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Metallic Bonds:

Learn about the fundamentals of metallic bonds using the Electron Sea Model and explore the intricacies of ionic crystals and lattice energy. Discover key properties of metals and ionic compounds such as conductivity, malleability, and high melting points.

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Metallic Bonds:

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  1. Metallic Bonds: • Metal atoms form bonds when the outer energy levels overlap. • This is called the Electron Sea Model. • It proposes that all the metal atoms in a metallic solid donate their electrons to form a “sea” of electrons. • These free moving electrons are also called delocalized electrons.

  2. Properties of Metals • Conduct electricity and heat • High melting and boiling points • Hard and dense • Metals are malleable (hammered into sheets) and ductile (drawn into a wire). • Form alloys (a mixture of elements that have metallic properties). • Examples: steel, bronze, cast iron, gold 10 carat, brass.

  3. IONIC CRYSTALS • In ionic compounds, the positive and negative ions are packed into a pattern. • This particle packing forms an ionic crystal. • Crystals require a large amount of energy to break apart.

  4. CRYSTAL LATTICE • Attraction between + and - ions results in a crystal lattice. • Each positive ion is surrounded by negative ions.

  5. LATTICE ENERGY • Lattice energy = the energy released when an ionic crystalline compound is formed. • The more negative the lattice energy, the stronger the force of attraction between ions • Smaller ions have more negative lattice energy • Higher charges make for more negative lattice energies (example: MgO has more lattice energy than NaF)

  6. Ionic Properties • Made of crystals • Have high melting points • Often soluble in water • Conduct electricity in water

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