T2: Oxidation, Reduction and Redox Reactions Flashcards
Oxidation definition
- loss of electrons
- oxidation state increases
Reduction definition
- gain of electrons
- oxidation state decreases
Reducing agent definition
- electron donor
- a reducing agent is itself oxidised
Oxidising agent definition
- electron acceptor
- an oxidising agent is itself reduced
oxidation state anagram
Under
My
Face
Here’s
Our
Chin
oxidation state assignments in order (what does the anagram stand for)
Uncombined elements (0)
Metals G1 = +1, G2 = +2 G3 = +3
Fluorine (-1)
Hydrogen (+1)
Oxygen (-2)
Chlorine (-1)
more positive oxidation state =
oxidation
more negative oxidation state =
reduction
if a substance is oxidised…
oxidation state increases
if a substance is reduced…
oxidation state decreases
in a reaction if the element has the same oxidation state (before and after the arrow) this means that…
the element is neither oxidised or reduced
rules for balancing half equations
- balance the main atom (not H or O) first
- Balance O using H2O
- Balance H using H+ ions
- Balance charge using electrons (add to more positive side)
steps to follow to combine half equations
1 multiply 1 or both the half equations until they contain the same amount of electrons
2 add the reactants from both half equations together
3 add the products from both half equations together
4 cancel out the electrons
roman numerals in oxidation states
I +1
II +2
III +3
IV +4
V +5
VI +6
VII +7
VIII +8
