Galvanic Cells and Redox Reactions Overview

Galvanic Cells

Devices converting chemical energy to electrical energy.

Oxidation

Loss of electrons in a chemical reaction.

Reduction

Gain of electrons in a chemical reaction.

Salt Bridge

Connects two half-cells, allowing ion flow.

Anode

Electrode where oxidation occurs, losing electrons.

Cathode

Electrode where reduction occurs, gaining electrons.

Oxidation Numbers

Indicate electron loss or gain by atoms.

Electrode Potential

Voltage associated with a half-cell reaction.

Standard Reduction Potential

Measure of tendency to gain electrons.

Electrolytic Cells

Use external power to drive non-spontaneous reactions.

Redox Reaction

Simultaneous oxidation and reduction processes.

Charge Conservation

Total charge remains constant in reactions.

Molarity

Concentration of solute in a solution.

Electronegativity Difference

Drives voltage in electrochemical cells.

Half-Reaction

Shows either oxidation or reduction separately.

Voltage Calculation

Difference in electrode potentials for reactions.

Ionic Compounds

Composed of cations and anions, electrically neutral.

Electrode Weight Change

Indicates ion concentration changes during reactions.

Chemical Reaction Force

E must be negative for spontaneous reactions.

Battery Lifespan Factors

Anode depletion, cathode ion depletion, salt bridge depletion.

Common Oxidation States

H=+1, O=-2, Ag=+1, Zn=+2.