What is the trend in thermal stability of Group 1 carbonates?

What is the trend in thermal stability of Group 1 carbonates?

In Group 1, lithium carbonate behaves in the same way – producing lithium oxide and carbon dioxide. The rest of the Group 1 carbonates don’t decompose at Bunsen temperatures, although at higher temperatures they will. The decomposition temperatures again increase as you go down the Group.

Which carbonate is the most stable to heat?

The thermal stability (measured by the temperature of decomposition) of these carbonates increases on moving down the group due to the increase of electropositive character of the metal or basicity of the metal hyroxide. Thus, BeCO3 is least thermally stable while BaCO3 is most thermally stable.

Are carbonate stable towards heat?

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.

Why does the stability of carbonates increase down Group 1?

As the positive ions get bigger down the group, they have less effect on the carbonate ions near them. To compensate, the compound must be heated more in order to force the carbon dioxide to break off and leave the metal oxide. In other words, carbonates become more thermally stable down the group.

Why does thermal stability of carbonates increase down Group 1?

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.

Why does thermal stability of Group 2 carbonates increase down the group?

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.

Does thermal stability increase down Group 1?

The thermal stability of most compounds of Group 1 elememts (hydroxides, carbonates, nitrates) increases down the group due to decrement in charge density of the cation.

Why does the stability of alkaline earth metal carbonates 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 carbonates of Group 1a elements are more thermally stable than those of group 2a?

Imagine that this ion is placed next to a positive ion. The positive ion attracts the delocalized electrons in the carbonate ion towards itself. If the positive ion only has one positive charge, the polarizing effect is lessened. This is why the Group 1 compounds are more thermally stable than those in Group 2.

Why are carbonates more thermally stable down the group?

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. This page offers two different explanations for these properties: polarizability and energetics.

Why do Group 1 compounds need to be heated more?

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. As the positive ions get bigger down the group, they have less effect on the carbonate ions near them.

How does heat affect the decomposition of carbonates?

Down the group, the carbonates require more heating to decompose. The carbonates become more thermally stable down the group. The effect of heat on the Group 2 Nitrates The Group 2 nitrates undergo thermal decomposition to the metal oxide, nitrogen dioxide and oxygen gas.

How stable are Group 1 hydrogen carbonates?

By contrast, the Group 1 hydrogen carbonates are stable enough to exist as solids, although they do decompose easily on heating. For example, this is the reaction for sodium hydrogen carbonate: Detailed explanations are given for the carbonates because the diagrams are easier to draw.

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