Water boils at a higher temperture than a non-polar solvent like either because?
Water boils at a higher temperature than non-polar solvents like ethanol or gasoline because of the differences in their intermolecular forces. To understand this, we need to consider the concept of intermolecular forces.
Intermolecular forces are attractive forces between molecules. They determine the physical properties of substances, including boiling points. In the case of water, it has hydrogen bonding, which is a strong intermolecular force. Non-polar solvents like ethanol or gasoline lack such strong intermolecular forces and primarily have weaker forces like London dispersion forces.
When a substance boils, it undergoes a phase change from a liquid to a gas. The boiling point is the temperature at which the vapor pressure of the liquid equals the atmospheric pressure, and boiling occurs. Substances with stronger intermolecular forces require more energy to break these forces and transition into the gas phase.
Water's high boiling point is primarily due to hydrogen bonding. Hydrogen bonding occurs when a hydrogen atom bonded to an electronegative atom (like oxygen in water) interacts with another electronegative atom. These intermolecular hydrogen bonds in water are relatively strong, requiring more energy to break them apart and convert water from a liquid to a gas.
In contrast, non-polar solvents like ethanol or gasoline lack strong hydrogen bonding. Their intermolecular forces, such as London dispersion forces, are weaker and less significant. As a result, these substances have lower boiling points than water.
To determine the boiling points of different substances, you can refer to reference material like handbooks, chemistry databases, or search online resources that provide data on the physical properties of various substances. These sources will provide you with the necessary information to compare and understand why water boils at a higher temperature than non-polar solvents.