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What are the trends in thermal stability of carbonates and nitrates of Group 2?
Both carbonates and nitrates of Group 2 elements become more thermally stable down the group. The larger compounds further down require more heat than the lighter compounds in order to decompose. All the carbonates in this group undergo thermal decomposition to the metal oxide and carbon dioxide gas.
Why does the stability of carbonates increase 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.
What is the trend in thermal stability of Group 1 carbonates?
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. The smaller the positive ion, the higher the charge density, and the greater the effect on the carbonate ion.
What is thermal stability of carbonates?
One common reaction of any metal carbonates is known as thermal decomposition. When metal carbonates are heated, they break down to form the metal oxide and carbon dioxide gas. This means that sodium carbonate is very stable and requires a high temperature to decompose.
What are the trends in thermal stability of nitrates down Group 2?
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.
Why is BaCO3 more stable than MgCO3?
As the atomic number increases, the difference in the stability of metal cation and the oxide anion increases. Hence, the stability of the carbonate increases. Thus, among the given carbonates, the order of thermal stability is BaCO3>CaCO3>MgCO3.
Why is na2co3 thermally stable?
All the alkali carbonates are stable to heat except lithium carbonate Li2CO3, because lithium carbonate is a covalent compound. Lithium ions are very small in size and carbonate ions are very large in size. Therefore, the small size lithium ion polarizes large size carbonate ions which forms more stable lithium oxide.
Why does thermal stability of Group 2 carbonates increase?
Is MgCO3 thermally stable?
MgCO3 is thermally more stable than CaCO3 .
Is BaCO3 thermally stable?
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 BaCO3>CaCO3>MgCO3.
Why are Group 2 carbonates more thermally stable?
As you go down the group the carbonates become more thermally stable. This trend is explained in terms of the Group II metal ions ability to polarise the anion, the carbonate ion. Small highly charged positive ions distort the electron cloud of the anion. The larger the anion the easier the distortion, as seen with the carbonate ion.
Which is more stable GP1 or 2 carbonates?
Revision:Thermal stability of gp1 and 2 carbonates Thermal Stability is the decomposition of a compound on heating. The higher the temperature needed to decompose something, the more thermally stable it is. In group 1 and 2, the nitrates and carbonates get more stable down the group.
What is the thermal stability of Group 2?
Thermal stability is the decomposition of compounds on heating. More the strong bonding more thermal stability. As we move down the group 2 the size of cations increases and sulphate is a big ion group according to its size. and big group of compounds are stable with big ionic group.
Which is more thermally stable nitrates or carbonates?
Both carbonates and nitrates of Group 2 elements become more thermally stable down the group. The larger compounds further down require more heat than the lighter compounds in order to decompose. All the carbonates in this group undergo thermal decomposition to the metal oxide and carbon dioxide gas. Click to see full answer.