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Atomic Structure of Metals
Metals have a unique atomic structure where atoms are arranged in a regular, closely-packed lattice. The outermost electrons (valence electrons) are loosely bound and can move freely throughout the metal, creating a "sea of electrons."
This free electron movement is the key to understanding all metallic properties!
Metallic Bond = Metal Ions + Sea of Electrons
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Why Metals Shine (Lustre)
When light hits a metal surface, the free electrons absorb and immediately re-emit photons. This rapid absorption and re-emission creates the characteristic metallic shine. The smoother the surface, the more uniform the reflection.
Polished metals reflect up to 95% of incident light!
Lustre ∝ Free Electron Density × Surface Smoothness
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Electrical Conductivity Mechanism
When a voltage is applied, free electrons drift in one direction, creating electric current. Unlike insulators, metals have no energy gap between valence and conduction bands, allowing electrons to move freely.
Silver is the best conductor, followed by copper and gold!
σ = n × e × μ (Conductivity = electron density × charge × mobility)
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Malleability & Ductility
The metallic bond is non-directional, meaning atoms can slide past each other without breaking bonds. When force is applied, layers of atoms slip over each other while maintaining the metallic bond through the sea of electrons.
Gold can be beaten into sheets only 0.0001mm thick!
Deformation = Slip of Atomic Layers (Bonds remain intact)
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Sonorous Nature Explained
When struck, metal atoms vibrate in a coordinated manner due to strong metallic bonds. These vibrations travel through the metal as sound waves with minimal energy loss, producing clear, sustained tones.
The metallic bond allows vibrations to travel efficiently!
Sound Quality ∝ Bond Strength × Atomic Mass