![]() 1.3.7 use the accepted structural model for metals to predict and explain their structure and physical properties including melting point, malleability, ductility and electrical conductivity.Unit C1: Structures, Trends, Chemical Reactions, Quantitative Chemistry and Analysis.C2.2d describe and compare the nature and arrangement of chemical bonds in: v.1.40 Explain the properties of metals, including malleability and the ability to conduct electricity.Explain chemical bonding in terms of electrostatic forces and the sharing of electrons.Explain how the bulk properties of materials are related to the different types of bonds they contain, their bond strengths and the ways in which their bonds are arranged, recognising that the atoms themselves do not have these properties.4.6 Interactions over small and large distances.5.2.1 Chemical bonds, ionic, covalent and metallic.5.2 Bonding, structure and the properties of matter.The bonding in metals may be represented in the following form: (each electron associated with a positive core sea of delocalised electrons).The sharing of delocalised electrons gives rise to strong metallic bonds.The electrons in the outer shell of metal atoms are delocalised and so are free to move through the whole structure.Metals consist of giant structures of atoms arranged in a regular pattern.4.2.1 Chemical bonds, ionic, covalent and metallic.4.2 Bonding, structure and the properties of matter. ![]() Manufacture of iron (blast furnace - chemical aspects) and steel.Transition metal elements: general chemical properties (colour, variable valency, use as catalysts).The electrochemical series (reactions of metals with acids, water and oxygen not required).Option 2B: Additional electrochemistry and the extraction of metals.Comparison between metals and non-metals (hardness, lustre, malleability, ductility, heat conductivity and electrical conductivity).Explanations in terms of atomic radius, screening effect and nuclear charge for general trends in proprties of elements in groups I and VII.Oxidation and reduction in terms of loss and gain of electrons. ![]()
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