Oxidation Reduction Redox
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What is an advantage of oxidation states over charges?
They can also be applied to covalent compounds
What is the first rule for calculating oxidation states?
Uncombined elements or elements only bonded to other elements of the same type for example, oxygen have an oxidation state of zero
What is the second rule of calculating oxidation states?
In a compound, the sum of oxidation states of all elements within it is 0
What’s the third rule of calculating oxidation states?
In a complex ion, the sum of oxidation states of all elements is equal to the charge on the ion (compound ion)
What is the fourth rule of calculating oxidation states?
Oxidation state of group one metals in a compound is always +1
What is the fifth rule of calculating oxidation states?
Oxidation state of group 2 metals in a compound is always +2
What is the sixth rule of calculating oxidation state?
Oxidation state of aluminium in a compound as always +3
What is the seventh rule of calculating oxidation state?
Oxidation state of hydrogen in a compound is plus one except in a metal hydride where it is minus one
What is the eighth rule of calculating oxidation states?
Oxidation state of oxygen in a compound is always-2 except in a peroxide where its -2
Describe the steps for writing half equations
• Balance the species with the variable oxidation state. • Balance oxygen through addition of water. • Balance hydrogen through addition of hydrogen ions. • Balance charge by adding electrons.
Define oxidation
A reaction in which an atom or group of atoms loses electrons
Define reducing agent
An electron donor (reduces another species)
Define reduction
Reaction in which an atom or group of atoms gains electrons
Define oxidising agent
An electron receptor (oxidises another species)
What does oil rig stand for?
Oxidation is loss of electrons or hydrogen Reduction is gaining of electrons or hydrogen
How do you know if something is oxidation?
If oxidation state increases its oxidation
How do you know if something is reduction?
If oxidation state decreases its reduction
What are the rules for combining half equations?
• One half equation must show oxidation (electrons added on the right hand side) and one must show reduction (electrons added on the left-hand side). • Before you combine them the number of electrons in each half equation must be equal (multiply them up to lowest common denominator.) • Add equations together all reactants and products from both equations included. • Remove spectator ions/electrons.
How do you know if something is the oxidising or reducing agent?
Oxidising agent is what’s reduced Reducing agent is what oxidised