Consider the following species: Ca2+(aq), Ca(s), I2(s) and I–(aq). What is the (i) strongest oxidant and (ii) strongest reductant?

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BlackTom AI · Accepted Answer

Question restatement: We are to identify (i) the strongest oxidant and (ii) the strongest reductant among Ca2+(aq), Ca(s), I2(s) and I–(aq).

Option a: (i) I2 and (ii) Ca
This option assigns I2 as the strongest oxidant, which is correct because I2 tends to gain electrons to form I–, reflecting its high oxidizing strength. It also assigns Ca(s) as the strongest reductant, which is correct because elemental calcium can readily lose electrons to become Ca2+. Therefore this option aligns with standard redox trends: I2 (oxidant) > I–; Ca(s) (reductant) > Ca2+.

Option b: (i) Ca and (ii) I2
This choice declares Ca(s) as the strongest oxidant. That is incorrect: Ca(s) is a superb reductant, not an oxidant, since it readily donates electrons to oxidize others. Conversely, I2 is a strong oxidant, not the strongest reductant, so this pairing reverses the roles.

Option c: (i) Ca2+ and (ii) I–
Here, Ca2+ is identified as the strongest oxidant. Ca2+ is the oxidized form of calcium and cannot accept electrons to become a higher oxidation state in this context; as a cation it does not act as an oxidizing agent under these conditions. I– is identified as the strongest reductant, but iodide ions are weak reducers compared to elemental calcium; also, I– would be oxidized to I2 rather than acting as a reductant to a stronger reducing agent in this setup. Overall, this option misassigns both roles.

Option d: (i) I– and (ii) Ca2+
This option sets I– as the strongest oxidant, which is incorrect because iodide is already in a reduced state and does not readily accept electrons to become I2 under standard conditions. It also sets Ca2+ as the strongest reductant, which is incorrect since Ca2+ cannot easily donate electrons to reduce other species; elemental Ca(s) is the strong reductant, not Ca2+. Thus both assignments are inconsistent with fundamental redox behavior.

Summary:
- I2 is the primary oxidizing agent among the species listed, because it accepts electrons to form I–. 
- Ca(s) is the primary reducing agent among the species listed, because it donates electrons to form Ca2+. 
- The other options misidentify either the oxidant or the reductant by swapping roles, mischaracterizing oxidation states, or misplacing electron transfer tendencies.

Consider the following species: Ca2+(aq), Ca(s), I2(s) and I–(aq). What is the (i) strongest oxidant and (ii) strongest reductant?

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