how do metals conduct heat

Metals conduct heat primarily due to the free-moving electrons within them. These electrons are not bound to any particular atom and can move freely throughout the metal's structure. When one end of a metal is heated, the electrons at that end gain thermal energy and start vibrating more rapidly. These energetic electrons then move through the metal, colliding with other atoms and electrons, effectively transferring heat energy from the hot end to the cold end. This mechanism allows metals to conduct heat much faster and more efficiently than non-metals, where heat is transferred only through vibrations of atoms. In addition, the regular crystal lattice structure of metals allows atoms to vibrate and pass energy efficiently, further aiding thermal conductivity. The extent of heat conduction varies among metals, largely depending on how freely electrons can move before colliding with impurities or lattice irregularities. Pure metals like copper, silver, and gold typically conduct heat better than alloys or impure metals because their electrons move with less resistance. In summary, the combination of free, mobile electrons and an orderly atomic lattice enables metals to be excellent heat conductors.