Structure 2.3: Flashcards
Master the definitions and trends.
Define Metallic Bonding
The electrostatic attraction between a lattice of positive ions (cations) and delocalized valence electrons.
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Why are metals malleable?
The bonding is non-directional. Layers of cations can slide over each other without breaking the attractive forces to the electron sea.
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Trend: Melting Point of Group 1 Metals
Decreases down the group. Ionic radius increases, weakening the attraction between the nucleus and the delocalized electrons (charge remains constant).
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Explain the high melting point of Aluminum vs Sodium
Al³⁺ has a higher charge and smaller radius than Na⁺. It also contributes 3 electrons to the sea vs 1. Higher charge density = stronger bond.
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Define Delocalization
Valence electrons are not associated with a single atom but are free to move throughout the entire lattice structure.
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Transition Metals vs s-block Melting Points (HL)
Transition metals have significantly higher melting points because they can delocalize 3d electrons as well as 4s electrons, increasing bond strength.
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Electrical Conductivity Mechanism
Mobile delocalized electrons move towards the positive terminal when a potential difference is applied, carrying charge.
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