Electronic configuration<\/strong><\/td>\nElectronic configuration = 1. Thus, 1electro in the outermost valence shell.<\/p>\n Example: \nH=1<\/strong>;\u00a0Li=2,\u00a01<\/strong>;\u00a0Na=2,8,1<\/strong>; K=2,8,8,1<\/strong><\/td>\n\n One electron less than the nearest noble gas.<\/p>\n Example: \nH= 1 (He=2) \nF= 2,7 (Ne=2,8) \nCl= 2,8,7 (Ar=2,8,8)<\/p>\n<\/td>\n<\/tr>\n | \nIon formation<\/strong><\/td>\nElectropositive character exhibited.<\/p>\n H 1e–<\/sup> \u2192 H1+ \n<\/sup>Li 1e–<\/sup>\u00a0\u2192 Li1+ \n<\/sup>Na 1e–<\/sup>\u00a0\u2192 Na1+<\/sup><\/td>\nElectronegative character exhibited.<\/p>\n H + 1e–<\/sup>\u00a0\u2192 H1- \n<\/sup>F + 1e–<\/sup>\u00a0\u2192 F1- \n<\/sup>Cl\u00a0+ 1e–<\/sup>\u00a0\u2192 Cl1-<\/sup><\/td>\n<\/tr>\n\nValency<\/strong><\/td>\nElectrovalency\u00a0of one exhibited.<\/p>\n H1+<\/sup>\u00a0,\u00a0Li1+\u00a0<\/sup>, Na1+<\/sup><\/td>\n\n Electrovalency\u00a0and\u00a0covalencyexhibited.<\/p>\n Hydrogen<\/strong>:<\/p>\nforms\u00a0NaH\u00a0(electrovalent)forms CH4<\/sub>(covalent)<\/p>\nChlorine<\/strong>:<\/p>\nforms\u00a0NaCl\u00a0(electrovalent) \nforms CCl4<\/sub>\u00a0(covalent)<\/p>\n<\/td>\n<\/tr>\n\nReactions<\/strong><\/td>\nStrong affinity for non-metals (example: O, S,\u00a0Cl)<\/p>\n Hydrogen<\/strong>: forms H2<\/sub>O; H2<\/sub>S;\u00a0HCl<\/p>\nSodium<\/strong>: forms Na2<\/sub>O; Na2<\/sub>S;\u00a0NaCl<\/td>\n__<\/td>\n<\/tr>\n | \nReducing agent<\/strong><\/td>\nActs as a reducing agent.<\/p>\n Hydrogen<\/strong>:<\/p>\nCuO\u00a0+\u00a0H2<\/sub>\u00a0\u2192 Cu\u00a0+\u00a0H2<\/sub>O<\/p>\nSodium<\/strong>:<\/p>\nCuO\u00a0+\u00a02Na \u2192\u00a0Cu\u00a0+\u00a0Na2<\/sub>O<\/td>\n__<\/td>\n<\/tr>\n | \nAtomicity<\/strong><\/td>\n__<\/td>\n | \n Diatomic molecules are formed. (Two atoms linked by a single bond)<\/p>\n Hydrogen \n<\/strong>H:H or H-H \u2192\u00a0H2<\/sub>\u00a0<\/p>\nChlorine \n<\/strong>Cl:Cl\u00a0or\u00a0Cl-Cl \u2192\u00a0Cl2<\/sub><\/p>\n<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\nResemblance with Halogens:<\/u><\/p>\n\n- Both exist in the form of diatomic molecules.<\/li>\n
- Both show gaseous nature.<\/li>\n
- Both have a valency of 1.<\/li>\n
- Both are non-metals.<\/li>\n
- Both lose electron to term anions.<\/li>\n<\/ol>\n
Solution 3.<\/strong><\/span><\/p>\n(a) Hydrogen is found in minute traces in the Earth’s crust and the Earth’s atmosphere. The atmosphere around the sun and stars is found to contain 1.1 % hydrogen.<\/p>\n (b) Henry Cavendish when prepared this gas from iron and dil. acids, he established its elementary nature and showed that when the gas burns in air, water is formed. It was on account of this property that Lavoisier in 1783 named it hydrogen (Greek word meaning water-former).<\/p>\n Solution 4.<\/strong><\/span><\/p>\n(a)\u00a0A\u00a0monovalent<\/span>\u00a0metal \n2Na\u00a0+\u00a0H2<\/sub>\u00a0\u2192 2NaH \n(Sodium hydride)<\/p>\n(b)\u00a0A divalent metal \nCa\u00a0+\u00a0H2<\/sub>\u00a0\u2192 CaH2 \n<\/sub>(Calcium hydride)<\/p>\nSolution 5.<\/strong><\/span><\/p>\n(a) Calcium:<\/strong>\u00a0is not used in lab preparation of hydrogen because:<\/p>\n\n- The reaction and very violent and exothermic hence dangerous.<\/li>\n
- The heat liberated ignites the hydrogen.<\/li>\n
- Calcium is expensive.<\/li>\n<\/ol>\n
(b) Iron:<\/strong>\u00a0Iron reacts slowly at ordinary temperatures, hence requires heating. The hydrogen produced also contain impurities like\u00a0sulphur\u00a0dioxide and hydrogen\u00a0sulphide. Hence, it is not used in lab preparation of hydrogen.<\/p>\n(c)\u00a0Aluminium:<\/strong>\u00a0It is not used in the lab preparation of hydrogen because oxides of this metal keep sticking to the surface of the metal. Thus the steam does not come in contact with metal and hence reaction stops.\u00a0.<\/p>\n(d) Sodium:<\/strong>\u00a0It is riot used in the lab preparation of hydrogen because the reaction is violent. The sodium melts into a globule and darts about freely on the surface of water hence the collection of hydrogen is difficult.<\/p>\nSolution 6.<\/strong><\/span><\/p>\nDepending upon the nature of reaction taking place between metals and substances like air, water and acids, metals are arranged in a vertical series in order of their activity. Such a series is called activity series of metals.<\/p>\n The metals places near the\u00a0top<\/strong>\u00a0of the series are the\u00a0most reactive<\/strong>, while those placed near the\u00a0bottom<\/strong>\u00a0are the\u00a0least reactive<\/strong>.<\/p>\nWhen dilute hydrochloric acid or dilute\u00a0sulphuric\u00a0acid react with the metals above hydrogen in the activity series, they produce hydrogen. But the metals below hydrogen in the activity series do not.<\/p>\n Solution 7.<\/strong><\/span><\/p>\n(a)\u00a0Reactants:<\/strong>\u00a0Nitrogen and hydrogen\u00a0(Haber process)<\/strong><\/p>\nChemical equation: \n \n<\/strong><\/p>\nObservation and conditions \n<\/strong>Three volumes of hydrogen and one volume of nitrogen react at temperature 450o<\/sup>C-500o<\/sup>C at the pressure of 200-900\u00a0atm, in presence of a finely divided iron which acts as a catalyst, and promoter molybdenum.<\/p>\n(b)\u00a0Reactants:<\/strong>\u00a0Chlorine and hydrogen<\/p>\nChemical equation:<\/strong> \n<\/p>\nObservation and conditions \n<\/strong>Hydrogen and chlorine (in their equal volumes) react slowly in diffused sunlight but reacts explosively in direct sunlight. A spontaneous reaction takes place with the release of a large amount of energy.<\/p>\n(c)\u00a0Reactants:<\/strong>\u00a0Sulphur\u00a0and hydrogen<\/p>\nChemical equation: \n<\/strong>H2<\/sub>\u00a0+ S \u2192\u00a0H2<\/sub>S \n<\/strong><\/p>\nObservation and conditions \n<\/strong>Hydrogen gas when passed through molten\u00a0sulphur, it reacts to give another gas, hydrogen\u00a0sulphide.<\/p>\n(d)\u00a0Reactants:<\/strong>\u00a0Oxygen and hydrogen<\/p>\nChemical equation: \n<\/strong>2H2<\/sub>\u00a0+ O2<\/sub>\u00a0\u2192 2H2<\/sub>O \n<\/strong><\/p>\nObservation and conditions \n<\/strong>Hydrogen burns with a\u00a0pop sound<\/strong>\u00a0in oxygen. It burns with a pale blue flame forming water.<\/p>\nSolution 8.<\/strong><\/span><\/p>\n(a)\u00a0<\/strong>Among the given metals Zinc is most suitable. \n(i) Copper: In case of copper, It is placed below hydrogen in the activity series. So it does not displace hydrogen from acid. \nCu +\u00a0HCl \u2192\u00a0No reaction \n(ii) In case of Mg; it is a very expensive metal. \n(iii) In case of sodium, it reacts with explosively and violently.<\/p>\n(b)\u00a0<\/strong>Among the given acids we prefer dilute\u00a0sulphuric\u00a0acid. \nWe reject concentrated\u00a0sulphuric, dilute nitric and concentrated nitric acid because these are powerful\u00a0oxidising\u00a0agents and oxygen formed due to its decomposition\u00a0oxidises\u00a0the hydrogen to water.<\/p>\n(c)\u00a0<\/strong>Modification: Collect the gas by downward displacement of water when all the air from the apparatus has been expelled. Drying Agent used is Calcium Chloride.<\/p>\nSolution 9.<\/strong><\/span><\/p>\n(a)\u00a0Iron reacts reversibly with steam. Hence the hydrogen formed is removed as it is released to prevent reduction of\u00a0triferric<\/span>\u00a0tetraoxide<\/span>. \nFe\u00a0+\u00a04H2<\/sub>O \u2192\u00a0Fe3<\/sub>O4<\/sub>\u00a0+\u00a04H2<\/sub>\u00a0? \n(Steam)<\/p>\n(b) \n<\/p>\n Solution 10.<\/strong><\/span><\/p>\n(a)\u00a0The metal is magnesium \n(b)\u00a0Mg\u00a0+\u00a0H2<\/sub>O \u2192\u00a0MgO\u00a0+\u00a0H2<\/sub><\/p>\nSolution 11.<\/strong><\/span><\/p>\n(a)<\/strong>\u00a0Substance A is\u00a0CuO\u00a0and substance B is Cu.<\/p>\n(b)<\/strong>\u00a0Test for water \n<\/u>(i) It is neutral to litmus \n(ii) It changes anhydrous copper\u00a0sulphate\u00a0into blue salt.<\/p>\n(c)<\/strong>\u00a0When substance\u00a0A\u00a0i.e,\u00a0CuO\u00a0reacts with hydrogen, it removes oxygen and we get free metal i.e. Cu.<\/p>\n(d)<\/strong>\u00a0CuO\u00a0+\u00a0H2<\/sub>\u00a0\u2192 Cu\u00a0+\u00a0H2<\/sub>O<\/p>\n(e)<\/strong>\u00a0No, there is no reaction between substance B and dilute hydrochloric acid because copper does not displace hydrogen from acids.<\/p>\n(f)<\/strong>\u00a0Cu +\u00a0HCl \u2192\u00a0No reaction<\/p>\nSolution 12.<\/strong><\/span><\/p>\nMagnesium lies above Hydrogen in reactivity series and can displace hydrogen from acid whereas, Mercury and silver lie below hydrogen in reactivity series and cannot displace hydrogen from acid and hence nothing happens.<\/p>\n Solution 13.<\/strong><\/span><\/p>\nSoap bubbles containing hydrogen rapidly rise up in air as hydrogen is lighter than air.<\/p>\n Solution 14.<\/strong><\/span><\/p>\nBosch Process \n<\/u><\/strong>Bosch process consists of following steps.<\/p>\nStep 1 :<\/strong><\/p>\nSteam is passed over a hot coke (at 1000o<\/sup>C) in a special type\u00a0of a furnaces\u00a0called converters. \nIn this step carbon reacts with water to form carbon monoxide and hydrogen gas. This mixture is called water gas.<\/p>\nStep 2 :<\/strong><\/p>\nIn this step excess of steam is mixed with water gas and entire mixture is passed over heated ferric oxide and chromic oxide. Ferric oxide acts as catalyst and chromic oxide as promoter. \n<\/p>\n Step 3 :<\/strong><\/p>\nIn this step removal of carbon dioxide from reaction mixture takes place. The mixture of carbon dioxide and hydrogen is forced through cold water under pressure\u00a0at 30 atmospheric pressure\u00a0or through caustic potash solution which dissolve carbon dioxide leaving behind hydrogen gas. | | | | | | | | | | | | |