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प्रश्न
Discuss the trend of the following:
The solubility and the nature of oxides of Group 2 elements.
उत्तर
All the alkaline earth metals form oxides of formula MO. The oxides are very stable due to high lattice energy and are used as refractory material. Except BeO (predominantly covalent), all other oxides are ionic and their lattice energy decreases as the size of cation increases.
The oxides are basic and basic nature increases from BeO to BaO (due to increasing ionic nature).
`ubrace(BeO <)_("Amphoteric") ubrace(MgO <)_("Weakly basic") ubrace(CaO < SrO < BaO)_("Strongly basic")`
BeO dissolves both in acid and alkalies to give salts and is amphoteric.
The oxides of the alkaline earth metals (except BeO and MgO) dissolve in water to form basic hydroxides and evolve a large amount of heat. BeO and MgO possess high lattice energy and thus are insoluble in water.
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संबंधित प्रश्न
Beryllium and magnesium do not give colour to flame whereas other alkaline earth metals do so. Why?
Assertion: BeSO4 is soluble in water while BaSO4 is not
Reason: Hydration energy decreases down the group from Be to Ba and lattice energy remains almost constant.
Substantiate Lithium fluoride has the lowest solubility among group one metal fluorides.
Some of the Group 2 metal halides are covalent and soluble in organic solvents. Among the following metal halides, the one which is soluble in ethanol is ______.
Why are BeSO4 and MgSO4 readily soluble in water while CaSO4, SrSO4 and BaSO4 are insoluble?
What is the structure of BeCl2 molecule in gaseous and solid state?
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Reason (R): Beryllium carbonate is unstable and decomposes to give beryllium oxide and carbon dioxide.
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Among the following alkaline earth metal halides, one which is covalent and soluble in organic solvents is ______.
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