Ionic Bonding (AQA GCSE Chemistry: Combined Science)

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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
  • This loss or gain of electrons takes place to obtain a full outer shell of electrons
  • The electronic structure of ions of elements in Groups 1, 2, 6 and 7 will be the same as that of a noble gas - such as helium, neon, and argon
  • Negative ions are called anions and form when atoms gain electrons, meaning they have more electrons than protons
  • Positive ions are called cations and form when atoms lose electrons, meaning they have more protons than electrons
  • All metals lose electrons to other atoms to become positively charged ions
  • All non-metals gain electrons from other atoms to become negatively charged ions

Diagram to show the formation of a sodium ion

sodium-atom-and-ion

Diagram showing the formation of the sodium ion

Diagram to show the formation of a chloride ion

Formation-of-negatively-charged-Chloride-ion

Diagram showing the formation of the chloride ion

  • The positive and negative charges are held together by the strong electrostatic forces of attraction between oppositely charged ions
    • This is what holds ionic compounds together

Dot & Cross Diagrams

  • These show the arrangement of the electrons in an ionic compound
  • The electrons are shown as dots and crosses
  • The charge of the ion is spread evenly which is shown by using brackets
  • The charge on each ion is written at the top right-hand corner

Dot and cross diagram of sodium chloride

diagram to show how oppositely-charged-ions-attraction-due-to-electrostatic-attraction-igcse-and-gcse-chemistry-revision-notes

Dot and cross diagram of sodium chloride

Examiner Tip

The number of electrons that an atom gains or loses is the same as the charge.

For example, if a magnesium atom loses 2 electrons, then the charge will be +2, if a bromine atom gains 1 electron then the charge will be -1.

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Representing ionic bonding

  • Ionic bonds can be represented diagrammatically using dot and cross diagrams
  • These are a simple and quick way to show the formation of an ionic compound
  • If there are more than two atoms, then hollow circles or other symbols / colours may be used to make it clear
  • The electrons from each atom should be represented by using solid dots and crosses
  • The large square brackets should encompass each atom and the charge should be in superscript and on the right-hand side, outside the brackets
  • For larger atoms with more electron shells, only the valence shell needs to be drawn

Forming the ionic bond in sodium chloride

Ionic bonding – Sodium Chloride

Diagram representing how the ionic bond in sodium chloride is formed

Example: Sodium Chloride

  • Sodium is a Group 1 metal so loses one outer electron to another atom to gain a full outer shell of electrons
  • A positive sodium ion with the charge 1+ is formed, Na+ 
  • Chlorine is a Group 7 non-metal so gains one electron to have a full outer shell of electrons
  • A negative chloride ion with a charge of 1- is formed, Cl
  • The ions are then attracted to one another and held together by electrostatic forces
  • The formula of the ionic compound is thus NaCl

Oppositely charged ions attraction due to electrostatic attraction, IGCSE & GCSE Chemistry revision notes

Dot-and-cross diagram of sodium chloride

Example: Magnesium oxide

  • Magnesium is a Group 2 metal so will lose two outer electrons to another atom to have a full outer shell of electrons
  • A positive ion with the charge 2+ is formed, Mg2+ 
  • Oxygen is a Group 6 non-metal so will need to gain two electrons to have a full outer shell of electrons
  • Two electrons will be transferred from the outer shell of the magnesium atom to the outer shell of the oxygen atom
  • Oxygen atom will gain two electrons to form a negative ion with charge 2-
  • The ions are then attracted to one another and held together by electrostatic forces
  • The formula of the ionic compound is thus MgO

Ionic bonding in magnesium oxide

Magnesium Oxide dot & cross diagram

Dot-and-cross diagram of magnesium oxide

Formula of ionic compounds

  • You may be asked to give the formula of an ionic compound from a given diagram
  • If it is a dot-and-cross diagram, then just count the number of atoms of each element
  • This is then equal to the empirical formula of the compound
  • If it is a 3D lattice structure, then look for how many ions are in the lattice
  • Write them down and balance the charges to find the formula for the compound

Examiner Tip

When describing ionic bonding:

  • State how many electrons the metal loses
  • State the resulting charge of the metal ion
  • State how many electrons the non-metal gains
  • State the resulting charge of the non-metal ion
  • State that the oppositely charged ions are held together by strong forces of attraction in ionic bonding
  • Careful: Sometimes you might need more than one metal ion, e.g. Na2O, or non-metal ion, e.g. MgCl2, so be sure to say how many of each ion are needed in these cases

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Stewart

Author: Stewart

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 Exam Questions and revision materials for Save My Exams. Stewart specialises in Chemistry, but has also taught Physics and Environmental Systems and Societies.