Similarities and Differences between Group One and Group Two Elements

Among the Group 1 Alkali Metals are the elements Magnesium, Calcium, Barium, Strontium, and Radium, which are soft silver metals with a less metallic character than the Group 1 Alkali Metals. Despite the fact that many characteristics are shared by the entire group, heavier metals such as Ca, Sr, Ba, and Ra are almost as reactive as the Group 1 Alkali Metals in terms of reactivity. A +2 oxidation state is achieved by all of the elements in Group 2 due to the presence of two electrons in their valence shells.

Elements from Group 1 vs Group 2 – a Summary

The difference between groups 1 and 2 is the number of electrons in their outermost orbital, which is different from one another. When comparing group 1 and group 2 elements, the most significant difference is that all group 1 elements have unpaired electrons in their outermost orbital, whereas all group 2 elements have paired electrons in their outermost orbital.

What are the Elements of Group 2 Referred to As

Alkaline earth metals are elements that are found in group 2 of the periodic table and are composed of alkaline earth elements. When combined with water, these metals produce an alkaline solution, which is why they are referred to as alkaline metals. They are referred to as earth metals because their oxides do not dissolve in water and do not heat when exposed to heat. Earth was a term used by scientists in the early centuries to refer to any material that possessed these two characteristics. It is impossible to dissolve all of the group 2 elements’ oxides in water, and they are all heat resistant. As a result, alkaline earth metals are designated as elements belonging to group 2.

The Characteristics of the Elements of Group 2

Group 2 elements’ properties are very similar especially in regards to their valence electrons, physical properties, and chemical properties. These will be discussed in the next few sections.

Conclusion

The electrons present in an atom occupy various sub-orbitals of available energy levels, which are arranged in increasing order of energy content. In an atom, the final electron can be found in any of the four subshells: the s, p, d, or f subshells. As a result, the s block elements are defined as the elements of the atom that have their last valence electron present in the s-suborbital at the time of formation.