Answer:
Step-by-step explanation:
The difference in the physical state of LiCl and NCl3 at room temperature is due to the difference in their intermolecular attractive forces.
LiCl has strong ionic bonds, which are strong attractive forces between positive and negative ions. These strong attractive forces result in a high melting and boiling point, making LiCl a solid at room temperature.
NCl3, on the other hand, has weaker covalent bonds, which are attractive forces between atoms in a molecule. These weaker attractive forces result in a lower melting and boiling point, making NCl3 a liquid with a relatively low boiling point at room temperature.
The strength of intermolecular forces is determined by the type of bond and the molecular structure. Ionic bonds are stronger than covalent bonds, and the stronger the bond, the higher the melting and boiling points of a substance.