Introduction to Redox Reactions and Oxidation

Vocabulary flashcards covering the introductory concepts of redox chemistry, focusing on the definition of oxidation, subatomic particle charge balances, and oxidation equations for magnesium and copper.

Oxidation

The loss of electrons in a chemical process.

Four Core Steps to Solving Redox Reactions

The four foundational concepts needed before solving redox equations: 1. Understanding what oxidation and reduction mean; 2. Identifying oxidation and reduction in a chemical equation; 3. Calculating oxidation numbers; 4. Balancing redox equations.

Neutral Magnesium Atom ($Mg$)

An uncharged atom containing 12 protons (positive charges) and 12 electrons (negative charges), with a net charge of zero ($12(+) - 12(-) = 0$).

Magnesium Oxidation Reaction

The oxidation process represented by the equation $Mg \rightarrow Mg^{2+} + 2e^{-}$, in which a neutral magnesium atom loses two electrons.

Magnesium Ion ($Mg^{2+}$)

A positively charged ion formed when a magnesium atom loses two electrons, leaving 12 protons and 10 electrons to yield an overall charge of $+2$ ($12(+) - 10(-) = +2$).

Copper Oxidation Reaction

The oxidation reaction represented by the equation $Cu \rightarrow Cu^{2+} + 2e^{-}$, in which copper loses two electrons.

Copper(II) Ion

The positively charged ion ($Cu^{2+}$) produced when a neutral copper atom loses two electrons via oxidation.