Question

what kind of intermolecular forces act between an ammonia molecule and a hydrogen peroxide (h₂o₂) molecule?
note: if there is more than one type of intermolecular force that acts, be sure to list them all, with a comma between the name of each force.

Explanation:

• Dipole - dipole forces: Both \(NH_3\) (ammonia) and \(H_2O_2\) (hydrogen peroxide) are polar molecules. A polar molecule has a permanent dipole moment due to the unequal distribution of electron density within the molecule. When two polar molecules interact, the positive end of one dipole is attracted to the negative end of another dipole. This is the dipole - dipole force.
• Hydrogen bonding: Hydrogen bonding is a special case of dipole - dipole interaction. For hydrogen bonding to occur, a hydrogen atom must be bonded to a highly electronegative atom (such as \(N\) in \(NH_3\) and \(O\) in \(H_2O_2\)). In \(NH_3\), \(H\) is bonded to \(N\) (\(N\) has a high electronegativity of \(3.04\)), and in \(H_2O_2\), \(H\) is bonded to \(O\) (\(O\) has an electronegativity of \(3.44\)). The \(H\) atom (which has a partial positive charge) in one molecule is attracted to the \(N\) or \(O\) atom (which has a partial negative charge) in another molecule.
• London dispersion forces: These forces exist between all molecules, whether they are polar or non - polar. They are caused by the temporary fluctuations in electron density within a molecule, which can induce dipoles in neighboring molecules. Even though \(NH_3\) and \(H_2O_2\) have stronger dipole - dipole and hydrogen bonding forces, London dispersion forces are also present.

Answer:

London dispersion forces, dipole - dipole forces, hydrogen bonding