> Electrical conductivity requires the movement of charged particles. Why Do Ionic Compounds Conduct Electricity? Ionic compounds cannot conduct electricity when solid, as their ions are held in fixed positions and cannot move. Consequently, ionic solids do not conduct electricity. One good example to prove this theory is during your chemistry lessons. The positive nuclei of the metal atoms is held together while all the electrons are free to move. the ionic compounds conduct when they are molten because their structure is loose and there are weakly shared pairs. In a liquid, the ionic compound dissociates into its respective ions. For electrolysis to work, the compound must contain ions. Answered by | 24th Jul, 2017, 04:20: PM Electricity is the flow of electrons. For a substance to conduct electricity, it needs to contain some sort of charge carrier - this could be an electron or an ion - that is free to move within the substance. Ionic compounds in their solid state have particles that are held tightly together, restricting all movement and preventing electrical current from forming. Covalent compounds cannot act as electrolytes because they contain neutral atoms . the metals conduct better because of a specific trait called "sea of electrons". or ions. The ionic solids are insulators in the solid state because the ions are entrapped in fixed places in the crystal lattice & cannot move when electric field is applied.However, in molten state,they become good conductors of electricity. 1:44 know that a covalent bond is formed between atoms by the sharing of a pair of electrons and metals conduct electricity because they have delocalized … Ionic compounds are usually solid in nature and free flow of ions is not possible . However , in molten state the ions are able to flow freely and thus conduct electricity. Not all ionic compounds conduct electricity, but the majority of them do. I kind of know the answers, i just cant put em in words :P i know ionic compounds conduct electricty because the ions are free to move.. but why does the fact that ions move make it conduct electricity? Why do ionic compounds conduct electricity when molten, and why does metal conduct electricity anyway? An example of an ionic compound is Sodium Chloride, NaCl, in which Sodium (NA) is the cation and Chlorine (Cl) is the anion. 1:42 understand why compounds with giant ionic lattices have high melting and boiling points; 1:43 Know that ionic compounds do not conduct electricity when solid, but do conduct electricity when molten and in aqueous solution (g) Covalent bonding. Solid ionic compounds do not have electrical conductivity because the ions are not free to move. Ionic compounds such as sodium chloride or magnesium chloride are in a fixed positions as a solid held together by their opposite charges in an ionic lattice. Water is a good conductor of electricity but alone it doesn’t have the means to create that electrical charge. The common unit for charge is the Coulomb ("C"). Explanation: Answer:Ionic compounds conduct electricity when molten (liquid) or in aqueous solution (dissolved in water), because their ions are free to move from place to place. Ionic compounds do not conduct electricity in the solid state because the electrostatic forces of attraction between ions in the solid state are very strong. When an ionic substance is molten or dissolved, the ions that make it up are free to move within the substance and carry charge through it, i.e. Why do ionic compounds conduct electricity when molten/dissolved in water? conduct electricity.

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