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(d). Answer: Due to smallest size, Li+ can polarize water molecules easily than the other alkali metal ions. Question 1. SOLUBILITY OF THE HYDROXIDES, SULPHATES AND CARBONATES OF THE GROUP 2 ELEMENTS IN WATER This page looks at the solubility in water of the hydroxides, sulphates and carbonates of the Group 2 elements - beryllium, magnesium, calcium, strontium and barium. All the alkaline earth carbonates will neutralize an acidic solution by. Answer: MgSO4,7H2O. Answer: Since group 1 hydroxides and carbonates due to large size contain higher hydration energy than the lattice energy so, they are easily soluble in water. Question 15. Why? 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. NCERT Solutions for Class 6, 7, 8, 9, 10, 11 and 12. To neutralize excess stomach acid that causes indigestion, would you use BeCO. (c) A brine solution is made to react with BaCO3 to produce Na2CO3 (iii) Sodium peroxide: Answer: (a) Na2O2 + 2H2O ——-> 2Na0H + H2O2 Since Ionization enthalpy of potassium is less than that of sodium, potassium is more reactive than sodium. What happens when Question 19. Question 4. Question 11. Alkali metal hydroxides LiOH, NaOH, KOH, CsOH are soluble, and their solutions are basic. (c) It is because reduction potential depends upon sublimation energy, ionisation energy and hydration energy. (Acetone is polar in nature). Thus Lil– has more covalent character than LiF. Question 8. Why are lithium salts commonly hydrated and those of the other alkali metal ions usually anhydrous? Hydroxides: As you go down the group the solubilities of the group 2 hydroxides increase. Answer:  Beryllium does not impart colour to a non-luminous flame. Answer: (i) Ionization enthalpy. The greater the ease of producing OH-ions, the more alkaline is the Question 11. Why are ionic hydrides of only alkali metals and alkaline earth metals are known? Berrylium hydroxide (Be (OH) 2) and magnesium hydroxide (Mg (OH) 2) are completely insoluble in water. They are less electropositive than alkali metals. (b) Lithium cannot be used in making photoelectric cells. They are thermally stable. Share 10. Answer: Benzene can be used to store an alkali metal because other substances react with alkali metal as: Explain. drying agent for removing water from the atmosphere—CaCl, Group 2 elements almost exclusively form ionic compounds containing the M. How many liters of chlorine gas will be released at standard temperature and pressure? (c) Due to small size, lithium does not form alums. The elements have very similar properties: they are all shiny, silvery-white, somewhat reactive metals at standard temperature and pressure.. At cathode: Heating a barium-containing alloy to high temperatures will cause some ionization to occur, providing the initial step in forming a spark. For Alkaline Earth metals Group 2. Alkaline earth metals hydroxides are less soluble in water as compared to alkali metals. Question 20. Note: The h ydroxides of group 2 (the alkaline earth metals) are slightly soluble. Topics and Subtopics in NCERT Solutions for Class 11 Chemistry Chapter 10 The s-Block Elements: NCERT Solutions Class 11 ChemistryChemistry Lab ManualChemistry Sample Papers. (ii) 2Na + O2 ———> Na2O2 All enzymes that utilise ATP in phosphate transfer require magnesium as a cofactor. are solved by group of students and teacher of NEET, which is also the largest student community of NEET. Why does the solubility of alkaline earth metal hydroxides in water increase down the group ? (a) Pb (b) Mg  (c) Ca (d) Al Although it describes the trends, there isn't any attempt to explain them on this page - for reasons discussed later. 7. What is the effect of heat on the following compounds (Give equations for the reactions)? 400+ SHARES. Alkali metals hydroxides are highly basic in nature. Question 3. Question 5. Hence, alkaline earth metal hydroxides have lower solubility than alkali metals. Answer:(i) NaNO3 (ii) CaCO3 (iii) NaCl. Reactions in Water. This is due to the high lattice energies of alkaline earth metals. Question 9. Question 7. ... Reactivity of with water (and solubility of metal hydroxides) increases down the group. Answer: 1. Cl– – e– ——->Cl The Questions and Answers of What is the solubility order of fluorides for alkaline earth metals? Hydroxides of alkali earth metals are much less soluble. Answer: Fused NaOH. Whereas  BeSO4 is ionic in nature and its hydration energy dominates the lattice energy. Question 9. (a) It is used in the manufacturing of soap paper, artificial silk etc. Extensively used in the manufacturing of high quality paper. Answer: Alkali metals have only one valence electron per metal atom. Solubility of hydroxides: The hydroxides of alkaline earth metals are less soluble than those of alkali metals. Answer: (i) Ionization enthalpy. Question 1. Question 2. (b) What happens when alkali metals are dissolved in ammonia? Discuss the general characteristics and gradation in properties of alkaline earth metals. Thus it undergoes hydrolysis to produce strong base NaOH and its aqueous solution is alkaline in nature. Which is more basic NaOH or Mg(OH)2? (a) and (d) 7. Metal hydroxide Ksp Metal hydroxide Ksp Be (OH)2 1.6 × 10-26 Sr (OH)2 3.2 × 10-4 When these electrons return to the ground state, the energy is emitted in the form of light. (i) caustic soda (ii) sodium carbonate (iii) quick lime Answer: Question 12. (c) 4. (a) Na (b) K (c) Rb (d) Cs Which of the following is used in photoelectric cells? Potassium carbonate cannot be prepared by Solvay process. If hydration energy is greater than lattice energy then the compound is soluble in water. 5.2.1 General characteristics of alkali metals: Alkali metals are highly reactive and are found in nature only as compounds. Answer: All the compounds are crystalline solids and their solubility in water is guided by both lattice enthalpy and hydration enthalpy. Share with your friends. Here we shall look at the solubilities of the hydroxides and sulfates of Group 2 metals. Question 8. What happens when it is added to water? It is prepared by heating CaC2 with N2 at high temperature. (b) and (d) 8. A Chloride 8 A Hydroxide C. A Carbonate H. A Nitrate D. An Iodide I. Compare the solubility and thermal stability of the following compounds of the alkali metals with those of the alkaline earth metals. Why are alkali metals soft? Compare the alkali metals and alkaline earth metals with respect to (i) ionization enthalpy, (ii) basicity of oxides, (iii) solubility of hydroxides. (b) a sodium amalgum reacts with water to produce NaOH which gives Na2CO3 on reacting with CO2 Question 6. Answer:  Because alkali and alkaline earth metals are themselves stronger reducing agents than the majority of other reducing agents. (b) Used in the purification of sugar and in the manufacturing of cement. Answer: (a) Nitrates of both group 1 and group 2 elements are soluble in water because hydration energy is more than the lattice energy. plays important roles in neuromuscular function. Therefore, these are soft and have low melting point. Why alkali and alkaline earth metals cannot be obtained by chemical reduction method? 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. Thus they show an oxidation state of +1 and are strongly electropositive. Question 10. Solubility of Hydroxides and Flourides INCREASES from top to bottom. Answer: Due to ammoniated electrons and cations. (iii) Sodium peroxide (iv) Sodium carbonate? Question 5. Because BeO and MgO are much more inert than the other group 2 oxides, they are used as refractory materials in applications involving high temperatures and mechanical stress. Answer:  Potassium and caesium have much lower ionization enthalpy than that of lithium. (i) Chile salt petre (ii) Marble (iii) Brine Question 5. (b) Lithium is the only alkali metal to form a nitride directly. MgCl2, CaCl2, SrCl2, BaCl2 How many hours will it take to process the magnesium metal if a total current of 1.00 × 10. At anode: Question 4. Find out the oxidation state of sodium in Na2O2. It is also soluble in acetone due to dipolar attraction. Thus Lil dissolves in ethanol more easily than the KI. Question 15. Question 31. (iii) Lil is more soluble than KI in ethanol. Question 23. Properties of alkali and alkaline earth metals hydroxides in periodic table. Alkali metals impart characteristic colours to the flame. Basicity of oxides of alkali metals are higher than that of alkaline earth metals. Answer: Since the atoms of alkali metals have bigger kernels and smaller number of valence electrons, the metallic bonds in them are very weak and hence are soft. Answer: Question 13. Question  21. 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. 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. When heated to 800°C, NaN03 gives, Question 4. To be familiar with the reactions, compounds, and complexes of the alkaline earth metals. Solubility in water is related to the ionic nature and size. The oxide of which of the following metals is amphoteric? Alkali metals are highly electropositive in nature. Group 1 These hydroxides are the strongest bases in the aqueous medium and are highly corrosive. In what ways lithium shows similarities to magnesium in its chemical behaviour? Question 28.Write balanced equations for reactions between. This means that the magnitude of hydration enthalpy is quite large. (ii) Sodium metal is heated in free supply of air? The elements in Group 2 are called the alkaline earth metals. Alkaline earth metals are (b) alkali metals are prepared by electrolysis of their fused chlorides? Question 2. Question 4. The alkaline earth metals are six chemical elements in group 2 of the periodic table.They are beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra). Answer: It is due to high lattice energy of LiF as compared to LiCl. Answer: (a) Na2CO3 is a salt of a weak acid, carbonic acid (H2CO3) and a strong base NaOH. (a) KO2(b) CrO5(c) Na2O2 (d) BaO2 Therefore, it is almost insoluble in water. Which alkali metal ion forms largest hydrated ion in aqueous solution? Question 20. Alkali metals exhibit +1 oxidation states in their compounds. Therefore, Lattice energy of Na2CO3 is higher than that of Li2CO3. (c) Na2O+ CO2 ———–>Na2CO3. Why do alkali metals give characteristic flame colouration? Mg is the main pigment for the absorption of light in plants. Why does the solubility of alkaline earth metal hydroxides on water increase down the group. 400+ VIEWS. Why is Li2CO3 decomposed at a lower temperature whereas Na2CO3 at higher temperature? Answer: (i) Lattice energy of BeO is compartively higher than the hydration energy. Alkali metals have low ionization enthalpies. (a) an ammoniacal brine solution is carbonated with CO2, forming NaHCO3 which on decomposition at 150°C produces Na2CO3 Which of the following is used in photoelectric cells? (a) Nitrates (b) Carbonates (c) Sulphates Describe two important uses of each of the following: , For solubility hydration, energy > lattice energy.Hydration energy varies inversely with size, ie, decreases with increase in size. The hydroxides become more soluble as you go down the Group. What is the mixture of CaC2 and N2 called? Solubility of the Hydroxides. Give the important uses of the following compounds. When heated to 800°C, NaN03 gives Question 19. Answer:  It is called Nitrolime. Answer:  Be and Mg. Answer: BeCl2 (vapour) (c) Ee for M2+ (aq) + 2e– —> M(s) (where M = Ca, Sr, or Ba) is nearly constant. On the other hand, in lithium chloride (LiCl) the lattice enthalpy is comparatively very small. Na + C2H5OH ——–> C2H5ONa + ½ H2. Why Solubility of Alkaline Earth Metals decreases down the Group? (i) Limestone (ii) Cement (iii) Plaster of Paris. Answer: Size of Cs is the biggest thus, its melting point is the lowest, (d) is correct. Why is LiF almost insoluble in water whereas LiCl soluble not only in water but also in acetone? Question 8. However, if you shake it with water, filter it and test the pH of the solution, you find that it is slightly alkaline. Answer: (i) 2Na + 2H2O ——–> 2NaOH + H2 Atomic size goes on increasing down the group. The oxide of which of the following metals is amphoteric? Why is the solution of alkali metals in liquid ammonia conducting in nature? (c) 10. As a result, the binding energy of alkali metal ions in the close-packed metal lattices are weak. They have a strong tendency to lose 1 electron to form unipositive ions. Question 7. Beryllium and magnesium do not give colour to flame whereas other alkaline earth metals do so.

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