Ionic Bonds: Dot & Cross Diagrams (Edexcel IGCSE Chemistry (Modular))
Revision Note
Dot and cross diagrams for ionic compounds
Ionic bonds can be represented diagrammatically using dot-and-cross diagrams
The electrons from each atom should be represented by using solid dots and crosses
If there are more than two atoms, then hollow circles or other symbols / colours may be used to make it clear
The large square brackets should encompass each atom and the charge should be in superscript and on the right-hand side, outside the brackets
Sodium chloride dot and cross diagram
Sodium is a Group 1 metal so will lose one outer electron to another atom to gain a full outer shell of electrons
A positive sodium ion with the charge 1+ is formed
Chlorine is a Group 7 non-metal so will need to gain an electron to have a full outer shell of electrons
One electron will be transferred from the outer shell of the sodium atom to the outer shell of the chlorine atom
A chlorine atom will gain an electron to form a negatively charged chloride ion with a charge of 1-
The formula of sodium chloride is NaCl
Dot and cross diagram for sodium chloride
Sodium loses one electron, and chlorine gains one electron.
Magnesium oxide dot and cross diagram
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
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 formula of magnesium oxide is MgO
Dot and cross diagram for magnesium oxide
Magnesium loses two electrons and oxygen gains two electrons.
Examiner Tip
For exam purposes you need only show the outer electrons in dot & cross diagrams.
You should be able to draw dot & cross diagrams for combinations of ions from groups 1,2,3,5,6 and 7.
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