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Introduction: What is Metallic Bonding?
Metallic bonds are a type of chemical bond found in metals and metallic alloys. They form when the valence electrons of atoms delocalize and freely flow within the formed lattice structure.
Delocalized Electrons: Electrons that aren't bound to a specific atom and can freely flow within a structure or molecule.
Nondirectional Bonding: Electrons aren't shared between specific atoms.
Lattice Structure: The atoms are arranged in a repeating pattern.
How Metallic Bonding Works
Metal atoms are capable of forming metallic bonds due to:
Loosely-bound electrons. (essential for delocalization)
Low electronegativity. (prevents electron localization)
Low electronegativity difference.
Metallic bonding makes lattice structure possible, yet lattice structures reinforce metallic bonding.
Metallic Alloys
Substitutional Alloy: Metallic elements with similar atomic radii replace atoms in the host metal's lattice, forming a relatively uniform structure. (e.g. brass, composed of copper and zinc)
Interstitial Alloy: Smaller atoms fit into the spaces between larger metal atoms in the lattice. (e.g. steel, consisting of iron and carbon)
Properties of Metallic Compounds
Bond Strength: Strong intramolecular forces due to electrostatic attraction between the ions and the electrons.
High melting point.
Polarity: Metallic bonds are considered nonpolar due to the delocalized, nondirectional "sea" of electrons.
Solubility: Depends on reactivity. More reactive metals may undergo redox reactions with solvents, forming aqueous ions.
Conductivity: Highly conductive due to the delocalized electrons within the metal.
Physical Property:
Malleable and ductile, as the "sea" of electrons gives the lattice flexibility under pressure.
Has relatively higher luster, as the abundance of delocalized electrons on the surface reflects light effectively.
More inert metals reflect more light due to resistance from oxidation.
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