Ch.11 - Liquids, Solids & Intermolecular ForcesWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: The table below shows some physical properties of halogenated liquids.LiquidExperimental Dipole Moment (D)Normal Boiling Point (˚C)CH2F21.93–52CH2Cl21.6040CH2Br21.4397Which of the following statements

The table below shows some physical properties of halogenated liquids.
LiquidExperimental Dipole Moment (D)Normal Boiling Point (˚C)

Which of the following statements best explains these data?
(a) The larger the dipole moment, the stronger the intermolecular forces, and therefore the boiling point is lowest for the molecule with the largest dipole moment.
(b) The dispersion forces increase from F to Cl to Br; since the boiling point also increases in this order, the dispersion forces must make a far greater contribution to intermolecular interactions than dipole–dipole interactions.
(c) The trend in electronegativity is F > Cl > Br; therefore, the most ionic compound (CH2F2) has the lowest boiling point, and the most covalent compound (CH2Br2) has the highest boiling point.
(d) Boiling point increases with molecular weight for these nonpolar compounds.