Intermolecular Forces
Intermolecular forces are the attractions between molecules, and OCR examines them in 2.2.2 and then reuses them for the halogens in 3.1.3, the alkanes in 4.1.2 and the alcohols in 4.2.1.
The section also covers ionic and metallic bonding, simple molecular and giant lattices, and intermolecular forces with hydrogen bonding and the anomalous properties of water.
Revision Notes
6 revision notes, in the order the specification teaches them.
London Forces
Revise how moving electrons create instantaneous and induced dipoles, and why electrons and shape decide their strength.
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Permanent Dipole-Dipole Forces
Revise which molecules have a permanent dipole, how they attract, and how to decide the forces in an unfamiliar molecule.
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Hydrogen Bonding
Revise the N-H, O-H and H-F requirement, the exam diagram, and predicting hydrogen bonding in other molecules.
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Anomalous Properties of Water
Revise why water has such a high boiling point, why ice floats and why water has a high surface tension.
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Boiling Point Trends
Revise boiling point trends for alkanes, branched isomers, alcohols and the hydrogen halides.
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Choosing Solvents
Revise hydration of ions, alcohols in water, why some polar molecules do not dissolve, and non-aqueous solvents.
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Download, print and revise the key facts of this topic at a glance.
Intermolecular Forces Map
OCR A Level Chemistry A · 2.2.2 Intermolecular forces
The whole section on one A4 page: bonds or forces, London forces, permanent dipoles, hydrogen bonds, H₂O, NH₃ and HF, and why water is odd.
Boiling Points and Solvents Map
OCR A Level Chemistry A · 2.2.2 Boiling points and solvents
The whole section on one A4 page: chain length, branching, alcohols against alkanes, the hydrogen halides, water as a solvent and other solvents.
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Specification
Every specification point in this topic, in the exam board's own words. Rate how confident you are with each one.
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2.2.2
- j (i) b
explanation of a permanent dipole within molecules containing covalently-bonded atoms with different electronegativities
Revise - l
hydrogen bonding as intermolecular bonding between molecules containing N, O or F and the H atom of –NH, –OH or HF
Revise - m (i)
explanation of the anomalous property of H2O resulting from hydrogen bonding: the density of ice compared with water
Revise - m (ii)
explanation of the anomalous property of H2O resulting from hydrogen bonding: its relatively high melting and boiling points
Revise - o i
explanation of the effect of structure and bonding on the melting and boiling points of covalent compounds with simple molecular lattice structures
Revise - o ii
explanation of the effect of structure and bonding on the solubility of covalent compounds with simple molecular lattice structures
Revise
3.1.3
- a ii
explanation of the trend in the boiling points of Cl2, Br2 and I2, in terms of induced dipole–dipole interactions (London forces) (see also 2.2.2 k)
Revise
4.1.2
- c i
explanation of the variations in boiling points of alkanes with different carbon-chain length, in terms of induced dipole–dipole interactions (London forces) (see also 2.2.2 k)
Revise - c ii
explanation of the variations in boiling points of alkanes with different branching, in terms of induced dipole–dipole interactions (London forces) (see also 2.2.2 k)
Revise
4.2.1
- a (i) c
an explanation, in terms of hydrogen bonding, of the relatively low volatility of alcohols compared with alkanes (see also 2.2.2 l and 4.1.2 c)
Revise
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