You are absolutely correct! While NaCl and C₄H₁₀ have similar molecular masses, their boiling points are vastly different. Here's why:

* Ionic vs. Covalent Bonding: NaCl is an ionic compound, meaning it forms a crystal lattice structure held together by strong electrostatic forces between positively charged sodium ions (Na⁺) and negatively charged chloride ions (Cl⁻). C₄H₁₀ (butane) is a covalent compound, with molecules held together by relatively weak Van der Waals forces.

* Strength of Intermolecular Forces: The electrostatic forces in ionic compounds are significantly stronger than the Van der Waals forces in covalent compounds. This difference in the strength of intermolecular forces is the primary reason for the huge boiling point disparity.

Here's how it translates to boiling point:

* NaCl: To break the strong ionic bonds in NaCl and cause it to boil, you need to supply a tremendous amount of energy, resulting in a very high boiling point (over 1400°C).

* C₄H₁₀: The weak Van der Waals forces in butane are easily overcome with relatively little energy, leading to a much lower boiling point (-0.5°C).

In summary:

* NaCl: Strong ionic bonds = high melting and boiling points

* C₄H₁₀: Weak Van der Waals forces = low melting and boiling points