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Bonding and structure: Atoms, molecules and lattices

Key ideas • General

Key concepts

What you'll likely be quizzed about

  • Ionic bonding occurs when one atom transfers electrons to another, generating positively charged cations and negatively charged anions.
  • The attraction between oppositely charged ions creates a regular arrangement known as a giant ionic lattice.
  • This structure possesses high melting and boiling points due to the strong electrostatic forces between ions, and ionic compounds are hard and brittle.
  • Ions are mobile when molten or dissolved, allowing electrical conductivity, which is absent in the solid state.

Flashcards

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Electrical conductivity of ionic solids

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Ionic solids do not conduct electricity because ions are fixed in place; conductivity occurs when molten or dissolved as ions can move.

Key notes

Important points to keep in mind

Ionic bonding results from electron transfer producing charged ions that attract in a lattice.

Covalent bonding involves shared electrons, with molecular size affecting melting points.

Metallic bonding's delocalised electrons provide conductivity and malleability.

Electron pair repulsion dictates molecular geometry and bond angles.

Lone pairs exert greater repulsion than bonding pairs, reducing bond angles.

Giant structures create bulk properties; simple molecules create molecular properties.

Conductivity requires mobile charged particles like ions or delocalised electrons.

Solubility depends on the balance between lattice attractions and solvent interactions.

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