds are the connections between atoms that allow the formation of molecules and compounds. Each type of bond has distinct characteristics and strengths, influencing how readily they break or form.
- Bond energy quantifies the strength of a bond: the higher the energy, the stronger the bond.- Types of bonds include ionic, covalent (like those in \(\mathrm{O}_{2}\)), and metallic bonds, each requiring different amounts of energy to break apart.- Understanding bond energies is crucial for predicting the outcomes of chemical reactions, particularly in processes like photodissociation, where bonds break under light energy.
Examining these interactions provides insight into how compounds behave under various conditions, such as heat, pressure, and light exposure.