Introduction
Metals are amongst the most important materials in society for their useful properties. This chapter looks at the underlying structure of metals and how these properties arise.
Structure 2.3.1 - A metallic bond is the electrostatic attraction between a lattice of cations and delocalized electrons.
- Explain the electrical conductivity, thermal conductivity and malleability of metals.
Guidance
- Relate characteristic properties of metals to their uses.
Tools and links
- Tool 1, Inquiry 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 2.3.2 - The strength of a metallic bond depends on the charge of the ions and the radius of the metal ion.
- Explain trends in melting points of s and p block metals.
Guidance
- A simple treatment in terms of charge of cations and electron density is required.
Tools and links
- Structure 2.4 - What are the features of metallic bonding that make it possible for metals to form alloys?
Structure 2.3.3 - Transition elements have delocalized d-electrons. (HL)
- Explain the high melting point and electrical conductivity of transition elements.
Guidance
- Chemical properties of transition elements are covered in Reactivity 3.4.
Tools and links
- Structure 3.1 - Why is the trend in melting points of metals across a period less evident across the d-block?