Retreival part 1

• Name the three types of chemical bond.

  Ionic, covalent and metallic
• Define ionic bonding.

  Electrostatic attraction between oppositely charged ions.
• Define covalent bonding.

  Electrostatic attraction between a positive nucleus and a shared pair of negative electrons
• Define metallic bonding.

  Electrostatic attraction between positively charged ions and delocalised electrons
• Define metallic bonding.

  Electrostatic attraction between positively charged ions and delocalised electrons.
• What type of atoms form ionic bonds?

  Non-metals with metals.
• What type of atoms form covalent bonds?

  Non-metals only.
• What type of atoms form metallic bonds?

  Metals only.
• What happens to the metal atoms in ionic bonding?

  They lose their outer shell electrons to have a full shell and form a positively charged ion.
• What happens to the non-metal atoms in ionic bonding?

  They gain outer shell electrons to fill their shell and become negatively charged ions.
• Why do atoms become ions?

  To attain a full outer electron shell.
• Name the first three halide ions.

  Fluoride, chloride and bromide.
• Name and write the formula of the GCSE molecular positive ion.

  Ammonium, NH4+.
• Name and write the formula of the GCSE molecular 1- ions.

  Hydroxide, OH- and nitrate, NO3-
• Name and write the formula of the GCSE molecular 2- ions.

  Sulfate, SO42- and carbonate, CO32-.
• Name and write the formula of the GCSE molecular 3- ion.

  Phosphate, PO43-.
• What are the limitations of the particle model?

  There are no forces, that all particles are represented as spheres and that the spheres are solid.
• What determines the melting and boiling point of a material?

  The strength of the forces between the particles.
• State the structure of an ionic compound

  Giant ionic lattice.
• Describe the bonding in an ionic material.

  Strong electrostatic attraction between oppositely charge ions in all directions.
• Describe the melting points of ionic materials.

  High.
• Describe the conduction of electricity of ionic solids.

  None because the ions are not able to move and carry the charge throughout the structure.
• Describe the conduction of electricity of ionic liquids or solutions.


  Good because the ions are able to move and carry the charge throughout the structure.
• State the structure of a covalent compound.

  Small molecule.
• Describe the bonding in a simple, covalent material.

  Weak intermolecular forces that require little energy to break. Strong covalent bonds that don't break easily.
• Describe the melting points of small molecules

  Weak.
• What is the typical state of a small molecule?

  Liquid or gas
• Describe the conduction of electricity in small molecules.

  None because there are no delocalised electrons or ions that can move and carry the charge throughout the structure.
• Compare the melting point of a smaller small molecule versus a larger small molecule.

  Larger small molecules have larger melting points
• What happens to the strength of a weak intermolecular force as molecules

  become larger?

  They get stronger.
• Name the materials that can be described as Giant Covalent Lattices.

  Diamond, Graphite, Silica and Graphene.
• Describe the bonding in Diamond.

  Each carbon is strongly, covalently bonded to 4 others.
• Describe the bonding in Graphite.

  Each carbon is strongly, covalently bonded to 3 others and has one delocalised electron. They form hexagonal layers that have weak intermolecular forces.
• Describe the bonding in Silica.

  Each silicon is strongly, covalently bonded to 4 oxygen atoms.
• What are the melting points like in giant covalent lattices?

  High.
• Which of the giant covalent materials conduct electricity?

  Graphite and graphene.
• Explain why two of the giant covalent materials conduct electricity.

  They have delocalised electrons that carry the charge throughout the structure.
• Compare conduction of electricity in graphite to a molten ionic compound.

  Graphite has delocalised electrons, ionic has ions that can move.
• What two properties are unique to graphite?

  Conducts electricity and soft and slippery.
• How does diamond differ from graphite in terms of electrical conductivity and hardness/softness?