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Volatility is a measure of how easily a substance evaporates. In essence, it tells us how readily molecules in a liquid escape into the gas phase. Imagine a liquid that quickly turns into vapor at room temperature; such substances are considered to be highly volatile. Volatility is primarily influenced by the strength of intermolecular forces within a substance. These forces act as a barrier against evaporation. When intermolecular forces are weak, molecules can escape the liquid phase easily, resulting in higher volatility. Conversely, strong intermolecular forces mean that more energy is needed for molecules to evaporate, leading to lower volatility.A key indicator of volatility is the boiling point. The lower the boiling point, the higher the volatility, because it implies that less heat is needed for evaporation to occur. This inverse relationship helps in comparing the volatility of substances like carbon tetrahalides. For example, since \( \mathrm{CCl}_{4} \) boils at a lower temperature than \( \mathrm{CBr}_{4} \), it is therefore more volatile.

The boiling point of a substance is the temperature at which its liquid phase converts to gas as rapidly as the pressure allows. At this temperature, the vapor pressure of the liquid becomes equal to the pressure exerted on the liquid by the surrounding environment, causing the liquid molecules to break free and form gas. Boiling points serve as an indicator of the strength of a substance's intermolecular forces. Specifically, the stronger these forces are, the more energy (and hence higher temperature) is necessary to transition into the gas phase. Hence, substances with higher boiling points tend to have stronger intermolecular forces.Several factors influence the boiling point:

• Molar Mass: Generally, an increase in molar mass results in higher boiling points due to greater London dispersion forces.
• Intermolecular Force Types: Forces like hydrogen bonding and dipole-dipole interactions can significantly raise boiling points.

Thus, in comparing \( \mathrm{CCl}_{4} \) and \( \mathrm{CBr}_{4} \), the higher boiling point of \( \mathrm{CBr}_{4} \) indicates its stronger intermolecular forces.

Vapor pressure is the pressure exerted by a vapor in equilibrium with its liquid or solid form. It reflects the tendency of molecules to escape from the liquid or solid into the gas phase. Generally, higher vapor pressures correspond to more volatile substances, as more molecules are in the vapor phase at a given time.Factors Influencing Vapor Pressure:

• Temperature: As temperature increases, vapor pressure rises because more molecules have the kinetic energy needed to escape into vapor.
• Intermolecular Forces: Weaker forces within a liquid allow more molecules to escape, resulting in higher vapor pressure.

To illustrate, consider carbon monoxide (\( \mathrm{CO} \)) and \( \mathrm{CBr}_{4} \). \( \mathrm{CO} \), having weaker intermolecular forces, exhibits higher vapor pressure than \( \mathrm{CBr}_{4} \). This makes \( \mathrm{CO} \) more conducive to evaporation while \( \mathrm{CBr}_{4} \) remains mostly in its liquid state at the same temperature.