Ever wonder why water boils at 100°C whilst other similar...
Chemistry198 views·Updated 21 Jun 2026·3 pagesUnderstanding Intermolecular Forces for AQA Chemistry
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Understanding Intermolecular Forces
Think of intermolecular forces as the "glue" that holds molecules together, though they're much weaker than the bonds within molecules themselves. These forces might be weak, but they're absolutely crucial for determining how substances behave in the real world.
There are three main types you need to know: Van der Waals forces (the weakest), permanent dipole-dipole interactions (medium strength), and hydrogen bonding (the strongest). Each one works differently and affects substances in unique ways.
Van der Waals forces are the most basic type - they exist between all molecules and even noble gas atoms. As molecules get larger, these forces become stronger because there's more surface area for attraction. This explains why helium boils at -269°C whilst xenon boils at -108°C.
Quick Check: Remember that molecular size directly affects Van der Waals forces - bigger molecules = stronger forces = higher boiling points!
2
of 3
Dipole Interactions and Hydrogen Bonding
Permanent dipole-dipole interactions occur when molecules have uneven charge distribution due to differences in electronegativity. Picture HCl molecules lining up so the slightly positive hydrogen end attracts the slightly negative chlorine end of neighbouring molecules.
Hydrogen bonding takes this concept further and creates the strongest intermolecular force. It only happens when hydrogen is bonded to fluorine, oxygen, or nitrogen - the three most electronegative elements. The hydrogen's positive charge attracts lone pairs of electrons on these atoms.
Water perfectly demonstrates hydrogen bonding in action. These special bonds give water its unique properties: ice is less dense than liquid water (creating the lattice structure that makes ice float), water has an unusually high boiling point, and it shows remarkable surface tension.
Real-World Connection: Without hydrogen bonding, water would boil at around -80°C, making life on Earth impossible!
3
of 3
Patterns in Hydrides and Key Rules
Looking at hydrides (compounds of hydrogen with other elements) reveals fascinating patterns. In Groups 5, 6, and 7, the first member always has a much higher boiling point than expected - NH₃, H₂O, and HF all break the trend because of hydrogen bonding.
For other hydrides moving down each group, two competing factors battle it out. Polarity decreases (weakening dipole forces) whilst molecular size increases (strengthening Van der Waals forces). The size effect usually wins, explaining why H₂Te boils higher than H₂S.
Here are the essential rules you need to remember: all molecules have Van der Waals forces as a baseline, polar molecules add dipole-dipole forces on top, and hydrogen bonding only occurs with F, O, or N. These forces directly determine physical properties like boiling points, melting points, and solubility.
Exam Tip: When predicting boiling points, first check for hydrogen bonding, then consider molecular size and polarity - this approach works every time!
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Chemistry198 views·Updated 21 Jun 2026·3 pagesUnderstanding Intermolecular Forces for AQA Chemistry
hammerbro@hammerbro
Ever wonder why water boils at 100°C whilst other similar molecules boil at much lower temperatures? It's all down to intermolecular forces - the invisible attractions between molecules that determine how substances behave. Understanding these forces will help you predict...
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of 3
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Understanding Intermolecular Forces
Think of intermolecular forces as the "glue" that holds molecules together, though they're much weaker than the bonds within molecules themselves. These forces might be weak, but they're absolutely crucial for determining how substances behave in the real world.
There are three main types you need to know: Van der Waals forces (the weakest), permanent dipole-dipole interactions (medium strength), and hydrogen bonding (the strongest). Each one works differently and affects substances in unique ways.
Van der Waals forces are the most basic type - they exist between all molecules and even noble gas atoms. As molecules get larger, these forces become stronger because there's more surface area for attraction. This explains why helium boils at -269°C whilst xenon boils at -108°C.
Quick Check: Remember that molecular size directly affects Van der Waals forces - bigger molecules = stronger forces = higher boiling points!
2
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Dipole Interactions and Hydrogen Bonding
Permanent dipole-dipole interactions occur when molecules have uneven charge distribution due to differences in electronegativity. Picture HCl molecules lining up so the slightly positive hydrogen end attracts the slightly negative chlorine end of neighbouring molecules.
Hydrogen bonding takes this concept further and creates the strongest intermolecular force. It only happens when hydrogen is bonded to fluorine, oxygen, or nitrogen - the three most electronegative elements. The hydrogen's positive charge attracts lone pairs of electrons on these atoms.
Water perfectly demonstrates hydrogen bonding in action. These special bonds give water its unique properties: ice is less dense than liquid water (creating the lattice structure that makes ice float), water has an unusually high boiling point, and it shows remarkable surface tension.
Real-World Connection: Without hydrogen bonding, water would boil at around -80°C, making life on Earth impossible!
3
of 3Sign up to see the content. It's free!
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Patterns in Hydrides and Key Rules
Looking at hydrides (compounds of hydrogen with other elements) reveals fascinating patterns. In Groups 5, 6, and 7, the first member always has a much higher boiling point than expected - NH₃, H₂O, and HF all break the trend because of hydrogen bonding.
For other hydrides moving down each group, two competing factors battle it out. Polarity decreases (weakening dipole forces) whilst molecular size increases (strengthening Van der Waals forces). The size effect usually wins, explaining why H₂Te boils higher than H₂S.
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