3.1.3
Bonding
AQA 3.1.3 covers ionic, covalent and metallic bonding, bonding and physical properties, shapes of molecules and ions, bond polarity and intermolecular forces. This topic links structure, bonding and forces to melting point, conductivity, crystal structure and molecular shape.
Revision Notes
Work through each part of AQA 3.1.3 in a structured sequence.
Bonding
Ionic Bonding
Electrostatic attraction between oppositely charged ions in a lattice, ionic formulae and properties.
Start revisingBonding
Covalent Bonding
Single, multiple and dative covalent bonds, including line and arrow representations.
Start revisingMolecules
Shapes of Molecules and Ions
Electron-pair repulsion, lone pairs, bond angles and shapes of simple molecules and ions.
Start revisingPolarity
Bond Polarity
Electronegativity, polar covalent bonds and why some molecules have permanent dipoles.
Start revisingMetallic Bonding
Attraction between delocalised electrons and positive ions arranged in a lattice.
Start revisingCovalent
Giant Covalent Structures
Macromolecular structures such as diamond and graphite, and their properties.
Start revisingMolecular
Simple Molecular Structures
Molecular substances such as iodine and ice, including melting point and conductivity.
Start revisingTypes
Structure Types
Giant ionic, giant metallic, giant covalent and simple molecular lattices compared: melting point, conductivity, solubility and energy changes on changes of state (3.1.3.4).
Start revisingForces
Intermolecular Forces
London forces, permanent dipole-dipole forces and hydrogen bonding.
Start revising3.1.3 Bonding – AQA A Level Chemistry
The following AQA specification points outline the knowledge and skills students are expected to demonstrate for Bonding.
3.1.3 Bonding
Ionic bonding involves electrostatic attraction between oppositely charged ions in a lattice.
The formulas of compound ions, eg sulfate, hydroxide, nitrate, carbonate and ammonium.
Students should be able to:
A single covalent bond contains a shared pair of electrons.
Multiple bonds contain multiple pairs of electrons.
A co-ordinate (dative covalent) bond contains a shared pair of electrons with both electrons supplied by one atom.
Students should be able to represent:
Metallic bonding involves attraction between delocalised electrons and positive ions arranged in a lattice.
The four types of crystal structure:
The structures of the following crystals as examples of these four types of crystal structure:
Students should be able to:
Bonding pairs and lone (non-bonding) pairs of electrons as charge clouds that repel each other.
Pairs of electrons in the outer shell of atoms arrange themselves as far apart as possible to minimise repulsion.
Lone pair-lone pair repulsion is greater than lone pair-bond pair repulsion, which is greater than bond pair-bond pair repulsion.
The effect of electron pair repulsion on bond angles.
Students should be able to:
Electronegativity as the power of an atom to attract the pair of electrons in a covalent bond.
The electron distribution in a covalent bond between elements with different electronegativities will be unsymmetrical. This produces a polar covalent bond, and may cause a molecule to have a permanent dipole.
Students should be able to:
Forces between molecules:
The melting and boiling points of molecular substances are influenced by the strength of these intermolecular forces.
The importance of hydrogen bonding in the low density of ice and the anomalous boiling points of compounds.
Students should be able to:
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