REDOX Flashcards
What does it mean for a substance to be oxidised?
The substance loses electrons
The substance gains oxygen
The substance loses hydrogen
The rule that applies depends on the stated equation
What does it mean for a substance to be reduced?
The substance gains electrons
The substance loses oxygen
The substance gains hydrogen
The rule that applies depends on the stated equation
What is an oxidising agent?
A substance that donates electrons or hydrogen to another substance in the reaction.
It is reduced during the reaction
What is a reducing agent?
A substance that accepts electrons and hydrogen or donates oxygenin the reaction.
It is oxidised during the formula
What are the general oxidation state rules?
The total of all oxidation states should be the same on both sides of the equation
What are the oxidation state rules with specific atoms and molecules?
The oxidation state is 0 for a pure element (O2, Cl2)
The oxidation state is equivalent to an ion’s ionic charge for simple ions
Oxidation state is mostly for halide ions
Oxidation state is mostly +1 for hydrogen and -2 for oxygen
What are some exceptions to oxidation state rules?
If the oxygen is part of a peroxide ion (O^2-), such as hydrogen peroxide (H2O2), each oxygen has a -1 oxidation state
Hydrogen can have a -1 oxidation state if part of a metal hydride
The more electronegative element in a compound has a negative oxidation state; for a compound like F2O, oxygen has a oxidation state of +2
What is a redox reaction?
A reaction where both oxidation and reduction both occur
What is a disproportionation reaction?
A redox reaction where the same element is oxidised and reduced
Chlroine is an example, when reacting with water to produce chloric acid and hydrochloric acid`
