Arrange the following oxidizing agents in order of increasing strength under standard-state conditions: Br2(aq), MnO4+(aq), Sn4+(aq).

Oxidizing agents are substances that gain electrons in a chemical reaction, causing another substance to be oxidized. Their strength is determined by their ability to accept electrons; stronger oxidizing agents can more readily oxidize other substances. Understanding the relative strength of different oxidizing agents is crucial for predicting the outcomes of redox reactions.

Standard-state conditions refer to a set of specific conditions used to measure and compare the properties of substances, typically defined as 1 bar of pressure and a specified temperature, usually 25°C. Under these conditions, the behavior of substances, including their reactivity as oxidizing agents, can be reliably assessed, allowing for consistent comparisons.

Electrode potentials, measured in volts, indicate the tendency of a species to be reduced (gain electrons) in an electrochemical reaction. The standard reduction potential values for various half-reactions can be used to rank oxidizing agents by their strength. A higher standard reduction potential corresponds to a stronger oxidizing agent, making it essential for arranging the agents in the question.