1. Ionic Bonding
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What is an ion?
An ion is an electrically charged atom or group of atoms formed by the loss or gain of electrons to obtain a full outer shell.
Ions Summary
• Anions = Negative ions (gain electrons, more electrons than protons) • Cations = Positive ions (lose electrons, more protons than electrons) • Metals → lose electrons → form cations • Non-metals → gain electrons → form anions
Group 1 metals
1+ (e.g. Na⁺)
Group 2 metals
2+ (e.g. Mg²⁺)
Group 3 metals
3+ (e.g. Al³⁺)
Silver
Ag⁺
Copper(II)
Cu²⁺
Iron(II)
Fe²⁺
Iron(III)
Fe³⁺
Lead(II)
Pb²⁺
Zinc(II)
Zn²⁺
Hydrogen
H⁺
Ammonium
NH₄⁺
Group 5 non- metals
3- (E.g. N3-)
Group 6 non- metals
2- (E.g. O2-)
Group 7 non- metals
1- (E.g. Cl-)
Hydroxide
OH⁻
Carbonate
CO₃²⁻
Nitrate
NO₃⁻
Sulfate
SO₄²⁻
What method is used when writing the Formulae for Ionic Compounds.
Swap and Drop Method
What is an ionic bond?
The strong electrostatic forces of attraction between the positive and negative ions in an ionic lattice.
Why do ionic compounds have high melting and boiling points?
• They have giant ionic lattices • There are strong electrostatic forces of attraction between oppositely charged ions in all directions • The forces need lots of energy to overcome them
Do greater charged ions have stronger electrostatic forces of attraction?
The greater the charge on the ions, the stronger the electrostatic forces and the higher the melting point will be.