Explanation
Thermal stability of metal carbonates increases as the electropositive character of the metal or the basicity of the metal hydroxide increases from Be(OH)2 to Ba(OH)2, Thus, BaCO3 is the most stable.
Due to small size of Li+ and F– ions, lattice enthalpy is much higher than hydration enthaalpy and hence LiF is least soluble among alkali metal Fluorides.
The solubility decreases as we move from CaSO4 to BaSO4.
The electrons of Be and Mg are so strongly bonded that they do not get excited in flame.
According to Fajan rules, polarity increases as the size of the cation increases.
Alkali metal oxides are most basic followed by alkaline earth metal oxides while transition metal oxides are least basic. Amongst alkali and alkaline earth metal oxides, basicity increases down the group. Thus, Cs2O is more basic than K2O and SrO is more basic than MgO. Therefore, the overall order is : NiO < MgO < SrO < K2O < Cs2O
The solubility of bicarbonates of alkali metals increases down the group but alkaline earth metal carbonates are insoluble in H2O.
CaO, CaCO3 and Ca(OH)2 are all bases and hence must dissolve in acetic acid to form calcium acetate only calcium oxalate does not dissolve in CH3COOH.
2 (Be, Mg)
6 [K2SO4, BeSO4, Li2SO4, MgSO4, Na2SO4, Rb2SO4]
1 [Be(OH)2]
Lithium does not form peroxide
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