Introduction:
In chemistry, a reducing agent is a substance that donates electrons during a chemical reaction, causing another substance to be reduced. On the other hand, an oxidant is a substance that accepts electrons during a chemical reaction, causing another substance to be oxidized. In this context, we will explore the reducing and oxidizing properties of two compounds, SnCl2 and PbCl2.

SnCl2 as a reducing agent:
SnCl2, also known as tin(II) chloride, behaves as a reducing agent due to the presence of Sn(II) ions. The reduction potential of Sn(II) is higher than that of H+ ions, allowing it to donate electrons and reduce other species. Here's a detailed explanation:

1. Oxidation state of Sn in SnCl2:
- Tin in SnCl2 has an oxidation state of +2. This means that each Sn atom donates two electrons to form Sn(II) ions.

2. Reduction of other species:
- Sn(II) ions can reduce various species by donating electrons to them. For example, in the presence of H+ ions, Sn(II) is oxidized to Sn(IV) while H+ is reduced to H2 gas:
Sn(II) + 2H+ → Sn(IV) + H2

- Similarly, Sn(II) can reduce other metal ions, such as Fe(III) or Cu(II), by donating electrons and causing their reduction.

3. Overall process:
- In any chemical reaction where SnCl2 is acting as a reducing agent, the Sn(II) ions are oxidized to Sn(IV), while the other species being reduced gains electrons.

PbCl2 as neither an oxidant nor a reductant:
PbCl2, also known as lead(II) chloride, does not exhibit significant oxidizing or reducing properties. Here's why:

1. Oxidation state of Pb in PbCl2:
- Lead in PbCl2 has an oxidation state of +2, similar to Sn in SnCl2. However, the reduction potential of Pb(II) is lower than that of Sn(II).

2. Lack of significant reducing properties:
- While Pb(II) can technically donate electrons, its reduction potential is not sufficient to effectively reduce other species. As a result, PbCl2 is not commonly used as a reducing agent.

3. Lack of significant oxidizing properties:
- Similarly, Pb(II) does not have a strong tendency to accept electrons and oxidize other species. Therefore, PbCl2 does not behave as an oxidant in most reactions.

Conclusion:
In summary, SnCl2 behaves as a reducing agent due to the ability of Sn(II) ions to donate electrons and reduce other species. On the other hand, PbCl2 does not significantly exhibit oxidizing or reducing properties, making it neither an oxidant nor a reductant in chemical reactions.