Metals are found to the left and towards the bottom of the periodic table.

The idea

Metals occupy the left-hand side and the lower portion of the periodic table. Group 1 metals such as lithium, sodium and potassium sit on the far left, Group 2 metals such as magnesium and calcium sit next to them, and the large central block contains the transition metals such as iron, copper and zinc. Moving down a group, metallic character becomes more pronounced, so elements lower in a group behave more typically as metals. This positional pattern lets you predict properties: an element on the left or low down is likely to conduct electricity, be malleable and form positive ions.

For example: Sodium in Group 1 and iron in the transition block are both clearly metallic, whereas elements towards the top right are not.

What earns the marks

• Locates metals on the left-hand side of the periodic table, including Groups 1 and 2.
• Recognises the central transition metal block as metallic.
• Notes that metallic character increases towards the bottom of a group.
• Uses position to predict metallic properties such as conduction and positive ion formation.
• Contrasts the metal region with the non-metal region at the top right.

Common mistakes and how to put them right

• Placing all metals only in Groups 1 and 2 and forgetting the large transition metal block in the centre.

• Thinking that position alone guarantees metallic behaviour at every point.

  Put it right: Hydrogen is an exception at the top left.

• Assuming metals are only found at the very bottom of the table rather than across the left and centre.

Exam tips

• Sketch a simple dividing line from the top of Group 13 down to the bottom of Group 16 to separate metals from non-metals.
• When predicting properties, state both the horizontal and vertical position, for example 'left of the table and low in the group'.
• Use named examples such as sodium, magnesium and iron to support a position-based answer.