It is used to predict whether a metal can displace another metal in a single displacement reaction (a reaction in which one element is displaced by another element in a compound).It allows us to ascertain how the metal will react.The reactivity series is useful in several ways: H + (Non-Metal, Reference for Comparison) The metals situated above hydrogen are more reactive than hydrogen and have the potential to displace hydrogen from water or acids to liberate H 2 gas.To isolate the metals from their ores and other compounds, a large amount of energy is consumed for metals at the top of the series.In addition to electro positivity, the electron-donating ability of the metal also reduces while travelling down the series.Hence, sodium is more electropositive than lithium but less electropositive than potassium. The electropositive nature of metals decreases as we move down the series.For example: Zinc can displace copper from the copper sulfate solution as it is placed above copper and therefore, is more reactive. A metal situated above in the reactivity series (more reactive) can displace the metal placed below it (less reactive) from its compound.Hence, the upper part of the series contains powerful reducing agents as they are easily oxidized, and corrode easily. The reducing power of the metals decreases as we move from the top of the table to its bottom.
REACTIVITY SERIES OF METALS FREE
The head of the reactivity series comprises the most reactive elements, which are not available in nature in the free state and the foot of the series includes the least reactive elements.The reactivity of Metals chart gives a detailed understanding of the reactivity of different metals with different elements.
Salient Features of the Reactivity Series
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