| Reactivity series of metals | | We have seen that some metals are more reactive than others are. From the study of periodic table of elements, we know seen that the reactivity of elements decreases as we go from the left to right in one periodic. |  | | In the alkali group (IA), as we go down the group we have elements Lithium (Li), Sodium (Na), Potassium (K), Rubidium (Rb), Cesium (Cs) and Francium (Fr). They have all only one electron in their outermost shells. All the elements show metallic properties and have valence +1. They give up electron easily. Reactivity or the ease with which these elements give off their electrons increases with the size of the atoms. The size of the atom increases from Li to Fr. The outermost electron is less loosely bound in Fr than in Li, as in Fr the distance between the last electron and the positive nucleus is large; this makes the attractive force binding or holding the electron to be less. Thus K will give up electron more easily than Na. This makes K more reactive than Na. | | Previous | Next |
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