Why is the boiling point of water lower than hydrogen peroxide

Hydrogen peroxied has a boiling point of 150 degrees while water is 100 degrees. Are there any inermolecular forces in these molecules causing this? please explain

While boiling point differences can be attributed to variations in the strengths of intermolecular forces, there are three types of forces which must be considered.

Hydrogen peroxide has more electrons, which gives a greater polariability for H2O2 and stronger London dispersion forces.

H2O2 has a much greater dipole moment than does water. H2O2 is 2.26 Debye vs 1.86 Debye for water. The greater dipole-dipole attraction also contributes to the increased boiling point.

H2O2 exibits hydrogen bonding and with one additional oxygen atom, compared to water, there are more sites available to form hydrogen bonds. With potentially more hydrogen bonding in H2O2, the boiling point will be greater.

The bottom line is that all three types of intermolecular forces are stronger for hydrogen peroxide than for water which accounts for the greater boiling point of H2O2.

============ Follow up =============

Ich will says, "OH, and let me clarify. Hydrogen bonds ARE NOT actually "bonds." They are called that because they are the strongest intermolecular force and were once thought to be a chemical bond due to their strength. No bonds are broken in phase changes, only IMF's."

To which we reply, "Wrong, wrong and wrong." Hydrogen bonds ARE bonds as recently clarified by the IUPAC. They are CURRENTLY thought to be bonds. Hydrogen bonds are broken during phase changes. This requires a lot of energy, which means that water has a much greater boiling point than H2S, for example, where there are no hydrogen bonds. Hydrogen bonds involve the formation of weakly covalent bonds between molecules where hydrogen is the bridging element.

Here is an excerpt from the recent redefinition of the hydrogen bond by the IUPAC, "The hydrogen bond is an attractive interaction between a hydrogen atom from a molecule or a molecular fragment X–H in which X is more electronegative than H, and an atom or a group of atoms in the same or a different molecule, in which there is evidence of bond formation. A typical hydrogen bond may be depicted as X–H•••Y–Z, where the three dots denote the hydrogen bond. .... arising from charge transfer between the donor and acceptor leading to partial covalent bond formation between H and Y."