What is the correct order of boiling points for the given hydrides?

The correct order of boiling points for the given hydrides illustrates the influence of molecular structure and intermolecular forces. In this case, water (H₂O) has the highest boiling point due primarily to hydrogen bonding, which is a strong type of dipole-dipole interaction that occurs when hydrogen is bonded to highly electronegative elements such as oxygen. This bonding significantly increases the energy required to transition from liquid to gas, resulting in a higher boiling point.

Following water, H₂Te (hydrogen telluride) has a higher boiling point than both H₂Se (hydrogen selenide) and H₂S (hydrogen sulfide) due to its larger molecular size and greater van der Waals forces. As you move down the group in the periodic table from sulfur to tellurium, the molecular weight increases, leading to stronger London dispersion forces, which in turn elevate the boiling points.

H₂Se then comes next in terms of boiling point, being lower than H₂Te but higher than H₂S. Hydrogen sulfide has the lowest boiling point among these hydrides due to its smaller size and weaker intermolecular forces relative to those of H₂Se and H₂Te.

Thus, the boiling point trend can be