The melting point of NaCl sodium chloride is 801C 1474F . This value is experimentally determined and does not require calculations. However, I can explain the factors that affect the melting point of this compound.1. Ionic bonds: Sodium chloride is an ionic compound formed by the electrostatic attraction between positively charged sodium ions Na+ and negatively charged chloride ions Cl- . The strength of the ionic bond is directly proportional to the charges of the ions and inversely proportional to the distance between them. In the case of NaCl, the ionic bond is strong due to the +1 and -1 charges of Na+ and Cl- ions, respectively. This strong ionic bond contributes to the high melting point of NaCl.2. Lattice structure: NaCl has a face-centered cubic lattice structure, which means that each ion is surrounded by six oppositely charged ions. This arrangement maximizes the electrostatic attraction between the ions, further contributing to the high melting point.3. Polarizability: The polarizability of an ion refers to its ability to distort its electron cloud in response to an electric field. In general, larger ions with more diffuse electron clouds are more polarizable. The polarizability of an ion can affect the strength of the ionic bond and, consequently, the melting point of the compound. In the case of NaCl, both Na+ and Cl- ions have relatively low polarizability, which results in a strong ionic bond and a high melting point.4. Presence of impurities: The presence of impurities can disrupt the regular arrangement of ions in the crystal lattice, which can weaken the ionic bonds and lower the melting point of the compound. For example, the addition of a small amount of another salt, such as calcium chloride CaCl2 , can lower the melting point of NaCl. This effect is known as freezing-point depression and is commonly used in applications like de-icing roads.In summary, the melting point of NaCl is 801C, and it is influenced by factors such as the strength of the ionic bonds, the lattice structure, the polarizability of the ions, and the presence of impurities.