Is hydrogen bonding strongest between molecules of H20 H2S H2Se or H2Te?

Hydrogen bonding can only occur between Hydrogen and N, O, or F nothing else

H2O

Hydrogen bonding is a type of intermolecular force that occurs when a hydrogen atom is bonded to a highly electronegative atom (such as oxygen, nitrogen, or fluorine) and is attracted to another electronegative atom in a nearby molecule.

To determine which molecule experiences the strongest hydrogen bonding, we need to consider the electronegativity and the number of hydrogen atoms available for bonding in each molecule.

Out of the given molecules (H2O, H2S, H2Se, and H2Te), water (H2O) experiences the strongest hydrogen bonding. This is because oxygen (O) is highly electronegative (3.44 on the Pauling scale), which creates a significant electrical difference between the hydrogen and oxygen atoms in water molecules. Water has two hydrogen atoms available for hydrogen bonding, resulting in strong intermolecular forces.

In comparison, while hydrogen sulfide (H2S), hydrogen selenide (H2Se), and hydrogen telluride (H2Te) also have hydrogen atoms bonded to highly electronegative atoms (sulfur, selenium, and tellurium), the electronegativities of these atoms are lower than that of oxygen. This leads to weaker hydrogen bonding.

Thus, the order of increasing strength of hydrogen bonding among the given molecules is: H2Te < H2Se < H2S < H2O.

The larger the anion the weaker the bond.