Group 2 on the periodic table: Alkaline earth metals - Electronic configuration, physical and chemical properties

 What are Alkaline Earth Metals?

The alkaline earth metals are all of the elements in the second column of the periodic table. This group includes beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra). The word 'alkaline' refers the basic nature of the compounds they form when bonded with oxygen. Alkaline earth metals have relatively low ionization energies for their first two electrons; because of this, alkaline earth metals exist with a 2+ charge most of the time.

Electronic configuration

Alkaline earth metals have a corresponding [Noble gas] ns2 electronic configuration. So, all alkali earth metals have two electrons in their outermost layer of electrons.   


Physical and chemical Properties

Group 2 elements are highly reactive metals because they tend to lose their two valence electrons to achieve a stable electron configuration. They have higher melting and boiling points than alkali metals because of their strong metallic bonding and well-arranged crystal structure. Group 2 elements are good conductors of heat and electricity. They react with dilute acids to form colourless solutions of metal salts. Also, form alkaline solutions with water and their ionization energy decreases as atomic size increases. Atomic and ionic radii increase as you move down the group in the periodic table. They are mainly used in fireworks, rescue flares, high-performance car engines, and more.

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