1. Ionic Bonding vs. Covalent Bonding:
* Copper(II) chloride (CuCl₂): This compound consists of copper ions (Cu²⁺) and chloride ions (Cl⁻) held together by strong electrostatic forces known as ionic bonds. These bonds require a large amount of energy to break, resulting in a high melting point.
* Ethane (C₂H₆): This molecule is held together by covalent bonds, where atoms share electrons. Covalent bonds are weaker than ionic bonds, requiring less energy to break.
2. Lattice Structure:
* Copper(II) chloride (CuCl₂): Forms a crystalline lattice structure with a repeating pattern of ions. This ordered arrangement contributes to the strong attraction between ions and further increases the melting point.
* Ethane (C₂H₆): Exists as individual molecules with relatively weak intermolecular forces (van der Waals forces) between them. These forces are easily overcome, resulting in a low melting point.
3. Polarity:
* Copper(II) chloride (CuCl₂): This compound is ionic and highly polar due to the large electronegativity difference between copper and chlorine. This polarity contributes to stronger interactions within the lattice.
* Ethane (C₂H₆): Ethane is a nonpolar molecule, meaning it has no significant separation of charges. This lack of polarity leads to weaker intermolecular forces.
In summary:
The strong ionic bonds, the ordered lattice structure, and the polarity of copper(II) chloride contribute to its high melting point compared to the weaker covalent bonds, lack of a rigid lattice, and nonpolar nature of ethane.
