Ch.4 - Chemical Quantities & Aqueous ReactionsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds
Solubility Rules
Molecular Equations
Gas Evolution Equations
Solution Stoichiometry
Complete Ionic Equations
Calculate Oxidation Numbers
Redox Reactions
Balancing Redox Reactions: Acidic Solutions
Balancing Redox Reactions: Basic Solutions
Activity Series
Additional Practice
Types of Chemical Reactions
Normality & Equivalent Weight
Additional Guides
Oxidation Reduction (Redox) Reactions
Oxidation Number
Net Ionic Equation
Jules Bruno

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.”

remember the difference between oxidation and reduction with LEO the lion goes GERLEO 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                     PO43–  Oxidation Number = – 3

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

Oxidation-Number-Group-1aOxidation States (Group 1A)

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

Oxidation-Number-Group-2aOxidation 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-Number-hydrogenOxidation States (Hydrogen)

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

Oxidation-Number-FluorineOxidation 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. 


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

Oxidation-Number-PeroxidesOxidation States (Peroxides)


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

Oxidation-Number-SuperoxidesOxidation States (Superoxides)

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

Oxidation-Number-HalogensOxidation 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-electron-transferRedox 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. 

loss-of-electrons-gain-of-electronsOxidation 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, Cr2O72-

dichromate-ion-oxidation-numberHow to Calculate Oxidation Number (Cr2O72-)

Oxidation numbers in ethanol, C2HOH. 

Ethanol-oxidation-numberHow to Calculate Oxidation Number (C2H5OH)

Oxidation numbers in carbon dioxide, C­O2

Carbon-dioxide-oxidation-numberHow to Calculate Oxidation Number (CO2)

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

Chromium (Cr) is transformed from Cr­2O72– to Cr3+ and has its oxidation number go from +6 to +3. Its oxidation number has decreased  and because Cr is a part of Cr­2O72– 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-ReplacementSingle Replacement Reaction

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


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-Reaction-rustCombustion ReactionDisproportionation

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

Disproportionation-gain-of-oxygen-loss-of-oxygensDisproportionation 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 cellsspontaneitystoichiometry and solution chemistry

Jules Bruno

Jules felt a void in his life after his English degree from Duke, so he started tutoring in 2007 and got a B.S. in Chemistry from FIU. He’s exceptionally skilled at making concepts dead simple and helping students in covalent bonds of knowledge.