Question 1. Which of the following best explains the relative boiling points for Cl2 and HCl? Cl2 has the higher boiling point because liquid Cl2 has stronger London-dispersion forces than liquid HCl. Cl2 has the higher boiling point because liquid Cl2 has stronger dipole-dipole forces than liquid HCl. HCl has the higher boiling point because liquid HCl has hydrogen-bonding interactions while liquid Cl2 has no hydrogen bonding interactions. HCl has the higher boiling point because liquid HCl has dipole-dipole forces while liquid Cl2 does not have dipole-dipole forces.
Question
1. Which of the following best explains the relative boiling points
for Cl2 and HCl?
Cl2 has the higher boiling point because liquid Cl2 has stronger London-dispersion forces than liquid HCl.
Cl2 has the higher boiling point because liquid Cl2 has stronger dipole-dipole forces than liquid HCl.
HCl has the higher boiling point because liquid HCl has hydrogen-bonding interactions while liquid Cl2
has no hydrogen bonding interactions.
HCl has the higher boiling point because liquid HCl has dipole-dipole forces while liquid Cl2 does not have dipole-dipole forces.
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