ionic bonding, metalic bonding and structure

• What is an ion?

  An atom that has lost/gained electrons
• Which kinds of elements form ionic bonds?

  Metals and non-metals
• What charges do ions from Group 1 form?

  1+
• What charges do ions from Group 2 form?

  2+
• What charges do ions from Group 6 form?

  2-
• What charges do ions from Group 7 form?

  1-
• What force holds oppositely charged ions together?

  Electrostatic force of attraction
• Describe the structure of a giant ionic lattice.

  Alternating positive/negative ions held by electrostatic forces
• Why do ionic substances have high melting points?

  Strong electrostatic forces need lots of energy
• Why don't ionic substances conduct electricity when solid?

  Ions are in fixed positions
• When can ionic substances conduct electricity?

  When melted or dissolved
• Why do ionic substances conduct electricity when melted/dissolved?

  Ions are free to move
• Describe the structure of a pure metal.

  Regular arrangement of positive ions
• Describe the bonding in a pure metal.

  Positive ions with delocalised electrons
• What are four properties of pure metals?

  Malleable, ductile, conductors, high melting points
• Explain why pure metals are malleable.

  Layers of ions can easily slide
• Explain why metals have high melting/boiling points.

  Strong metallic bonds need much energy
• Why are metals good conductors of electricity and thermal energy?

  Delocalized electrons carry charge/energy
• What is an alloy?

  A mixture of two or more metals
• Explain why alloys are harder than pure metals.


  Disrupt layers, so they can't slide
• Which groups form 1+ ions?

  Group 1
• Which groups form 2+ ions?

  Group 2
• Which group forms 2- ions?

  Group 6
• Which group forms 1- ions?

  Group 7
• Why do ionic compounds have high boiling points?

  Strong electrostatic attraction between ions
• What force holds ions together in a crystal lattice?

  Electrostatic force of attraction
• What structure do ionic compounds form?

  Giant ionic lattice structure
• What type of ions are in a lattice structure?

  Alternating positive and negative ions
• What force holds ions together in a lattice structure?

  Electrostatic force of attraction
• Why do ionic bonds require lots of energy to break?

  Electrostatic force of attraction is strong
• Why are ions fixed in position in a solid ionic compound?

  Ions cannot move in solid state
• Do solid ionic compounds contain delocalized electrons?

  No, there are no delocalised electrons
• How does the movement of ions change when an ionic compound melts or dissolves?

  Ions are free to move and carry charge
• What surrounds layers of positive metal ions in metals?

  Delocalised electrons
• What is the nature of the attractive forces in metals?

  Electrostatic forces between ions and electrons
• What are the typical properties of metals?

  • Malleable
  • High melting/boiling points
  • Good conductors of electricity
  • Good conductors of thermal energy
• Why are metals malleable?

  Layers can slide over each other easily
• Why do metals have high melting points?

  Strong electrostatic forces require much energy to break
• How do delocalized electrons contribute to electrical conductivity?

  They are free to move through the metal
• What is a metal alloy?

  Mixture of a metal with another element