4 x 1 hour lessons

This module links particle models to measurable properties of gases and solids. First, you’ll develop fluency with the ideal gas equation and see how molecular collisions give rise to gas pressure and why real gases deviate from ideal behaviour. Then we switch to solids, comparing giant ionic, simple molecular, giant molecular, and giant metallic lattices, and explaining how bonding and structure control melting point, electrical conductivity and solubility. You’ll finish by deducing structure type from experimental information.

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By the end of this module you will be able to:

• explain gas pressure in terms of molecule–wall collisions

• state the assumptions for an ideal gas (zero particle volume, no intermolecular attractions) and apply pV=nRT in calculations, including determining Mr

• describe lattice structures of crystalline solids: giant ionic (e.g. NaCl, MgO), simple molecular (iodine, C₆₀, ice), giant molecular (SiO₂, graphite, diamond) and giant metallic (copper)

• explain trends in melting/boiling point, conductivity, and solubility from bonding and structure

• deduce the bonding/structure type of an unknown from given data

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CIE Syllabus Points (9701):

• 4.1 The gaseous state: ideal and real gases and pV=nRT

• 4.2 Bonding and structure