Thermal decomposition is the term given to splitting up a compound by heating it. Polarising-Power-and-the-Stability-of-Carbonates. More the strong bonding more thermal stability. The carbonates of group-2 metals and that of lithium decompose on heating, forming an oxide and carbon dioxide . Discuss the trend of the following : (i) Thermal stability of carbonates of Group 2 elements . * Due to same reason, carbonates of group-1 are more stable than those of group-2. (i) All the alkaline earth metals form carbonates (MCO 3). Calculate the loss in mass of each metal carbonate. What is the word equation for thermal decomposition? 900+ SHARES. Cation of greater polarizing power distort the carbonate ion more easily and easily decompose it than the cation of lower polarizing power. Thermal stability is the decomposition of compounds on heating. This means that the enthalpy change from the carbonate to the oxide becomes more negative so more heat is needed to decompose it. 5.2 ACIDS, BASES AND SALTS 2. Stability of carbonates increases down group I (alkali) and group II (alkaline earth) metals. MgCO3 decomposes at 540 C. CaCO3 decomposes at 900 C. SrCO3 decomposes at 1290 C. BaCO3 decomposes at 1360 C. This is because of the increasing size of the cation (ionised metal) as we go down the group. Explanations. As we go down the group, the carbonates have to be heated more strongly before they will decompose. Thermal decomposition is the term given to splitting up a compound by heating it. Eight resources on the thermal decomposition of the group 1 and 2 nitrates and carbonates. However, carbonate of lithium, when heated, decomposes to form lithium oxide. Source(s): https://shrinke.im/a8pDM. The electron cloud of anion is distorted to a lesser extent. so, the correct order of thermal stability of given carbonates is: BeCO 3 < MgCO 3 < CaCO 3 < K 2 CO 3 Be, Mg and Ca present in second group and K present in the first group. That's entirely what you would expect as the carbonates become more thermally stable. Why na2co3 does not decompose on heating? Nitrates of both group 1 and group 2 metals are soluble in water. Explanation: In all cases, for a particular set of e.g. The thermal stability … The rest of group 1 follow the … Thermal Stability is the decomposition of a compound on heating. This trend is explained in terms of the Group II metal ions ability to polarise the anion, the carbonate ion. Also, does thermal stability increase or decrease as you go down group 1 (with explanation please)? The solubility of carbonates in water decreases as the atomic number of the metal ion increases. Group 1 or Group 2 compounds, the thermal stability increases down the group as the ionic radius of the cation increases, and its polarising power decreases. Charge Density and Polarising Power of Group 2 Metal Cations. It also identifies and explains the trend in the solubility and thermal stability of group 2 metal compounds. The size of the group 2 ions gets bigger as we go down the group. So, solubility should decrease from Li to Cs. It however shows reversible decomposition in closed container All the carbonates in this Group undergo thermal decomposition to give the metal oxide and carbon dioxide gas. It describes and explains how the thermal stability of the compounds changes as you go down the Group. The carbonates of group-2 metals and that of lithium decompose on heating, forming an oxide and carbon dioxide . Thermal decomposition is the term given to splitting up a compound by heating it. Why is lithium carbonate thermally unstable. Info. Asked By: Piedraescrita Italia | Last Updated: 19th March, 2020, Cation of greater polarizing power distort the. Thermal stability of carbonates increases in a group as we move from top to bottom and decreases in a period as we move from left to right. Exactly the same arguments apply to the nitrates. This decreases the charge density and the ability of the cation to polarize the anion. All these carbonates decompose on heating to give CO 2 and metal oxide. What's the difference between Koolaburra by UGG and UGG? As you go down the group the carbonates become more thermally stable. Click to see full answer Also know, how does the thermal stability of alkaline earth metal carbonates vary down the group explain? The nitrates also become more stable to heat as you go down the Group. I am a metal and placed above iron in the activity series. Thermal stability: * Carbonates are decomposed to carbon dioxide and oxide upon heating. 3. Products: barium oxide, nitrogen dioxide (nitrogen(IV) oxide) and oxygen d) lower 2. M C O 3 → M O + C O 2 On moving down the group, the stability of alkaline earth metal carbonates increases. The ones lower down have to be heated more strongly than those at the top before they will decompose. The term "thermal decomposition" describes splitting up a compound by heating it. You should look at your syllabus, and past exam papers -. Asked by Wiki User. 0 0 0. Thermal decomposition is the breakdown of a compound into two or more different substances using heat; Thermal decomposition of carbonates. To test what you've learned from this lesson- Answer to question 23 the calcium ion has a larger charge (2+) thatn the potassium ion (1+). You can see that the reactions become more endothermic as you go down the Group. Lets take a look at the trend in how group 2 carbonates decompose. About this resource. The ones lower down have to be heated more strongly than those at the top before they will decompose. All of these carbonates are white solids, and the oxides that are produced are also white solids. Group-2 carbonates are fairly soluble in the solution of CO 2; Thermal Stability. Thermal decomposition is the term given to splitting up a compound by heating it. Hey guys, I had a question on why thermal stability increases down Group 2? (ii) Carbonates. docx, 35 KB. The carbonates become more stable to heat as you go down the Group. At an elementary level, the relative thermal stability of the carbonates of the metals cannot easily be explained in terms of simple ideas of bonding in these compounds. It describes and explains how the thermal stability of the compounds changes as you go down the Group. To test what you've learned from this lesson- Answer to question 23 the calcium ion has a larger charge (2+) thatn the potassium ion (1+). Story home 1 2 story home Post ; Gervald F. 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