is it true that CO2 is a gas whereas SiO2 is a solid.

Explanation

To determine whether the statement "CO2 is a gas whereas SiO2 is a solid" is true, we can analyze the properties of both compounds based on their molecular structure and intermolecular forces.

### Step-by-Step Solution:

1. **Identify the State of CO2 at Room Temperature:**
- Carbon dioxide (CO2) is a molecular compound. At room temperature (approximately 25°C), CO2 exists as a gas. This is due to the weak intermolecular forces (dispersion forces) that hold the CO2 molecules together, which are not strong enough to keep them in a solid state.

2. **Identify the State of SiO2 at Room Temperature:**
- Silicon dioxide (SiO2), on the other hand, is a network solid. In SiO2, each silicon (Si) atom is covalently bonded to four oxygen (O) atoms in a tetrahedral arrangement, forming a three-dimensional network. This strong covalent bonding results in a solid structure with a high melting point.

3. **Compare the Intermolecular Forces:**
- The weak dispersion forces in CO2 allow it to exist as a gas, while the strong covalent bonds in SiO2 result in a solid state. The difference in the type of bonding and structure is key to understanding their physical states.

4. **Conclusion:**
- Based on the analysis, we can conclude that the statement "CO2 is a gas whereas SiO2 is a solid" is indeed true.

### Final Answer:
Yes, it is true that CO2 is a gas whereas SiO2 is a solid.

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