Most elements form oxides and hydroxides with different characteristics. Often, regular periodic trends are observed in these oxides and hydroxides. Hydroxides of `Na` and `Mg` are distinctly alkaline, while oxides of `N` and `S` are distinctly acidic.
Draw the structure of sulfur dioxide

Answer

To draw the structure of sulfur dioxide (SO₂), we can follow these steps:

### Step 1: Determine the number of valence electrons
- Sulfur (S) has 6 valence electrons.
- Oxygen (O) has 6 valence electrons, and since there are two oxygen atoms, we multiply by 2.
- Total valence electrons = Valence electrons of S + 2 × Valence electrons of O = 6 + 2(6) = 18.

### Step 2: Calculate the number of bond pairs and lone pairs
- We divide the total number of valence electrons (18) by 2 to find the number of electron pairs.
- Number of electron pairs = 18 / 2 = 9.
- Each bond pair contributes 1 to this count, and each lone pair also contributes 1.
- To find the number of bond pairs (b) and lone pairs (l), we can use the formula:
- b + l = 9.
- The number of bond pairs can be determined by considering the typical bonding in SO₂. Since sulfur typically forms two double bonds with oxygen, we can assume 2 bond pairs.
- Therefore, the number of lone pairs = 9 - 2 = 7.

### Step 3: Identify the hybridization
- The hybridization can be determined from the number of bond pairs and lone pairs.
- In this case, with 2 bond pairs and 1 lone pair, the hybridization is sp².

### Step 4: Determine the molecular geometry
- According to VSEPR theory, the presence of 2 bond pairs and 1 lone pair results in a bent or V-shaped molecular geometry.

### Step 5: Draw the structure
- Place the sulfur atom in the center.
- Draw two oxygen atoms bonded to the sulfur atom with double bonds.
- Indicate the lone pair of electrons on the sulfur atom.

The final structure of sulfur dioxide (SO₂) can be represented as follows:

```
O
||
S -- O
:
```