Metallic Bonding

• What type of structures does metallic bonding occur in?

  Giant lattice structures
• What happens to the outer electrons in metallic bonding?

  They become delocalized and move freely
• What forms the 'sea of electrons' in metallic bonding?

  Delocalized electrons surrounding metal ions
• What creates strong electrostatic forces in metallic bonding?

  The attraction between electrons and metal ions
• What is a characteristic property of metals regarding melting points?

  They generally have high melting points
• Why do metals with more delocalized electrons have stronger metallic bonds?

  More delocalized electrons create stronger attractions
• How do smaller metal ions affect metallic bonding?

  They increase charge density and strengthen bonds
• What is the melting point of gold described as?

  Very high melting point
• Why are metals ductile?

  Metal ions can slide past each other
• What is copper widely used for due to its properties?

  Electrical wiring
• Why are metals excellent conductors of electricity?

  Delocalized electrons move freely
• Are metals soluble in water?

  No, they are generally insoluble
• What is silver known for in terms of conductivity?

  Outstanding conductor of electricity
• What happens to particles in a solid?

  They are closely packed and vibrate in place
• What occurs when solids are heated?

  They melt into liquids as particles gain energy
• How do particles behave in a liquid?

  They move around each other but stay in contact
• What happens to liquids when heated?

  They evaporate or boil into gases
• How do gas particles behave?

  They move rapidly and independently
• What occurs when gases are cooled?

  They condense into liquids
• What is the structure of particles in a solid?

  They are tightly packed in a fixed structure
• How do particles in a liquid behave compared to solids?

  They can move around each other
• What is the arrangement of particles in a gas?

  Particles are far apart and move freely
• What are the two types of covalent substances?

  Simple molecular and giant covalent
• Why do simple molecular substances have low melting points?

  Weak intermolecular forces need to be overcome
• At what temperature does water boil?

  100°C
• Why do giant covalent structures have very high melting points?

  Extensive strong covalent bonds require much energy
• What is the melting point of diamond?

  About 3550°C
• How does each carbon atom bond in diamond?

  Each bonds to four others in a lattice
• How do the physical properties of materials relate to their bonding types?

  • Ionic: High melting/boiling points, conducts when molten or dissolved, generally soluble in water.
  • Giant covalent: Very high melting/boiling points, generally does not conduct, generally insoluble in water.
  • Simple molecular: Low melting/boiling points, does not conduct, solubility depends on polarity.
  • Metallic: Generally high melting/boiling points, conducts in solid state, generally insoluble in water.
• What type of bonding results in high melting and boiling points?

  Ionic and giant covalent bonding
• What determines the solubility of simple molecular substances?

  Polarity of the molecules and solvents
• Why do metallic substances conduct electricity?

  They have delocalized electrons that move
• What is the general solubility of metallic substances in water?

  Generally insoluble