Classify each of the following unbalanced half-reactions as either an oxidation or a reduction. (d) CH₃O→H(aq) CH₂O(aq)

Verified step by step guidance

1. Identify the oxidation states of the carbon atom in both CH_3OH and CH_2O.
2. In CH_3OH, the carbon is bonded to three hydrogens and one oxygen. Calculate the oxidation state of carbon considering the typical oxidation states of hydrogen (+1) and oxygen (-2).
3. In CH_2O, the carbon is bonded to two hydrogens and one oxygen. Calculate the oxidation state of carbon in this compound.
4. Compare the oxidation states of carbon in CH_3OH and CH_2O to determine if the carbon is being oxidized or reduced.
5. If the oxidation state of carbon increases, it is an oxidation reaction. If it decreases, it is a reduction reaction.

Key Concepts

Oxidation and Reduction

Oxidation and reduction are chemical processes that involve the transfer of electrons between species. Oxidation refers to the loss of electrons, resulting in an increase in oxidation state, while reduction involves the gain of electrons, leading to a decrease in oxidation state. These processes are often coupled, as one species is oxidized while another is reduced.

Half-Reactions

Half-reactions are equations that show either the oxidation or reduction process separately. They are useful for balancing redox reactions and understanding the electron transfer involved. Each half-reaction includes the species undergoing oxidation or reduction, along with the electrons gained or lost, allowing for a clearer analysis of the overall reaction.

Balancing Redox Reactions

Balancing redox reactions involves ensuring that the number of atoms and the charge are equal on both sides of the reaction. This can be achieved by separating the reaction into its oxidation and reduction half-reactions, balancing each for mass and charge, and then combining them. Understanding how to balance these reactions is crucial for accurately representing the chemical changes occurring.