Volatility of (CH₃)₂CO vs. (CH₃)₃SiO
The difference in volatility between acetone ((CH₃)₂CO) and trimethylsiloxy ((CH₃)₃SiO) can be attributed to their molecular structures and intermolecular forces.

1. Molecular Structure
- (CH₃)₂CO (Acetone) has a simple carbonyl group (C=O) flanked by two methyl groups.
- (CH₃)₃SiO (Trimethylsiloxy) contains a silicon atom bonded to three methyl groups and an oxygen atom, leading to a more complex structure.

2. Intermolecular Forces
- Acetone exhibits significant dipole-dipole interactions due to its polar carbonyl group, which allows for relatively strong interactions between molecules.
- However, the forces are not as strong as those found in larger or more complex molecules.
- In contrast, trimethylsiloxy has stronger van der Waals forces due to its larger size and the presence of silicon.
- The silicon-oxygen bond contributes to a more stable structure, resulting in weaker volatility compared to acetone.

3. Boiling Point
- Acetone has a boiling point of approximately 56 °C, which allows it to readily evaporate at room temperature.
- Trimethylsiloxy has a higher boiling point, attributed to its stronger intermolecular forces, making it less volatile.

4. Conclusion
- The combination of molecular structure and the nature of intermolecular forces dictates the volatility of these compounds.
- Acetone's simple structure and weaker interactions lead to its volatility, while trimethylsiloxy's complex structure and stronger forces result in lower volatility.