As the carbon dioxide is in solid form(dry ice) so it has gained all the properties of solid i.e. now they have highest intermolecular force between them.

Intermolecular Forces of Attraction

Intermolecular forces of attraction are the forces that hold molecules together in a substance. These forces determine the physical properties of the substance, such as boiling point, melting point, and viscosity.

There are several types of intermolecular forces, including hydrogen bonding, dipole-dipole interactions, and London dispersion forces. Hydrogen bonding is the strongest type of intermolecular force, followed by dipole-dipole interactions, and then London dispersion forces.

Comparing the Intermolecular Forces of Attraction

Let's compare the intermolecular forces of attraction for the given substances:

Liquid Water (option A)
- Water molecules are polar due to the electronegativity difference between oxygen and hydrogen atoms.
- The hydrogen atoms in one water molecule are attracted to the oxygen atoms in neighboring water molecules through hydrogen bonding.
- Hydrogen bonding is a strong intermolecular force, making liquid water have a relatively high boiling point and surface tension.

Liquid Ethyl Alcohol (option B)
- Ethyl alcohol (C2H5OH) molecules are also polar due to the electronegativity difference between oxygen and hydrogen atoms.
- Like water, ethyl alcohol molecules can form hydrogen bonds, but they are not as strong as those in water.
- Therefore, the intermolecular forces of attraction in liquid ethyl alcohol are weaker compared to liquid water.

Gaseous CO2 (option C)
- Carbon dioxide (CO2) molecules are nonpolar because the two oxygen atoms are symmetrically arranged around the carbon atom, resulting in a linear molecule.
- Nonpolar molecules like CO2 do not have permanent dipoles and cannot form hydrogen bonds or dipole-dipole interactions.
- The only intermolecular force present in gaseous CO2 is London dispersion forces, which are relatively weak.

Solid CO2 (option D)
- Solid CO2, also known as dry ice, is composed of CO2 molecules arranged in a lattice structure.
- The intermolecular forces of attraction in solid CO2 are stronger than in gaseous CO2 because the molecules are held together in a solid state.
- Although solid CO2 does not exhibit hydrogen bonding or dipole-dipole interactions, it experiences London dispersion forces, which become significant in the solid state due to close proximity of the molecules.

Therefore, solid CO2 (option D) has the highest intermolecular forces of attraction among the given substances.