`SnCl2` acts as a reducing agent because

Options

A. `SnCl_(2)` can accept electrons readily
B. `Sn^(3+)` is more stable than `Sn^(2+)`
C. `Sn^(4+)` is more stable than `Sn^(2+)`
D. `Sn^(2+)` can be readily converted to metallic tin.

Answer

To understand why SnCl2 acts as a reducing agent, we can break down the explanation into a series of steps:

### Step 1: Identify the oxidation states of tin in SnCl2
- In SnCl2, tin (Sn) has an oxidation state of +2. This is because each chlorine (Cl) atom has an oxidation state of -1, and there are two chlorine atoms, giving a total of -2. To balance this, tin must be +2.

### Step 2: Understand the electronic configuration of tin
- The electronic configuration of tin (Sn) is [Kr] 4d10 5s2 5p2. This shows that tin has four electrons in its outermost shell (5s and 5p orbitals).

### Step 3: Determine the stable oxidation state of tin
- The stable oxidation state of tin is +4 (Sn4+). This means that tin can lose additional electrons to achieve a more stable electronic configuration.

### Step 4: Explain the process of oxidation and reduction
- A reducing agent is a substance that donates electrons to another species, causing that species to be reduced while itself being oxidized. In this case, SnCl2 can oxidize itself from Sn2+ to Sn4+, meaning it loses two electrons.

### Step 5: Conclude why SnCl2 is a reducing agent
- Since SnCl2 can lose electrons (oxidize itself to Sn4+) and in the process, it can reduce other species (by donating those electrons), it acts as a reducing agent.

### Summary
SnCl2 acts as a reducing agent because it can oxidize itself from Sn2+ to Sn4+, thereby donating electrons to reduce other species.

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