* Stronger intermolecular forces: Water molecules form strong hydrogen bonds with each other. Hydrogen bonds are the strongest type of intermolecular forces, requiring significant energy to break. In contrast, CCl4 molecules only exhibit weak London dispersion forces, which are easily overcome.
* Higher boiling point: Water's strong hydrogen bonds result in a significantly higher boiling point (100°C) compared to CCl4 (76.7°C). This means water needs more energy to transition from liquid to gas.
* Polarity: Water is a highly polar molecule due to the electronegativity difference between oxygen and hydrogen. This polarity enhances hydrogen bonding, further contributing to its lower volatility. CCl4, on the other hand, is nonpolar, lacking the strong dipole-dipole interactions that would increase its volatility.
In summary, the strong hydrogen bonding in water molecules makes it more difficult for them to escape into the gas phase, leading to its lower volatility compared to carbon tetrachloride.
