Thermal stability of BaCO3, CaCO3 and MgCO3 is (a) BaCO3>CaCO3>MgCO3 (b) BaCO3>MgCO3>CaCO3 (c) M

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Thermal stability of BaCO3, CaCO3 and MgCO3 is (a)...

Thermal stability of $\mathrm{BaCO}_{3}, \mathrm{CaCO}_{3}$ and $\mathrm{MgCO}_{3}$ is (a) $\mathrm{BaCO}_{3}>\mathrm{CaCO}_{3}>\mathrm{MgCO}_{3}$ (b) $\mathrm{BaCO}_{3}>\mathrm{MgCO}_{3}>\mathrm{CaCO}_{3}$ (c) $\mathrm{MgCO}_{3}>\mathrm{CaCO}_{3}>\mathrm{BaCO}_{3}$ (d) $\mathrm{CaCO}_{3}>\mathrm{MgCO}_{3}>\mathrm{BaCO}_{3}$

Thermal stability of $\mathrm{BaCO}_{3}, \mathrm{CaCO}_{3}$ and $\mathrm{MgCO}_{3}$ is
(a) $\mathrm{BaCO}_{3}>\mathrm{CaCO}_{3}>\mathrm{MgCO}_{3}$
(b) $\mathrm{BaCO}_{3}>\mathrm{MgCO}_{3}>\mathrm{CaCO}_{3}$
(c) $\mathrm{MgCO}_{3}>\mathrm{CaCO}_{3}>\mathrm{BaCO}_{3}$
(d) $\mathrm{CaCO}_{3}>\mathrm{MgCO}_{3}>\mathrm{BaCO}_{3}$

Key Concepts

Ionic Size and Charge Density

The size of the metal cation and its corresponding charge density significantly affect the stability of the carbonate. Smaller cations tend to have higher charge densities, which result in stronger polarization effects on the carbonate ion. As the ionic radius increases, the polarizing ability decreases, contributing to enhanced thermal stability of the carbonate.

Thermal Decomposition of Carbonates

This concept involves the breakdown of a metal carbonate into metal oxide and carbon dioxide upon heating. The decomposition temperature is a measure of the thermal stability of the carbonate, indicating how much heat energy is required to overcome the bonds in the crystal lattice and release CO2.

Lattice Energy

Lattice energy refers to the energy released when ions in the gas phase come together to form an ionic solid. In carbonates, a higher lattice energy usually translates into greater stability as more energy is needed to break apart the ionic structure. The magnitude of the lattice energy is influenced by the sizes and charges of the ions involved.

Polarizing Power

Polarizing power is the ability of a cation to distort the electron cloud of the anion. Smaller cations with higher charge densities, such as Mg2+, have greater polarizing power relative to larger cations like Ba2+. This increased polarization weakens the bonds within the carbonate ion, often leading to lower thermal stability.

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