Which is of the following is TRUE for deviations from ideal gas behavior?
Real gases can exhibit no deviation whatsoever from ideal gas behavior whatsoever at the proper values for $P$, $V$, $T$, and $n$.
At higher pressures and temperatures, real gases deviate more from ideal behavior because the atoms and molecules of the gas do not have enough energy to overcome their intermolecular forces.
The volume of gas particles is irrelevant in considering their behavior because a gas can only fill its container, regardless of the volume of the particles themselves. Since gas particles always fill their container, the volume of the container itself is all that is necessary to describe the behavior of the gas.
It is not possible for real gases to be completely described by the ideal gas model because some intermolecular attraction is inevitable. If no such attraction existed, gases could never condense into liquids or freeze into solids.