This activity introduces oxidation numbers by giving a conceptual foundation for them in terms of electron accounting and polar bonds. It then shows how the model used so far needs refining.
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Oxidation numbers
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Chemistry for the gifted and talented: oxidation numbers
Level
Specification
- Republic of Ireland
- Wales
- Northern Ireland
- England
- A/AS level
- AQA Chemistry
- Physical Chemistry
- Bonding
- Bond polarity
- 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: use partial charges to show that a bond is polar.
- Bond polarity
- Oxidation, reduction and redox equations
- Bonding
- Physical Chemistry
- Edexcel Chemistry
- Topic 2: Bonding and Structure
- Topic 3: Redox I
- 1. know what is meant by the term ‘oxidation number’
- 2. be able to calculate the oxidation number of elements in compounds and ions. The use of oxidation numbers in peroxides and metal hydrides is expected.
- 3. understand oxidation and reduction in terms of electron transfer and changes in oxidation number, applied to reactions of s- and p-block elements
- OCR Chemistry A
- Module 2: Foundations in chemistry
- 2.1 Atoms and reactions
- 2.2 Electrons, bonding and structure
- 2.2.2 Bonding and structure
- i) electronegativity as the ability of an atom to attract the bonding electrons in a covalent bond; interpretation of Pauling electronegativity values
- j) explanation of: a polar bond and permanent dipole within molecules containing covalently-bonded atoms with different electronegativities; a polar molecule and overall dipole in terms of permanent dipole(s) and molecular shape
- 2.2.2 Bonding and structure
- Module 2: Foundations in chemistry
- AQA Chemistry
- A/AS level
- Scotland
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