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1.
The nature of the element
Alkaline earth metals are silver-white, with metallic luster, good conductivity and ductility
.
Alkaline earth metals have two valence electrons, so the metal bond of alkaline earth metals is stronger than that of alkali metals
.
The melting point, boiling point, hardness, and density of alkaline earth metals are much higher than that of alkali metals
The reactivity of alkaline earth metals from Be to Ba metal increases in turn, and its reactivity is manifested in strong reducibility
.
Alkaline earth metals can directly combine with many non-metallic elements to form ionic compounds
3Mg+N 2 =Mg 3 Ne 2
The strong reducibility of alkaline earth metals can be used to prepare precious metals or rare metals
.
Ca, Sr, and Ba in alkaline earth metals can react with H 2 to form corresponding hydrides at high temperatures , and react with water to form hydroxides
.
Calcium , strontium , and barium react mildly with water
.
The reason is that the metal has a high melting point and does not melt when reacting with water; the solubility of hydroxide is small, and the generated hydroxide covers the surface of the metal to hinder the contact between the metal and water and slow down the reaction rate
Because Be and Mg form a dense oxide protective film on the surface, they do not react with water at room temperature
.
2.
Preparation of simple substance
All alkaline earth metals can be prepared by electrolytically molten chloride
Metal beryllium can be produced by electrolytic melting of BeCl 2 , and NaCl or CaCl 2 needs to be added during the production process to increase the conductivity of the molten salt
Metal beryllium can also be prepared by thermal reduction method, usually by reducing BeF2 with magnesium metal at high temperature