bonding

• what sort of elements are involved in metallic bonding?

  metals
• Explain the melting points of metals

  Strong electrostatic attraction between positive metal ions and negative delocalised electrons which takes a lot of energy to break
• explain why metals are used to make ovens and wires

  Thermal conductivity

  Strength

  Ductile

  Electrostatic conductivity
• What forces hold metals atoms in place in their structure?

  electrostatic forces of attraction
• define ductile

  drawn into wires
• malleable


  can be hammered into shape
• Why are the layers in metal structures useful?

  They can easily slide over one another so they can change shape without breaking bonds
• what is an alloy?

  Mixture of metals
• Why are metals good conductors of electricity

  They have delocalised electrons which allows them to carry change + more
• what are free/delocalised electrons?

  electrons which are not held in place and can move around a structure
• Why are metals good conductors of heat?

  They contain delocalised electrons which can move and carry thermal energy
• what type of elements are involved in ionic bonding?

  metals and non-metals
• what is the formula of magnesium oxide?

  MgO
• what is the formula of sodium chloride?

  NaCl
• what is the formula of aluminium oxide?

  Al2O3
• what is the formula of zinc bromide?

  ZnBr2
• describe the melting point of ionic compounds

  high as they contain strong ionic bonds
• do ionic compounds conduct electricity when solid? Explain your answer

  No because they don't contain any delocalised electrons - ions are fixed in position and can't move
• explain what happens during the formation of sodium chloride

  sodium have one free electron whereas chlorine needs one electron to have a full outer shell. So sodium transfers one electron to chlorine. A Na+ and Cl- ion are formed
• explain why ionic compounds have high melting points

  strong electrostatic forces of attraction between oppositely charged ions which require lots of energy to break
• how strong are the bonds between each of the ions in an ionic compounds?

  very strong
• describe the ionic structure of sodium chloride

  giant ionic lattice

  alternating positive and negative ions in a regular arrangement in a fixed position
• what do the Noble gases not react?

  they already contain a full outer shell
• what type of elements are involved in covalent bonding?

  non-metals
• describe the bonding in a diamond

  strong electrostatic attraction between a shared pair of electrons and the bonded nuclei
• do covalent compounds conduct electricity. Explain why

  no as electrons are not free to move except in graphite
• why do simple covalent compounds have low boiling points?

  contain weak intermolecular forces which don't require much energy to break
• what type of structure are diamonds, graphite and SiO2

  giant covalent
• why do giant covalent compounds have high melting points?

  strong electrostatic attraction between a shared pair of electrons and the bonded nuclei
• why doesn't diamonds conduct electricity?

  It doesn't contain delocalised electrons as it reacts with 4 carbons- electrons are fixed and can't move
• why does graphite conduct electricity?

  as each molecule only reacts with 3 carbons, it has one delocalised electron
• Describe the bonding in graphite

  weak forces (NOT INTERMOLECULAR) between layers allowing the to slide

  Strong covalent bonds between carbon atoms

  each molecule is bonded to 3 other carbon molecules
• describe the bonding in SiO2

  Strong covalent bonds (1:2 ratio)

  strong electrostatic attraction between shared pair of electrons and the bonded nuclei
• what is an ionic lattice

  regular arrangement of positive and negative ions which repeats in all directions
• what do ionic compounds made with 2 different elements end with


  -ide
• what do ionic compounds with 3 or more elements end in?


  -ate