| Characteristics
of Groups |
| In the first group, called group I A, we have Hydrogen (H), Lithium (Li), Sodium (Na), Potassium (K), Rubidium (Rb), Cesium (Cs) and Fransium (Fr). They have all only one electron in their outermost shells. H is an exception in this group and has to be dealt separately. So other than H all the elements show metallic properties and have valence +1. They give up an electron easily. They are highly metallic. The group is known as the alkali metals. |
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| The second group (group II A) has Beryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), Barium (Ba) and Radium (Ra). They have two electrons in their last shell and their valence is +2 as they give up two electrons to form compounds. The elements in group II A are not as metallic as the alkali metals. They form oxides easily and are known as alkali earth metals. |
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