IB Chemistry HL: Mastering Redox Reactions Quiz

In order to determine whether an element undergoes oxidation or reduction in reactions using oxidation numbers, it is important to understand the principles behind LEORA and GEROA. These incorrect answers provide alternative options that may confuse individuals who are trying to deduce oxidation or reduction reactions.

When deducing oxidation and reduction half-equations for a redox reaction, it is important to focus on the half equations rather than the full balanced equation, colors, or using a calculator.

When deducing redox equations using half-equations, it is important to utilize H+ and H2O to balance the equations in acid solution. Balancing equations in alkaline solution is not necessary for assessment purposes. Incorrect answers provide information that does not align with the standard practice of balancing half-equations in redox reactions.

The correct definitions of oxidizing agent and reducing agent involve the concepts of electron transfer and oxidation numbers as described in the correct answer. The incorrect answers provided do not accurately define these terms.

In redox reactions, the oxidizing agent gets reduced by accepting electrons while the reducing agent gets oxidized by losing electrons. The correct answer provides a mnemonic device 'LEORA' for loss electrons, oxidation, reducing agent and 'GEROA' for gain electrons, reduction, oxidizing agent.

The feasibility of a redox reaction can be deduced from a reactivity series, which is a simplified form of a table of standard electrode potentials showing the relative reactivities of chemicals. However, students are not expected to recall a specific reactivity series, as understanding the concept is sufficient.

A voltaic cell converts chemical energy into electrical energy through a spontaneous redox reaction. The more reactive metal is the negative electrode, not the positive electrode, and the cell is used specifically for producing electricity and not for separating mixtures or exchanging heat energy.

In an electrolytic cell, oxidation always occurs at the anode (negative electrode) where electrons are lost, and reduction occurs at the cathode (positive electrode) where electrons are gained. This is a fundamental principle in electrochemistry.

Electrolytic cells require electrical energy, not heat, light, or mechanical energy, to drive the non-spontaneous chemical reactions involved in electrolysis.

In an electrochemical cell, oxidation occurs at the positive electrode, which is called the anode. Reduction occurs at the negative electrode, known as the cathode. Electrons flow from the anode to the cathode through the external wires connecting the electrodes.

Electrolysis of a molten electrolyte is often used to obtain reactive metals from their ores. Half-equations showing the formation of products at each electrode will be assessed to determine the products of the electrolysis process.