Chapter U5.18, Problem 2E

Interpretation Introduction

Interpretation: The reason of less stability of more active metals needs to be explained.

Concept introduction: The reactivity series of metal in the order of increasing reactivity is,

Gold < Silver < Mercury < Bismuth < Antimony < Hydrogen < Lead < Tin < Nickel < Cobalt < Cadmium < Iron < Chromium < Zinc < Manganese < Aluminium < Calcium < Strontium < Barium < Lithium < Sodium < Potassium

Answer to Problem 2E

The metals that are more active also considered less stablebecause they lose electrons and they easily form a metal oxide generating an impure metal.

Explanation of Solution

The reactivity series of metal in the order of increasing reactivity is,

Gold < Silver < Mercury < Bismuth < Antimony < Hydrogen < Lead < Tin < Nickel < Cobalt < Cadmium < Iron < Chromium < Zinc < Manganese < Aluminium < Calcium < Strontium < Barium < Lithium < Sodium < Potassium

The active metals are usually less stable because they lose electrons and they easily form a metal oxide generating an impure metal. This is because, metal high in the activity series reacts in a vigorous way with compounds and gives up electrons to form positive ions easily and also easily undergoes corrosion. While, a metal low in the activity series, does not vigorously reacts with chemicals and does not easily give up electrons to form positive and undergo corrosion easily.

Conclusion

The metals that are more active also considered less than the metals that are less active.