all metals, generally soft and highly reactive. (c) Lithium on being heated in air mainly forms the monoxide and not the peroxide. Answer: Question 3. (c) Sulphates of group 1 are soluble in water except Li2SO4. Alkali metals dissolve in liquid ammonia to form blue and conducting solution. (a) a solution of Na2CO3 is alkaline? Although it describes the trends, there isn't any attempt to explain them on this page - for reasons discussed later. However, in case of corresponding magnesium and calcium compounds, the cations have smaller sizes and more magnitude of positive charge. Question 6. (c) Lithium does not form alums. (iii) Sodium peroxide: (iii) Na2O2 + 2H20 ———> 2NaOH + H2O2. (d)Since, among alkali metals, lithium has the most negative electrode potential (E° = -3.04 V) so, it is the strongest reducing agent in the aqueous solution. (ii) Sodium carbonate (b) Used in the purification of sugar and in the manufacturing of cement. The Questions and Answers of What is the solubility order of fluorides for alkaline earth metals? What happens when sodium metal is heated in free supply of air? Why? Whereas BeSO4 is ionic in nature and its hydration energy dominates the lattice energy. What happens when it is added to water? Answer: Soda ash is anhydrous sodium carbonate (Na2CO3). State as to why Question 24. Solubility of sulphates of group 2 decreases down the group because Lattice energy dominates over hydration energy. Solubility of hydroxides: The hydroxides of alkaline earth metals are less soluble than those of alkali metals. (ii) BaO is soluble but BaSO4is insoluble in water. (b) and (d) 8. Answer: (a) According to Fazan’s rule, Li+ ion can polarise l– ion more than the F– ion due to bigger size of the anion. are solved by group of students and teacher of NEET, which is also the largest student community of NEET. All the alkaline earth carbonates will neutralize an acidic solution by. … 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 hydration energy of the cation remains almost unchanged. Give the chemical equation also. Question 12. They are thermally stable. What happens when crystals of washing soda are exposed to air? (b) Carbonates of group 1 elements are soluble in water except Li2CO3 They are also thermally stable except Li2CO3 Thus, LiCO3 is decomposed at a lower temperature. (a) Lithium iodide is more covalent than lithium fluoride. The increasing solubility of the hydroxides on moving down the group is evident from their solubility products. (b) 2KO2 + 2H2O ———-> 2K0H + O2+ H2O2 (ii) 2Na + O2 ———> Na2O2 Question 8. Sodium hydroxide, NaOH, also known as caustic soda or lye, is of great industrial importance. What is dead burnt plaster? Which alkali metal ion forms largest hydrated ion in aqueous solution? As a component of the alloy in an automotive spark plug electrode, would you use Be, Ca, or Ba? Due to this, K and Cs are used in photoelectric cells rather than lithium. Therefore lithium chloride dissolves in water. Question 9. Therefore, Lattice energy of Na2CO3 is higher than that of Li2CO3. (a) It is used in the manufacturing of soap paper, artificial silk etc. Question 7. (ii) Sodium hydroxide is manufactured by electrolysis of an aqueous solution of NaCl (brine) in Castner-Kellner cell. Answer: (i) Lattice energy of BeO is compartively higher than the hydration energy. 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Discuss the general characteristics and gradation in properties of alkaline earth metals. Name the alkali metal which shows diagonal relationship with magnesium? Na 2 S + H 2 O → 2NaOH + H 2 S. P block metal sulfides solubility and colors. Reactions in Water. For Alkaline Earth metals Group 2. (d) 3. (b) Lithium cannot be used in making photoelectric cells. Question 21. (c) Due to small size, lithium does not form alums. Answer: Sodium ions: Question 25. Alkali metal hydroxides LiOH, NaOH, KOH, CsOH are soluble, and their solutions are basic. (a) Used in the softening of water, for laundry and cleaning purposes. (i) CaC03 (ii) CaSO4 2H2O That is why these metals are not obtained by chemical reduction methods. Below is a metal hydroxide solubility curve showing the solubility of the common heavy metal ions and their respective solubility versus pH. (i) NaHCO3 (ii) NaOH It is prepared by heating CaC2 with N2 at high temperature. 800+ VIEWS. The hydroxides become more soluble as you go down the Group. Question 20. Answer: (a) The unusual properties of lithium as compared to other alkali metals is due to its exceptionally small size of atom and its ion and its high polarising power. Beryllium ion is the most soluble and the solubility decreases with increasing size so that Barium ion is the least water-soluble alkaline earth metal ion. (a) 2. Both react with nitrogen to form nitrides. The extent of hydration decreases in the order. In what ways lithium shows similarities to magnesium in its chemical behaviour? Compare the solubility and thermal stability of the following compounds of the alkali metals with those of the alkaline earth metals. CaC2 + N2 ——–> CaCN2 + C, Question 1. The explanation for the trends in solubility is given in chapter 3.17 enthalpies of solution The pH of an aqueous solution of a hydroxide depends on the extent to which the metal hydroxide can be split to produce independent ions. LiCl is soluble in water because its hydration energy is higher than its lattice energy. Question 1. Answer: Alkali metals dissolve in liquid ammonia and give deep blue solutions which are conducting in nature because ammoniated electrons absorb energy in the visible region of light and impart blue colour. Lithium shows a diagonal relationship with, (a) sodium (b) silicon (c) nitrogen (d)magnesium, (a) an ammoniacal brine solution is carbonated with CO, (b) a sodium amalgum reacts with water to produce NaOH which gives Na, (c) A brine solution is made to react with BaCO. (ii) Sodium metal is heated in free supply of air? Why is LiF almost insoluble in water whereas LiCl soluble not only in water but also in acetone? Answer: Question 3. Both lattice enthalpy and hydration enthalpy decreases down the group as the size of the cation increases but lattice enthalpy decreases more rapidly than the hydration enthalpy and hence the solubility increases down the group. Their resultant is almost constant for these ions. (i) Sodium metal (ii) Sodium hydroxide Answer: Beryllium does not impart colour to a non-luminous flame. Here we shall look at the solubilities of the hydroxides and sulfates of Group 2 metals. Why does the solution of alkali metals becomes blue in liquid ammonia? Atomic size goes on increasing down the group. Alkali metals are highly electropositive in nature. Therefore, these are soft and have low melting point. Question 3. (a) Share 10. The elements in Group 2 are called the alkaline earth metals. A Chloride 8 A Hydroxide C. A Carbonate H. A Nitrate D. An Iodide I. (iii) Solubility of hydroxides: Alkaline earths have larger lattice energies than alkali metals due to small size and high charge. Why are alkali metals not found in nature? The reducing property of alkali metals follows the order, (a) Na < K < Rb < Cs < Li (b) K < Na < Rb < Cs < Li, (c) Li < Cs < Rb < K < Na (d) Rb < Cs < K < Na < Li. The hydroxides and carbonates of sodium and potassium are easily soluble in water while the corresponding salts of magnesium and calcium are sparingly soluble in water. When heated to 800°C, NaN03 gives Solubility of group 2. Answer: 1. (a) sodium (b) silicon (c) nitrogen (d)magnesium Question 5. Only strontium hydroxide (Sr (OH) 2) and barium hydroxides (Ba (OH) 2) are completely soluble from alkaline earth metals. (a) Pb (b) Mg (c) Ca (d) Al In case of sodium and potassium compounds, the magnitude of lattice enthalpy is quite small as compared of sodium and potassium that are mentioned, readily dissolve in water. Answer: They are always univalent because after losing one electron, they aquire nearest inert gas configuration.Li+ forms largest hydrated cations because it has the highest hydration energy. For example, quicklime ( CaO ) reacts with water to give lime... Carbonate H. a Nitrate D. an Iodide i ionization enthalpy of LiF is maximum among all the alkaline earth.! 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Period with diagonally situated element of second period with diagonally situated element second... Are weak return to the rest of the first element of neighbouring element is called diagonal relationship in periodic?...
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