Ionic Bonding (Oxford AQA International A Level Chemistry)
Revision Note
Written by: Philippa Platt
Reviewed by: Stewart Hird
Ionic Bonding
Ionic bonding is defined as the electrostatic attraction between oppositely charged ions in a lattice
It involves the transfer of electrons from a metallic element to a non-metallic element
Transferring electrons usually leaves the metal and the non-metal with a full outer shell
Metals lose electrons from their valence shell forming positively charged cations
Na+, K+, Mg2+, Ca2+
Non-metal atoms gain electrons forming negatively charged anions
F-, Cl-, O2-, N3-
The number of electrons lost or gained will be the same as the charge
Na loses one electron to form the Na+ ion
Once the atoms become ions, their electronic configurations are the same as a noble gas
Argon has the electronic configuration 1 s2 2s2 2p6 3s2 3p6
Table of electronic configurations of atoms and ions
atom | ion | |
---|---|---|
sodium | 1 s2 2s2 2p6 3s1 | 1 s2 2s2 2p6 |
chlorine | 1 s2 2s2 2p6 3s2 3p5 | 1 s2 2s2 2p6 3s2 3p6 |
Ionic bonding formation in NaCl
The ions form a lattice structure which is an evenly distributed crystalline structure
Ions in a lattice are arranged in a regular repeating pattern so that positive charges cancel out negative charges
The attraction between the cations and anions is occurring in all directions
Each ion is attracted to all of the oppositely charged ions around it
Therefore the final lattice is overall electrically neutral
Ionic crystal
Formulas of Ionic Compounds
The charge for an ion can be determined by the group number:
Table showing the relationship between group number and charge
Group | Ion | Example |
---|---|---|
1 | 1+ | K+ |
2 | 2+ | Sr2+ |
3 | 3+ | Al3- |
5 | 3- | N3- |
6 | 2- | S2- |
7 | 1- | I- |
You need to know the formulas for ions that compound
Names and formulas of compound ions
Name | Overall charge | Formula |
---|---|---|
sulfate | 2- | SO42- |
hydroxide | 1- | OH- |
nitrate | 1- | NO3- |
carbonate | 2- | CO32- |
ammonium | 1+ | NH4+ |
Worked Example
Write the formula for the following ionic compounds:
Sodium carbonate
Copper(II) nitrate
Ammonium sulfate
Magnesium hydroxide
Answers:
Sodium carbonate
Sodium is a 1+ ion, Na+ and carbonate is a 2- ion, CO32- two sodium ions are required to form the electronically neutral ionic compound
Na2CO3
Copper(II) nitrate
Copper is a 2+ ion, Cu2+, and nitrate is a 1- ion, NO3-two nitrate ions are required to form the electronically neutral ionic compound
Cu(NO3)2
Ammonium sulfate
Ammonium is a 1+ ion, NH4+ and sulfate is a 2- ion, SO42- two ammonium ions are required to form the electronically neutral ionic compound
(NH4)2SO4
Magnesium hydroxide
Magnesium is a 2+ ion, Mg2+, and hydroxide is a 1- ion, OH- two hydroxide ions are required to form the electronically neutral ionic compound
Mg(OH)2
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