**Boiling point and Intermolecular Forces:**
The boiling point of a compound is determined by the strength of its intermolecular forces. Intermolecular forces are the attractive forces between molecules that hold them together in the liquid or solid phase. The stronger the intermolecular forces, the higher the boiling point of a compound.

**Comparing Intermolecular Forces:**
When comparing the boiling points of the given compounds (SnCl4, GeCl4, SiCl4, and CCl4), we need to consider the type of intermolecular forces present.

1. **SnCl4 (Tin(IV) chloride):**
Tin(IV) chloride is a covalent compound. It contains polar covalent bonds between tin and chlorine atoms. However, the molecule as a whole is non-polar because the dipole moments cancel each other out. The main intermolecular force in SnCl4 is London dispersion forces, which are relatively weak. Therefore, SnCl4 has a relatively low boiling point.

2. **GeCl4 (Germanium(IV) chloride):**
Similar to SnCl4, Germanium(IV) chloride is also a covalent compound with polar covalent bonds. However, the molecule as a whole is non-polar due to the symmetrical arrangement of the chlorine atoms around the central germanium atom. The main intermolecular force in GeCl4 is London dispersion forces, which are relatively weak. Therefore, GeCl4 also has a relatively low boiling point.

3. **SiCl4 (Silicon(IV) chloride):**
Silicon(IV) chloride is another covalent compound with polar covalent bonds. However, unlike SnCl4 and GeCl4, the molecule is tetrahedral in shape, which means it is not symmetrical. As a result, SiCl4 has a permanent dipole moment and experiences stronger dipole-dipole interactions compared to SnCl4 and GeCl4. Therefore, SiCl4 has a higher boiling point than the previous two compounds.

4. **CCl4 (Carbon tetrachloride):**
Carbon tetrachloride is a covalent compound with non-polar covalent bonds. The molecule is tetrahedral and symmetrical, resulting in a cancellation of dipole moments. The only intermolecular force present in CCl4 is London dispersion forces, which are weaker than dipole-dipole interactions. Therefore, CCl4 has a relatively low boiling point.

**Conclusion:**
Among the given compounds, SiCl4 has the highest boiling point because it has stronger dipole-dipole interactions due to its non-symmetrical molecular shape. On the other hand, SnCl4, GeCl4, and CCl4 have weaker intermolecular forces (London dispersion forces) and therefore lower boiling points.