Oxidation And Reduction
Oxidation and Reduction
Mnemonic: OILRIG
Oxidation Is Loss, Reduction Is Gain
Oxidation → the loss of electrons from an atom or an ion→ always happens at anode (positive electrode) → think anOde (O2 in the electrolysis of water xp)
Redox reactions: Reactions involving the transfer of electrons
e.g. burning, rusting, photosynthesis, respiration and the browning of apples.
happens in three types of reactions:
1. addition of oxygen
2. removal of hydrogen
3. increase in valency (how easily an atom can combine with other chemical species)
Reduction → the gain of electrons → always happens at cathode (negative electrode) → think catHode (H2 produced in the electrolysis of water xp)
An oxidising agent is a substance that allows oxidation (the loss of electrons) to occur by being reduced
(by taking in those electrons) e.g. hydrogen peroxide (hair bleaching), oxygen (respiration)
Real Life Application of Oxidation:
Swimming-pool water treatment
Chlorine or chlorine compounds such as Ca(ClO)2 (Calcium Hypochlorite - usually used) and NaClO
(Sodium Hypochlorite) are added to water to form HOCl. HOCL is an oxidising agent and it kills microorganisms by oxidising them (by being reduced itself)
When chlorine acts as an oxidising agent it
is reduced to the chloride (Cl-) ion
A reducing agent is a substance that allows reduction (the gain of electrons) to occur by being oxidised
(losing electrons for the other thing to take in) e.g. sulfur dioxide (bleaching), hydrogen (reduction of organic compounds). 2Na(s)+Cl2(g) → 2NaCl(s)
Redox Reaction Experiments (Displacement Reactions)
Halogens with Halides (Halogen Ions)
Cl > Br > I
(all ions added are in solution with other ions so that they are in ionic form don't confuse bromine solution with sodium bromide). Silver nitrate can be used to test for halides (Cl- = white precipitate, Br- = pale cream precipitate, I- = pale yellow precipitate) Ammonia solution is added to the precipitates. Further testing involves adding dilute
Mnemonic: OILRIG
Oxidation Is Loss, Reduction Is Gain
Oxidation → the loss of electrons from an atom or an ion→ always happens at anode (positive electrode) → think anOde (O2 in the electrolysis of water xp)
Redox reactions: Reactions involving the transfer of electrons
e.g. burning, rusting, photosynthesis, respiration and the browning of apples.
happens in three types of reactions:
1. addition of oxygen
2. removal of hydrogen
3. increase in valency (how easily an atom can combine with other chemical species)
Reduction → the gain of electrons → always happens at cathode (negative electrode) → think catHode (H2 produced in the electrolysis of water xp)
An oxidising agent is a substance that allows oxidation (the loss of electrons) to occur by being reduced
(by taking in those electrons) e.g. hydrogen peroxide (hair bleaching), oxygen (respiration)
Real Life Application of Oxidation:
Swimming-pool water treatment
Chlorine or chlorine compounds such as Ca(ClO)2 (Calcium Hypochlorite - usually used) and NaClO
(Sodium Hypochlorite) are added to water to form HOCl. HOCL is an oxidising agent and it kills microorganisms by oxidising them (by being reduced itself)
When chlorine acts as an oxidising agent it
is reduced to the chloride (Cl-) ion
A reducing agent is a substance that allows reduction (the gain of electrons) to occur by being oxidised
(losing electrons for the other thing to take in) e.g. sulfur dioxide (bleaching), hydrogen (reduction of organic compounds). 2Na(s)+Cl2(g) → 2NaCl(s)
Redox Reaction Experiments (Displacement Reactions)
Halogens with Halides (Halogen Ions)
Cl > Br > I
(all ions added are in solution with other ions so that they are in ionic form don't confuse bromine solution with sodium bromide). Silver nitrate can be used to test for halides (Cl- = white precipitate, Br- = pale cream precipitate, I- = pale yellow precipitate) Ammonia solution is added to the precipitates. Further testing involves adding dilute