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I used Fajan's rule to check for ionic character but … Thus more basic hydroxides down the group also thermal stability of hydroxide increases down the group. Next, high temperature and pressure curing conditions were designed to ensure a higher degree of M-A-H conversion in the samples after 2 years of curing. The salt containing one or more atoms of oxygen such as oxides ,hydroxides ,carbonate ,bicarbonate ,nitrite ,nitrate ,sulphates ,oxalates and phosphates are called oxo salts. Thermal stability 1. Correct option: (d) Ba(OH) 2 < Sr(OH) 2 < Ca(OH) 2 < Mg(OH) 2 Explanation: Stability of ionic compounds decreases with decrease in lattice enthalpy. 2. Thermal stability increases on descending the group. This decreases the charge density and the ability of the cation to polarize the anion. 3) Anhydrous CaCl 2 is also used as a desiccant ( drying agent in laboratory). The effect of curing time on the thermal stability of hydroxyl group of the hardened samples was studied by thermal analysis at 140.-days, 255.-days and 2-year of hydration at room temperature. The hydroxides of the Group II metals, which may be used in thermochemical water-splitting cycles, have been investigated thermoanalytically. Decomposition becomes more difficult and thermal stability increases. 3. Thus stability of alkaline earth metal hydroxides decreases with decrease in lattice enthalpy as the size of alkali earth metal cations increases down the group. 2. EL8: Group 1 and group 2 metals, ionisation enthalpy, charge density and thermal stability, oxides and hydroxides of group 2 What are group 1 and group 2 metals cal… What is … When the hydroxides of the s-block metals are discussed, it's easier to separate between the group 1 elements and the group 2 elements. Henry's law constant for CO 2 in water is 1.67 x 10 8 Pa at 298 K. Calculate the quantity of CO 2 in 500 mL of soda water when packed under 2.5 atm CO 2 pressure at 298 K. Q:- Calculate the mole fraction of benzene in solution containing 30% by mass in carbon tetrachloride. This is an example of the diagonal relationship. So what causes this trend? Charge Density and Polarising Power of Group 2 Metal Cations. Thus stability of alkaline earth metal hydroxides decreases with decrease in lattice enthalpy as the size of alkali earth metal cations increases down the group. iii) Reaction with hydrogen: Hydrogen reacts with alkali metals to form hydride M+H-. Decomposition temperatures and decomposition enthalpies of the four hydroxides increase with increasing atomic weight of the compounds. 4) Anhydrous MgCl 2 is used in the electronic extraction of magnesium.. Solubility and thermal stability of Oxo salts. Why is it that thermal stability of alkali metal hydrides decreases down the group, but for carbonates, it increases? Lithium often follow the pattern of Group II rather than Group I. Mg 2+ has a small size and high charge so its charge density is considered high in Group 2. Going down group II, the ionic radii of cations increases. The electron cloud of anion is distorted to a lesser extent. Group 1 These hydroxides are the strongest bases in the aqueous medium and are highly corrosive. Reactivity increases down the group as electro positive character increases down the group. 1. group increases. 3. The increasing thermal stability of Group 2 metal salts is consistently seen. Solution: Stability of ionic compounds decreases with decrease in lattice enthalpy. Let's use MgCO 3 as an example. Even for hydroxides we have the same observations. The respective TG- and DSC-curves are represented. Carbonates and hydroxides of Group I metals are as a whole more stable than those of Group II. 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