Ideal gases behave ideally with negligible intermolecular forces

Steps:

• Recall ideal gas law: PV = nRT assumes point particles with no interactions.
• Identify deviations: Real gases deviate due to intermolecular forces and molecular volume.
• Evaluate conditions: High pressure and low temperature enhance attractions, increasing deviations.
• Assess properties: Weaker forces reduce attractions, making behavior closer to ideal.

Why D is correct:

• Ideal gas model defines gases as having zero intermolecular forces; weaker forces minimize deviations from PV = nRT.

Why the others are wrong:

• A: Higher pressure compresses molecules, amplifying intermolecular attractions and volume effects.
• B: Lower temperature slows molecules, strengthening relative impact of attractive forces.
• C: More polar molecules increase dipole-dipole attractions, causing larger deviations.

Final answer: D