Topic 1 of 6 · Form 5
Atomic structure, bonding and states of matter
Subatomic particles; isotopes; electronic configuration with s, p, d orbitals (Cr and Cu exceptions); ionisation energies and their trends; evidence for shells from successive ionisation energies.
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Atomic structure
Subatomic particles; isotopes; electronic configuration with s, p, d orbitals (Cr and Cu exceptions); ionisation energies and their trends; evidence for shells from successive ionisation energies.
Bonding
Ionic, covalent (σ and π bonds; hybridisation sp, sp², sp³), dative, metallic; electronegativity and bond polarity; VSEPR shapes (linear, trigonal planar, tetrahedral, trigonal pyramidal, bent, trigonal bipyramidal, octahedral); intermolecular forces (London dispersion, permanent dipole, hydrogen bonding).
States of matter
Ideal gas equation pV = nRT and deviations from ideality (high pressure, low temperature); lattice structures (giant ionic, giant covalent, giant metallic, simple molecular).
Worked example: Find the molar mass of a gas if 0.50 g occupies 400 cm³ at 300 K and 101 kPa.
n = pV/RT = (101 000 × 4.0 × 10⁻⁴)/(8.31 × 300) = 0.0162 mol → M = 0.50 ÷ 0.0162 = 30.9 g mol⁻¹
Check yourself
- State the shape and bond angle of SF₆.
- Why does the first ionisation energy fall from Mg to Al?
- Under which conditions do real gases deviate most from ideal behaviour?
Show answers
- Octahedral, 90°.
- Al's outer electron is in a 3p orbital, higher in energy and more shielded than the 3s electron of Mg.
- High pressure and low temperature.
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