Which of the following oxides of nitrogen is solid? (a) \(\mathrm{N}_{2} \mathrm{O}_{5}\) (b) \(\mathrm{N}_{2} \mathrm{O}\) (c) \(\mathrm{N}_{2} \mathrm{O}_{3}\) (d) \(\mathrm{NO}_{2}\)

When considering the physical state of nitrogen oxides, it's important to note that room temperature and atmospheric pressure play crucial roles. Dinitrogen pentoxide, abbreviated as (N_2O_5), exists as a solid under these conditions. This stands in contrast to most other oxides of nitrogen, which are typically gaseous at room temperature.

Moreover, (N_2O_5) is quite unique among its counterparts as it demonstrates relatively low volatility. This feature stems from its high molar mass and the substantial intermolecular forces present within its structure, which we will delve into further in subsequent sections of the article. If you are ever presented with various oxides of nitrogen and prompted to determine which is solid, remember that it's (N_2O_5) that exists in this state at standard room conditions.

Nitrogen oxides are a group of compounds that show a diverse range of chemical properties due to differences in their molecular structure and oxidation states of nitrogen. One such property of nitrogen oxides, which includes (N_2O_5), is their ability to act as oxidizing agents. This characteristic is especially prominent in (N_2O_5) due to the nitrogen's +5 oxidation state, which is the highest among the common oxides.

Other noteworthy chemical properties include reactivity with water. For instance, (N_2O_5) reacts with water to produce nitric acid, a reaction that is significant for the nitrogen cycle in the environment. These compounds also play critical roles in atmospheric chemistry, contributing to phenomena such as acid rain, ozone depletion, and air pollution. Understanding these properties helps in realizing the implications of nitrogen oxides on both the environment and industrial processes.

Intermolecular forces are the forces of attraction or repulsion which act between neighboring particles (atoms, molecules, or ions). They determine the physical properties of compounds, including their phase at room temperature. When we talk about (N_2O_5) being a solid at room temperature, it's all about the strong intermolecular forces at play.

In (N_2O_5), the dominant intermolecular force is the London dispersion force. These forces increase with the size of the molecules and the number of electrons. Since (N_2O_5) has a relatively large molecular structure and a higher electron count compared to other oxides of nitrogen, it exhibits stronger London dispersion forces, leading to its solid state at room temperature.

Additionally, (N_2O_5) can form polymeric structures through covalent bonds and possibly exhibit some dipole-dipole interactions due to its molecular geometry, further contributing to its solid state. Indeed, intermolecular forces are a key concept in understanding how substances behave and transform from one phase to another. They are central to topics ranging from materials science to meteorology and are crucial for the students to grasp in order to predict the physical state of compounds.