In each pair of compounds, pick the one with the higher boiling point. Explain your reasoning. a. NH₃ or CH₄ c. CO₂ or NO₂

Verified step by step guidance

1. Identify the type of intermolecular forces present in each compound. NH_3 has hydrogen bonding due to the N-H bond, while CH_4 has only London dispersion forces.
2. Compare the strength of intermolecular forces: Hydrogen bonds in NH_3 are stronger than the London dispersion forces in CH_4, leading to a higher boiling point for NH_3.
3. For CO_2 and NO_2, identify the molecular geometry and polarity. CO_2 is linear and nonpolar, while NO_2 is bent and polar.
4. Determine the types of intermolecular forces: CO_2 has London dispersion forces, whereas NO_2 has both dipole-dipole interactions and London dispersion forces.
5. Compare the strength of intermolecular forces: The presence of dipole-dipole interactions in NO_2 makes its intermolecular forces stronger than those in CO_2, resulting in a higher boiling point for NO_2.