Which of the following is most stable BaCO3 MgCO3 SrCO3 CaCO3?

Which of the following is most stable BaCO3 MgCO3 SrCO3 CaCO3?

⇒ The increasing order of the size of cations of the given carbonates: Mg < Ca < Sr < Ba Hence, the increasing order of the thermal stability is: MgCO3 < CaCO3 < SrCO3 < BaCO3 ⇒ Thus, among alkaline earth metal carbonates, option (D), BaCO3 is thermally the most stable.

Which carbonate is thermally most stable MgCO3 CaCO3 BaCO3 SrCO3?

MgCO3 is most stable alkaline earth metal because it is present in first period. Due to this its nuclear charge is less as compare to other. Due to its less nuclear charge its bond length is small thus it is more stable.

Which is more thermally stable BaCO3 or CaCO3?

As the atomic number increases down the group, the difference in the stability of metal cation and the oxide anion increases. Hence, the stability of carbonate increases. Therefore, the thermal stability of carbonates increases down the group. Therefore, the order of stability is \[BaC{O_3} > CaC{O_3} > MgC{O_3}\] .

Which is more thermally stable MgCO3 or CaCO3?

MgCO3 is thermally more stable than CaCO3 .

Which is the correct order of thermal stability SrCO3?

MgCO3

Which is more stable BaCO3 MgCO3 CaCO3 BeCO3?

BaCO3 is more thermally stable because polarising power of Ba2+ is less than other alkaline earth metals and thermal stability is inversely proportional to polarising power of action when compound containing polyatomic anion and here carbonate is polyatomic anion.

Is Rb2CO3 thermally stable?

Correct option a Li2CO3Explanation:Since the alkali metals are highly electropositive their carbonates are highly stable towards heat. As the electropositivity increases down the group the stability is in order of :Cs2CO3 >Rb2CO3 > K2CO3 > Na2CO3 > Li2CO3Lithium carbonate decomposes on heating.

Which is more stable Na2CO3 or CaCO3?

Since sodium is smaller in size than calcium and two sodium ions are bonded to carbonate group, sodium carbonate is more polarised than calcium carbonate. So, lesser heat is required to break sodium carbonate than calcium carbonate. Thus, calcium carbonate is more stable than sodium carbonate.

Why is BaCO3 more stable than MgCO3?

The increasing order of thermal stability of carbonates is as follows: Hence, carbonate of alkaline earths decompose into oxide and CO2. Large cations like Ba2+ have low ionic potential and are unable to polarise the electrons of O atom due to which carbonates of large cations are more stable.

Which of the following carbonates is least stable MgCO3 CaCO3 BaCO3 srco3?

Why is baco3 more stable than MgCO3?

Why do carbonates become more thermally stable down the group?

The smaller the positive ion is, the higher the charge density, and the greater effect it will have on the carbonate ion. As the positive ions get larger down the group, they affect on the carbonate ions near them less. In other words, the carbonates become more thermally stable down the group.

What are the factors affecting the thermal stability of BaCO3?

> Thermal stability of BaCO3,… (i) More be the ionic nature, more be the attractive force between the species. (ii) More be the attractive force, more be the thermal stability. (iii) Ionic character for the same anionic species, increases down the group.

What is the Order of thermal stability of carbonate?

Thus, the stability of the decomposition product metal oxide decreases, as close packing is not possible. Hence, the stability of the carbonate increases. Thus, among the given carbonates, the order of thermal stability is BaCO 3 . Was this answer helpful? Select the correct order of density.

Why is MgCO3 thermally less stable than CaCO3?

Originally Answered: MgCO3 is thermally less stable than CaCO3? First, Mg (period 2) is in a lower period than Ca (period 3), which means that the ionic radius of magnesium will be smaller than calcium’s.

How does atomic number affect the stability of carbonates?

On moving down the group of alkaline earth metals, the thermal stability of carbonates increases. As the atomic number increases, the difference in the stability of metal cation and the oxide anion increases. Thus, the stability of the decomposition product metal oxide decreases, as close packing is not possible.