Final answer:
CH₃F exhibits London dispersion forces, dipole-dipole forces, and hydrogen bonding. Therefore, the correct answer is D) All of the above.
Step-by-step explanation:
CH₃F, or methyl fluoride, is a molecule composed of carbon (C), hydrogen (H), and fluorine (F) atoms. To identify the intermolecular forces present, we need to consider the nature of the bonds and the overall molecular geometry.
A) London Dispersion Forces: These forces arise from temporary fluctuations in electron distribution, leading to temporary dipoles. In CH₃F, fluorine is more electronegative than carbon and hydrogen, creating an uneven distribution of electrons. This uneven distribution induces temporary dipoles in neighboring molecules, resulting in London dispersion forces.
B) Dipole-Dipole Forces: CH₃F is a polar molecule due to the significant electronegativity difference between fluorine and the other atoms. This polarity results in permanent dipoles, and dipole-dipole forces occur between the positive end of one molecule and the negative end of another.
C) Hydrogen Bonding: Hydrogen bonding occurs when hydrogen is directly bonded to a highly electronegative atom (like fluorine, nitrogen, or oxygen). In CH₃F, there is a hydrogen atom bonded to fluorine, making hydrogen bonding possible.
CH₃F exhibits London dispersion forces, dipole-dipole forces, and hydrogen bonding due to its molecular composition and geometry. These intermolecular forces collectively contribute to the substance's physical properties, such as boiling point and solubility.