As a specialist in the field of materials science, I can provide you with a comprehensive understanding of how metals conduct electricity and their behavior in aqueous solutions.

Metals are known for their excellent electrical conductivity, which is primarily due to the presence of free electrons within their atomic structure. These electrons are not tightly bound to any particular atom but are free to move throughout the metal lattice. When an electric field is applied across a metal, these electrons move in response to the field, creating an electric current. This movement of electrons is what allows metals to conduct electricity effectively.

However, when we discuss metals in an aqueous solution, the situation becomes more complex. An aqueous solution is a mixture in which the solute, in this case, the metal, is dissolved in a solvent, typically water. The solubility of metals in water varies greatly, with some metals being insoluble or only slightly soluble, while others can form ions that dissolve readily.

The solubility and subsequent conductivity of a metal in water depend on several factors, including the metal's reactivity and the pH of the solution. Reactive metals, such as sodium, potassium, and calcium, react vigorously with water to form metal hydroxides and hydrogen gas. This reaction can disrupt the metal's ability to conduct electricity because the metal is no longer present in its metallic form but has been converted into ions.

On the other hand, less reactive metals, such as copper, silver, and gold, do not react with water under normal conditions and are considered insoluble in water. These metals will not dissolve to form ions that can conduct electricity. However, if these metals are already in the form of ions, they can contribute to the conductivity of the solution. For example, a solution of copper sulfate contains copper ions that can move to conduct electricity.

It is important to note that the presence of ions in a solution is what facilitates its conductivity. Pure water, as mentioned, has very few ions and thus is a poor conductor of electricity. The addition of salts, such as table salt (sodium chloride), increases the number of ions in the solution, enhancing its ability to conduct electricity. When table salt dissolves in water, it dissociates into sodium and chloride ions, which are free to move and carry charge, thus increasing the solution's conductivity.

In summary, metals conduct electricity due to the movement of free electrons within their structure. In an aqueous solution, the conductivity of metals depends on their solubility and the ability to form ions that can move freely. Reactive metals that form ions upon reacting with water can contribute to the solution's conductivity, while less reactive metals that do not dissolve will not. The presence of ions in a solution, whether from dissolved salts or metal ions, is crucial for its electrical conductivity.

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When a metal conducts electricity, the charge is carried by electrons moving through the metal. ... Pure water contains very few ions, so it does not conduct electricity very well. When table salt is dissolved in water, the solution conducts very well, because the solution contains ions.read more >>