You are correct! The boiling point of hydrogen sulfide (H₂S) is slightly higher than that of hydrogen selenide (H₂Se).

Here's why:

* Intermolecular forces: The primary forces holding molecules together in the liquid state are Van der Waals forces. These forces increase with the size and polarizability of the molecule.

* Size and Polarizability: Selenium is larger and more polarizable than sulfur. This means that the electron cloud in a hydrogen selenide molecule is easier to distort, leading to stronger temporary dipoles (London dispersion forces).

* Hydrogen Bonding: While not as strong as in water, hydrogen sulfide exhibits weak hydrogen bonding, which contributes to a slightly higher boiling point compared to hydrogen selenide.

However:

While H₂S has a higher boiling point than H₂Se, it is still a relatively low boiling point compound due to the weak intermolecular forces involved.

Here are the approximate boiling points:

* Hydrogen sulfide (H₂S): -60°C (-76°F)

* Hydrogen selenide (H₂Se): -41°C (-42°F)