Question 14. Note concerning #7 just above: Some older sources might include ammonium hydroxide (NH4OH) as a soluble hydroxide. (a)Na + N2 + O2 (b) NaNO2 + O2 (c) Na2O + O2 + N2 (d)NaN3 + O2 (c) It is because reduction potential depends upon sublimation energy, ionisation energy and hydration energy. Answer: Alkali metals have only one valence electron per metal atom. Which statement is true? Explain the following: That is why these metals are not obtained by chemical reduction methods. Melting point nad boiling point of particular alkali metal follow the order Fluorides > Chlorides > Bromides > Iodides. Na is liberated at the cathode. Name the alkali metal which shows diagonal relationship with magnesium? Which alkali metal cation has the highest polarising power? In the Solvay process Answer: (i) Sodium metal is manufactured by electrolysis of a fused mass of NaCl 40% and CaCl2 60% in Down’s cell at 873 K, using iron as cathode and graphite as anode. Compare the solubility and thermal stability of the following compounds of the alkali metals with those of the alkaline earth metals. Lithium shows a diagonal relationship with, (a) sodium (b) silicon (c) nitrogen (d)magnesium, (a) an ammoniacal brine solution is carbonated with CO2, forming NaHCO3 which on decomposition at 150°C produces Na2CO3, (b) a sodium amalgum reacts with water to produce NaOH which gives Na2CO3 on reacting with CO2, (c) A brine solution is made to react with BaCO3 to produce Na2CO3. Question 9. Solubility rules that apply to water solution: (1) All alkali metal (lithium, sodium, potassium, rubidium, and cesium) and ammonium compounds are soluble. Therefore lithium chloride dissolves in water. (3) Silver, lead, and mercury(I) compounds are insoluble. Magnesium atom has small size so electrons are strongly bound to the nucleus. (iii) Na2O2 + 2H20 ———> 2NaOH + H2O2. Question 2. (ii) Basicity of oxides. (d) 3. The solubility of metal halides depends on their nature, lattice enthalpy and hydration enthalpy of the individual ions. 2Cl– (melt) ——-> Cl2 (g) + 2e–. You can disable footer widget area in theme options - footer options, NCERT Solutions for Class 11 Chemistry Chapter 10 The s-Block Elements, NCERT Class 11 Chemistry Textbook Solved Questions, NCERT Solutions for Class 11 Chemistry Chapter 10 Very Short Answer Type Questions, NCERT Solutions for Class 11 Chemistry Chapter 10 Short Answer Type Questions, Question 1. Silver nitrite and potassium perchlorate are considered slightly soluble. (b) Lithium is the only alkali metal to form a nitride directly. (b) a sodium amalgum reacts with water to produce NaOH which gives Na2CO3 on reacting with CO2 Question 30. In the vapour state, it exists as a chlorobridged dimer. (iv)Sodium carbonate is obtained by Solvay ammonia process. Alkali salts are all ionic which refers to the bonding mechanism of the crystalline solid. Why is the solution of alkali metals in liquid ammonia conducting in nature? Give the chemical formula of Epsom salt. (a) Na (b) K (c) Rb (d) Cs What do you mean by diagonal relationship in periodic table? (c) Li < Cs < Rb < K < Na (d) Rb < Cs < K < Na < Li Silver nitrite and potassium perchlorate are considered slightly soluble. 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. (c) more oxidizing (d) less basic than alkali metals. Answer: Alkali metals and alkaline earth metals are most electropositive due to low ionization ethalpy therefore they form ionic hydrides, e.g. v) Solubility in liquid ammonia Why are alkali metals not found in nature? (c) 4. (iii) Quick lime Why is LiF almost insoluble in water whereas LiCl soluble not only in water but also in acetone? Answer: Limestone: Question 22. (i) NaHCO3 (ii) NaOH Question 8. Name the compounds used for the manufacture of washing soda by Solvay process. (ii) Solubility : All the carbonates of alkali metals are generally soluble in water and their solubility increase rapidly on descending the group. Question 28.Write balanced equations for reactions between. (c) MgCl2 is electrolysed. (b) high lattice enthalpy. So, solubility should decrease from Li to Cs. Question 18. Question 5. Carbonates, hydroxides, sulfates, phosphates, and heavy metal salts are often insoluble. 2. (a) 9. Answer: Question 3. At anode: Question 6. Nitrates and acetates are generally soluble. 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. Basicity of oxides of alkali metals are higher than that of alkaline earth metals. For example, a typical Group 2 nitrate like magnesium nitrate decomposes this way: (1) 2 M g (N O 3) 2 (s) → 2 M g O (s) + 4 N O 2 (g) + O 2 (g) Answer: This is due to the reason that potassium bicarbonate (KHCO3) formed as an intermediate (when CO2 gas is passed through ammoniated solution of potassium chloride) is highly soluble in water and cannot be separated by filtration. Why are alkali metals soft and have low melting points? Na (am) + e- (am) + NH3(l) ——–> NaNH2(am) + —1/2 H2(g). Answer:  Potassium and caesium have much lower ionization enthalpy than that of lithium. Due to this, K and Cs are used in photoelectric cells rather than lithium. (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. The rules form a list so when they seem to contradict, the higher one takes precedent. The exceptions are the alkali metal hydroxides and Ba (OH) 2. Answer: Sodium ions: Question 25. All nitrates are soluble. Thus, LiCO3 is decomposed at a lower temperature. Nitrate and Alkali Metal rule 3. 5. The most important slightly soluble substance is calcium hydroxide, Ca(OH)2. Most halogen (Cl¯, Br¯, I¯) salts are soluble. (a) Alkali metals show only +1 oxidation state. The Solubility Rules. The solubility results were obtained in water or aqueous solutions. (ii) Sodium carbonate (b) A cation is highly polarising if its charge/ size ratio is very high. Thus it undergoes hydrolysis to produce strong base NaOH and its aqueous solution is alkaline in nature. Sodium Nitrate. Answer: 1. 2M(NO 3) … Why is Li2CO3 decomposed at a lower temperature whereas Na2CO3 at higher temperature? The exceptions are the alkali metal hydroxides and Ba(OH) 2. Atomic size goes on increasing down the group. (i) caustic soda (ii) sodium carbonate (iii) quick lime (a) a solution of Na2CO3 is alkaline? (b) and (d) 8. Part 2. Each rule has exceptions and the important ones are noted. Essentially, all alkali metal (Li +, Na +, K +, Rb +, Cs +) and ammonium (NH 4 +) salts are soluble. Which is more basic NaOH or Mg(OH)2? Question 9. 2Na- Hg + 2H20——>2NaOH +H2 +Hg In dentistry, in ornamental work for making statues. Question 1. Potassium carbonate cannot be prepared by Solvay process. Carbonates of metal: Thermal stabilityThe carbonates of alkali metals except lithium carbonate are stable to heat. At anode: Answer: It is anhydrous calcium sulphate (CaSO4). Group 2 carbonates are insoluble in water because their Lattice energy are higher than hydration energy. Nitrates , carbonates and sulphates of Alkali metals are soluble in water . (b) Na and K impart colour to the flame but Mg does not. (b) It is used in glass manufacturing. 6. Why alkali and alkaline earth metals cannot be obtained by chemical reduction method? In fact, these metals can precipitate from their salt solutions as carbonates.Nitrates: Thermal stabilityNitrates of alkali metals,except LiNO3, decompose on strong heating forming nitrites and oxygen. In the transport of sugars and amino acids into cell. Silver and lead ion are mostly soluble, except when paired with nitrate, acetate and… Heating the nitrates. 2. compounds of the alkali metals and the ammonium ion are generally soluble. Most hydroxides (OH-) are insoluble.. 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. Lead and Silver rule 1. Give two examples. Alkali metal and nitrate salts are never soluble. (iii) Since the size of Li+ ion is very small in comparison to K+ ion, it polarises the electron cloud of I– ion to a great extent. Keep in mind that there will be slight variations from table to table. Thermal stability of carbonates of group 2 increases down the group because Lattice energy goes no increasing due to increase in ionic character. Question 7. Question 20. 1. All alkali metals hydroxides are soluble in water. Answer: Soda ash is anhydrous sodium carbonate (Na2CO3). Most hydroxides (OH -) are insoluble. osti.gov journal article: solubility in ternary water-salt systems containing cerium nitrates and alkali metal nitrates (c) more oxidizing (d) less basic than alkali metals Answer: Alkali metals are highly reactive in nature. (a) Nitrates (b) Carbonates (c) Sulphates Answer: (a) Nitrates of both group 1 and group 2 elements are soluble in water because hydration energy is more than the lattice energy. Explain the significance of sodium, potassium, magnesium and calcium in biological fluids. Halogen rule 7. 4. Which of the following is used in photoelectric cells? Answer: It is due to high lattice energy of LiF as compared to LiCl. Question 5. Extensively used in the manufacturing of high quality paper. For example,Li2CO3 +heat -> Li­2O +CO2MgCO3 +Heat -> MgO +CO2Na2CO3 +heat -> no effect.The stabilities of carbonates of alkaline earth metals increase on … Solubility of sulphates of group 2 decreases down the group because Lattice energy dominates over hydration energy. Solubilities of the halides, nitrates, carbonates, sulfates, and some perchlorates of all the alkali metals and alkaline earth metals in methanol at room temperature have been determined. Using this idea, how can we order the three rules we have so far to remove any contradictions? 2Na + Hg ——->Na – Hg + 2H20 Nitrates are soluble in water. ‘ … Alkali earth metals. Question 1. b) Alkali metal and nitrate salts are never soluble. Lithium Nitrate , JPCRD, 2010 , 39 , 033104. 2. Answer:  Alkali metals. What is the effect of heat on the following compounds (Give equations for the reactions)? 3. Name the alkaline earth metals whose salt do not impart colour to a non-luminous flame. However, in case of corresponding magnesium and calcium compounds, the cations have smaller sizes and more magnitude of positive charge. Question 20. Therefore, a large amount of energy is needed to excite their valence electron, and that’s why they do not impart colour to the flame. [ M = Be, Mg, Ca, Sr, Ba] (b) Carbonates- Na+ + e– —–> Na (l) Which alkali metal ion forms largest hydrated ion in aqueous solution? (a) What makes lithium to show properties uncommon to the rest of the alkali metals? Question 5. NCERT Solutions Class 11 Business Studies, NCERT Solutions Class 11 Entrepreneurship, NCERT Solutions Class 11 Indian Economic Development, NCERT Solutions Class 11 Computer Science. On the other hand, in lithium chloride (LiCl) the lattice enthalpy is comparatively very small. (a) Why Cs is considered as the most electropositive element? Question 14. Question 2. This means that the magnitude of hydration enthalpy is quite large. 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. Alkali metals are highly reactive in nature. Thus, it has the highest charge density and hence attracts the water molecules more strongly. (a) Sr (b) Ca (c) Be (d) Mg On heating, Beryllium nitrate forms nitrite and, other nitrates yield oxide, liberating brown fumes of nitrogen dioxide. Na + H2O —–> NaOH + 1/2H2 Nitrates , carbonates and sulphates of Alkali metals are soluble in water . In the final analysis, the table your teacher wants you to use is the most correct one for you to use. (a) Li (b) Na (c) K (d) Cs Why is LiF almost insoluble in water whereas LiCl soluble not only in water but also in acetone? (b) When is a cation highly polarising? Solubility. Question 8. (ii) Sodium hydroxide is manufactured by electrolysis of an aqueous solution of NaCl (brine) in Castner-Kellner cell. 3. At anode: All nitrates are soluble, even if it’s a lead nitrate. Volume 89: Jitka Eysseltová and Violetta Timofeevna Orlova Alkali Metal Nitrates (two parts) IUPAC Project Part 1. Alkali metals have low ionization enthalpies. As a result, the binding energy of alkali metal ions in the close-packed metal lattices are weak. Question 2. (i) Limestone (ii) Cement (iii) Plaster of Paris. Question 13. of alkaline earth metals are higher than those of the corresponding alkali metals. Order of Size of alkali metal ions in aqueous; Why alkali metals r soluble in water n thermally stable? Lead and Silver rule 2. Discuss the general characteristics and gradation in properties of alkaline earth metals. Why do alkali metals give characteristic flame colouration? EXCEPT those of ammonium (NH 4+) and Alkali metal (Group 1, or, Group IA) cations. Question 12. The oxides of calcium, strontium, and barium are basic and the hydroxides are strongly basic. (a) Na2O2 and water (a) KO2(b) CrO5(c) Na2O2 (d) BaO2 Question 3. Question 16. Explain the following: Silver acetate, mercurous acetate, and lead acetate are moderately soluble. Which out of the following can be used to store an alkali metal? Answer: BeCl2 (vapour) Halogen rule 1. Question 6. 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. Why are alkali metals always univalent? Comment on each of the following observations: Alkali metals are highly electropositive in nature. Answer: Li2CO3 is a covalent compound whereas Na2CO3 is an ionic compound. 3. Indeed, I found one website with four terms. Describe the importance of the following: Mg is the main pigment for the absorption of light in plants. Why? EXCEPT those of ammonium (NH 4+ ), … Which one of the following alkaline earth metal carbonates is thermally most stable? Thus Lil– has more covalent character than LiF. Find out the oxidation state of sodium in Na2O2. Question 9. Question  21. 1. The most common definition for solubility is this: This definition means there are only two categories: soluble and insoluble. (ii) Both BaO and BaSO4 are ionic compounds but the hydration energy of BaO is higher than the lattice energy therefore it is soluble in water. Their solubility in water increases on moving down the group because their lattice enthalpies decrease more rapidly than the hydration enthalpies. Why does the solution of alkali metals becomes blue in liquid ammonia? (i) CaC03 (ii) CaSO4 2H2O Nitrates of both group 1 and group 2 elements are thermally unstable but they decompose differently except LiCO3 e.g. (a) MgCO3 (b) CaCO3 (c) SrCO3 (d) BaCO3 That’s why they always exist in combined state in nature. At cathode: Alkali metals impart characteristic colours to the flame. Electropositive character increases on going down the group. [ Thus they need large amount of energy for excitation of electrons to higher 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. 2Cl-(aq) – 2e- ———> Cl2(g). Answer:  Sodium peroxide is formed. plays important roles in neuromuscular function. (iii) Lil is more soluble than KI in ethanol. Answer:  (i) Caustic soda Which alkaline earth metals do not impart colour to the flame? This website has definitions for soluble, insoluble and slightly soluble plus a good set of rules for solubility at the end of the file. Data on some, such as cesium and rubidium fluoride, nitrate, carbonate, and sulfate, appear to be reported for the first time. 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