Which of the following species is the strongest oxidizing agent under standard state conditions?

a. Ag+(aq)
b. H2(g)
c. H+(aq)
d. Cl2(g)
e. Al3+(aq)

An oxidizing agent is a substance that gains electrons in a redox chemical reaction.

I think Al3+ has a very high electron affinity and should pull electrons to it in a chemical reaction.

Is Al3+ the best choice for this problem?

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To determine the strongest oxidizing agent under standard state conditions, we need to consider the reduction potential values (E°) for each species.

The reduction potential measures the tendency of a species to gain electrons and acts as an indicator of its oxidizing power. Species with higher reduction potentials are stronger oxidizing agents.

Looking at the given choices:

a. Ag+(aq) has a reduction potential of +0.80 V (Ag+(aq) + e- → Ag(s)).
b. H2(g) has a reduction potential of 0.00 V (2 H+(aq) + 2 e- → H2(g)).
c. H+(aq) has an infinite reduction potential since it cannot be reduced further.
d. Cl2(g) has a reduction potential of +1.36 V (Cl2(g) + 2 e- → 2 Cl-(aq)).
e. Al3+(aq) has a reduction potential of -1.66 V (Al3+(aq) + 3 e- → Al(s)).

Comparing the reduction potentials, we can see that Cl2(g) has the highest value at +1.36 V, indicating that it is the strongest oxidizing agent among the given choices. Therefore, the correct answer is d. Cl2(g).

To determine the strongest oxidizing agent, we need to consider the reduction potential of each species. The species with a higher reduction potential value is more likely to gain electrons and, therefore, is a stronger oxidizing agent.

To find the reduction potential values, we can use standard reduction potential tables. These tables provide the reduction potential values for half-cell reactions under standard conditions. The higher the reduction potential value, the greater the tendency that species has to be reduced (meaning it acts as an oxidizing agent).

Let's consult the standard reduction potential table to determine the reduction potential values for the given species:

a. Ag+(aq): The reduction potential for Ag+ is +0.799 V.
b. H2(g): The reduction potential for H2 is 0 V since it is used as the reference electrode.
c. H+(aq): The reduction potential for H+ is 0 V since it is used as the reference electrode.
d. Cl2(g): The reduction potential for Cl2 is +1.36 V.
e. Al3+(aq): The reduction potential for Al3+ is -1.66 V.

From these values, we can observe that Cl2 has the highest reduction potential at +1.36 V, indicating it is the strongest oxidizing agent under standard state conditions among the given species.

Therefore, the correct choice for the strongest oxidizing agent in this case would be d. Cl2(g).