Step 1: Understanding the Question:
This is a conceptual question asking to identify a false statement regarding the properties of ionic and covalent bonding.
Step 2: Detailed Explanation:
Statement (A): Correct. Ionic bonds are purely electrostatic attractions between oppositely charged ions. These forces act equally in all directions (spherically symmetric). Therefore, ionic bonds are non-directional.
Statement (B): Correct. For most common stable molecules involving s and p block elements, atoms can share up to 3 pairs of electrons to form a triple bond (e.g., \(N_2\), acetylene). Higher bond orders are exceptionally rare and typically involve transition metals.
Statement (C): Incorrect. Covalent compounds are formed by the sharing of electrons, resulting in neutral molecules. Even in a fused (liquid/molten) state, they exist as molecules and do not dissociate into ions. Because they lack free charge carriers (ions or mobile electrons), they are insulators. It is ionic compounds that conduct electricity when fused.
Statement (D): Correct. Many ionic compounds are soluble in polar solvents like water because the high dielectric constant of water can overcome the lattice energy of the crystal and solvate the ions.
Step 3: Final Answer:
The statement that covalent compounds conduct electricity in the fused state is incorrect.