Week 10 (Redox Reactions and Spectroscopy)

Question 1

Disproportionation

Answer 1

-Self Oxidation Reduction
-a chemical reaction where a single substance acts as both the oxidizing agent and reducing agent
-only one reactant is involved, which splits into two different products, one oxidized and one reduced
-the oxidation state of the same element changes in both the oxidized and reduced product

Question 2

Reducing and Oxidizing agents and O.N.s

Answer 2

-when an atom is at its lowest O.N., it can only be a reducing agent (get rid of electrons, ex. Cl= -1)
-when an atom is at its highest O.N., it can only be an oxidizing agent (gain electrons, ex. Cl= +7)

Question 3

Examples of disproportionation reactions

Answer 3

-O in H₂O₂ is both a reducing and oxidizing agent
-2H₂O₂ –> 2H₂O + O₂
-H₂O is reduced (O goes from -1 to -2)
-O₂ is oxidized (O goes from -1 to 0)
-causes H₂O₂ to disproportionate

Question 4

A substance as both oxidizing and reducing agent

Answer 4

-for an element that has multiple stable oxidation states (S, N, halogens), in an intermediate oxidation state, it can act as either an oxidizing or reducing agent (oxidizing (gain) when reacting with less electronegative, reducing (lose) when reacting with more electronegative)
-Many halogen-containing substances with a halogen oxidation number in the mid-range (XO₃⁻, XO₂⁻, XO⁻, X₂) can disproportionate (be both oxidizing and reducing agent) under suitable conditions