Start studying Reactions of Group 2 Oxides and Hydroxides, and trends in solubility. But the answer to your question is no, they are not soluble, they react. Name an element from Group 2 which forms an amphoteric oxide and a water soluble sulphate. As a result, going down the group, the alkalinity of the solution formed increases when Group 2 oxides react with water Going down the group, the solubility of the hydroxides increases which means that the solutions formed from the reactions of the Group 2 metal oxides and water become more alkaline going down the group In water, the small highly charged oxide ions strongly attract water molecules and hydration is followed by hydrolysis. Calcium hydroxide is reasonably soluble in water. O 2-(aq) + H 2 O (l) → 2OH-(aq). (ii) The solubility and the nature of oxides, of Group 2 elements. Alkali (and not Alkalie!) M(s) + H 2 O(l) --> M(OH) 2 (aq) + H 2 (g) This is another example of a redox reaction. As a result, BeS0 4 is highly soluble in water. If the ions are more attracted to each other than the water then the compound will be insoluble. Reactions of the hydroxides of group 2 elements with acids 2HCl (a q) + Mg(O H)2 (a q) MgCl2 (a q)+ 2H2O (l) Solubility of hydroxides Group II hydroxides become more soluble down the group. The substances are listed in alphabetical order. Why are BeSO 4 and MgSO 4 readily soluble in water while CaSO 4, SrSO 4 and BaSO 4 are insoluble? Group 2 oxides REACT with water. Metal Oxides that are formed from elements in group IA and IIA, except for Be and Mg, react with water to create Hydroxides. The group 2 metal is oxidised from an oxidation state of zero to an oxidation state of +2. Discuss the trend of the following: (i) Thermal stability of carbonates of Group 2 elements. Q34. A group 2 oxide would form water instead of hydrogen gas, and as for if it dissolves, I think it depends on is the metal hydroxide is a solid or aqeous as it could form a precipitate. The balance between the attraction of oppositely charged ions to one another and the attraction of separate ions to water dictates the solubility of ionic compounds. The table below provides information on the variation of solubility of different substances (mostly inorganic compounds) in water with temperature, at one atmosphere pressure.Units of solubility are given in grams per 100 millilitres of water (g/100 ml), unless shown otherwise. As you can probably see from the periodic table, these elements are Li, Na, K, Rb, Cs, Ca, Sr, Ba. Today we're covering: Properties of Group 2 compounds Reactions Oxides with water Carbonates with acid Thermal decomposition Carbonates Nitrates Solubility Hydroxides Sulfates Let's go! The majority of compounds formed by group II elements are ionic. Contents Discuss the trend of the following: (i) Thermal stability of carbonates of Group 2 elements. The ionic oxides of Na 2 O and MgO, are soluble in water, although MgO is only slightly. All Group II hydroxides when not soluble appear as white precipitates. Group 2 elements all react with water in a similar way: Metal + Water --> Metal Hydroxide + Hydrogen. Here we will be talking about: Oxides Hydroxides Carbonates Nitrates Sulfates Group 2 Oxides Characteristics: White ionic solids All are basic oxides EXCEPT BeO BeO: amphoteric The small Be2+ … CaO + H 2 O --> Ca(OH) 2 But as the solubility of the hydroxides decreases ascending the group magnesium oxide reacts only slowly with water. Sol: (i) All the alkaline earth metals form carbonates (MC0 3). Sodium ions, with only +1 charge and a relatively large radius, hence have a low charge density and hydrolysis does not occur. 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