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I hear you asking, "Wait a minute, what exactly are oxidising agents? Are there also reducing agents if there are oxidising agents? So what exactly are reducing agents?
Take a chill pill. Because the information on this content page has the answers to these queries.
So let's explore oxidising and reducing agents in further detail.
TABLE OF CONTENTS
Example:
In this equation, H2SO4 act as an oxidising agent. It oxidises Zn and itself gets reduced.
- - Oxidation
- Reduction
Example:
In this equation, O2 acts as an oxidising agent. It oxidises Cu and itself gets reduced.
- Oxidation
- Reduction
Example:
In this equation, F2 act as an oxidising agent. It oxidises NaCl and itself gets reduced.
- Oxidation
- Reduction
Example:
In this equation, H2O2 act as an oxidising agent. It oxidises PbS and itself gets reduced.
- Oxidation
- Reduction
Example:
In this equation, HCl act as a reducing agent. It reduces F2 and itself gets oxidised
- Oxidation
- Reduction
Example:
In this equation, Li acts as a reducing agent. It reduces F2 and itself gets oxidised.
- Oxidation
- Reduction
Example:
In this equation, acts as a reducing agent. It reduces and itself gets oxidised.
- Oxidation
- Reduction
Example:
Observe the given reaction. When lead (Pb) reacts with copper sulphate solution, lead (Pb) is converted to lead sulphate (PbSO4) and copper sulphate (CuSO4) to copper (Cu). There is an increase in the oxidation state of lead, confirming its oxidation, and a decrease in the oxidation state of copper, confirming its reduction.
In a redox reaction, the oxidising agent undergoes reduction i.e. it gains electrons, and the reducing agent undergoes oxidation i.e. it loses electrons.
In the given reaction, the oxidising agent is copper sulphate (CuSO4) as copper (Cu) goes from +2 to 0 oxidation state i.e it accepts 2 electrons from lead (Pb) and undergoes reduction.
Similarly, the reducing agent in this reaction is lead (Pb) as it goes from 0 to +2 oxidation state i.e it donates 2 electrons to copper (Cu) and undergoes oxidation.
Q1. Which will behave as an oxidising agent in the given reaction?
A. PbSO4(aq)
B. Zn(s)
C. Pb(s)
D. Both (A) and (C)
Answer: A)
Solution: The oxidation state of Pb in PbSO4(aq) is +2, and the oxidation state of Pb in Pb(s) is 0 i.e. Pb2+ accepts two electrons from Zn and becomes Pb. Therefore Pb2+ (PbSO4) undergoes reduction, or in other words, it acts as an oxidising agent.
(reduced/oxidising agent)
The oxidation state of Zn in Zn(s) is 0 and the oxidation state of Zn in ZnSO4(aq) is +2 i.e. Zn donates two electrons to Pb2+ and becomes Zn2+. Therefore, Zn undergoes oxidation, or in other words, it acts as a reducing agent.
(oxidised/redducing agent)
Hence, PbSO4(aq) is the oxidising agent in the given reaction.
So, option A) is the correct answer.
Q2. Which of the following will act as a reducing agent in the given reaction?
A. HNO3(aq)
B. Cu(s)
C. Cu(NO3)2
D. 2H2O(aq)
Answer: B)
Solution: The oxidation state of N in HNO3(aq) is +5, and the oxidation state of N in NO2(g) is +4 i.e. N5+ accepts an electron from Cu and becomes N4+. Therefore N5+ (HNO3) undergoes reduction, or in other words, it acts as an oxidising agent.
(reduced/oxidising agent)
The oxidation state of Cu in Cu(s) is 0 and the oxidation state of Cu in Cu(NO3)2(aq) is +2 i.e. Cu donates two electrons and becomes Cu2+. Therefore, Cu undergoes oxidation, or in other words, it acts as a reducing agent.
(oxidised/reducing agent)
Hence, Cu (s) is the reducing agent in the given reaction.
So, option B) is the correct answer.
Q3. For the reaction , pick out the correct statement.
A. CuCl2 is reduced and H2 is oxidised.
B. CuCl2 is oxidised and H2 is reduced.
C. CuCl2 is both oxidised and reduced.
D. H2 is both oxidised and reduced.
Answer: A)
Solution: The oxidation state of Cu in CuCl2 is +2, and the oxidation state of Cu in Cu is 0 i.e. Cu2+ accepts two electrons and becomes Cu. Therefore, Cu2+ (CuCl2) undergoes reduction, or in other words, it acts as an oxidisng agent.
(reduced/oxidising agent)
The oxidation state of H in H2 is 0, and the oxidation state of H in HCl is +1 i.e. H donates an electron and becomes H+. Therefore H (H2) undergoes oxidation, or in other words, it acts as a reducing agent.
(oxidised/reducing agent)
Thus, CuCl2 is reduced and H2 is oxidised in the given reaction.
So, option A) is the correct answer.
Q4. Which of the following will act as both a reducing agent and an oxidising agent in the given reaction?
A. Cl2(g)
B. Cl-(aq)
C.
D. All of these
Answer: A)
Solution: The oxidation state of Cl in Cl2(g) is 0, and the oxidation state of Cl in Cl-(aq) is -1 i.e Cl accepts an electron and becomes Cl-(aq). Therefore, Cl undergoes reduction, or in other words, it acts as an oxidising agent.
(reduced/oxidising agent)
The oxidation state of Cl in Cl2(g) is 0, and the oxidation state of Cl in is +7 i.e. Cl donates 7 electrons and becomes Cl+7(aq). Therefore, Cl undergoes oxidation, or in other words, it acts as a reducing agent.
(oxidised/reducing agent)
Hence, Cl2(g) gets reduced and oxidised, and can therefore act as both a reducing and an oxidising agent.
So, option A) is the correct answer.
Q1. Is there a difference between a reducing agent and an anti-oxidant?
Answer: Antioxidant agents can stop a chain reaction by getting rid of the free radical intermediates. Antioxidants can be thought of as reducing agents since they are oxidised while acting as antioxidants. Examples include polyphenols, thiols and ascorbic acid.
Q2. What biological effects do oxidising agents have?
Answer: The harmful effects of oxidants include damage to lipids, proteins and DNA, as well as the acceleration of atherosclerosis, rheumatoid arthritis, and cataract development. Additionally, oxidants are to blame for the ischemia-reperfusion syndrome.
Q3. Why are metals referred to as reducing agents?
Answer: Because all metals are relatively electropositive and have low ionisation energies, they lose electrons relatively quickly. As a result of their tendency to donate electrons and become oxidised, metals act as reducing agents.
Q4. What effect do oxidants have on respiration?
Answer: High doses of oxidants like ozone and nitrogen dioxide result in death from lung oedema. Worsening of asthma (acute effects) and effects on lung growth are well-established effects on the respiratory system (chronic effects). Long-term exposure to oxidising agents such as ozone has recently been linked to negative cardiovascular outcomes, including increased mortality.