Why can metals bend without breaking and conduct electricity so effectively?
In short: Metallic properties like conductivity and malleability are rooted in atomic structure. This video explores how delocalized electrons and crystal lattice imperfections dictate how metals behave, react, and interact with the world around us.
Metals are defined by their ability to conduct heat and electricity, their malleability, and their reflectivity. At the atomic level, these traits arise because metal atoms typically have fewer than half the electrons needed to fill their outermost shell. In simple metals, these valence electrons become delocalized, moving freely throughout the solid as a collective, which explains their high conductivity. In transition metals, this behavior is further explained by band theory, which accounts for interactions with d electrons.
The physical durability of metals—their ability to be shaped without shattering—is often due to imperfections within their crystalline structure. The absence of specific atomic layers allows metals to deform plastically rather than fracturing. While most metals are found in ores, some, such as gold and platinum, exist in a free state due to their low chemical reactivity. Conversely, highly reactive metals like lithium and potassium readily combine with nonmetals like oxygen.
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Sources
- Summary by Intellect · source: Properties of metals | HS Chemistry | Khan Academy
- Also: Metal | Definition, Characteristics, Types, & Facts | Britannica
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