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CAIE IGCSE Chemistry Ionic Properties from Structure and Bonding

Practise explaining ionic melting points and conductivity from electrostatic attraction in a lattice and the mobility of ions in different states.

Syllabus
2026–2028
Course
Chemistry 0620

Exam points

  • link high melting and boiling points to strong attractions between oppositely charged ions
  • state that solid ionic compounds do not conduct because lattice ions cannot move
  • explain molten or aqueous conduction through mobile positive and negative charge carriers

2.4.7—Ionic compound properties from question 1

[Maximum number: 3]

Fluorine is a Group VII element. Fluorine forms compounds with metals and non-metals.

Tetrafluoromethane and lead(II) fluoride are fluorides of Group IV elements. Some properties of tetrafluoromethane and lead(II) fluoride are shown in the table.

Table for Question 2.4.7—Ionic compound properties from question 1 — CAIE IGCSE Chemistry

Explain, in terms of attractive forces between particles, why lead(II) fluoride has a much higher melting point than tetrafluoromethane.

In your answer refer to the types of attractive forces between particles and their relative strengths.

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