Question

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Class 11th Chemistry...

Chapter - Redox Reactions...

So here are the questions..

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(i) Explain Redox Reactions on the basis of electron transfer. Use suitable examples.

(ii) Why does fluorine do not show disproportionation reaction?

(iii) Which method can be used to find out strength of reductant/ oxidant in solution? Explain with the help of example.

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Answer 1

♠ ANSWER ;
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➊. REDOX REACTIONS ( on the basis of electron transfer ) :

The species which loses electrons is said to be oxidised and the species which gains electrons is said to be reduced.

Since there cannot be a net gain or loss of electrons in a chemical reaction, this means that all chemical Changes involving the loss and gain of electrons occur simultaneously. THAT'S WHY OXIDATION TAKES PLACE AT THE COST OF REDUCTION AND VICE VERSA..

Hence, it is called REDOX reaction.

▶ EXAMPLE :
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4 Na (s) + O₂ ( g ) ➝ 2 Na₂ O ( s )

2 Na ( s ) + S ( s ) ➝ Na₂ S.

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➋. Like Chlorine, bromine and iodine also undergo similar disproportionation reactions. However, Fluorine does not show this behaviour. This is because FLUORINE IS THE MOST ELECTRONEGATIVE AND STRONGEST OXIDISING AGENT and therefore, it does not show positive oxidation states. That's why fluorine do not show disproportionation reaction.

▶ EXAMPLE :
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2 F₂ ( g ) + 2 OH^- ( aq ) ➝ 2 F ^- ( aq ) + OF₂ ( g ) + H ₂ O ( l ).

Here, F₂ also reacts with water to produce some oxygen.
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➌. E . M. F. or Potential of a cell is the method by which we can determine the strength of reductant and oxidant in a solution.

The difference between the electrode potentials of the two electrodes constituting an electrochemical cell is known as ELECTROMOTIVE FORCE ( E. M. F ) or cell potential.

If standard electrode potential is more than zero, then its reduced form will be more stable compared to hydrogen gas . And will act as strong OXIDISING AGENT..

On the other hand , if standard electrode potential is negative than hydrogen, then hydrogen gas is more stable than the reduced form of the species. And hence, will act as a strong REDUCING AGENT.

Similarly, we can compare two species.

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