QuestionJuly 24, 2025

The boiling point of bromine is 59^circ C Which of the following best predicts the boiling point of iodine monochloride, a polar compound? Higher than 59^circ C because dipole-dipole interactions in iodine monochloride are stronger than dispersion forces in bromine. Lower than 59^circ C because ionic bonding in bromine is stronger than covalent bonding in iodine monochloride. Lower than 59^circ C because dipole-dipole interactions in iodine monochloride are weaker than in bromine. Higher than 59^circ C because ionic bonding in iodine monochloride is stronger than H-bonding in bromine.

The boiling point of bromine is 59^circ C Which of the following best predicts the boiling point of iodine monochloride, a polar compound? Higher than 59^circ C because dipole-dipole interactions in iodine monochloride are stronger than dispersion forces in bromine. Lower than 59^circ C because ionic bonding in bromine is stronger than covalent bonding in iodine monochloride. Lower than 59^circ C because dipole-dipole interactions in iodine monochloride are weaker than in bromine. Higher than 59^circ C because ionic bonding in iodine monochloride is stronger than H-bonding in bromine.
The boiling point of bromine is 59^circ C Which of the following best predicts the boiling point of iodine monochloride, a polar compound? Higher than 59^circ C because dipole-dipole interactions in iodine monochloride are stronger than dispersion forces in bromine. Lower than 59^circ C because ionic bonding in bromine is stronger than covalent bonding in iodine monochloride. Lower than 59^circ C because dipole-dipole interactions in iodine monochloride are weaker than in bromine. Higher than 59^circ C because ionic bonding in iodine monochloride is stronger than H-bonding in bromine.

Solution
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Answer

Higher than 59^{\circ }C because dipole-dipole interactions in iodine monochloride are stronger than dispersion forces in bromine. Explanation 1. Identify Intermolecular Forces Bromine (Br_2) is nonpolar with dispersion forces. Iodine monochloride (ICl) is polar with dipole-dipole interactions. 2. Compare Strength of Interactions Dipole-dipole interactions in ICl are generally stronger than dispersion forces in Br_2. 3. Predict Boiling Point Stronger intermolecular forces typically result in a higher boiling point.

Explanation

1. Identify Intermolecular Forces<br /> Bromine ($Br_2$) is nonpolar with dispersion forces. Iodine monochloride (ICl) is polar with dipole-dipole interactions.<br /><br />2. Compare Strength of Interactions<br /> Dipole-dipole interactions in ICl are generally stronger than dispersion forces in $Br_2$.<br /><br />3. Predict Boiling Point<br /> Stronger intermolecular forces typically result in a higher boiling point.
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