In its compounds . Tin exhibits the oxidation numbers .

Options

A. ` +2`
B. `+4`
C. ` +6`
D. `+3`

Answer

To determine the oxidation numbers exhibited by tin (Sn) in its compounds, we can follow these steps:

### Step 1: Identify the Group and Electronic Configuration
Tin (Sn) belongs to Group 14 of the periodic table, also known as the carbon family. Its electronic configuration is:
\[ \text{[Kr]} 4d^{10} 5s^2 5p^2 \]

### Step 2: Understand the Valence Electrons
In Group 14, the general outer electronic configuration is \( ns^2 np^2 \). This means that tin has 4 valence electrons (2 from the \( 5s \) subshell and 2 from the \( 5p \) subshell).

### Step 3: Determine Possible Oxidation States
To achieve a stable electronic configuration (similar to that of noble gases), tin can either lose all four of its valence electrons or just the two \( p \) electrons. Therefore, the possible oxidation states for tin are:
- **+4**: When tin loses all four valence electrons.
- **+2**: When tin loses only the two \( p \) electrons and retains the two \( s \) electrons.

### Step 4: Explain the Inert Pair Effect
The existence of these two oxidation states is influenced by the inert pair effect, which is more pronounced in heavier elements of the group. This effect arises due to the poor shielding of the \( s \) electrons by the intervening \( d \) or \( f \) electrons, making it energetically less favorable for the \( s \) electrons to participate in bonding.

### Conclusion
Thus, in its compounds, tin exhibits the oxidation numbers **+2 and +4**.

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