Edexcel IGCSE Chemistry Ionic Bonding

This page contains the detailed and easy notes for Edexcel  IGCSE Chemistry Ionic Bonding for revision and understanding.

IONIC BONDING: Metals and Non Metals

  • It is between a metal and a non metal
  • Metal loses an electron and become positively charged.
  • Non- Metal gains an electron and becomes negatively charged.
  • There is a strong electrostatic force of attraction between opposite charged ions resulting in ionic bonding.

Dot and Cross Diagram

  • Write the symbols
  • Write electronic configuration
  • show outer electrons
  • show transfer
  • show charges

Example –  Aluminium Fluoride

Al = 2,8,3

F = 2,7

Example – Magnesium chloride

Mg = 2,8,2

Cl = 2,8,7

Ionic Bonding

Edexcel IGCSE Chemistry Ionic Bonding

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PROPERTIES OF IONIC COMPOUNDS

Ionic Compound Properties

  • Brittle solids with definite crystal shapes

In Ionic compounds, there is a strong electrostatic force of attraction between the opposite charged ions. This results in the formation of giant ionic lattice.

  • Good insulators in solid form, but become good conductors in liquid or dissolved form.

In the solid form, the ions are not free to move as they are held together by strong electrostatic force of attraction. In molten or when they are dissolved in water the ions are free to move and conduct electricity.

  • High melting and boiling point compared to molecular compounds


In Ionic compounds, there is a strong electrostatic force of attraction between the opposite charged ions. This results in the formation of giant ionic lattice. Large amount of energy is required to overcome the strong electrostatic force of attraction. Therefore, ionic compounds have high melting and boiling point.

Greater the charge of an ionic lattice, stronger is the electrostatic force of attraction. Greater the melting and bp.

For éx – Aluminium chloride > Magnesium chloride > sodium chloride

FORMULAE OF IONIC COMPOUNDS

  • Write the Symbols
  • Write the charges
  • (Upto group the charge is same as the group number. After group 4 it is group number -8)
  • Criss Cross
  1. a) Sodium Oxide = Na2O
  2. b) Magnesium Nitride = Mg3N2
  3. c) Calcium Oxide = CaO
  4. d) Sodium Sulphide = N2S
  5. e) Sodium Chloride = NaCl
  6. f) Magnesium chloride = MgCl2
  7. g) Aluminium Chloride = ACl3

FORMULAE OF COMPLEX IONS

a) Magnesium HydroxideAl2(SO4)3
b) Aluminium SulphateAl2(SO4)3
c) Calcium PhosphateCa3(PO4)2
d) Magnesium nitrateMg(NO3)2
e) Calcium CarbonateCaCO3
f) Sodium PhosphateNa3PO4

Positive 

 

 

Negative

 

Ammonium = NH4+


 

Carbonate = CO32-
 Sulphate = SO42-
 Nitrate = NO3–
 Phosphate = PO43-
 Hydroxide = OH–




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