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Why do metals conduct electricity? — Let’s start with “electron gas”
In chemistry and physics, we often say that the electrons in metals are "active." But what exactly is going on?
According to electron theory, the valence electrons in metals are actually loosely bound to the atomic nuclei. Unlike in molecules, they are not tightly bound, but can freely "jump" from one atom to another.
These freely mobile electrons form a cloud of "electron gas" within the metal. While the name sounds a bit abstract, it's essentially a group of electrons roaming around, behaving somewhat like ordinary gas molecules.
At the same time, atoms that have lost their valence electrons become positively charged metal ions. These ions don't just wander around; they're neatly arranged at the junctions of the metal's crystal lattice.
So, we can think of metals as:
On one side, neatly arranged metal ions; on the other, a freely moving electron gas.
This structure explains some important properties of metals, such as:
Conductivity: This is because the electron gas can move in a directed manner under an applied electric field.
Heat conduction: The movement of electrons quickly transfers energy.
Ductile: ions can slide relative to each other in the lattice, and the electron gas acts as a "lubricant."
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