Which of the following species would NOT function as an oxidizing agent?
a. MnO4-
b. Mn+2
c. H+
d. S
e. Br-
An oxidizing agent must be reduced and that means a gain of electrons. So it must go from whatever oxidation state is shown to a lower positive value; i.e., it must gain electrons. For example, MnO4^- is +7 for Mn and it goes to +2, a decrease in positive value (a gain of 5 electrons) and that makes it reduced. Do the others the same way.
Is the ans b?
To identify which species would NOT function as an oxidizing agent, we need to understand the concept of oxidation and reduction.
An oxidizing agent is a species that gains electrons and gets reduced in a chemical reaction, causing another species to lose electrons and get oxidized.
On the other hand, a reducing agent is a species that loses electrons and gets oxidized, causing another species to gain electrons and get reduced.
In this case, we need to find the species that cannot gain electrons or act as an oxidizing agent.
Let's analyze each option:
a. MnO4-: This is the permanganate ion, and it has a high oxidation state for manganese (+7). It can gain electrons and get reduced, so it can act as an oxidizing agent.
b. Mn+2: This is the manganese ion with a +2 oxidation state. It can lose electrons and get oxidized, so it cannot act as an oxidizing agent.
c. H+: Hydrogen ions are usually not involved in redox reactions. While they can gain electrons and get reduced, they do not work as effective oxidizing agents.
d. S: Sulfur is commonly found in various oxidation states (-2, +2, +4, +6) and can act as both an oxidizing agent and a reducing agent. It depends on the specific reaction and the oxidation state of sulfur in that reaction.
e. Br-: Bromide ion has a -1 oxidation state and can potentially gain electrons and get reduced, making it capable of acting as an oxidizing agent.
Based on the analysis, option b. Mn+2 would NOT function as an oxidizing agent, as it cannot gain electrons and get reduced.
To determine which species would not function as an oxidizing agent, we need to understand what an oxidizing agent is.
An oxidizing agent is a substance that accepts electrons from another substance during a chemical reaction, causing the other substance to undergo oxidation (lose electrons). In other words, an oxidizing agent is itself reduced (gains electrons) in the reaction.
To identify which species would not function as an oxidizing agent, we need to find the species that does not have the ability to accept electrons or undergo reduction.
a. MnO4-: This is the permanganate ion, which readily accepts electrons to be reduced to Mn+2 in reactions. It can function as an oxidizing agent.
b. Mn+2: This is the reduced form of manganese. Since it has already lost electrons to become positively charged, it cannot accept more electrons from another substance. It would not function as an oxidizing agent.
c. H+: Hydrogen ions are typically not strong oxidizing agents as they do not readily accept electrons from other substances. They typically function as reducing agents instead.
d. S: Sulfur is a non-metal element that does not have the ability to accept electrons readily. It would not function as an oxidizing agent.
e. Br-: Bromide ions have the ability to accept electrons and be reduced to Br2 in reactions. They can function as an oxidizing agent.
Therefore, the species that would NOT function as an oxidizing agent is (b) Mn+2.