Hydrogen bonds are generally stronger than coordinate bonds. Hydrogen bonds are formed between a hydrogen atom and an electronegative atom such as nitrogen, oxygen, or fluorine. The electronegative atom attracts the electrons in the hydrogen bond, creating a partial positive charge on the hydrogen atom and a partial negative charge on the electronegative atom. This electrostatic attraction is what holds the hydrogen bond together.

Coordinate bonds, also known as dative bonds, are formed when one atom donates a pair of electrons to another atom. The atom that donates the electrons is called the Lewis base, and the atom that accepts the electrons is called the Lewis acid. Coordinate bonds are weaker than hydrogen bonds because the electrostatic attraction between the two atoms is weaker. This is because the electrons in a coordinate bond are not shared equally between the two atoms, as they are in a hydrogen bond.

In general, hydrogen bonds are about 10 times stronger than coordinate bonds. However, the strength of a hydrogen bond or a coordinate bond can vary depending on the specific atoms involved.