Silicon is the second most abundant element `(~27.2%)` in the earth's after oxygen `(45.5 %)` Carbon. Silicon, germanium, tin and lead constitute the group `14` of the periodic table. Chemistry of silicon is distinctly different from that of carbon.
For example, under standard conditions `CO_(2)` is a gas whereas `SiO_(2)` is a covalent solid.
Draw the structures of `CO_(2)` and `SiO_(2)`

Answer

To draw the structures of carbon dioxide (CO₂) and silicon dioxide (SiO₂), we will follow these steps:

### Step 1: Draw the Lewis Structure for Carbon Dioxide (CO₂)

1. **Identify the central atom**: Carbon (C) is the central atom because it is less electronegative than oxygen (O).
2. **Count the valence electrons**: Carbon has 4 valence electrons, and each oxygen has 6 valence electrons. Therefore, the total number of valence electrons is:
\[ 4 \text{ (from C)} + 2 \times 6 \text{ (from O)} = 16 \text{ valence electrons} \]
3. **Arrange the atoms**: Place carbon in the center and the two oxygen atoms on either side.
4. **Form bonds**: Connect the carbon atom to each oxygen atom with a double bond to satisfy the octet rule for all atoms. Each double bond consists of 4 electrons (2 pairs).
5. **Distribute remaining electrons**: After forming double bonds, each oxygen will have 4 electrons remaining as lone pairs.

The Lewis structure of CO₂ can be represented as:
```
O=C=O
```
Where each "=" represents a double bond.

### Step 2: Draw the Lewis Structure for Silicon Dioxide (SiO₂)

1. **Identify the central atom**: Silicon (Si) is the central atom, similar to carbon in CO₂.
2. **Count the valence electrons**: Silicon has 4 valence electrons, and each oxygen has 6 valence electrons. Therefore, the total number of valence electrons is:
\[ 4 \text{ (from Si)} + 2 \times 6 \text{ (from O)} = 16 \text{ valence electrons} \]
3. **Arrange the atoms**: Place silicon in the center and the two oxygen atoms on either side.
4. **Form bonds**: Connect the silicon atom to each oxygen atom with a double bond.
5. **Distribute remaining electrons**: After forming double bonds, each oxygen will have 4 electrons remaining as lone pairs.

The Lewis structure of SiO₂ can be represented as:
```
O=Si=O
```
Where each "=" represents a double bond.

### Final Structures

- **Carbon Dioxide (CO₂)**:
```
O=C=O
```

- **Silicon Dioxide (SiO₂)**:
```
O=Si=O
```