Intermolecular forces drive deviations from ideal gas behavior

Steps:

• Ideal gases assume no intermolecular attractions or molecular volume; real gases deviate more with stronger forces or larger sizes at room temperature (25°C, 1 atm).
• Evaluate gases by polarity and bonding: nonpolar/monatomic gases behave ideally; polar gases with hydrogen bonding deviate most.
• Compare options: H₂ and Ne are nonpolar/small; CO₂ has weak dipole-induced forces; NH₃ has strong hydrogen bonding.
• NH₃ shows greatest deviation due to its polarity and intermolecular attractions, confirmed by higher compressibility factor deviation.

Why D is correct:

• NH₃ exhibits strong hydrogen bonding (N-H...N), violating ideal gas law's zero-interaction assumption, leading to largest PV/RT deviation per van der Waals equation.

Why the others are wrong:

• A. CO₂: Linear molecule with weak London dispersion forces, minimal deviation.
• B. H₂: Nonpolar diatomic with negligible forces and small size, nearly ideal.
• C. Ne: Monatomic noble gas with no intermolecular forces, closest to ideal.

Final answer: D