Why carbonates of group 1A element are more thermally stable than those of group 2a?

Why carbonates of group 1A element are more thermally stable than those of group 2a?

Polarizing the carbonate ion If the positive ion only has one positive charge, the polarizing effect is lessened. This is why the Group 1 compounds are more thermally stable than those in Group 2. The Group 1 compound must be heated more because the carbonate ion is less polarized by a singly-charged positive ion.

Does solubility of Group 2 carbonates increase down the group?

Solubility of the carbonates The carbonates become less soluble down the group. All the Group 2 carbonates are very sparingly soluble. Magnesium carbonate, for example, has a solubility of about 0.02 g per 100 g of water at room temperature.

Why is group 1A more soluble in water?

Salts of the Group 1A elements tend to be extremely soluble in water. Because the alkali metal ions are relatively large (compared to other ions from the same period), their charges densities are low, and they are easily separated from their anions and solvated by polar solvents like water.

Why do Group 2 carbonates decrease in solubility?

while for group 2, ie., Alkaline earth metals, solubility of carbonates in water decreases down the group as the decrease in hydration energy is more than the decrease in lattice energy..

What is unique about group 1a metal carbonates?

In Group 1, lithium carbonate behaves in the same way – producing lithium oxide and carbon dioxide. The rest of the Group 1 carbonates don’t decompose at Bunsen temperatures, although at higher temperatures they will. The decomposition temperatures again increase as you go down the Group.

Are group 1 carbonates soluble?

Group 1: Alkali Metals and Carbonates (X2CO3) All except Lithium are soluble in water and stable to heat. Uses: drug development. Chemical Characteristics: Low solubility in water.

Why does the solubility of Group 2 sulfates decrease down the group?

Since the hydration enthalpy decreases faster than the lattice enthalpy in the case of Group 2 sulphates, the solubility of Group 2 sulphates decreases while progressing down the group.

Why do Group 2 carbonates become more stable?

The thermal stability increases as you go down Group 2. This is because the Group 2 ion has lower charge density, and thus distorts the carbonate ion less. The less distorted the carbonate ion is, the more stable it is, and so a higher temperature is required to decompose the carbonate.

Are all group 1 carbonates soluble?

A saturated solution has a concentration of about 1.3 g per 100 g of water at 20°C. The other carbonates in the group are very soluble, with solubilities increasing to an astonishing 261.5 g per 100 g of water at this temperature for cesium carbonate. Solubility of the carbonates increases down Group 1.

What carbonates are soluble?

g) All carbonates are insoluble except those of sodium, potassium and ammonium. Magnesium carbonate is slightly soluble. Many hydrogen carbonates, such as Ca(HCO3)2 and Mg(HCO3)2, are soluble.

Does solubility increase down group 1?

The hydroxides The other hydroxides in the group are even more soluble. Solubility of the hydroxides increases down Group 1.

Are group 2 sulfates soluble?

Solubility of the sulphates 4H2O is soluble. (The Data Books agree on this – giving a figure of about 39 g dissolving in 100 g of water at room temperature.)

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