Question

Why is the photodissociation of \(\mathrm{N}_{2}\) in the atmosphere relatively unimportant compared with the photodissociation of \(\mathrm{O}_{2} ?\)

Short answer

The photodissociation of N2 is relatively unimportant compared to O2 in the atmosphere for three main reasons: (1) N2 has a stronger bond and requires higher energy (9.8 eV) for photodissociation compared to O2 (5.2 eV), (2) the photons with enough energy to break N2 bonds are mostly in the extreme UV range, which is scarce in Earth's sunlight and poorly penetrates the atmosphere, and (3) N2 photodissociation produces relatively unreactive nitrogen atoms, while O2 photodissociation forms reactive oxygen atoms that contribute to ozone formation and other significant atmospheric processes.

Step-by-step solution

Understanding Photodissociation

Photodissociation is a process in which a molecule absorbs a photon of light, which causes the molecule to break apart into its constituent atoms or smaller molecules. In the context of the atmosphere, photodissociation of N2 and O2 is important as it results in the formation of reactive species that play a role in various atmospheric processes.

Energy Requirements for Photodissociation

The energy required to break the bond in a molecule can be represented as the bond dissociation energy. In order to break the bond, the molecule must absorb a photon with at least equal energy to the bond dissociation energy. For N2, the bond dissociation energy is around 9.8 eV, while for O2, it is around 5.2 eV. Since N2 has a stronger bond, it requires more energy to be photodissociated compared to O2.

Wavelengths of Light Absorbed

The energy of a photon is inversely proportional to its wavelength. Since the photodissociation of N2 requires more energy, the corresponding photons must have shorter wavelengths. The photons with enough energy to photodissociate N2 are mostly in the ultraviolet (UV) range, particularly the extreme UV range below 200 nm. However, these photons are not very abundant in the Earth's sunlight, as they are mostly absorbed by other molecules or scattered before reaching the Earth's surface. On the other hand, O2 absorbs photons in a wider range of wavelengths, with the energy requirement met by UV-B (280-320 nm) and UV-C (100-280 nm) photons. These wavelengths are more plentiful in sunlight and can penetrate deeper into the atmosphere.

Consequences of Photodissociation

When N2 undergoes photodissociation, it forms nitrogen atoms (N) which are relatively unreactive and do not cause any significant impact on the atmosphere. On the other hand, photodissociation of O2 forms reactive oxygen atoms (O) which further react with other O2 molecules to form ozone (O3). This ozone plays a crucial role in absorbing UV radiation and protecting the Earth's surface from harmful UV radiation. Moreover, ozone is also involved in various other chemical reactions in the atmosphere contributing to the Earth's weather and climate.

Conclusion

The photodissociation of N2 is relatively unimportant compared with the photodissociation of O2 in the atmosphere due to three main reasons: (1) higher energy requirements for N2 photodissociation, (2) the scarcity of short-wavelength UV photons needed to break the N2 bonds, and (3) the lack of any significant atmospheric consequences resulting from the photodissociation of N2 compared to the various roles played by O2 and its photodissociated products like ozone.

Key concepts

Bond Dissociation Energy

Bond dissociation energy is a crucial concept in understanding why certain molecules are more likely to be photodissociated than others. It represents the amount of energy needed to break a specific chemical bond within a molecule. In simpler terms, it's the energy required for a molecule to separate into its individual atoms. This energy is typically measured in electronvolts (eV). Let's put it into context:

• The bond dissociation energy for \(_2\) is approximately 9.8 eV.
• For \(_2\), it's about 5.2 eV.

These values help us understand which molecules are harder or easier to dissociate. Because \(_2\) has a higher bond dissociation energy, it means the bonds holding nitrogen atoms together are quite strong. These stronger bonds require more energy to be broken. Conversely, the bond dissociation energy for \(_2\) is lower. This means it needs less energy to come apart, making the bonds easier to break. Therefore, molecules like \(_2\) with lower bond dissociation energy are more commonly photodissociated in the atmosphere.

UV Radiation

Understanding ultraviolet or UV radiation is key to knowing how photodissociation occurs in the atmosphere. When a molecule absorbs a photon of light, the energy of that photon can cause the molecule to dissociate. The energy of a photon is inversely related to its wavelength: shorter wavelengths have more energy. Let's look at some details:

• Molecules requiring more energy to dissociate, like \(_2\), need photons with shorter wavelengths, specifically in the extreme UV range below 200 nm.
• These photons are scarce in Earth's sunlight because they are mostly absorbed by the atmosphere before reaching the ground.
• Molecules with lower energy requirements for dissociation, like \(_2\), can absorb slightly longer wavelengths in the UV-B (280-320 nm) and UV-C (100-280 nm) range.

This is why O2 undergoes photodissociation more readily than \(_2\) in our atmosphere. The UV photons that can effectively dissociate oxygen are more abundant in sunlight and penetrate deeper into the atmospheric layers.

Ozone Formation

Ozone formation is a fascinating process that significantly impacts life on Earth. It is intricately linked to photodissociation, particularly of \(_2\). When \(_2\) is dissociated by UV radiation, it splits into two oxygen atoms (O). These reactive oxygen atoms quickly latch onto other \(_2\) molecules to form ozone (\(_3\)). Here's why this is important:

• Ozone plays a critical role in blocking harmful UV-radiation from the sun, protecting living organisms on the Earth's surface.
• It participates in numerous chemical reactions in the atmosphere, influencing weather and climate patterns.

The photodissociation of \(_2\) and the subsequent formation of ozone showcases how energy from the sun drives crucial chemical changes in our atmosphere. While nitrogen molecules tend to remain stable, oxygen molecules contribute to the dynamic and vital process of ozone development, underscoring the essential function of photodissociation in ecological balance and protection.