the alkaline earth metal is Be → Sr : form only monoxide(MO) Ba : form peroxide BaO2 under pressure; Solubility increases from BeO to BaO BeO,MgO,SrO,BaO → increasing solubility; All oxides are base (BeO is amphoteric) Hydroxides of the lighter alkaline earth metals are insoluble in water, but their solubility increases as the atomic number of the metal increases. Solubility in liquid ammonia. Solubility Patterns in the Periodic Table continued 2 216 linn Scientiic nc ll ihts esered 4. Get an answer for 'Describe the relationship between the solubility of the salts containing alkaline earth metal ions and the position of the metals in the periodic table.' 2) sodium or ammonium carbonate is added to the solution of alkaline earth metal salt such as CaCl 2. CaCl 2 + Na 2 CO 3 ——> CaCO 3 + 2 NaCl. _____ _____ _____ _____ 3. 10. Oxides and Hydroxides Because BeO and MgO are much more inert than the other group 2 oxides, they are used as refractory materials in applications involving high temperatures and mechanical stress. What trend in solubility did you observe for the alkaline earth metals? An alkaline earth metal gives a salt with chlorine which is sparingly soluble in water at room tempreture but fairly soluble in boiling water. 2. PHYSIAL PROPERTIES. All metal oxides are ionic (except BeO) divalent metal ions are sufficiently polarizing to make peroxide when heated in pure oxygen. It also forms a sulphate whose mixture with a sulphate of a transition metal is called 'lithopone' and is used as white pigment. The alkaline earth metals comprise the group 2 elements. All the alkaline earth metals have two electrons in their valence shell, so they lose two electrons to form cations with a 2+ charge. A metal M readily forms water-soluble sulphate M S O 4 ,water-insoluble hydroxide M (O H) 2 and oxide MO which becomes inert on heating.The hydroxide is soluble in NaOH,The M is: View solution Property of all the alkaline earth metals that increases with their atomic number is: 9. The ammoniates are good conductors of electricity and decompose at high temperature. Properties of the Alkaline Earth Metals . All the discovered alkaline earth metals occur in nature. Reactions of Alkaline Earth Metals. The alkaline earth metals are the elements that correspond to group 2 of the modern periodic table. Properties . This group of elements includes beryllium, magnesium, calcium, strontium, barium, and radium.The elements of this group are quite similar in their physical and chemical properties. Hydroxides of the lighter alkaline earth metals are insoluble in water, but their solubility increases as the atomic number of the metal increases. The precipitations of alkaline‐earth metal and transition metal oxalates, from aqueous solution and from excess alkali metal oxalate solution, are surveyed: also the coprecipitations of transition metal oxalates together with alkaline‐earth metal oxalates. Like alkali metals, alkaline earth metals dissolve in liquid ammonia giving coloured solutions. The alkaline earths possess many of the characteristic properties of metals.Alkaline earths have low electron affinities and low electronegativities.As with the alkali metals, the properties depend on the ease with which electrons are lost.The alkaline earths have two electrons in the outer shell. When the metal ammonia solutions are evaporated, hexammoniates [M (NH 3) 6] 2+ are formed. Because BeO and MgO are much more inert than the other group 2 oxides, they are used as refractory materials in applications involving high temperatures and mechanical stress. 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