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: Explain why the boiling point of Br 2 (59 °C) is lower than that of iodine monochloride, ICl (97 °C), even thought they have nearly the same molar mass.a) Br2 is larger the ICl.b) ICl is ionic.c) The

Problem

Explain why the boiling point of Br 2 (59 °C) is lower than that of iodine monochloride, ICl (97 °C), even thought they have nearly the same molar mass.

a) Br2 is larger the ICl.

b) ICl is ionic.

c) The molar mass dependence of a liquid's boiling point is not an absolute rule, and it should not be applied to all compounds.

d) It is impossible to say without further informations.

e) The molar mass is not identical, the molar mass of Br 2 is only 159.80 g/mol compared to 162.35 g/mol for ICl. 

f) ICl is polar while Br2 is nonpolar.