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Chemistry

1. Principles of Chemistry
1.2 Elements, Compounds & Mixtures>1.3 Atomic Structure>1.4 The Periodic Table>1.5 Chemical Formulae, Equations and Calculations>1.6 Ionic Bonding>1.7 Covalent Bonding>1.8 Metallic Bonding>1.9 Electrolysis>

2. Inorganic Chemistry

2.1 Group 1 (Alkali Metals) – Lithium, Sodium and Potassium >2.2 Group 7 (Halogens) – Chlorine, Bromine and Iodine >2.3 Gases in the Atmosphere >2.4 Reactivity Series >2.5 Extraction and Uses of Metals >2.6 Acids, Alkalis and Titrations >2.7 Acids, Bases and Salt Preparations >2.8 Chemical Tests >

3. Physical Chemistry

3.1 Energetics >3.2 Rates of Reaction >3.3 Reversible Reactions and Equilibria >

4. Organic Chemistry

4.1 Introduction >4.2 Crude Oil >4.3 Alkanes >4.4 Alkenes >4.5 Alcohols >4.6 Carboxylic Acids >4.7 Esters >4.8 Synthetic Polymers >

1.8 Metallic Bonding

1.8.1C Know how to represent a metallic lattice by a 2-D diagram

RECALL

Metals tend to lose electrons to form full electron shells
They form positive cations

Metal ions are held together strongly by metallic bonding

Atoms are arranged in a lattice
Electrons lost by the metal atoms are delocalised
The delocalised electrons move freely between the positive metal ions like a sea of electrons

1.8.2C Understand metallic bonding in terms of electrostatic attractions

Metallic Bonding

Electrostatic attraction forces between positive metal ions lattice and negative delocalised electrons

1.8.3C Explain typical physical properties of metals, including electrical conductivity and malleability

Metals have high melting and boiling points due to strong metallic bonds that require high levels of energy to break.
Metals are malleable (can be hammered into thin sheets) as layers of positive ions can slide over each other without breaking the metallic bonds.