Oxidation Reduction (Redox) Reactions (IGNORE)

In an Oxidation Reduction (Redox) Reaction we have the transferring of an electron(s) between reactants. The reactant that gains electrons is reduced and represents the oxidizing agent, while the reactant that loses electrons is oxidized and represents the reducing agent. 

Oxidation Reduction (Redox) Reactions

Redox reactions are characterized by a gain or loss of electrons and to remember the difference between oxidation and reduction just say “LEO the lion goes GER.”

LEO GER ChartCalculating Oxidation Numbers

In oxidation vs reduction reactions, examining how the oxidation numbers of the reactants change is key to determining which one has been oxidized or reduced. When calculating the oxidation number of an element or compound we can use the following rules. 

Rule 1: When an element is in its standard state its oxidation number is equal to zero. 

Na (s)             Br₂ (l)              S₈ (s)              F­₂ (g)              Ne (g)             Ca (s)

Rule 2: The charge of an ion or polyatomic ion is equal to its oxidation number. 

Ca²⁺  Oxidation Number = +2                     PO₄^3–  Oxidation Number = – 3

Rule 3: For metals from Group 1A, their oxidation number is equal to +1 when connected to other elements.

Oxidation States (Group 1A)

Rule 4: For metals from Group 2A, their oxidation number is equal to +2 when connected to other elements. 

Oxidation States (Group 2A)

Rule 5: For hydrogen, the oxidation number is +1 when connected to non-metals and -1 when connected to boron or a metal. 

Oxidation States (Hydrogen)

Rule 6: For fluorine, the oxidation number is always -1 when connected to other elements. 

Oxidation States (Fluorine)

Rule 7: For oxygen, the oxidation number is -1 when it’s a peroxide, -1/2 when it’s a superoxide and -2 in most other cases. 

Peroxide 

A peroxide represents a compound containing two elements from Group 1A bonded to two oxygen atoms. 

Oxidation States (Peroxides)

Superoxide 

A superoxide represents a compound containing one element from Group 1A bonded to two oxygen atoms. 

Oxidation States (Superoxides)

Rule 8: For the halogens of Cl, Br, and I their oxidation numbers are -1 unless they are connected to oxygen. 

Oxidation States (Halogens)

So now let’s take a look at redox reaction to determine which reactant has been oxidized and which reactant has been reduced. 

PRACTICE: Identify the reducing agent and oxidizing agent from the following redox reaction.

Redox Reaction example

STEP 1: Identify the monoatomic ions because their charges equal their oxidation numbers.

H⁺  Oxidation Number = +1                     Cr³⁺  Oxidation Number = + 3

STEP 2: Assign oxidation numbers to the elements in compounds with known values based on the rules we’ve just reviewed. 

Oxidation Numbers (H₂O)

STEP 3: If an element doesn’t have a rule to calculate its oxidation number then assigned it an “x” and then solve. 

Oxidation numbers in dichromate ion, Cr₂O₇^2-. 

How to Calculate Oxidation Number (Cr₂O₇^2-)

Oxidation numbers in ethanol, C₂H_5­OH. 

How to Calculate Oxidation Number (C₂H₅OH)

Oxidation numbers in carbon dioxide, C_­O₂. 

How to Calculate Oxidation Number (CO₂)

STEP 4: Look to see which element or compound was reduced. 

Chromium (Cr) is transformed from Cr­₂O₇^2– to Cr³⁺ and has its oxidation number go from +6 to +3. Its oxidation number has decreased  and because Cr is a part of Cr­₂O₇^2– we would say that the entire compound has been reduced and represents the oxidizing agent. 

STEP 5: Look to see which element or compound was oxidized. 

Carbon (C) is transformed from C₂H₅OH to CO₂ and has its oxidation number go from +2 to +4. Its oxidation number has increased and because C is a part of C₂H₅OH we would say that the entire compound has been oxidized and represents the reducing agent. 

Types of Redox Reactions

Different types of chemical reactions will also fall under the classification of being a redox reaction. 

Single Displacement or Replacement Reactions

In a single displacement reaction we have one element replacing another element within a compound. To determine if an element can replace another element we use an activity series chart. 

Single Replacement Reaction

A very common example is the displacement of a hydrogen atom by magnesium when reacting with hydrochloric acid.

Combustion 

When following the traditional defintion this involves O₂ reacting with a compound made of (C & H) or (C, H & O) to produce CO₂ and H₂O.

Combustion ReactionDisproportionation

A disproportionation reaction is one where the reactant compound is both oxidized and reduced.

Disproportionation Reaction

Redox Reactions play an important role in many reactions you will see in your chemistry and biology courses. In addition to recognizing the oxidizing agent and reducing agent you will learn about balancing redox reactions, the connections to electrochemical cells, spontaneity, stoichiometry and solution chemistry.