Reactivity series of metals

The reactivity series arranges metals in order of how readily they lose electrons and react. Once you know the order, you can predict a whole set of exam answers: whether a metal reacts with water or acid, whether one metal will displace another from its salt, and how the metal is extracted from its ore. This reference gives the standard SPM order together with the behaviour that goes with each position, arranged as the DSKP expects.

Scope note

The series below is the standard KSSM reference used in SPM Chemistry. Carbon and hydrogen are shown in their usual positions as reference points, even though they are non-metals, because so many exam questions are decided by whether a metal sits above or below them. Keep the order in mind and read across each row to recall the reaction and extraction method.

The series

Order	Metal	Symbol	Reaction with water	Reaction with dilute acid	Usual extraction
1 (most reactive)	Potassium	K	Vigorous with cold water	Violent, dangerous	Electrolysis
2	Sodium	Na	Vigorous with cold water	Violent, dangerous	Electrolysis
3	Calcium	Ca	Reacts with cold water	Rapid	Electrolysis
4	Magnesium	Mg	Slow in cold water; burns in steam	Rapid	Electrolysis
5	Aluminium	Al	Reacts with steam	Moderate	Electrolysis
,	Carbon	C	,	,	(reference point)
6	Zinc	Zn	Reacts with steam	Moderate	Reduction by carbon
7	Iron	Fe	Reacts with steam (reversible)	Moderate	Reduction by carbon
8	Tin	Sn	No reaction	Slow	Reduction by carbon
9	Lead	Pb	No reaction	Very slow	Reduction by carbon
,	Hydrogen	H	,	,	(reference point)
10	Copper	Cu	No reaction	No reaction	Heating the ore
11	Silver	Ag	No reaction	No reaction	Found native / simple heating
12 (least reactive)	Gold	Au	No reaction	No reaction	Found native

How to use the series

Use the two reference lines to unlock most questions. A metal above hydrogen displaces hydrogen from a dilute acid, so it fizzes and produces hydrogen gas; a metal below hydrogen (copper, silver, gold) does not react with dilute acid. A metal below carbon can be extracted by heating its oxide with carbon, because carbon is more reactive and reduces the oxide; a metal above carbon is too reactive for this and must be extracted by electrolysis. For displacement, a more reactive metal displaces a less reactive metal from its salt solution, for example, zinc displaces copper because zinc is higher in the series.

Worked reasoning

Suppose a question asks whether magnesium reacts with copper(II) sulfate solution. Magnesium is higher than copper, so it is more reactive and displaces copper: Mg(s) + CuSO₄(aq) gives MgSO₄(aq) + Cu(s), and you would see the blue solution fade and a reddish-brown deposit of copper form. Reverse the metals and nothing happens, because copper is less reactive than magnesium and cannot push it out. Reading the series turns this from guesswork into a one-line deduction.

Common mistakes to avoid

• Placing aluminium as unreactive because of its oxide layer. Aluminium is actually reactive; the oxide coat just protects the surface.
• Saying copper reacts with dilute acid. It does not, because it sits below hydrogen.
• Getting displacement backwards. Only a higher (more reactive) metal displaces a lower one.
• Forgetting that very reactive metals need electrolysis, not carbon reduction.

How we help

Our online one-to-one teachers connect the series to the questions that use it, so you stop memorising a list and start reading it like a tool. Lessons are in English, one to one, from RM50 per hour, with a paid one-hour trial. Because reactivity underlies extraction of metals, displacement, and much of redox chemistry, a secure grasp of this one table pays off across Form 4 and Form 5 answers.