Ionic Bonding (Oxford AQA International A Level Chemistry)

Revision Note

Philippa Platt

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

A diagram to show the formation of an ionic bond in NaCl
When sodium and chlorine react, an electron is transferred from the Na atom to the Cl atom to form two oppositely charged ions which bond together
  • 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

Chemical Bonding Ionic Lattice, downloadable AS & A Level Chemistry revision notes
A typical ionic crystal structure

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:

  1. Sodium carbonate

  2. Copper(II) nitrate

  3. Ammonium sulfate

  4. 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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Philippa Platt

Author: Philippa Platt

Expertise: Chemistry

Philippa has worked as a GCSE and A level chemistry teacher and tutor for over thirteen years. She studied chemistry and sport science at Loughborough University graduating in 2007 having also completed her PGCE in science. Throughout her time as a teacher she was incharge of a boarding house for five years and coached many teams in a variety of sports. When not producing resources with the chemistry team, Philippa enjoys being active outside with her young family and is a very keen gardener

Stewart Hird

Author: Stewart Hird

Expertise: Chemistry Lead

Stewart has been an enthusiastic GCSE, IGCSE, A Level and IB teacher for more than 30 years in the UK as well as overseas, and has also been an examiner for IB and A Level. As a long-standing Head of Science, Stewart brings a wealth of experience to creating Topic Questions and revision materials for Save My Exams. Stewart specialises in Chemistry, but has also taught Physics and Environmental Systems and Societies.