Bonding

• Infinite Lattice


  The network structure of a giant covalent substance continues indefinitely in three dimensions.
• Hard and Brittle

  Giant covalent substances are typically hard and brittle, meaning they break easily and are prone to cracking.
• High Melting and Boiling Points


  Giant covalent substances have high melting and boiling points due to the strong covalent bonds between atoms.
• High Thermal Conductivity


  Giant covalent substances are good heat conductors, meaning they efficiently transfer heat.
• Ionic Compounds

  Metals (low electron affinity) lose electrons, nonmetals (high electron affinity) gain electrons, leading to formation of ionic compounds
• Simple molecular substances cannot conduct electricity because they have no charge
• Intermolecular forces are Weak attractive forces between molecules. When a simple molecular substance melts or boils, it is the intermolecular forces that are broken (not the covalent bonds in each molecule).
• Fullerenes

  Giant covalent substance that forms a large hollow shape

  A) Hollow

  B) hexagonal rings

  C) strong structure

  D) cant conduct electricity

  E) lubricants

  F) no unpaired electrons

  
• Graphene

  A giant covalent substance made of layers of hexagonal rings

  A) high melting + boiling points

  B) soft, weak forces

  C) good electricity conductor

  D) unbonded electrons

  E) good heat conductor

  
• Diamond

  A giant covalent substance with a tetrahedral shape to it

  A) rigid structure

  B) doesnt conduct electricity

  C) high melting point

  D) high thermal conductivity

  
• Metallic bonding occurs between metal atoms where they lose electrons to form positive ions that are held together by electrostatic attraction.
• Covalent bonds are formed when two atoms share their outermost electron shells, forming a molecule with an overall neutral charge.
• The metallic lattice has delocalised electrons which can move freely throughout the whole solid. This gives metals their electrical and thermal conductivity.
• In ionic solids, the ions are arranged in a regular repeating pattern known as a crystal lattice.
• Ionic compounds consist of positively charged ions called cations and negatively charged ions called anions. The ions are held together by electrostatic attractions.
• 


  Covalent- Non-metals only

  Ionic- Metals and non metals

  Metallic- Metals only
• Ionic bonding


  When there is a strong electrostatic attraction between positive and negative ions.
• Covalent bonding


  A shared pair of electrons
• Metallic bonding


  A strong electrostatic attraction between positive ions and negative delocalised ions