* Low boiling point: This suggests weak intermolecular forces between the molecules of the compound.

* Insoluble in water: This implies that the compound is non-polar or has very weak interactions with water molecules. Water is a polar solvent, so it prefers to dissolve other polar molecules.

* Standard pressure (STP): This just tells us the conditions we're working under, but it doesn't directly influence the type of compound.

Putting it together:

Considering the clues, the compound is most likely a non-polar covalent molecule. Here's why:

* Weak Intermolecular Forces: Non-polar molecules primarily experience weak London Dispersion forces, which are responsible for their low boiling points.

* Insolubility in Water: The "like dissolves like" rule applies here. Water is polar, and non-polar molecules are not attracted to it, leading to insolubility.

Examples of such compounds could include:

* Small hydrocarbons: Like methane (CH4) and ethane (C2H6)

* Gases: Many gases exist as non-polar molecules at standard pressure (e.g., nitrogen (N2), oxygen (O2))

Important Note: There are exceptions. While many non-polar molecules exhibit these properties, some compounds may have other factors influencing their behavior. For instance, a large molecule with a non-polar backbone could still have some polar functional groups that might lead to weak water solubility.