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Reactivity Series of Metals

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Reactivity Series of Metals

The reactivity series is a list of metals arranged in order of their reactivity from highest to lowest. It is also known as the activity series. Metals at the top are highly reactive, while those at the bottom are least reactive.

Factors Affecting Reactivity:

a. Electron Configuration: Metals lose electrons to form positively charged ions.

b. Atomic Size: Metals with larger atomic size have loosely held outer electrons, making them more reactive.

c. Position in the Series

  • Highly reactive metals (K, Na, Ca, Mg, Al) react with water and acids.
  • Moderately reactive metals (Zn, Fe, Pb, Cu) react with acids but not with water.
  • Less reactive metals (Ag, Au, Pt) do not react under normal conditions.

Reactivity series of metals

Salient Features of the Reactivity Series:

1. Electropositivity Decreases Down the Series

  • Metals at the top are more electropositive.
  • Potassium is the strongest reducing agent.

2. Reaction with Acids: Metals above hydrogen in the series can displace hydrogen from acids.

3. Displacement Reactions: A more reactive metal displaces a less reactive metal from its salt solution.

Example: Fe + CuSO₄ → FeSO₄ + Cu

4. Metal Extraction

  • Highly reactive metals are extracted by electrolysis.
  • Moderately reactive metals (Zn to Hg) are extracted by reducing their oxides.

5. Electron Donation Capacity Decreases Down the Series: Metals at the top donate electrons more readily than those at the bottom.

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Related QuestionsVIEW ALL [48]

Metal ‘A’ has electronic configuration 2, 8, 1 and metal ‘B’ has electronic configuration 2, 8, 8, 2. Out of these, which metal is more reactive? Write the reaction of this metal with dilute HCl acid.

Complete the statement by filling in the blank with the correct word:

The metal which reacts with steam and the reaction is reversible is ________.

Classify the following metals based on their reactivity.
Cu, Zn, Ca, Mg, Fe, Na, Li, Hg

More reactive Moderately reactive Less reactive
     
     

Of the three metals X, Y and Z. X reacts with cold water, Y with hot water and Z with steam only. Identify X, Y and Z and also arrange them in order of increasing reactivity.

Write a chemical equation for the following event.

Zinc oxide is dissolved in dilute hydrochloric acid.

In preparation of Aqua regia hydrochloric acid and _______ acid are mixed.

Write chemical equation for the event.
Aluminium came in contact with air.

Three metal samples of magnesium, aluminium and iron were taken and rubbed with sandpaper. These samples were then put separately in test tubes containing dilute hydrochloric acid. Thermometers were also suspended in each test tube so that their bulbs dipped in the acid. The rate of formation of bubbles was observed. The above activity was repeated with dilute nitric acid and the observations were recorded.

Answer the following questions:

(i) When the activity was done with dilute hydrochloric acid, then in which one of the test tubes was the rate of formation of bubbles the fastest and the thermometer showed the highest temperature?

(ii) Which metal did not react with dilute hydrochloric acid? Give reason.

(iii) Why is hydrogen gas not evolved when a metal reacts with dilute nitric acid? Name the ultimate products formed in the reaction.

OR

Name the type of reaction on the basis of which the reactivity of metals is decided. You have two metals X and Y. How would you decide which is more reactive than the other?

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