Explain why the melting point of methyl fluoride, CH3 F (-142^∘ C), is higher than the melting p

step 1 Methyl fluoride has a higher melting point because it has stronger intermolector forces. If we d

Explain why the melting point of methyl fluoride, CH3 F...

Explain why the melting point of methyl fluoride, $\mathrm{CH}_{3} \mathrm{F}$ $\left(-142^{\circ} \mathrm{C}\right),$ is higher than the melting point of methane, $\mathrm{CH}_{4}\left(-182^{\circ} \mathrm{C}\right)$.

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Key Concepts

Intermolecular Forces

Intermolecular forces determine the energy required to overcome the attraction between molecules in a solid state. Molecules that experience stronger interactions, such as dipole-dipole attractions in addition to dispersion forces, require more energy to melt, hence resulting in a higher melting point.

Molecular Polarity and Dipole Moment

The introduction of a highly electronegative atom into a molecule can create a permanent dipole moment. The presence of a dipole means that, in addition to the typical London dispersion forces, there are dipole-dipole interactions that enhance the overall intermolecular attraction, influencing the melting point.

Electronegativity and Substitution Effects

Replacing a less electronegative atom in a molecule with a more electronegative one alters the electron distribution, resulting in increased molecular polarity. This change can lead to stronger intermolecular attractions due to dipole-dipole interactions, thereby affecting the melting point relative to a molecule without such a substitution.

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