Reactivity Series
Section: 9. Metals | Syllabus: Cambridge AS Level Physics 9702
What is the Reactivity Series? Reactivity Series A list of metals arranged in order of their reactivity, from most reactive (top) to least reactive (bottom). The reactivity series is one of the most important tools in chemistry.
It allows us to: Predict which metals will react with water, acids, and oxygen Predict displacement reactions between metals and metal compounds Determine how metals should be extracted from their ores Understand corrosion and how to prevent it The Complete Reactivity Series Interactive Diagram Vertical reactivity series chart showing metals from most reactive (top) to least reactive (bottom).
Include color coding: most reactive metals (K, Na, Ca, Mg) in red/orange, medium reactive (Al, Zn, Fe) in yellow, and least reactive (Cu, Ag, Au) in green. Show arrows indicating "More reactive" at top and "Less reactive" at bottom.
Include small icons showing: Group 1 metals react explosively with water, transition metals have varying reactivity, noble metals don't corrode easily. Metal Symbol Reactivity Level Key Properties Potassium K Most reactive Reacts violently with water and air Sodium Na Very reactive Reacts vigorously with water Calcium Ca Very reactive Reacts readily with water Magnesium Mg Reactive Reacts slowly with cold water, rapidly with steam Aluminium Al Reactive Protected by oxide layer Carbon C (Non-metal reference point for extraction) Zinc Zn Moderately reactive Reacts with steam and acids Iron Fe Moderately reactive Rusts in moist air, reacts with acids Hydrogen H (Non-metal reference point for acid reactions) Copper Cu Low reactivity Does not react with water or dilute acids Silver Ag Very low reactivity Does not corrode easily Gold Au Least reactive Unreactive - does not corrode at all Memory Aid Please Send Charlie's Monkeys And Cute Zebras Into Hot Countries Signed Gordon P otassium, S odium, C alcium, M agnesium, A luminium, C arbon, Z inc, I ron, H ydrogen, C opper, S ilver, G old Reference Points in the Series 1.
Carbon (C) Carbon is included as a reference point because: Metals above carbon cannot be extracted by reduction with carbon Metals below carbon can be extracted by reduction with carbon This determines the extraction method for each metal 2.
Hydrogen (H) Hydrogen is included as a reference point because: Metals above hydrogen will react with dilute acids to produce hydrogen gas Metals below hydrogen will NOT react with dilute acids This helps predict acid-metal reactions Position Reaction with Dilute Acids Examples Above hydrogen React to produce H₂ gas Mg + H₂SO₄ → MgSO₄ + H₂ Below hydrogen No reaction Cu + HCl → No reaction Reactions with Water Metal Group Reaction with Cold Water Observation K, Na, Ca (Most reactive) React vigorously Fizzing, heat produced, metal may melt or ignite Forms metal hydroxide + hydrogen Mg Reacts very slowly with cold water Rapid reaction with steam Few bubbles in cold water White powder (MgO) forms with steam Al, Zn, Fe No reaction with cold water React with steam Metal oxide + hydrogen gas produced Cu, Ag, Au (Least reactive) No reaction No change Example Equations: Sodium + water: 2Na(s) + 2H₂O(l) → 2NaOH(aq) + H₂(g) Very vigorous reaction - sodium melts, moves around, may ignite Magnesium + steam: Mg(s) + H₂O(g) → MgO(s) + H₂(g) White magnesium oxide powder forms Reactions with Dilute Acids Metals above hydrogen in the reactivity series react with dilute acids: General equation: Metal + Acid → Salt + Hydrogen Examples: Metal Acid Equation Observation Magnesium Hydrochloric acid Mg + 2HCl → MgCl₂ + H₂ Rapid fizzing, metal dissolves Zinc Sulfuric acid Zn + H₂SO₄ → ZnSO₄ + H₂ Steady fizzing Iron Hydrochloric acid Fe + 2HCl → FeCl₂ + H₂ Slow fizzing Copper Hydrochloric acid No reaction No change (below H in series) Reactivity Trend The more reactive the metal, the faster and more vigorous the reaction with acid.
Magnesium reacts much more rapidly than iron because it is higher in the reactivity series. Displacement Reactions Displacement Reaction A reaction where a more reactive metal displaces (pushes out) a less reactive metal from its compound.
The Rule: Key Principle A more reactive metal will displace a less reactive metal from its compound (salt solution or oxide). A less reactive metal cannot displace a more reactive metal. Examples of Displacement: Zinc displaces copper from copper sulfate: Zn(s) + CuSO₄(aq) → ZnSO₄(aq) + Cu(s) ✓ Works because Zn is more reactive than Cu Observation: Blue solution fades, brown copper deposits on zinc Magnesium displaces copper from copper oxide: Mg(s) + CuO(s) → MgO(s) + Cu(s) ✓ Works because Mg is more reactive than Cu Very exothermic - sparks and bright light produced Iron with magnesium sulfate: Fe(s) + MgSO₄(aq) → No reaction ✗ Does not work because Fe is less reactive than Mg Interactive Activity Drag-and-drop displacement reaction predictor.
Students drag metal cards (Mg, Zn, Fe, Cu, Ag) onto compound cards (MgSO₄, ZnSO₄, FeSO₄, CuSO₄, AgNO₃). When dropped, the interface sh…
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