Define reduction in terms of (i) electron transfer, (ii) change in oxidation number. $$ClO^- + SO_2^{2-} + OH^- \rightarrow Cl^- + SO_4^{2-} + H^+$$ Assign oxidation numbers in the first equation above to identify (iii) the reducing reagent, (iv) the oxidising reagent. $$ClO^- + Br^- + H^+ \rightarrow Cl^- + Br_2 + H_2O$$ Using oxidation numbers, or otherwise, balance either equation.

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Define reduction in terms of (i) electron transfer, (ii) change in oxidation number - Leaving Cert Chemistry - Question b - 2016

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Define reduction in terms of (i) electron transfer, (ii) change in oxidation number. $$ClO^- + SO_2^{2-} + OH^- \rightarrow Cl^- + SO_4^{2-} + H^+$$ Assign oxidati... show full transcript

Worked Solution & Example Answer:Define reduction in terms of (i) electron transfer, (ii) change in oxidation number - Leaving Cert Chemistry - Question b - 2016

Step 1

(i) electron transfer

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Answer

Reduction is defined as the gain of electrons. In a redox reaction, the species undergoing reduction receives electrons from the oxidizing agent.

Step 2

(ii) change in oxidation number

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Answer

Reduction can also be defined as a decrease in oxidation number. When a substance is reduced, its oxidation state decreases, indicating a gain of electrons.

Step 3

(iii) the reducing reagent

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In the equation $ClO^- + SO_2^{2-} + OH^- \rightarrow Cl^- + SO_4^{2-} + H^+$ , the reducing agent is $SO_2^{2-}$ . This species donates electrons to the $ClO^-$ , leading to the reduction of chlorine.

Step 4

(iv) the oxidising reagent

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In the same equation, the oxidizing agent is $ClO^-$ . It accepts electrons from the $SO_2^{2-}$ , thus causing the oxidation of sulfur.

Step 5

Using oxidation numbers, or otherwise, balance either equation

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To balance the equation $4ClO^- + SO_2^{2-} + 4OH^- \rightarrow 4Cl^- + 2SO_4^{2-} + 2H^+$ , we first determine the oxidation states:

Chlorine in $ClO^-$ is +1, and in $Cl^-$ is -1.
Sulfur in $SO_2^{2-}$ is +4, and in $SO_4^{2-}$ is +6.

The balanced equation maintains conservation of mass and charge, ensuring that the number of each type of atom and the charges are equal on both sides.

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Define reduction in terms of (i) electron transfer, (ii) change in oxidation number - Leaving Cert Chemistry - Question b - 2016

Worked Solution & Example Answer:Define reduction in terms of (i) electron transfer, (ii) change in oxidation number - Leaving Cert Chemistry - Question b - 2016

(i) electron transfer

(ii) change in oxidation number

(iii) the reducing reagent

(iv) the oxidising reagent

Using oxidation numbers, or otherwise, balance either equation

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