The compound with the highest boiling point will be which of the following?

A.CH3Cl
B.CH3Br
C.CH4
D.CH3F

To determine which compound has the highest boiling point, we need to consider the molecular structure and intermolecular forces present in each compound.

Among the options given, CH3Cl, CH3Br, CH4, and CH3F, the compound with the highest boiling point would be CH3Br.

The boiling point of a compound is primarily determined by the strength of the intermolecular forces. In general, larger molecules and compounds with more polar bonds tend to have higher boiling points.

In this case, CH3Br has a larger molecular size compared to CH3Cl and CH3F due to the presence of the heavier bromine atom. This increased molecular size results in stronger dispersion forces between CH3Br molecules, leading to a higher boiling point compared to the other compounds.

Therefore, option B, CH3Br, is the compound with the highest boiling point among the given options.

To determine which compound has the highest boiling point among A(CH3Cl), B(CH3Br), C(CH4), and D(CH3F), we need to analyze the intermolecular forces within each compound. Boiling point largely depends on the strength of these intermolecular forces.

CH3Cl (option A) and CH3Br (option B) are both halogen compounds, and they have dipole-dipole interactions due to the difference in electronegativity between carbon and the halogen atom. However, CH3Br has a larger molecular mass compared to CH3Cl, which leads to stronger van der Waals forces. These stronger intermolecular forces result in a higher boiling point for CH3Br.

CH4 (option C) is a nonpolar molecule and only has weak London dispersion forces as intermolecular forces. Since London dispersion forces are typically weaker than dipole-dipole interactions, CH4 will have the lowest boiling point among the given options.

CH3F (option D) is a polar molecule, like CH3Cl and CH3Br, and also has dipole-dipole interactions. However, fluorine is the most electronegative atom among these halogens, meaning that CH3F has the largest dipole moment. This larger dipole moment leads to stronger intermolecular forces and a higher boiling point compared to CH3Cl (option A) but lower than CH3Br (option B).

Therefore, the compound with the highest boiling point among the given options is B(CH3Br).

The educated guess is to go with the one with the highest molar mass.