9.4 Reactivity Series
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19. List the metals and non-metals in the reactivity series in order from most reactive to least reactive.
The full syllabus sequence is:
Potassium, Sodium, Calcium, Magnesium, Aluminium, [Carbon], Zinc, Iron, [Hydrogen], Copper, Silver, Gold.
Potassium, Sodium, Calcium, Magnesium, Aluminium, [Carbon], Zinc, Iron, [Hydrogen], Copper, Silver, Gold.
20. Describe the reaction, if any, of potassium, sodium, and calcium with cold water.
These highly reactive metals interact vigorously/explosively with cold water to produce an alkaline metal hydroxide solution and hydrogen gas.
21. Describe the reaction between magnesium and steam.
Magnesium reacts rapidly with steam to create a bright white flame, producing solid magnesium oxide (MgO) and hydrogen gas.
22. Which metals from the reactivity series react with dilute hydrochloric acid?
Magnesium, zinc, and iron dissolve with effervescence in dilute hydrochloric acid. Copper, silver, and gold lie below hydrogen and do not react.
23. How are the reactions of metals with water and acids explained?
They are dictated directly by the relative position of the elements in the reactivity series. Metals higher up displace hydrogen more easily.
24. How can an order of reactivity be determined experimentally?
By measuring and comparing reaction kinetics, such as observing the rate of gas effervescence or recording temperature changes during displacement.
25. Describe the relative reactivities of metals in terms of ion formation.
Reactivity reflects a metal's tendency to lose valence electrons to form stable positive ions (cations). More reactive metals oxidize into ions more readily.
26. How can displacement reactions be used to determine the relative reactivity of metals?
By combining a solid metal with aqueous solutions of alternative metal salts (specifically magnesium, zinc, iron, copper, and silver). A more reactive metal will displace the ions of a less reactive metal from solution.
27. Explain the apparent unreactivity of aluminium despite its high position in the reactivity series.
Aluminium reacts instantly with atmospheric oxygen to form a tough, highly adherent, non-porous oxide layer (Al2O3) that shields the underlying metal from further chemical attack.