GENERAL PROPERTIES

Physical state: 

* Carbonates and bicarbonates are solids at room temperature. Carbonates of group-1 and group-2 elements are colorless. Whereas, the carbonates of transition elements may be colored.

* The polarizing power of the group-1 metal ions (M+) is less than the polarizing power of group-2 metal ions (M2+). Hence group-2 carbonates are more covalent than the carbonates of group-1. 

Whereas the polarizing power decreases down the group with increase in the size of metal ion. Hence the ionic nature increases down the group.

* NaHCO3 and KHCO3 can exist in the solid state. But the bicarbonates of group-2 elements are only known in aqueous solutions.

Solubility in water:

* Except Li2CO3, The group-1 carbonates are fairly soluble in water.  The solubility increases down the group as the ionic nature nature increases.

* Group-2 carbonates are sparingly soluble in water as their lattice energies are higher (it is due to increase in covalent nature). There is no clear solubility trend observed down this group. 

But group-2 carbonates are soluble in a solution of CO2 due to formation of HCO3-.

Thermal stability:

* Carbonates are decomposed to carbon dioxide and oxide upon heating. Whereas bicarbonates give carbonate, water and carbon dioxide.

* Thermal stability of group-1 and group-2 carbonates (also of bicarbonates) increases down the group as the polarizing power of the metal ion decreases.

* Due to same reason, carbonates of group-1 are more stable than those of group-2.

* Small and highly charged metal ions possess more polarizing power and hence facilitates the decomposition of carbonate ion into carbon dioxide and oxide ion.

 

CHEMICAL REACTIONS

The most important reaction shown by these anions is 'decomposition' by liberating carbon dioxide either upon heating or by adding acids. Water or oxide are the other products.

2HCO3- --------> CO3

2- + CO2 + H2O    (upon heating)

HCO3- + H+ --------> CO2 + H2O    (in acidic medium)

 

CO32- --------> CO2 + O2-      (upon heating)

CO32- + 2H+ ---------> CO2 + H2O    (in acidic medium)

Illustrations:

i) 2NaHCO3   -------->  Na2CO3 + CO2 + H2O    (upon heating)

ii) NaHCO3  + H+ -------->  Na+ + CO2 + H2O   

Application: That is why baking soda (NaHCO3) is used as leavening agent to raise cookies, cakes

etc.,. It is decomposed to CO2 and water upon heating. This makes the cookies porous and palatable.

 

iii) Ca(HCO3)2  -------->  CaCO3 + CO2 + H2O    (upon heating)

    Mg(HCO3)2  -------->  MgCO3 + CO2 + H2O    (upon heating)

Application: Temporary hardness of water is due to presence of bicarbonates of Ca and Mg. It is

possible to remove temporary hardness by boiling water. Upon boiling, the soluble bicarbonates are

decomposed to insoluble carbonates, which can be filtered off.

 

iv) CaCO3   -------->  CaO + CO2    (upon heating)

Application: This reaction is used to get quick lime (CaO), in lime kilns, which is further used in the

preparation of slaked lime, Ca(OH)2. This is also one of the reaction occurring in the manufacture of

Portland cement. Technically this type of reaction is called calcination.

 

v) CaCO3  + 2HCl -------->  CaCl2 + H2O + CO2   

vi) MgCO3  + 2HCl -------->  MgCl2 + H2O + CO2   

or in general 

CO32- + 2H+ ---------> CO2 + H2O

Comment: This reaction is the principle involved in the detection of carbonate ion present in a

given salt. 

Calcium carbonate is present in the marble stone. This is decomposed to carbon dioxide when

come into contact with acids. Hence the effervescence is observed when acids are dropped on the

floor. Lime juice contains citric acid, which liberates carbon dioxide and forms insoluble calcium citrate,

which appears as white marking.

Note: Effervescence is observed sometimes on granite floor which may rarely contain carbonates.

This may be originated from lichens lived on them.

STUDY OF SOME INDIVIDUAL CARBONATES AND BICARBONATES

Li2CO3: 

* Lithium carbonate is a colorless salt with polymeric nature. 

* It is sparingly soluble in water and its solubility decreases with increase in temperature. But it dissolves in presence of carbon dioxide due to the formation of LiHCO3.

* It is used in psychiatry to treat mania. The lithium ions interfere the sodium pump and inhibit the activity of protein kinase C (PKC).

* It is also used in the preparation of lithium cobalt oxide - which is present in lithium ion battery cathodes.

 

Na2CO3: 

* Sodium carbonate is a colorless salt.  

* It is fairly soluble in water.

* It is also called as washing soda.

* It is used mainly in laundries and in softening hard water.

* It is also used in making glass.