Single Choice

It is because of inability of $$ns^2$$ electrons of the valence shell to participate in bonding that:

A$$Sn^{4+}$$ is reducing while $$Pb^{4+}$$ is oxidising
B$$Sn^{2+}$$ is reducing while $$Pb^{4+}$$ is oxidising
Correct Answer
C$$Sn^{2+}$$ is oxidising while $$Pb^{4+}$$ is reducing
D$$Sn^{2+}$$ and $$Pb^{2+}$$ are both oxidising and reducing

Solution

$$\displaystyle Sn^{2+}$$ is reducing while $$\displaystyle Pb^{4+}$$ is oxidising.

$$\displaystyle Pb^{2+}$$ compounds are more stable than $$\displaystyle Pb^{4+}$$.

$$\displaystyle Pb^{4+}$$ compounds are easily reduced to stable $$\displaystyle Pb^{2+}$$ compounds.

$$Sn^{2+}$$ can be oxidise to $$Sn^{4+}$$ making it reducing agent.

SIMILAR QUESTIONS

Redox Reactions

The compound that cannot act both as oxidising and reducing agent is:

Redox Reactions

In the reaction, $$8Al+3Fe_{3}O_{4}\rightarrow 4Al_{2}O_{3}+9Fe$$ the number of electrons transferred from the reductant to the oxidant is:

Redox Reactions

Fluorine reacts with ice and results as follows: H2O(s)+F2(g)→HF(g)+HOF(s) Justify that this reaction is a redox reaction.

Redox Reactions

The compound AgF2 is unstable compound. However, if formed, the compound acts as a very strong oxidising agent. Why ?

Redox Reactions

$$2S_2O^{2-}_3\,(aq)+I_2(s)\rightarrow S_4O^{2-}_6(aq)+2I^{-}(aq)$$ $$S_2O^{2-}_3(aq)+2Br_2(l)+5H_2O(l)\rightarrow 2SO^{2-}_4(aq)+4Br^{-}(aq)+10H^{+}(aq)$$ Why does the same reductant, thiosulphate react differently with iodine and bromine?

Redox Reactions

Which of the following statements is not true ?

Redox Reactions

Which of the following statements is correct regarding redox reactions?

Redox Reactions

The number of moles of $$K_2Cr_2O_7 $$ reduced by one moles of $$Sn^{2+}$$ ions is:

Redox Reactions

Identify the reducing agent in the following reaction. $$H_{2} O+F_{2} \rightarrow H F+H O F$$

Redox Reactions

Identify the oxidising agent (oxidant) in the following reactions $$\text { (d) } V_{2} O_{5}+5 C a \rightarrow 2 V+5 C a O$$

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