Why does the solubility of carbonates of alkali metals increase down the group?

Why does the solubility of carbonates of alkali metals increase down the group?

On going down the group, the size of the cation increases and the salt becomes more ionic in nature. So, the solubility also increases down the group. Thus, the solubility of fluorides of alkali metals increases down the group.

Why the solubility of carbonates and bicarbonates of alkali metals increases down the group?

Solubility of carbonates and bicarbonates of alkali metal increases down the group for the alkali metal . Thus, the cleavage of Metal carbonate or metal bicarbonate bond occurs more easily as we move down the group. This make the carbonate and bicarbonate of metal to show increase in solubility in water down the group.

Why carbonates of alkaline earth metal are not soluble in water?

Group II metal oxide basicity and hydroxide solubility in water increase as you go down the column….Metal Oxide Basicity.

Element	Electronegativity	∆Electronegativity
Be	1.57	1.87
Mg	1.31	2.13
Ca	1.00	2.44
Sr	0.95	2.49

Why does the stability of alkaline earth metal carbonates and sulphates decrease down the group?

The size of anions being much larger compared to cations, the lattice enthalpy will remain almost constant within a particular group. Since the hydration enthalpies decrease down the group solubility will decrease as found for alkaline earth metal carbonates and sulphates.

Why does the solubility of carbonates decrease down the group?

Why does the solubility of alkaline earth metal carbonates and sulphates in water decrease down the group? Since the hydration enthalpies decrease as the size of the cation increases down the group , the solubility of carbonates and sulphates of alkaline earth metals decreases down the group .

Why does stability of carbonates increases down the group?

As the positive ions get larger down the group, they affect on the carbonate ions near them less. More heat must be supplied for the carbon dioxide to leave the metal oxide. In other words, the carbonates become more thermally stable down the group.

Why does the stability of carbonates increase down the group?

All the carbonates in this group undergo thermal decomposition to the metal oxide and carbon dioxide gas. Down the group, the carbonates require more heating to decompose. The carbonates become more thermally stable down the group.

Why are alkali carbonates soluble?

In general, the most common main group elements used as carbonates are the Alkali and Alkaline metals. All main group carbonates, except Na, K, Rb and Cs are unstable to heat and insoluble in water. Usually all carbonates are soluble in acid, because of the formation of bicarbonate ion.

Why does solubility of alkaline earth metal sulphates decrease down the group?

The solubility of the sulphates of alkaline earth metals in water decreases down the group in the periodic table. This is because as we move down the group the hydration enthalpy of the elements increases faster as compared to the relative decrease in their lattice enthalpy.

Why does the decomposition of carbonates decrease down the group?

Explaining the relative falls in lattice enthalpy The lattice enthalpies of both carbonates and oxides fall as you go down the Group because the positive ions are getting bigger. The inter-ionic distances are increasing and so the attractions become weaker.

Why are alkali metal carbonates stable?

As the electropositive character increase down the group, the stability of alkali carbonates increases. Hence more thermal energy required for the decomposition of alkali carbonates down the group. Hence, Rb2CO3 have more thermal stability than others. Q3.

Why are alkaline earth metals soluble?

With salts that contain these types of ions the attraction between the positive ion (alkali metal ion) and the negatively charged ion is weak enough for water molecules to be able to separate, therefore allowing the compound to be soluble.