Can someone explain the electrical conductivity of melted and of aqueous solutions of ionic compounds. An explain it using the characteristics of ionic compounds.
ThankS A Whole lot.. In Advance
I suggest you go to the site recommended by Ms.Sue. Here is a brief summary but this summary may help put the entire article in perspective.
When an ionic compound, for example NaCl, dissolves in water, the solid crystal structure is broken and the NaCl dissolves, leaving sodium ions (Na^+) and chloride ions (Cl^-) in solution. When electrodes are placed into the solution, the positive electrode will attract the negative ions (the chloride ions) and the negative electrode will attract the positive ions (the sodium ions).(Unlike charages attract.) This movement of ionic particles in solution is what conducts the electric current from one electrode to the other. In molten NaCl (which must be heated to a high temperature--I think about 800 or so degrees C--to melt), the liquid consists of Na^+ and Cl^- and, again, these ionc conduct electricity from one electrode to the other. The solid crystal actually consists of Na^+ and Cl^- but they are locked into position by the forces that hold the ions in their crystalline lattice. As such, the solid does not conduct electrcity because the ions are not free to move abouat. The conduction by the molten material confirms that the solid consists of ions. I hope this helps you get started.
The electrical conductivity of melted and aqueous solutions of ionic compounds can be explained using the characteristics of ionic compounds.
Ionic compounds are made up of positively charged ions (cations) and negatively charged ions (anions) that are held together by strong electrostatic forces in a crystal lattice structure. In the case of NaCl (sodium chloride), for example, it consists of sodium ions (Na+) and chloride ions (Cl-) arranged in a repeating pattern.
When an ionic compound dissolves in water, the crystal lattice structure breaks apart, and the individual ions separate from each other. In the case of NaCl, when it dissolves, it dissociates into sodium ions and chloride ions in the solution.
In an aqueous solution of an ionic compound, the positively charged ions (cations) are attracted to the negative electrode (cathode), while the negatively charged ions (anions) are attracted to the positive electrode (anode). This movement of ions in the solution allows for the flow of electric current.
The movement of ions in the solution is facilitated by the presence of water molecules. The water molecules surround the ions and help to separate them from each other, allowing them to move freely in the solution.
In the case of melted ionic compounds, such as molten NaCl, the solid crystal lattice structure is completely broken down, and the sodium ions and chloride ions are free to move throughout the liquid. The liquid molten NaCl can therefore conduct electricity because the ions are mobile and can carry the electric charge from one electrode to the other.
It should be noted that in the solid state, where the ions are tightly locked into the crystal lattice structure, the ionic compound does not conduct electricity because the ions are not free to move.
In conclusion, the electrical conductivity of melted and aqueous solutions of ionic compounds can be explained by the dissociation of the compound into individual ions in the solution, allowing for the movement of ions and the flow of electric current.