5.) Which of the following is the strongest oxidizing agent?
a.) Zn(s)
b.) Mg(s)
c.) Al3+(aq)
d.) Mg2+(aq)
Go to Google and type in"activity series".
The metals at the top are the top reducing agent. Metal ions at the bottom are the top oxidizing agents.
This was actually helpful, thank you!
To determine which of the given options is the strongest oxidizing agent, we need to consider their oxidation states. The atom or ion that undergoes the highest positive oxidation state is typically the strongest oxidizing agent because it readily accepts electrons during a redox reaction.
Here's how to find the oxidation state for each option:
a.) Zn(s): Zinc is a transition metal and typically has an oxidation state of +2 in its compounds. However, in elemental form (Zn(s)), its oxidation state is 0 since atoms in their natural state have an oxidation state of 0.
b.) Mg(s): Magnesium is an alkaline earth metal and typically has an oxidation state of +2 in its compounds. However, in elemental form (Mg(s)), its oxidation state is also 0.
c.) Al3+(aq): Aluminum is a metal, and the +3 charge on the ion indicates that its oxidation state is +3. This means that aluminum is already oxidized and cannot readily accept any more electrons, making it a weaker oxidizing agent compared to the other options.
d.) Mg2+(aq): Magnesium ion has an oxidation state of +2. Like the metallic form, Mg2+ has already lost electrons and cannot accept more electrons as easily.
Based on their oxidation states, we can conclude that the strongest oxidizing agent from the given options is Al3+(aq) because it has the highest oxidation state.