Chemical Bonds

• Giant Covalent Structure ( main characteristics)

  • high b.p. + m.p.
  • non metal to non metal bond
  • examples=diamond, graphite,
  • can't conduct electricity (except graphite)
• Simple Covalent Structure (main characteristics)


  • non metal to non metal bond
  • low m.p + b.p. as the intermolecular forces are weak so not a lot of energy is required to break these down
  • can't conduct electricity (?)
• Metallic Bonds (main characteristics)

  • high m.p. + b.p.
  • metal to metal bonds
  • can conduct thermal energy + electricity
• Ionic Compounds (main characteristics)


  • metal to non metal bond
  • can only conduct electricity when molten or dissolved in an aqueos solution
  • high m.p +b.p.
• Giant Covalent Structure


  Arrangement of atoms in a molecule where a large number of atoms are bonded together through covalent bonds
• High Boiling Point & Melting Point


  Strong intermolecular forces between covalently bonded atoms
• Non-Metal to Non-Metal Bond


  Atoms from the same group or family on the periodic table, but not metals
• Diamond & Graphite


  Both are giant covalent structures; diamond is extremely hard and rigid, while graphite is soft and slippery
• Poor Electrical Conductivity (except Graphite)


  Molecules held together tightly, making it difficult for electrons to move freely; graphite is an exception
• Ionic Compound


  A type of compound formed by the transfer of electrons from a metal to a nonmetal, resulting in the formation of positive and negative ions.
• Metal-to-Nonmetal Bond

  The attractive force that holds positive ions (cations) and negative ions (anions) together in a crystal lattice structure, forming an ionic compound.
• Conductivity of Ionic Compounds


  Ionic compounds are poor conductors of electricity in their solid state, but they can conduct electricity when melted or dissolved in an aqueous solution.
• Melting Point (m.p.) + Boiling Point (b.p.) of Ionic Compounds


  High due to the strong electrostatic attractive forces between the ions in the crystal lattice structure of the ionic compound.
• High Melting Point


  Metallic bonds have a high melting point due to strong atomic bonds
• High Boiling Point


  Metallic bonds have a high boiling point due to strong atomic bonds
• Metal-to-Metal Bonds


  Metallic bonds occur between metal atoms, not metal and non-metal atoms
• Conduct Thermal Energy

  Metallic bonds allow for easy transfer of thermal energy
• Conduct Electricity

  Metallic bonds facilitate the flow of electricity due to free-moving electrons
• Non-Metal to Non-Metal Bond


  A type of bond formed between two non-metal atoms, where each atom shares one or more valence electrons to form a molecule.
• Low Molar Mass


  The sum of the atomic masses of the atoms in a covalent compound is typically low compared to ionic compounds.
• Low Melting Point (m.p.) and Boiling Point (b.p.)


  The weak intermolecular forces in covalent compounds require relatively little energy to overcome, resulting in lower melting and boiling points.
• Poor Electrical Conductivity


  Covalent compounds usually do not conduct electricity because the electrons involved in the bond are localized within the molecules and are not free to move.
• Ionic Compound


  A compound formed from ions, atoms or groups of atoms that have gained or lost electrons.
• Cation


  A positive ion, formed when an atom loses one or more electrons.
• Anion


  A negative ion, formed when an atom gains one or more electrons.
• Metal-to-Nonmetal Bond


  The attractive force between cations and anions that holds them together in a crystal lattice structure.
• Crystal Lattice Structure


  A regular, repeating pattern of atoms or molecules that make up a solid crystal.