Redox Chemistry Lecture Notes

Comprehensive vocabulary flashcards covering the fundamental concepts, definitions, and specific examples of redox chemistry as presented in the lecture.

Redox reactions

Chemical reactions that involve the transfer of electrons and consist of two reactions, reduction and oxidation, occurring simultaneously.

Reduction

The gain of electrons by a species. In a half-equation, electrons are written on the left side of the arrow.

Oxidation

The loss of electrons by a species. In a half-equation, electrons are written on the right side of the arrow.

OIL RIG

An acronym used to remember redox processes: Oxidation Is Loss, Reduction Is Gain (of electrons).

Corrosion

A societal application of redox reactions, such as the rusting of iron represented by the equation: $4Fe(s) + 3O_2(g) \rightarrow 2Fe_2O_3(s)$.

Oxidant (oxidising agent)

A species that enables another species to be oxidised by accepting electrons; the oxidant itself undergoes reduction.

Reductant (reducing agent)

A species that enables another species to be reduced by losing electrons; the reductant itself undergoes oxidation.

Half-equations

Equations representing reduction and oxidation independently; they must show states and have balanced elements and charges (using electrons).

Overall redox equation

An equation that combines two half-equations with balanced electrons so that no electrons appear in the final equation.

Conjugate redox pair

A reactant and the product it forms during a redox reaction (e.g., $Zn(s)$ and $Zn^{2+}(aq)$).

KOHES

The method or sequence used for balancing complex half-equations, particularly in acidic conditions.

Solid substances in redox

Substances like $MgO(s)$ that cannot be separated into ions in equations (e.g., they cannot be written as $Mg^{2+}(s)$ and $O^{2-}(s)$).

Acidic solution reduction of $MnO_4^-$

The process where permanganate ions ($MnO_4^-$) gain electrons to form $Mn^{2+}$ in the presence of acid.

Acidic solution reduction of $Cr_2O_7^{2-}$

The process where dichromate ions ($Cr_2O_7^{2-}$) are reduced to form $Cr^{3+}(aq)$ in acidic conditions.