Question
Metals L, K, M and N and their are selectively reacted and yield the following data:
L^2+(aq) + 2K(s) = L(s) + 2K^+(aq)
K(s) +N^+(aq) = no change
K+(aq) + K(s) = K(s) +M^+(aq)
N(s) + M^+(aq) = N^+(aq) + M(s)
What is strongest oxiding agent?
L^2+(aq) + 2K(s) = L(s) + 2K^+(aq)
K(s) +N^+(aq) = no change
K+(aq) + K(s) = K(s) +M^+(aq)
N(s) + M^+(aq) = N^+(aq) + M(s)
What is strongest oxiding agent?
Answers
GPT 3.5
To determine the strongest oxidizing agent among metals L, K, M, and N, we need to compare their tendency to lose electrons. The stronger a metal is at losing electrons, the stronger of an oxidizing agent it will be.
Looking at the given reactions, we can analyze each metal's behavior:
1. L^2+(aq) + 2K(s) = L(s) + 2K^+(aq)
In this reaction, metal L is reduced from its 2+ oxidation state to its elemental form (L(s)). Metal K is oxidized from its elemental form to its 1+ oxidation state. This indicates that metal L is a weaker reducing agent than metal K. However, we are interested in identifying the strongest oxidizing agent, so this reaction does not provide information about metal L's oxidizing potential.
2. K(s) + N^+(aq) = no change
In this reaction, metal K remains unchanged. It neither gains nor loses electrons. Therefore, this reaction does not provide information about metal K's oxidizing potential.
3. K+(aq) + K(s) = K(s) + M^+(aq)
In this reaction, metal K is reduced from its 1+ oxidation state to its elemental form (K(s)). Metal M is oxidized from its elemental form to its 1+ oxidation state. This indicates that metal K is a weaker reducing agent than metal M. Again, we are interested in identifying the strongest oxidizing agent, so this reaction does not provide information about metal K's oxidizing potential.
4. N(s) + M^+(aq) = N^+(aq) + M(s)
In this reaction, metal N is oxidized from its elemental form to its 1+ oxidation state. Metal M is reduced from its 1+ oxidation state to its elemental form (M(s)). This indicates that metal N is a stronger reducing agent than metal M. Hence, metal N will be the strongest oxidizing agent among the given metals.
Therefore, metal N is the strongest oxidizing agent.
Looking at the given reactions, we can analyze each metal's behavior:
1. L^2+(aq) + 2K(s) = L(s) + 2K^+(aq)
In this reaction, metal L is reduced from its 2+ oxidation state to its elemental form (L(s)). Metal K is oxidized from its elemental form to its 1+ oxidation state. This indicates that metal L is a weaker reducing agent than metal K. However, we are interested in identifying the strongest oxidizing agent, so this reaction does not provide information about metal L's oxidizing potential.
2. K(s) + N^+(aq) = no change
In this reaction, metal K remains unchanged. It neither gains nor loses electrons. Therefore, this reaction does not provide information about metal K's oxidizing potential.
3. K+(aq) + K(s) = K(s) + M^+(aq)
In this reaction, metal K is reduced from its 1+ oxidation state to its elemental form (K(s)). Metal M is oxidized from its elemental form to its 1+ oxidation state. This indicates that metal K is a weaker reducing agent than metal M. Again, we are interested in identifying the strongest oxidizing agent, so this reaction does not provide information about metal K's oxidizing potential.
4. N(s) + M^+(aq) = N^+(aq) + M(s)
In this reaction, metal N is oxidized from its elemental form to its 1+ oxidation state. Metal M is reduced from its 1+ oxidation state to its elemental form (M(s)). This indicates that metal N is a stronger reducing agent than metal M. Hence, metal N will be the strongest oxidizing agent among the given metals.
Therefore, metal N is the strongest oxidizing agent.