The carbonates of group-2 metals and that of lithium decompose on heating, forming an oxide and carbon dioxide . This trend is explained in terms of the Group II metal ions ability to polarise the anion, the carbonate ion. Know of a thumb rule. All of these carbonates are white solids, and the oxides that are produced are also white solids. Join Yahoo Answers and get 100 points today. The salt containing one or more atoms of oxygen such as oxides ,hydroxides ,carbonate ,bicarbonate ,nitrite ,nitrate ,sulphates ,oxalates and phosphates are called oxo salts. When a smaller 2+ ion comes near a carbonate or nitrate ion, it pulls the electrons of the anion toward itself, and thus electrons are more concentrated on one particular oxygen of the anion that is closest to the 2+ cation; it polarizes the anion. The carbonates and nitrates of group 2 elements carbonates become more thermally stable as you go down the Group. Revision:Thermal stability of gp1 and 2 carbonates Thermal Stability is the decomposition of a compound on heating. The result is that the thermodynamics of the process are broadly similar for each of the Group 1 metals, and this reflected by the similar reduction potentials. Stability of oxides decreases down the group. Hence, more is the stability of oxide formed, less will be stability of carbonates. Results show that the acidity of C2H of an imidazolium ring is one of the key factors controlling the thermal stability. The higher the temperature needed to decompose something, the more thermally stable it is. The thermal stability of the hydrides of group 16 elements decreases down the group, i.e., H 2 O > H 2 S > H 2 Se > H­ 2 Te > H 2 Po. All M2O have the antifluorite structure (except Cs2O). As the cation increases in size down the group, the thermal stability of compounds with large complex ions increases. The oxides of metals having high positive reduction potentials are not stable towards heat. The s-metals consist of the Alkali Metals (Group 1) and the Alkaline Earth Metals (Group 2). Solution for group 1 elements with that of group 2 on the basis of the following:… Thermal decomposition is the term given to splitting up a compound by heating it. … 4) Anhydrous MgCl 2 is used in the electronic extraction of magnesium.. Solubility and thermal stability of Oxo salts. In group 1 and 2, the nitrates and carbonates get more stable down the group. If "X" represents any one of the elements, the following describes this decomposition: \[XCO_3(s) \rightarrow XO(s) + CO_2(g)\] Down the group, the carbonates require more heating to decompose. The structures of Be2+ often contain the cation in a tetrahedral environment: it is small and highly charged, and so has a high polarizing power and tends to form bonds with a high degree of directionality, ie. Still have questions? (8) 5) Compare and contrast the chemistry of group 1 elements with that of group 2 on the basis of the following: a) Nature of oxides b) Solubility and thermal stability c) Polarizing power of cations d) Reactivity and reducing power 6) Groups 1 and 2 metals could form (i) hydroxides and (ii) sulphates. As the electropositivity increases from top to bottom, the thermal stability of the oxide also increases from top to bottom. it displays a high covalency, Wavefunctions and the Born Interpretation, Electronic Transitions and the d2 Configuration, The total enthalpy change for the process depends on. As the group is descended, the enthalpies of ionization and sublimation both decrease, which favours oxidation, but this is balanced by the less exothermicenthalpy of solvation, which disfavours oxidation. This is because M-H bond dissociation energy decreases down the group with the increase in the size of a central atom. Reactivity increases down the group. Praseodymium-doped indium zinc oxide (PrIZO) channel materials have been fabricated by a solution process with conventional chemical precursor. It reacts with cold water to produce an alkaline solution of calcium hydroxide and hydrogen gas is released. Phosphoric acid and thermal treatments reveal the peculiar role of surface oxygen anions in lithium and manganese-rich layered oxides Oxidized On-species (0