(d) 3. Question 5. Heating a barium-containing alloy to high temperatures will cause some ionization to occur, providing the initial step in forming a spark. 2Na + Hg ——->Na – Hg + 2H20 Which out of the following can be used to store an alkali metal? Explain the significance of sodium, potassium, magnesium and calcium in biological fluids. For Alkaline Earth metals Group 2. This means that the magnitude of hydration enthalpy is quite large. They are thermally stable. Why are alkali metals not found in nature? Answer: Question 13. The elements have very similar properties: they are all shiny, silvery-white, somewhat reactive metals at standard temperature and pressure.. (c) Ee for M2+ (aq) + 2e– —> M(s) (where M = Ca, Sr, or Ba) is nearly constant. (c) 4. Answer: Monohydrate (Na2CO3– H2O) is formed as a result of efflorescence. Hydroxides of alkali earth metals are much less soluble. Alkali metals are highly reactive in nature. Question 4. Which alkaline earth metals do not impart colour to the flame? Na2CO3(s) + H2O(l)———–>2NaOH Na is liberated at the cathode. (c) more oxidizing (d) less basic than alkali metals. 7 3 alkaline earth metals difference between alkali and metal alkaline earth metal oxides solved 3 the following were exe Introduction The Elements In Which Last Electron EntersGroup 2 Alkaline Earth Metals ScienceaidAlkali And Alkaline Earth MetalsXps Results For The Alkali And Alkaline Earth Oxides Hydrox IdesAlkaline Earth Hydroxides In Water And Aqueous Solutions VolumeFor… Question 10. They are less electropositive than alkali metals. (a)Na + N2 + O2 (b) NaNO2 + O2 (c) Na2O + O2 + N2 (d)NaN3 + O2 (b) a sodium amalgum reacts with water to produce NaOH which gives Na2CO3 on reacting with CO2 Question 8. Question 32. Question 5. Solubility of the Hydroxides. (c) A brine solution is made to react with BaCO3 to produce Na2CO3 Answer: (i) Ionization enthalpy. (c) Since potassium is move reactive than sodium and it is found in nature to a less extent than Na, sodium is found to be more useful. Explain the reason for this type of colour change. (ii) Basicity of oxides. Why are alkali metals always univalent? The solubility of the alkaline earth metal hydroxides in water increases with increase in atomic number down the group. Answer:  Beryllium does not impart colour to a non-luminous flame. Answer: All the compounds are crystalline solids and their solubility in water is guided by both lattice enthalpy and hydration enthalpy. Question 20. (a) Compare four properties of alkali metals and alkaline earth metals. Question 10. Answer: (a) Na2CO3 is a salt of a weak acid, carbonic acid (H2CO3) and a strong base NaOH. Since Ionization enthalpy of potassium is less than that of sodium, potassium is more reactive than sodium. The hydroxides of the alkali metals, lithium, sodium, potassium, rubidium, and cesium, are the strongest bases and the most stable and most soluble of the hydroxides. In dentistry, in ornamental work for making statues. Which of the following is not a peroxide? They form oxides and hydroxides and these compounds are basic in nature. Magnesium atom has small size so electrons are strongly bound to the nucleus. When heated to 800°C, NaN03 gives (c) Na2O and CO2 alkali metals with those of the alkaline earth metals. Why is LiF almost insoluble in water whereas LiCl soluble not only in water but also in acetone? Question 30. 800+ SHARES. A Chloride 8 A Hydroxide C. A Carbonate H. A Nitrate D. An Iodide I. Why? Reactions in Water. Question 3. (a) What makes lithium to show properties uncommon to the rest of the alkali metals? How is it prepared? Explain the following: Question 1. (d) 5. Question 29. Alkali metals due to lower ionization enthalpy are more electropositive than the corresponding group 2 elements. (c) Sulphates of group 1 are soluble in water except Li2SO4. Li+ ion has the highest polarising power. (a) Pb (b) Mg  (c) Ca (d) Al It is also soluble in acetone due to dipolar attraction. Question 9. Alkali metals have low ionization enthalpies. Question 3. Explain. NaH, KH and CaH2, Question  8. Group 2 carbonates are insoluble in water because their Lattice energy are higher than hydration energy. To neutralize excess stomach acid that causes indigestion, would you use BeCO. Answer:  (a) Alkali metals have low ionization enthalpies. What are the common physical and chemical features of alkali metals? Answer: Size of Cs is the biggest thus, its melting point is the lowest, (d) is correct. When added to water, the first alkaline earth metal (Beryllium) is totally unreacative, and doesn't even react with steam.Then as you move down the group, the reactions become increasingly vigourous.. As an example, the following reaction takes place between magnesium and water, an alkali earth metal hydroxide and hydrogen gas is produced. 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? Question 2. Write the chemical formula of the following compounds. 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. (iii) Sodium peroxide (iv) Sodium carbonate? Question 19. Solubility of Carbonates and Sulphates DECREASES from top to bottom. Na (am) + e- (am) + NH3(l) ——–> NaNH2(am) + —1/2 H2(g). Question 11. Question 8. (iii) Quick lime (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. Rubidium and caesium are found associated in minute quantities with minerals of other alkali metals. Question 4. 6. (ii) Sodium hydroxide is manufactured by electrolysis of an aqueous solution of NaCl (brine) in Castner-Kellner cell. Answer: Due to small size, the ionization enthalpies of Be and Mg are much higher than those of other alkaline earth metals. (d) Li is the best reducing agent in aqueous solution. Sodium hydroxide, NaOH, also known as caustic soda or lye, is of great industrial importance. (a) and (d) 7. Alkali metals exhibit +1 oxidation states in their compounds. Atomic size goes on increasing down the group. Answer: Alkali metals and alkaline earth metals are most electropositive due to low ionization ethalpy therefore they form ionic hydrides, e.g. In what ways lithium shows similarities to magnesium in its chemical behaviour? (c) Sodium is found to be move useful than potassium? 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. All the alkaline earth carbonates will neutralize an acidic solution by. Question 2. 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. State as to why Question 31. Describe the importance of the following: 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. 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