* Ionic Bonding: Sodium chloride is an ionic compound. It forms a strong crystal lattice held together by electrostatic forces between positively charged sodium ions (Na+) and negatively charged chloride ions (Cl-). These strong bonds require a lot of energy to break, resulting in a high melting point (801°C).
* Hydrogen Bonding: Ethyl alcohol is a covalent compound with hydrogen bonding. While hydrogen bonding is a strong intermolecular force, it is significantly weaker than the ionic bonds in sodium chloride. The weaker bonds in ethyl alcohol require less energy to break, giving it a much lower melting point (-114°C).
In summary: The strong ionic bonds in sodium chloride make it a solid at room temperature and give it a very high melting point. Ethyl alcohol, with its weaker hydrogen bonds, is a liquid at room temperature and melts at a much lower temperature.
