Summary Intermolecular Forces, Electronegativity & Bond Properties
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Course
Chemistry
Institution
Junior / 11th Grade
The text discusses intermolecular forces, particularly focusing on hydrogen bonding, bond polarity, and Van der Waals’ forces within the context of CIE AS Chemistry. It explains hydrogen bonding as the strongest form of intermolecular bonding, requiring a highly electronegative atom like oxygen o...
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CIE AS Chemistry Your notes
3.6 Intermolecular Forces, Electronegativity & Bond
Properties
Contents
Hydrogen Bonding
Bond Polarity & Dipole Moments
Van der Waals' Forces
Inter & Intramolecular Forces
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Hydrogen Bonding
Your notes
Hydrogen Bonding
Hydrogen bonding
Hydrogen bonding is the strongest form of intermolecular bonding
Intermolecular bonds are bonds between molecules
Hydrogen bonding is a type of permanent dipole – permanent dipole bonding
For hydrogen bonding to take place the following is needed:
A species which has an O or N (very electronegative) atom with an available lone pair of electrons
A species with an -OH or -NH group
When hydrogen is covalently bonded to an electronegative atom, such as O or N, the bond becomes
very highly polarised
The H becomes so δ+ charged that it can form a bond with the lone pair of an O or N atom in another
molecule
Polarity of the OH bond
The electronegative atoms O or N have a stronger pull on the electrons in the covalent bond with
hydrogen, causing the bond to become polarised
For hydrogen bonding to take place, the angle between the -OH/-NH and the hydrogen bond is 180o
The number of hydrogen bonds depends on:
The number of hydrogen atoms attached to O or N in the molecule
The number of lone pairs on the O or N
Hydrogen bonding in ammonia
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Your notes
Ammonia can form a maximum of one hydrogen bond per molecule
Hydrogen bonding in water
Water can form a maximum of two hydrogen bonds per molecule. Two hydrogen bonds on the δ-
oxygen atom and one on each δ+ hydrogen atom
Properties of water
Hydrogen bonding in water, causes it to have anomalous properties such as high melting and boiling
points, high surface tension and anomalous density of ice compared to water
High melting & boiling points
Water has high melting and boiling points which is caused by the strong intermolecular forces of
hydrogen bonding between the molecules
In ice (solid H2O) and water (liquid H2O) the molecules are tightly held together by hydrogen bonds
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