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Why are metals good conductors?
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Metals are good conductors of electricity and heat due to their unique atomic structure and the presence of delocalized electrons.
- Atomic Structure: Metals have a structure where the outermost electrons of the atoms are not tightly bound to individual atoms. Instead, they are free to move throughout the entire metal lattice.
- Delocalized Electrons: These free electrons, also known as delocalized electrons or a "sea of electrons," can move easily when an electric field or heat is applied.
- Electrical Conductivity: When a voltage is applied across a metal, these delocalized electrons drift in a specific direction, creating an electric current. The ease with which these electrons move determines the metal's electrical conductivity.
- Thermal Conductivity: Similarly, when one part of a metal is heated, the delocalized electrons gain kinetic energy and transfer this energy to other electrons and atoms throughout the metal, resulting in efficient heat conduction.
Examples of highly conductive metals include copper, silver, gold, and aluminum.
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