Why do real gases not behave exactly like ideal gases?

An ideal gas is a hypothetical gas consisting of identical particles of negligible volume, with no intermolecular forces. Also the atoms or molecules of the gas undergo perfectly elastic collisions with the walls of the container and each other. Real gases do not exhibit these exact properties.

because the particals will not move the same as real gases

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the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.