Structure 2.3 The metallic model
Structure 2.3.1 and 2.3.2
- 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).
- 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).
- 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).
- 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?
HL content (2.3.3 only)
- Transition elements have delocalized d-electrons.
- Explain the high melting point and electrical conductivity of transition elements.
- Chemical properties of transition elements are covered in Reactivity 3.4.
- Structure 3.1 Why is the trend in melting points of metals across a period less evident across the d- block?
Video coming soon.