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Reactivity series and ordering metals

Chemical changes • Reactivity of metals

Key concepts

What you'll likely be quizzed about

  • Reactivity of a metal describes how readily the metal atom loses electrons to form a positive ion (cation).
  • Metal atoms lose outer electrons resulting in the formation of M+ or M2+ ions.
  • This process leads to chemical changes and energy release.
  • Limiting factors include experimental conditions such as temperature, concentration, surface area, and the presence of oxide layers, which affect the observed speed and vigor of reactions.

Flashcards

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How does a displacement reaction show relative reactivity?

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A more reactive metal displaces the ion of a less reactive metal from solution, indicating a greater tendency to form positive ions.

Key notes

Important points to keep in mind

Reactivity equals ease of forming positive ions.

More reactive metals lose electrons readily and react vigorously with water and acids.

Displacement reactions provide direct evidence: a more reactive metal displaces a less reactive metal ion.

Control temperature, concentration, and surface area when comparing reactivity.

Common order from most to least reactive: K > Na > Li > Ca > Mg > Zn > Fe > Cu.

Copper lies below hydrogen and does not react with dilute acids under standard conditions.

Hydrogen production and bubbling indicate an acid-metal or water-metal reaction.

Compare several experiments to deduce order.

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