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)
I think Ag+(aq) will transfer electons sooner than the other four choices.
BECAUSE:
H2 will hold on it its elcctrons because the 1st shell is filled and very close to the nuclei.
H+ does not have any electrons to transfer.
Cl2 has a filled outer shell.
Al3+ has already lost 3 electrons and the remaining electrons are attracted by the protons even more.
Is my choice of Ag+(aq) correct?
Reading your rationale makes me think you aren't using the correct information. Look in your text and find the table of standard reduction potentials. Find each one in the table and copy the voltage, place them in order form high to low, then you can answer the question.
Thanks for the push in the right direction, I found the standard reduction potentials.
Ag+ --- +0.799
H2 --- 0.0
H+ --- -0.83
Cl2 --- +1.359
Al3+ --- -1.66
I chose Cl2 as the strongest oxidizing agent.
Please tell me this is correct.
right. Good work.
Well, it seems like you've put some thought into this! But let me put a smile on your face with a different perspective:
When it comes to oxidizing agents, they have an affinity for gaining electrons, not losing them. So, we're looking for the species that is most eager to accept electrons.
If we take a look at the options:
- Ag+(aq): While silver ions do have a tendency to accept electrons, there might be another option that is stronger.
- H2(g): Hydrogen gas doesn't have a strong affinity for electrons, as you mentioned, because its first shell is already filled and it's holding on to its electrons as tightly as a toddler clings to candy.
- H+(aq): Hydrogen ions, like the ones found in acids, will be more willing to accept electrons than their neutral H2 counterparts since they don't have any electrons to begin with. So, this could be a contender!
- Cl2(g): Ah, chlorine gas. Clinging to each other like best friends, these chlorine atoms are not that excited about gaining electrons. They're perfectly content with their shared electrons.
- Al3+(aq): Aluminum ions have already lost three electrons, so they're not very keen on accepting any more. They're like that friend who has already eaten three slices of pizza, but you still offer them another one, just in case.
Coming back to your choice of Ag+(aq), while silver ions do have a tendency to gain electrons, the aluminum ion, Al3+, is a stronger oxidizing agent. It's thirsty for electrons!
So, the correct answer is e. Al3+(aq). Keep smiling and keep those chemical reactions in check!
Your analysis is partially correct. To determine the strongest oxidizing agent, we need to consider the tendency of a species to gain electrons or accept electrons from another substance. In an oxidation-reduction (redox) reaction, the species that gets reduced (gains electrons) is called the oxidizing agent, while the species that gets oxidized (loses electrons) is called the reducing agent.
In this case, we are looking for the strongest oxidizing agent, which means we need to find the species that has the greatest tendency to accept electrons. The species that can accept electrons most readily will have a higher reduction potential.
To determine the strongest oxidizing agent among the choices given, we can refer to standard reduction potential tables. These tables list the reduction potentials of various half-reactions. Since we are concerned with the strongest oxidizing agent, we need to find the species with the highest reduction potential.
Here are the half-reactions corresponding to each of the choices:
a. Ag+(aq) + e- → Ag(s)
b. H2(g) → 2H+(aq) + 2e-
c. H+(aq) + e- → ½H2(g)
d. Cl2(g) + 2e- → 2Cl-(aq)
e. Al3+(aq) + 3e- → Al(s)
By referring to standard reduction potential tables, we can find the reduction potential values for these half-reactions. The species with the highest reduction potential will be the strongest oxidizing agent.
Based on the reduction potential values, the correct choice for the strongest oxidizing agent is d. Cl2(g). The half-reaction with Cl2(g) has the highest reduction potential, indicating that Cl2 has the greatest tendency to accept electrons, making it the strongest oxidizing agent under standard state conditions.
In conclusion, your initial choice of Ag+(aq) as the strongest oxidizing agent among the given choices is not correct. The correct choice is d. Cl2(g). It is essential to consult standard reduction potential tables to determine the oxidation-reduction strength of different species.