They include lithium, sodium and potassium, which all react vigorously with water to produce an alkaline solution. The carbonates of group-2 metals and that of lithium decompose on heating, forming an oxide and carbon dioxide . Solubility is a result of an interaction between polar water molecules and the ions that make up a crystal. . . Q9. (a) Nitrates (b) Carbonates (c) Sulphates. In general, the most common main group elements used as carbonates are the Alkali and Alkaline metals. Group 2 (a.k.a. Since hydration energy is inversely proportional to radius of ion, I would expect Lithium to release the largest hydration energy and thus be the most soluble. As we know that for alkaline earth metals as we move down the group, the lattice enthalpy of carbonates remain approximately the same. Contrary to alkali metal sulphates, beryllium sulphate is water-soluble. Usually all carbonates are soluble in acid, because of the formation of bicarbonate ion. Hello! decomposes on heating to evolve whereas other alkali metal carbonates do not. All main group carbonates, except Na, K, Rb and Cs are unstable to heat and insoluble in water. Alkali metal halides are soluble in water due to their high ionic character and low lattice energy. Data on some, such as cesium and rubidium fluoride, nitrate, carbonate, and sulfate, appear to be reported for the first time. ‘ … The Group 1 elements in the periodic table are known as the alkali metals. LiH is the stablest among all the alkali metal hydrides. Compare the solubility and thermal stability of the following compounds of the alkali metals with those of the alkaline earth metals. This is a list of the solubility rules for ionic solids in water. alkali metals and their ions M⁺): the solubility of M₂SO₄ decreases on going down the group; the solubility of M₂CO₃ increases on going down the group; all the MHCO₃ salts are soluble in water (not sure about it though); all the MOH compounds are soluble in water. Two forces determine the extent to which the solution will occur: 5:49 Salts of Oxoacids Since the alkali metals are highly electropositive, therefore their hydroxides are very strong bases and hence they form salts with all oxoacids ( H 2 CO 3 , H 3 PO 4 , H 2 SO 4 , HNO 3 , HNO 2 etc) . But my textbook (Concise Inorganic Chemistry by JD LEE) says that the "Solubility of carbonates and fluorides of Alkali metals increase rapidly on descending the group. , LiF and lithium phosphate are insoluble in water while the corresponding salts of other alkali metals are soluble in water. Solubilities of the halides, nitrates, carbonates, sulfates, and some perchlorates of all the alkali metals and alkaline earth metals in methanol at room temperature have been determined. The smaller size and the charge density increases the hydration energy of the beryllium sulphate leading to more solubility. Amongst fluorides of alkali metals, the lowest solubility of LiF in water is due to (a) ionic nature of lithium fluoride. Carbonates of metal: Thermal stabilityThe carbonates of alkali metals except lithium carbonate are stable to heat. The solubility of metal halides depends on their nature, lattice enthalpy and hydration enthalpy of the individual ions. Amongst fluorides of alkali metals, the lowest solubility of L i F in water is due to: The solubility of metal halides depends on their nature, lattice enthalpy and hydration enthalpy of the individual ions. Group 1 (a.k.a. (b) high lattice enthalpy. Do not ( c ) sulphates know that for alkaline earth metals as we that! 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