JIPMER 2014: The correct order of solubility of the sulphates of alkaline earth metals in water is Be > Mg > Ca > Sr > Ba. The ionic mobility of alkali metal ions in aqueous solution is maximum for KO2 (potassium super oxide) is used in oxygen cylinders in space and submarines One mole of magnesium nitride on the reaction The outermost shell has electrons which experience lesser nuclear charge as the radius goes on increasing. Ionic radius b) lonization enthalpy Density d) Melting point Electropositive character 5) Compare and contrast the chemistry of group 1 elements with that of group 2 on the basis of the following: Nature of oxides b) Solubility and thermal stability Polarizing power of cations Reactivity and reducing power 6) Groups 1 and 2 metals could form (1) hydroxides and (m) sulphates. The Nuffield Data Book quotes anyhydrous beryllium sulfate, BeSO 4, as insoluble, whereas the hydrated form, BeSO 4.4H 2 O is soluble, with a solubility of about 39 g of BeSO 4 per 100 g of water at room temperature. Correct order of acidic strength is : View solution. This trend can be explained by the decrease in the lattice energy of the hydroxide salt and by the increase in the coordination number of the metal ion as you go down the column. This is because some magnesium hydroxide has dissolved. Have questions or comments? Since hydration energy is inversely proportional to radius of ion, I would expect Lithium to release the largest hydration energy and thus be the most soluble. The atomic radiusis: Find out the solubility of $Ni(OH)_2$ in 0.1 M NaOH. In Wolff‐Kishner reduction, the carbonyl group of aldehydes and ketones is converted into. The bicarbonate of alkali metal which does not exist in solid state is: Barium hydroxide is soluble enough to produce a solution with a concentration around 0.1 mol dm. As far as the solubility of sulphates of alkaline earth metal in water is concerned BeSO 4 and MgSO 4 are highly soluble , CaSO 4 is sparingly soluble, but the sulphates of Sr, Ba and Ra are virtually insoluble. Hence the solubility of sulphates of alkaline earth metal decreases down the group mainly due to decreasing hydration enthalpy from Be2+ to Ba2+. Of the following, which species is primarily obtained in a solution containing $ KHF_2 $ ? This is due to the fact that the lattice energy decreases down the group due to increase in size of the alkaline earth metals cation whereas the … MO + SO 3 ↑ (ii) The sulphates of alkaline metals Na and K are soluble in water. Thus the order: Concerning a) CaSO 4 , although sulfates tend to be soluble, Rule #5 indicates that calcium sulfate is an important exception to this rule. As a result atomic density increases. Case 1: As we go down the periodic group of alkaline earth metal, the size of atoms increase. All alkali metal and alkaline earth (Be 2+, Mg 2+, Ca 2+, Sr 2+, Ba 2+, Ra 2+) sulfides are soluble. This is due to (A) decreasi The lattice energy remains constant because sulphate ion is so large, so that small change in cationic sizes do not make any difference. Log in. The oxides of calcium, strontium, and barium are basic and the hydroxides are strongly basic. Each of these elements contains two electrons in their outermost shell. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. This is due to, In the periodic table, the period number corresponds to, First ionisation enthalpy of $\ce{Al}$ is lower than that of $\ce{Mg}$. Included in these metals are beryllium(Be), magnesium(Mg), strontium(Sr), barium(Ba) and radium(Ra). Solubility of sulphates: The solubility of sulphates of alkaline earth metals decreases as we move down the group from Be to Ba due to the reason that ionic size increases down the group. Physics. Data on some, such as cesium and rubidium fluoride, nitrate, carbonate, and sulfate, appear to be reported for the first time. … Magnesium carbonate, for example, has a solubility of about 0.02 g per 100 g of water at room temperature. The correct order of the solubility of alkaline- earth metal sulphates in water is : The correct order of the solubility of alkaline- earth metal sulphates in water is : Skip navigation Watch the recordings here on Youtube! MgO is basic and Mg(OH)2 is weakly basic and do not dissolve in NaOH solution. The solubility of alkaline metal carbonates and sulphates decreases with decrease in hydration energy as we move down the group. Which of the following is the weakest base? As far as the solubility of sulphates of alkaline earth metal in water is concerned BeSO 4 and MgSO 4 are highly soluble , CaSO 4 is sparingly soluble, but the sulphates of Sr, Ba and Ra are virtually insoluble. Thus, order is Contrary to alkali metal sulphates, beryllium sulphate is water-soluble. The smaller size and the charge density increases the hydration energy of the beryllium sulphate leading to more solubility. Although it describes the trends, there isn't any attempt to explain them on this page - for reasons discussed later. Thus the order: Identify compound X in the following sequence of reactions: Identify a molecule which does not exist. As you can see the electronegativities of the metals decrease down the column making the change in electronegativities increases down the group. Notice that a solution, and not a precipitate, is formed, implying that magnesium sulfate is soluble. Chemistry. Since hydration energy is inversely proportional to radius of ion, I would expect Lithium to release the largest hydration energy and thus be the most soluble. MO + SO 3 ↑ (ii) The sulphates of alkaline metals Na and K are soluble in water. 5.4k SHARES. The volume strength of $3.0\, N\, H_2O_2$ is, Non-stoichiometric hydrides are formed by, The correct order of solubility of the sulphates of alkaline earth metals in water is $Be > Mg > Ca > Sr > Ba$. The LibreTexts libraries are Powered by MindTouch® and are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. The heat of formation of the reaction, $\ce{ SO_{2} +\frac{1}{2}O_{2} -> SO_3}$ will be. 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