Write balanced chemical equations for each of the following reactions: (a) The nitric oxide molecule undergoes photodissociation in the upper atmosphere. (b) The nitric oxide molecule undergoes photoionization in the upper atmosphere. (c) Nitric oxide undergoes oxidation by ozone in the stratosphere.

Verified step by step guidance

1. Identify the reactants and products involved in the photoionization of nitric oxide (NO).
2. Understand that photoionization involves the absorption of a photon by a molecule, resulting in the ejection of an electron and the formation of a positive ion.
3. Write the chemical equation for the photoionization of nitric oxide: NO + hv → NO⁺ + e⁻, where 'hv' represents the photon energy.
4. Ensure that the equation is balanced in terms of both mass and charge. In this case, the number of atoms and the overall charge are balanced on both sides of the equation.
5. Review the concept of photoionization, which is a process where a molecule absorbs light energy and loses an electron, forming a cation.

Key Concepts

Photoionization

Photoionization is the process in which an atom or molecule absorbs a photon and subsequently loses an electron, resulting in the formation of a positively charged ion. This phenomenon is significant in atmospheric chemistry, particularly in the upper atmosphere where high-energy ultraviolet (UV) radiation is prevalent. In the case of nitric oxide (NO), the absorption of UV light leads to its ionization, which can affect various atmospheric processes.

Balanced Chemical Equations

A balanced chemical equation represents a chemical reaction where the number of atoms for each element is the same on both the reactant and product sides. Balancing equations is crucial for obeying the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. This ensures that the equation accurately reflects the stoichiometry of the reaction, allowing for proper calculations of reactants and products.

Nitric Oxide (NO) in the Atmosphere

Nitric oxide (NO) is a significant molecule in atmospheric chemistry, playing a role in the formation of smog and acid rain. It is produced from various sources, including combustion processes and lightning. In the upper atmosphere, NO can undergo reactions that lead to the formation of nitrogen dioxide (NO2) and other nitrogen oxides, which are important for understanding air quality and the chemistry of the ozone layer.