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Bonding and Structure, (Ionic Bonding**) - Coggle Diagram
Bonding and Structure
3. Metallic Bonding
- Occurs between metal atoms where electrons are delocalized, forming a "sea" of free-moving electrons around positively charged metal ions.
- A regular arrangement of positive metal ions surrounded by a sea of delocalized electrons.
- High Melting and Boiling Points:
- Due to strong metallic bonds between ions and delocalized electrons.
- Metals conduct electricity well due to the movement of delocalized electrons.
- Good conductors of heat as energy is transferred through the free-moving electrons.
- Malleability and Ductility:
- Metals can be hammered into shapes (malleable) and drawn into wires (ductile) because layers of atoms can slide over each other without breaking the metallic bond.
- Shiny surface due to reflection of light by delocalized electrons.
- Generally insoluble in water, though some metals can react with water.
2. Covalent Bonding
- Occurs between non-metal atoms where electrons are shared between atoms to achieve a full outer electron shell.
- Simple Molecular Structures:
- Water (H₂O), Carbon Dioxide (CO₂), Methane (CH₄).
- Low Melting and Boiling Points:
- Due to weak intermolecular forces (Van der Waals forces, dipole-dipole interactions, or hydrogen bonds).
- Do not conduct electricity because molecules have no overall charge and no free electrons or ions.
- Often gases or liquids at room temperature.
- Generally insoluble in water (exceptions include polar molecules like H₂O).
- Giant Covalent Structures:
- Diamond (C), Graphite (C), Silicon Dioxide (SiO₂).
- High Melting and Boiling Points:
- Due to strong covalent bonds throughout the structure.
- Very hard substances (e.g., diamond is the hardest natural material).
- Generally poor conductors (e.g., diamond), except graphite which has delocalized electrons that can move and conduct electricity.
- Insoluble in water and organic solvents due to strong covalent bonds.
- Occurs between metals and non-metals where electrons are transferred from the metal to the non-metal, resulting in the formation of oppositely charged ions.
- Regular, repeating 3D arrangement of positive and negative ions.
- High Melting and Boiling Points:
Due to strong electrostatic forces of attraction between oppositely charged ions, requiring a lot of energy to break.
- Conducts electricity when molten or dissolved in water because the ions are free to move.
- Does not conduct in solid form as ions are fixed in place.
- Generally soluble in polar solvents like water due to interaction between ions and polar molecules.
- Hardness and Brittleness:
- Hard due to strong ionic bonds.
- Brittle because any force that shifts the lattice causes ions of like charges to come together and repel, causing the structure to fracture.
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