Here's a breakdown:
Water (H₂O):
* Stronger intermolecular forces: Water molecules are polar, meaning they have a slightly positive end (hydrogen) and a slightly negative end (oxygen). This allows them to form strong hydrogen bonds with each other.
* Hydrogen bonding: Hydrogen bonds are a type of strong dipole-dipole interaction where a hydrogen atom bonded to a highly electronegative atom (like oxygen) forms a bond with an electronegative atom in a neighboring molecule.
* High boiling point: The strong hydrogen bonds require a lot of energy to break, leading to a relatively high boiling point of 100°C.
Ammonia (NH₃):
* Weaker intermolecular forces: While ammonia is also a polar molecule, it forms weaker hydrogen bonds than water. This is because the nitrogen atom is less electronegative than oxygen, leading to weaker attractions between molecules.
* Lower boiling point: The weaker intermolecular forces require less energy to break, resulting in a much lower boiling point of -33.34°C.
Room Temperature:
Since room temperature is typically around 20-25°C, water's strong hydrogen bonds keep it in a liquid state. On the other hand, ammonia's weaker intermolecular forces allow it to exist as a gas at room temperature.
In summary: Water's strong hydrogen bonds are responsible for its liquid state at room temperature, while ammonia's weaker hydrogen bonds lead to its gaseous state.
