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Edexcel A Level Chemistry

Ionic Bonding

Ionic compounds form when electrons are transferred and oppositely charged ions attract each other in a giant ionic lattice.

Exam Papers
Paper 1 & 2
9CH0/01 and 9CH0/02
Specification Points
2.1 – 2.27
9 points covered
Sub-topics
3 lessons
Revision notes available
Exam Board
Edexcel
Pearson 9CH0

Revision Notes

3 revision notes, in the order the specification teaches them.

One electron passing from a metal atom to a non-metal atom
1

Nature of Ionic Bonding

Revise electron transfer, ion formation and the electrostatic attraction between oppositely charged ions in ionic compounds.

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A small cation pulling a large anion out of shape
2

Polarisation of Ions

Learn how small highly charged cations can distort anion electron clouds, giving some ionic compounds partial covalent character.

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A crystal splitting cleanly when ion layers shift
3

Physical Properties of Ionic Compounds

Connect giant ionic lattice structure with melting temperature, solubility, brittleness and electrical conductivity.

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Summary Map

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Summary map

Download, print and revise the key facts of this topic at a glance.

Illustration of a summary map: compounds joined by reaction arrows
Summary map · PDF

Ionic Bonding Map

Edexcel A Level Chemistry · Topic 2 Bonding and Structure · Ionic Bonding

The whole section on one A4 page: forming ions, dot-and-cross diagrams, lattices and their strength, ionic radii and the evidence for ions.

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Virtual Lessons

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Topic 2A Ionic Bonding taught by a specialist chemistry teacher, in 2 recorded video lessons that follow the specification.

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MCQ Bank

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4 exam-style multiple-choice papers, MCQ (A) to (D): 77 questions on Topic 2A Ionic Bonding, written the way the exam asks them.

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Written, drawn and worked exam practice on this topic, marked by a specialist chemistry teacher.

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Written and drawn answers: 3 papers

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3 exam papers, (A) to (C): 39 questions on Topic 2A Ionic Bonding with no multiple choice. You write explanations, work out calculations and draw answers: structures, mechanisms and diagrams.

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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

  1. A.1

    know that ionic bonding is the strong electrostatic attraction between oppositely charged ions

    Revise
  2. A.2 a

    understand the effect of ionic radius on the strength of ionic bonding

    Revise
  3. A.2 b

    understand the effect of ionic charge on the strength of ionic bonding

    Revise
  4. A.3 a

    understand the formation of cations in terms of electron loss

    Revise
  5. A.3 b

    understand the formation of anions in terms of electron gain

    Revise
  6. A.4 a

    be able to draw electronic configuration diagrams of cations using dot-and-cross diagrams

    Revise
  7. A.4 b

    be able to draw electronic configuration diagrams of anions using dot-and-cross diagrams

    Revise
  8. A.5 a

    understand reasons for trends in ionic radii down a group

    Revise
  9. A.5 b

    understand reasons for trends in ionic radii for a set of isoelectronic ions such as N3- to Al3+

    Revise
  10. A.6 a

    understand that physical properties of ionic compounds provide evidence for the existence of ions

    Revise
  11. A.6 b

    understand that migration of ions provides evidence for the existence of ions

    Revise
  12. A.7

    know that a covalent bond is the strong electrostatic attraction between two nuclei and the shared pair of electrons between them

    Revise
  13. A.8i

    be able to draw dot-and-cross diagrams to show electrons in covalent substances, including: molecules with single, double and triple bonds

    Revise
  14. A.8ii

    be able to draw dot-and-cross diagrams to show electrons in covalent substances, including: species exhibiting dative covalent (coordinate) bonding, including Al2Cl6 and ammonium ion

    Revise
  15. A.9

    understand the relationship between bond lengths and covalent bond strengths

    Revise
  16. A.10 a

    understand that the shape of a simple molecule is determined by repulsion between electron pairs around a central atom

    Revise
  17. A.10 b

    understand that the shape of a simple ion is determined by repulsion between electron pairs around a central atom

    Revise
  18. A.11 a

    understand reasons for the shape of, and bond angles in, BeCl2

    Revise
  19. A.11 b

    understand reasons for the shape of, and bond angles in, BCl3

    Revise
  20. A.11 c

    understand reasons for the shape of, and bond angles in, CH4

    Revise
  21. A.11 d

    understand reasons for the shape of, and bond angles in, NH3

    Revise
  22. A.11 e

    understand reasons for the shape of, and bond angles in, NH4+

    Revise
  23. A.11 f

    understand reasons for the shape of, and bond angles in, H2O

    Revise
  24. A.11 g

    understand reasons for the shape of, and bond angles in, CO2

    Revise
  25. A.11 h

    understand reasons for the shape of, and bond angles in, PCl5(g)

    Revise
  26. A.11 i

    understand reasons for the shape of, and bond angles in, SF6(g)

    Revise
  27. A.11 j

    understand reasons for the shape of, and bond angles in, related molecules and ions

    Revise
  28. A.11 k

    understand reasons for the shape of, and bond angles in, simple organic molecules in this specification

  29. A.12 a

    be able to predict the shapes of simple molecules analogous to specified examples using electron-pair repulsion theory

    Revise
  30. A.12 b

    be able to predict the bond angles in simple molecules analogous to specified examples using electron-pair repulsion theory

    Revise
  31. A.12 c

    be able to predict the shapes of simple ions analogous to specified examples using electron-pair repulsion theory

    Revise
  32. A.12 d

    be able to predict the bond angles in simple ions analogous to specified examples using electron-pair repulsion theory

    Revise
  33. A.13

    know that electronegativity is the ability of an atom to attract the bonding electrons in a covalent bond

    Revise
  34. A.14 a

    know that ionic and covalent bonding are the extremes of a continuum of bonding type

    Revise
  35. A.14 b

    know that electronegativity differences lead to bond polarity in bonds

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  36. A.14 c

    know that electronegativity differences lead to bond polarity in molecules

    Revise
  37. A.15 a

    understand that molecules with polar bonds may not be polar molecules

    Revise
  38. A.15 b

    be able to predict whether or not a given molecule is likely to be polar

    Revise
  39. A.16i

    understand the nature of intermolecular forces resulting from the following interactions: London forces (instantaneous dipole – induced dipole)

    Revise
  40. A.16ii

    understand the nature of intermolecular forces resulting from the following interactions: permanent dipoles

    Revise
  41. A.16iii

    understand the nature of intermolecular forces resulting from the following interactions: hydrogen bonds

    Revise
  42. A.17 a

    understand interactions in H2O that give rise to hydrogen bonding

    Revise
  43. A.17 b

    understand interactions in liquid NH3 that give rise to hydrogen bonding

    Revise
  44. A.17 c

    understand interactions in liquid HF that give rise to hydrogen bonding

    Revise
  45. A.18i

    understand the following anomalous properties of water resulting from hydrogen bonding: its relatively high melting temperature and boiling temperature

    Revise
  46. A.18ii

    understand the following anomalous properties of water resulting from hydrogen bonding: the density of ice compared to that of water

    Revise
  47. A.19

    be able to predict the presence of hydrogen bonding in molecules analogous to those mentioned above

    Revise
  48. A.20i

    understand, in terms of intermolecular forces, physical properties shown by materials, including: the trends in boiling temperatures of alkanes with increasing chain length

    Revise
  49. A.20ii

    understand, in terms of intermolecular forces, physical properties shown by materials, including: the effect of branching in the carbon chain on the boiling temperatures of alkanes

    Revise
  50. A.20iii

    understand, in terms of intermolecular forces, physical properties shown by materials, including: the relatively low volatility (higher boiling temperatures) of alcohols compared to alkanes with a similar number of electrons

    Revise
  51. A.20iv

    understand, in terms of intermolecular forces, physical properties shown by materials, including: the trends in boiling temperatures of the hydrogen halides, HF to HI

    Revise
  52. A.21i

    understand factors that influence the choice of solvents, including: water, to dissolve some ionic compounds, in terms of the hydration of the ions

    Revise
  53. A.21ii

    understand factors that influence the choice of solvents, including: water, to dissolve simple alcohols, in terms of hydrogen bonding

    Revise
  54. A.21iii

    understand factors that influence the choice of solvents, including: water, as a poor solvent for compounds (to include polar molecules such as halogenoalkanes), in terms of inability to form hydrogen bonds

    Revise
  55. A.21iv

    understand factors that influence the choice of solvents, including: non-aqueous solvents, for compounds that have similar intermolecular forces to those in the solvent

    Revise
  56. A.22

    know that metallic bonding is the strong electrostatic attraction between metal ions and the delocalised electrons

    Revise