Hydrogen peroxide \(\left(\mathrm{H}_{2} \mathrm{O}_{2}\right)\) is a syrupy liquid with a relatively low vapor pressure and a normal boiling point of \(152.2^{\circ} \mathrm{C} . \mathrm{Ra}-\) tionalize the differences of these physical properties from those of water.

First, let's examine the molecular structure of both hydrogen peroxide and water. Water has a simple structure with one oxygen atom bonded to two hydrogen atoms at a 104.5-degree angle forming a bent geometry. It is a polar molecule. Hydrogen peroxide is more complex, with a shape resembling an open book - two oxygen atoms are joined by a single bond, and each oxygen atom is bonded to a hydrogen atom. This molecule also has a nonplanar structure, which makes it a polar molecule.

Now, let's discuss the intermolecular forces (IMF) that explain the differences in physical properties of hydrogen peroxide and water. The key intermolecular force in both molecules is hydrogen bonding. Hydrogen bonds are generally stronger than other intermolecular forces like dipole-dipole interactions and London dispersion forces. In water, the polar nature of the H₂O molecule combined with the relatively high electronegativity of oxygen leads to strong hydrogen bonds between water molecules. In hydrogen peroxide, stronger hydrogen bonds are also observed due to the presence of two oxygen atoms in the molecule. The nonplanar structure of hydrogen peroxide enables the presence of more hydrogen bonding sites than a water molecule.

Given that hydrogen peroxide has more hydrogen bonding sites when compared to water, it means that there are stronger forces between hydrogen peroxide molecules. These stronger intermolecular forces result in a higher boiling point for hydrogen peroxide. Regarding vapor pressure, the stronger intermolecular forces in hydrogen peroxide also play a role. Since the molecules are strongly attracted to each other, fewer molecules become a gas at a given temperature, which leads to a lower vapor pressure for hydrogen peroxide.

Lastly, let's compare their boiling points explicitly. Water has a boiling point of \(100^{\circ} \mathrm{C}\), while hydrogen peroxide has a higher boiling point of \(152.2^{\circ} \mathrm{C}\). This can be explained by the stronger hydrogen bonds in hydrogen peroxide. In conclusion, the differences in the physical properties of hydrogen peroxide and water can be rationalized by the differences in their molecular structures and intermolecular forces. Hydrogen peroxide has more hydrogen bonding sites and stronger hydrogen bonds than water, leading to its higher boiling point and lower vapor pressure compared to water.