This lesson provides the precise, step-by-step methodology for balancing chemical equations by inspection. You will learn how to adjust stoichiometric coefficients to enforce the conservation of mass principle across synthesis, decomposition, and displacement reactions. Mastering this foundational skill is mandatory for all subsequent stoichiometric calculations.

This lesson presents the algebraic method for balancing complex chemical equations unsuitable for simple inspection. You will learn to assign unknown coefficients, form a system of simultaneous equations based on elemental conservation, and solve for the minimum integer coefficients. This technique guarantees balance for challenging reactions.

This lesson introduces the change in oxidation number method for balancing complex redox reactions. You will learn to assign oxidation numbers to identify the atoms that are oxidised and reduced, then use the change in these numbers to determine the precise stoichiometric ratio of reactants required for conservation of charge and mass. This method is an alternative to the half-reaction approach.

This lesson defines and contrasts molecular, total ionic, and net ionic equations for reactions in aqueous solution. You will learn the rules for identifying strong electrolytes that dissociate into spectator ions, enabling the accurate derivation of the net ionic equation which represents only the chemically relevant species. Mastering this is crucial for understanding reaction mechanisms.

This lesson rigorously defines oxidation-reduction (redox) reactions based on the core concepts of electron transfer and changes in oxidation state. You will learn the precise relationship between oxidation and reduction, establishing the necessary foundational understanding for assigning oxidation numbers. Mastery of these fundamental definitions is critical for all subsequent redox analysis.

This lesson focuses on identifying the roles of the oxidizing and reducing agents in any redox reaction. You will learn the reciprocal relationship between the species that is oxidised and the species that causes reduction, and vice versa. Clearly identifying these agents is necessary for understanding the direction and potential of electrochemical cells.

This lesson presents the full set of rules for the unambiguous assignment of oxidation numbers to elements in compounds or ions. You will learn the hierarchy of rules governing common elements like oxygen, hydrogen, and halogens, and how to use the sum of these values to determine the oxidation state of the central atom. Accurate assignment is the first mandatory step for balancing all redox equations.

This lesson precisely correlates changes in oxidation state with the process of oxidation and reduction. You will learn that an increase in oxidation state defines oxidation, while a decrease defines reduction. Correctly tracking these changes across a reaction is the necessary starting point for balancing all complex redox equations.

This lesson introduces the half-reaction method, the universal technique for balancing complex redox reactions in aqueous solution. You will learn to separate the overall reaction into oxidation and reduction half-reactions, balance mass and charge independently in each half, and then combine them to yield the final balanced equation. This method is crucial for quantitative electrochemistry.

This lesson focuses specifically on balancing redox reactions under acidic conditions using the half-reaction method. You will learn the precise steps for balancing oxygen atoms using water and hydrogen atoms using H+. Mastering this protocol is vital for accurately quantifying reactions performed in acid solutions.

This lesson builds on the half-reaction method by providing additional complex examples of balancing redox equations in acidic media. We will focus on reactions involving polyatomic ions and multiple electron transfers to solidify your procedural fluency. Completing this ensures you can confidently apply the acidic medium balancing rules to any undergraduate problem.

This lesson introduces the specific protocol for balancing redox reactions occurring in alkaline (basic) medium using the half-reaction method. You will learn the final step of adding OH- ions to neutralise the H+ ions used in the acidic balancing process. Mastering this technique is necessary for accurately quantifying reactions in non-acidic aqueous environments.

This lesson provides additional complex examples of balancing redox equations in basic medium, reinforcing the procedural steps. We focus on reactions where the conversion from acidic to basic medium requires careful charge checking. Completing these examples ensures robust mastery of the basic medium half-reaction technique.

This lesson provides a final synthesis of all equation-balancing techniques, from simple inspection to complex redox half-reactions in varying media. You will apply these methods to integrated problems to confirm your mastery of mass and charge conservation before progressing to solution stoichiometry.