Structure 2.3 The metallic model 
Structure 2.3.1 and 2.3.2
Understandings:
  • A metallic bond is the electrostatic attraction between a lattice of cations and delocalized electrons (2.3.1).
  • The strength of a metallic bond depends on the charge of the ions and the radius of the metal ion (2.3.2).
Learning outcomes:
  • Explain the electrical conductivity, thermal conductivity and malleability of metals (2.3.1).
  • Explain trends in melting points of s and p block metals (2.3.2).
Additional notes:
  • Relate characteristic properties of metals to their uses (2.3.1).
  • A simple treatment in terms of charge of cations and electron density is required (2.3.2).
Linking questions:
  • Structure 3.1 What experimental data demonstrate the physical properties of metals, and trends in these properties, in the periodic table?
  • Reactivity 3.2 What trends in reactivity of metals can be predicted from the periodic table?
  • Structure 2.4 What are the features of metallic bonding that make it possible for metals to form alloys?
This video covers metallic bonding and the properties of metals. 
HL content (2.3.3 only)
Structure 2.3.3
Understandings:
  • Transition elements have delocalized d-electrons.
Learning outcomes:
  • Explain the high melting point and electrical conductivity of transition elements.
Additional notes:
  • Chemical properties of transition elements are covered in Reactivity 3.4.
Linking questions:
  • Structure 3.1 Why is the trend in melting points of metals across a period less evident across the d- block?
Video coming soon.