Which of the following facts is evidence for the existence of induced dipole-induced dipole interactions between molecules?
Answer
>>>Ions in water become surrounded by water molecules and this is what we observe as "dissolving."
Water freezes into a solid made up of molecules in a three-dimensional lattice.
or >>>>Molecules with O-H bonds can interact with each other and make the boiling point of the molecule of which they are a part very high.
Noble gases can be liquefied. Because they can be liquids, noble gas atoms must have some attraction for one another.
I'm not sure I like the way these are stated but the answer probably comes the closest to the last one; i.e, the noble gas atoms, especially He atoms.
The noble gas one is correct
The choice that provides evidence for the existence of induced dipole-induced dipole interactions between molecules is:
>>> Molecules with O-H bonds can interact with each other and make the boiling point of the molecule of which they are a part very high.
Explanation:
Induced dipole-induced dipole interactions, also known as London dispersion forces, occur between non-polar molecules or atoms. These forces result from temporary fluctuations in electron distribution that create temporary dipoles. The strength of these interactions increases with the size and shape of molecules.
In the given option, molecules with O-H bonds (such as water) can interact with each other through hydrogen bonding. Hydrogen bonding is a special case of dipole-dipole interaction in which a hydrogen atom bonded to an electronegative atom (like oxygen) interacts with another electronegative atom in a different molecule. This interaction leads to a strong attraction between water molecules, resulting in high boiling points for substances like water.
Since hydrogen bonding is a type of dipole-dipole interaction, it is a form of induced dipole-induced dipole interaction between molecules. Therefore, this fact provides evidence for the existence of induced dipole-induced dipole interactions.