Advertisements
Advertisements
Question
Use the information and data given below:
• Strength of London forces increases with the number of electrons in the molecule.
Looking at the trend of boiling points of \[\ce{HCl, HBr and HI}\], explain out of dipole-dipole interaction and London interaction, which one is predominant here.
Advertisements
Solution
The electronegativity decreases from \[\ce{Cl, Br}\] and I so the dipole-dipole interaction will also decrease as \[\ce{HCl > HBr > HI}\] and it is contrary to the boiling point order which is \[\ce{HCl < HBr < HI}\]. This confirms that the London interaction is predominant.
APPEARS IN
RELATED QUESTIONS
The interaction energy of London force is inversely proportional to sixth power of the distance between two interacting particles but their magnitude depends upon
Use the information and data given below:
• Stronger intermolecular forces result in higher boiling point.
Which type of intermolecular forces are present in the molecules \[\ce{HF, HCl, HBr and HI}\]?
______ interaction is predominant between a polar molecule having permanent dipole moment and non-polar molecule with zero dipole moment.
The interaction energy of London forces between two particles is proportional to rx, where r is the distance between the particles. The value of x is ______.
The predominant intermolecular forces present in ethyl acetate, a liquid, are ______.
