Final answer:
The half-reaction K → K+ + e− represents oxidation because electrons are lost. Oxidation and reduction half-reactions are balanced separately by atoms and charge, with an equal number of electrons lost and gained, then combined into a balanced overall reaction.
Step-by-step explanation:
The half-reaction K → K+ + e− represents the process of oxidation because electrons are lost. In this half-reaction, a potassium atom loses an electron and is transformed into a potassium ion (K+). This is indicative of oxidation, as the loss of electrons characterizes this process. It’s essential to balance the redox reaction where another species is reduced by the electrons lost during the oxidation process.
Different half-reactions can represent either a reduction or an oxidation process in a redox reaction. When balancing these reactions, electrons are added to one side of a half-reaction to balance charge, ensuring that the electrons lost by the oxidizing agent equal the electrons gained by the reducing agent. This allows for the two half-reactions to be correctly combined into a full balanced chemical equation.
For example, multiplying the oxidation half-reaction by a coefficient to balance the number of electrons lost with those gained in the reduction half-reaction is a critical step.
Once balanced, the half-reactions are then added together to yield an overall balanced equation, showcasing that the redox reaction as a whole is electrically neutral.