{"id":37608,"date":"2023-01-12T10:00:26","date_gmt":"2023-01-12T04:30:26","guid":{"rendered":"https:\/\/www.aplustopper.com\/?p=37608"},"modified":"2023-01-13T10:18:53","modified_gmt":"2023-01-13T04:48:53","slug":"plus-two-chemistry-notes-chapter-7","status":"publish","type":"post","link":"https:\/\/www.aplustopper.com\/plus-two-chemistry-notes-chapter-7\/","title":{"rendered":"Plus Two Chemistry Notes Chapter 7 The p Block Elements"},"content":{"rendered":"

Plus Two Chemistry Notes Chapter 7 The p Block Elements is part of Plus Two Chemistry Notes<\/a>. Here we have given Plus Two Chemistry Notes Chapter 7 The p Block Elements.<\/p>\n\n\n\n\n\n\n\n\n\n
Board<\/strong><\/td>\nSCERT, Kerala<\/td>\n<\/tr>\n
Text Book<\/strong><\/td>\nNCERT Based<\/td>\n<\/tr>\n
Class<\/strong><\/td>\nPlus Two<\/td>\n<\/tr>\n
Subject<\/strong><\/td>\nChemistry Notes<\/td>\n<\/tr>\n
Chapter<\/strong><\/td>\nChapter 7<\/td>\n<\/tr>\n
Chapter Name<\/strong><\/td>\nThe p Block Elements<\/td>\n<\/tr>\n
Category<\/strong><\/td>\nPlus Two Kerala<\/a><\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n

Kerala Plus Two Chemistry Notes Chapter 7 The p Block Elements<\/h2>\n

The p-Block – Elements of group 13 to 18 of the periodic table. The outer electronic configuration of a p-block element is ns2<\/sup>np1-6<\/sup>.<\/p>\n

Anomalous behaviour of the first element of a group: This is due to<\/p>\n

    \n
  1. Small in size<\/li>\n
  2. High electronegativity,<\/li>\n
  3. High ionisation enthalpy and<\/li>\n
  4. Non-availability of d – orbitals.<\/li>\n<\/ol>\n

    Diagonal Relationship:
    \nIn some cases, the first element of a group resembles diagonally with the element of the next group and of the next period.<\/p>\n

    Group 15 – Elements – Nitrogen Family:<\/span>
    \nElements are – N, P, As, Sb, Bi
    \nN2<\/sub> comprises 78% by volume of the atmosphere. N and P are essential constituents of animals and plants. N – Present in proteins, P – Present in bones.<\/p>\n

    Characteristics:
    \n1. Atomic radii increases with increase in Atomic Number.<\/p>\n

    2. Ionisation Enthalpy decreases down the group due to gradual increase in atomic size. Because of the extra stable half-filled p orbitals electronic configuration and smaller size, the ionisation enthalpy is less than that of group 14 elements in the corresponding periods.<\/p>\n

    3. Electronegativity decreases down the group.<\/p>\n

    Physical Properties:
    \nAll are polyatomic, metallic character increases from N to Bi, density increases from N to Bi, M.P. and B.P. increases down the group, except N all other elements show allotropy.<\/p>\n

    Chemical Properties:
    \nOxidisation states and trends in chemical reactivity:
    \nThe common oxidation states of 15 group elements are (-3), (+3) and (+5). The stability of +5 oxidisation state decreases and that of +3 state increases down the group due to inert pair effect. Nitrogen exhibits +1, +2, +4 oxidation states also when it react with O2<\/sub>.<\/p>\n

    The maximum covalence of N restricted to 4 since only 4 orbitals (one S and three P) are available for bonding.<\/p>\n

    Anomalous Properties of Nitrogen:
    \nIt is due to its small size, high electronegativity, high ionisation enthalpy and non-availability of \u2018d\u2019 orbitals. Nitrogen has unique ability to form p\u03c0 – p\u03c0 multiple bond. It cannot form d\u03c0 – p\u03c0 bond. P and A scan form d\u03c0 – d\u03c0 bond.<\/p>\n

    (i) Reactivity towards hydrogen:
    \nEH3<\/sub> hydrides, the central atom is sp3<\/sup> hybridised, molecules assume trigonal pyramidal geometry with a lone pair on the central atom. Stability-decreases from NH3<\/sub> to BiH3<\/sub>.<\/p>\n

    This is because, down the group the E-H bond dissociation enthalpy decreases due to increase in size of the central atom. Consequently, reducing character increases from NH3<\/sub> to BiH3<\/sub>. The basicity decreases in the order NH3<\/sub> > PH3<\/sub> > AsH3<\/sub> > SbH3<\/sub>> BiH3<\/sub>.<\/p>\n

    As the electronegativity of the central atom decreases on moving down the group, the bond pair-bond pair repulsion decreases. Hence the bond angle decreases in the order NH3<\/sub> > PH3<\/sub> > AsH3<\/sub>.<\/p>\n

    (ii) Reactivity towards oxygen:
    \nThey form E2<\/sub>O3<\/sub> & E2<\/sub>O5<\/sub> type oxides. The oxide in the higher oxidisation state of the element is more acidic than that in lower oxidation state.<\/p>\n

    (iii) Reactivity towards halogens:
    \nThey form EX3<\/sub> and EX5<\/sub> type halides. Nitrogen does not form pentahalide due to non-availability of d-orbital.<\/p>\n

    (iv) Reactivity towards Metals:
    \nThey react with some metals exhibiting – 3 oxidation state, e.g. Calcium nitrate (Ca3<\/sub>N2<\/sub>), Calcium phosphide (Ca3<\/sub>P2<\/sub>), Sodium arsenide (Na3<\/sub>As2<\/sub>).<\/p>\n

    Dinitrogen (N2<\/sub>):<\/span>
    \nIt is produced commercially by the liquefaction and fractional distillation of air.
    \nIn laboratory, N2<\/sub> is prepared by<\/p>\n

    NH4<\/sub>Cl(aq) + NaNO2<\/sub>(aq) \u2192 N2<\/sub>(g) + 2 H2<\/sub>O(l)+ NaCl(aq)
    \n\"Plus
    \nProperties:
    \nColourless, odourless, non-toxic gas; inert at room temperature because of high bond enthalpy of N \u2261 N.<\/p>\n

    Uses:
    \nManufacture of NH3<\/sub>, liquid N2<\/sub> is used as refrigerant to preserve biological materials, food items and in cryosurgery.<\/p>\n

    Ammonia:<\/span>
    \nLaboratory preparation:
    \n2NH4<\/sub>Cl + Ca(OH)2<\/sub> \u2192 2NH3<\/sub> + 2H2<\/sub>O\u00a0+ CaCl2<\/sub>
    \n(NH4<\/sub>)2<\/sub>SO4<\/sub> + 2NaOH \u2192 2NH3<\/sub> + 2H2<\/sub>O\u00a0+ Na2<\/sub>SO4<\/sub><\/p>\n

    Industrial (large scale) preparation by Haber\u2019s process:
    \nN2<\/sub>(g) + 3H(g) \u21cc NH3<\/sub>(g); \u0394f<\/sub>H\u24bd<\/sup> = -46.1 kJ\/mol-1<\/sup> Catalyst used earlier- spongy iron with molybdenum promoter. Catalyst used now – iron oxide with small amounts of K2<\/sub>O and Al2<\/sub>O3<\/sub>.<\/p>\n

    High pressure and low temperature will favour the formation of NH3<\/sub> as the forward reaction is exothermic and is accompanied by decrease in number of moles (Le Chatelier\u2019s principle). Hence, a pressure of 200 \u00d7 105<\/sup> Pa (about 200 atm) and a temperature of ~ 700 K are employed to increase the yield of NH3<\/sub>.<\/p>\n

    Properties:
    \nColourless, pungent smelling gas, trigonal pyramidal geometry, highly soluble in water.
    \nNH3<\/sub>(g) + H2<\/sub>O(l) \\(\\rightleftharpoons\\) NH+<\/sup>4<\/sub>(aq) + OH–<\/sup>(aq)
    \nLewis base – due to the presence of a lone pair of electrons on N. It can form complex compounds with metal ions. This finds application in the detection of
    \nCu2+<\/sup> and Ag+<\/sup>.<\/p>\n

    Uses:
    \nTo produce various nitrogeneous fertilizers, manufacture of inorganic nitrogen compounds (e.g. HNO3<\/sub>), liquid NH3<\/sub> is used as a refrigerant.<\/p>\n

    Oxides of Nitrogen:<\/span><\/p>\n

      \n
    1. Dinitrogen oxide (N2<\/sub>O) or laughing gas – Oxdation state (+1) – Colourless gas, neutral.<\/li>\n
    2. Nitrogen monoxide(NO) – Oxdation state (+2) colourless gas, neutral.<\/li>\n
    3. Dinitrogen Trioxide(N2<\/sub>O3<\/sub>) – Oxdation state (+3), blue solid, acidic in nature.<\/li>\n
    4. Nitrogen dioxide(NO2<\/sub>) – Oxdation state (+4) brown gas, acidic. It contains odd number of valence electrons. On dimerisation, it is converted to stable N2<\/sub>O4<\/sub> molecule with even number of electrons.<\/li>\n
    5. Dinitrogen tetroxide(N2<\/sub>O4<\/sub>) – Dimer of NO2<\/sub> – Oxdation state (+4), colourless solid\/liquid, acidic.<\/li>\n
    6. Dinitrogen pentoxide (N2<\/sub>O5<\/sub>) – Oxdation state (+5), colourless solid, acidic.<\/li>\n<\/ol>\n

      \"Plus<\/p>\n

      Nitric Acid:<\/span>
      \nIt is the most important oxoacid of N.
      \nLaboratory preparation:
      \nKNO3<\/sub>\/NaNO3<\/sub> + H2<\/sub>SO4<\/sub>(conc.) \u2192 KHSO4<\/sub>\/NaHSO4<\/sub> + HNO3<\/sub>
      \nIndustrial preparation – Ostwald\u2019s process:
      \n(1) NH3<\/sub> oxidised to NO by air.
      \n\"Plus<\/p>\n

      (2) NO is converted to NO2<\/sub>
      \n2NO(g) + O2<\/sub>(g) \u21c4 2NO2<\/sub>(g)<\/p>\n

      (3) NO2<\/sub> dissolved in water to give HNO3<\/sub>
      \n3NO2<\/sub>(g) + H2<\/sub>O(l) \u2192 2HNO3<\/sub> (aq) + NO(g)<\/p>\n

      Properties:
      \nColourless liquid, strong acid in aqueous solution. Concentrated HNO3<\/sub> is a strong oxidising agent and attacks most metals except noble metals like Au and Pt. The products of oxidation depend upon the concentration of the acid, temperature and the nature of the material undergoing oxidation, e.g.<\/p>\n

        \n
      • 3Cu + 8HNO3<\/sub>(dilute) \u2192 3Cu(NO3<\/sub>)2<\/sub> + 2NO + 4H2<\/sub>O<\/li>\n
      • Cu + 4HNO3<\/sub>(conc.) \u2192 CuCu(NO3<\/sub>)2<\/sub> + 2NO2<\/sub> + 2H2<\/sub>O<\/li>\n
      • 4Zn + 10HNO3<\/sub>(dilute) \u2192 4Zn(NO3<\/sub>)2<\/sub> + 5H2<\/sub>O + N2<\/sub>O<\/li>\n
      • Zn + 4HNO3<\/sub>(conc.) \u2192 Zn(NO3<\/sub>)2<\/sub> + 2H2<\/sub>O + 2N2<\/sub>O<\/li>\n<\/ul>\n

        Some metals (e.g., Cr, Al) do not dissolve in concentrated nitric acid because of the formation of a passive film of oxide on the surface.<\/p>\n

        Structure:
        \nIn the gaseous state, HNO3<\/sub>\u00a0exists as a planar molecule.
        \n\"Plus<\/p>\n

        Uses:
        \nManufacture ammonium nitrate (fertilizer), preparation of explosives, preparation of nitroglycerine, pickling of stainless steel, etching of metals, oxidiser in rocket fuels.<\/p>\n

        Phosphorus:<\/span>
        \nAllotropic forms – White P, red P and black P
        \n\"Plus<\/p>\n

        White Phosphorus:
        \nTransient white waxy solid, poisonous, insoluble in water, soluble in CS2<\/sub>, glows in dark (chemiluminescence), kept underwater, less stable and therefore more reactive than other solid phases under normal conditions because of angular strain in discrete tetrahedral P4<\/sub> molecules (angle 60\u00b0), readily catches fire in air and gives dense while fumes of P4<\/sub>O10<\/sub>.
        \nP4<\/sub> + 5O2<\/sub> \u2192 P4<\/sub>O10<\/sub><\/p>\n

        Red Phosphorus:
        \nObtained by heating white P at 573 K in an inert atm for several days, possesses iron grey lustre, odourless, non-poisonous, less reactive than white P, does not glow in dark, polymeric consisting of chains of P4<\/sub> tetrahedra.
        \n\"Plus<\/p>\n

        Black Phosphorus:
        \nObtained when red P is heated under high pressure, two forms \u03b1 – black phosphorus (formed when red P is heated in a sealed tube at 803 K) and \u03b2 – black phosphorus (prepared by heating white P at 473 K under high pressure).<\/p>\n

        Phosphine (PH3<\/sub>):<\/span>
        \nPrepared by the reaction of calcium phosphide with water or dilute HCl.
        \nCa3<\/sub>P2<\/sub> + 6H2<\/sub>O \u2192 3Ca(OH)2<\/sub> + 2PH3<\/sub>
        \nCa3<\/sub>P2<\/sub> + 6HCl \u2192 3CaCl2<\/sub> + 2PH3<\/sub><\/p>\n

        Laboratory preparation:
        \nBy heating white P with concentrated NaOH solution in an inert atmosphere of CO2<\/sub>.
        \nP4<\/sub> + 3NaOH + 3H2<\/sub>O \u2192 PH3<\/sub> + 3NaH2<\/sub>PO2<\/sub><\/p>\n

        Properties:
        \nColourless gas with a rotten fishy smell, highly poisonous, weakly basic, the structure is similar to NH3<\/sub> and gives phosphonium compounds with
        \nacids. PH3<\/sub> + HBr \u2192 PH4<\/sub>Br
        \nUses: in Holme\u2019s signals, in smoke screens.<\/p>\n

        Phosphorus Halides:<\/span>
        \nIt forms two types of halids PX3<\/sub> and PX5<\/sub> (X = F, Cl, Br)<\/p>\n

        Phosphorus Trichloride (PCl3<\/sub>):
        \nObtained by passing dry Cl2<\/sub> overheated white P.
        \nP4<\/sub> + 6Cl2<\/sub> \u2192 4PCl3<\/sub><\/p>\n

        Or, by the action of thionyl chloride on white P,
        \nP4<\/sub> + 8SOCl2<\/sub> \u2192 4PCl3<\/sub> + 4SO2<\/sub> + 2S2<\/sub>Cl2<\/sub><\/p>\n

        Properties
        \nColourless oily liquid, hydrolyses in the presence of moisture giving fumes of HCl.
        \nP4<\/sub> + 3H2<\/sub>O \u2192 H3<\/sub>PO3<\/sub> + 3HCl
        \nIt has pyrimidal shape and P is sp3 hybridised.
        \n\"Plus<\/p>\n

        Phosphorus Pentachloride (PCl5<\/sub>):
        \nPreparation:
        \nWhite P4<\/sub> + 10Cl2(dry)<\/sub> \u2192 4PCl5<\/sub><\/p>\n

        Properties:
        \nyellowish white powder. In moist air it hydrolysed giving POCl3<\/sub> and finally gets converted to phosphoric acid (H3<\/sub>PO4<\/sub>)
        \nPCl5<\/sub> + H2<\/sub>O \u2192 POCl3<\/sub> + 2HCl
        \nPOCl3<\/sub> + 3 H2<\/sub>O \u2192 H3<\/sub>PO4<\/sub> + 3 HCl
        \nIn gaseous and liquid phases, the shape of the molecule is trigonal bipyramidal. There are two types of P-Cl bonds, equatorial bond and axial bond. Axial bonds are longer than equitorial bonds due to more repulsion. In solid state it exits as ionic solid, [PCl4<\/sub>]+<\/sup>[PCl6<\/sub>]–<\/sup>.<\/p>\n

        Oxoacids of Phosphorus:<\/span><\/p>\n

          \n
        • Hypophosphorous\/Phosphinic acid(H3<\/sub>PO2<\/sub>) – Monobasic<\/li>\n
        • Orthophosphorous\/Phosphonic acid(H3<\/sub>PO3<\/sub>) – Dibasic<\/li>\n
        • Pyrophosphorous acid(H4<\/sub>P2<\/sub>O5<\/sub>) – Dibasic<\/li>\n
        • Hypophosphoric acid(H4<\/sub>P2<\/sub>O6<\/sub>) – Tetrabasic<\/li>\n
        • Orthophosphoric acid(H3<\/sub>PO4<\/sub>) – Tribasic<\/li>\n
        • Pyrophosphoric acid(H4<\/sub>P2<\/sub>O7<\/sub>) – Tetrabasic<\/li>\n
        • Metaphosphoric acid(HPO3<\/sub>)n<\/sub> – Tribasic<\/li>\n<\/ul>\n

          The p-H bonds are not ionisable and have no role in basicity. Only those H atoms in P-OH form are ionisable and cause basicity.<\/p>\n

          These acids in +3 oxidation state of P tend to disproportionate to higher and lower oxidation states, e.g. Orthophosphorous acid on heating disproportionates to give orthophosphoric acid (P in +5 state) and phosphine
          \n\"Plus<\/p>\n

          The acids with P-H bond .have strong reducing property, e.g. H3<\/sub>PO2<\/sub>. It reduces AgNO3<\/sub> to Ag.<\/p>\n

          Structure of Oxoacids:
          \n\"Plus<\/p>\n

          Group 16 Elements (Chalcogens):
          \n<\/span>O, S, Se, Te and Po.<\/p>\n

          1. Occurrence:
          \nO2 <\/sub>– Most abundant element on earth crust (46.6%), dry air contains 21% by volume. S – Present as sulphates, sulphides (e.g. CaSO4<\/sub>, PbS, ZnS). Se &Te-in metal selenides and tellurides, Po-radio active, formed by the decay of thorium and uranium minerals.<\/p>\n

          2. 6 General electronic configuration-ns2<\/sup>np4<\/sup>. In group:
          \nAtomic and ionic radii increases, ionisation enthalpy, electron gain enthalpy and electronegativity decreases – O has the highest electronegativity next to F.<\/p>\n

          3. Physical Properties:
          \nO is a diatomic gas, non metal. S-solid, non-metal. Se and Te are metalloids. Po-radioactive metal.<\/p>\n

          4. Chemical Properties:
          \nOxidation states and trends in chemical activity – exhibits variable oxidation states, stability of -2 oxidation state decreases down the group. O-shows +2 in OF2<\/sub>, -1 in peroxides and – 2 in other compounds. Other elements show +2, +4, +6 states.<\/p>\n

          5. Anomolous Behaviour of Oxygen:
          \nIt is due to small size high electronegativity, non availability of d-orbital and high polarising power.<\/p>\n

          (i) Reactivity with Hydrogen:
          \ngroup 16 elements form H2<\/sub>E type hydrids (E = O, S, Se, Te, Po). Their acidic character increases from H2<\/sub>O to H2<\/sub>Te due to decrease in H-E bond dissociation enthalpy. All hydride except H2<\/sub>O posses reducing property. Reducing nature increases from H2<\/sub>S to H2<\/sub>Te.<\/p>\n

          Due to small size and high electro naegativity of oxygen, H2<\/sub>O molecules are highly associated through hydrogen bonding resulting in its liquid state and high boiling point.<\/p>\n

          While, due to large size and low electronegativity of S association through hydrogen bonding is hot possible in H2<\/sub>S. Hence it exists as a gas and has low boiling point than H2<\/sub>O.<\/p>\n

          (ii) Reactivity with Oxygen:
          \nThey form EO2<\/sub> & EO3<\/sub> type oxides. Ozone, O3<\/sub> and SO2<\/sub> are gases. Both type of oxides are acidic in nature.<\/p>\n

          (iii) Reactivity Towards the Halogens:
          \nThey form EX2<\/sub>, EX4<\/sub> and EX6<\/sub> type halides. The stability of halides decrease in the order F–<\/sup> > Cl–<\/sup> > Br > l–<\/sup><\/p>\n

          Dioxygen (O2<\/sub>):<\/span>
          \nPreparation:
          \n(i) Heating KClO3<\/sub>, KMnO4<\/sub>, KNO3<\/sub> etc.
          \n\"Plus<\/p>\n

          (ii) Thermal decomposition of metal oxides.
          \n2Ag2<\/sub>O \u2192 4Ag + O2<\/sub>
          \n2PbO2<\/sub> H \u2192 2PbO + O2<\/sub><\/p>\n

          (iii) Decomposition of H202
          \n2H2<\/sub>O2<\/sub> \u2192 2H2<\/sub>O + O2<\/sub>.<\/p>\n

          Large scale preparation:
          \nElectrolysis of water, O2<\/sub> liberated at anode.<\/p>\n

          Properties:
          \nColourless, odourless gas; paramagnetic, directly reacts with nearly all metals except Au and Pt.<\/p>\n

          Simple Oxides:<\/span>
          \nBinary compound of O with another element, e.g. MgO, Al2<\/sub>O3<\/sub>. Basic oxide – oxide that combine with water give a base. e.g. MgO. Acidic oxide – oxide that combine with water to give acid, e.g. SO2<\/sub>, CO2<\/sub>.
          \nSO2<\/sub> + H2<\/sub>O \u2192 H2<\/sub>SO3<\/sub>
          \nIn general, metallic oxides are basic and non-metallic oxides are acidic.<\/p>\n

          Ozone (O3<\/sub>):<\/span>
          \nAllotropic form of O, too reactive, prepared by passing a slow dry stream of O2<\/sub> through a silent electrical discharge.
          \n3O2<\/sub> \u2192 2O3<\/sub>
          \n\u0394H = +142 kJ mol-1<\/sup><\/p>\n

          Properties:
          \nPure O3<\/sub> is a pale blue gas, dark blue liquid and violet-black solid, thermodynamically unstable compared to O2<\/sub>.<\/p>\n

          Oxidising property:
          \nDue to the ease with which it liberates atoms of nascent oxygen 03 acts as a powerful oxidising agent.
          \nO3<\/sub> \u2192 O2<\/sub> + [O]
          \ne.g. It oxidises lead sulphide to lead sulphate.
          \nPbS(s) + 4O3<\/sub>(g) \u2192 PbSO4<\/sub>(s) + 4O2<\/sub>(g)<\/p>\n

          Estimation of O3<\/sub>:
          \nWhen O3<\/sub> reacts with excess of Kl solution buffered with a borate buffer (pH 9.2), l2<\/sub> is liberated which can be titrated against a standard solution of sodium thiosulphate.
          \n2l–<\/sup>(aq) + H2<\/sub>O(l) + O3<\/sub>(g) \u2192 2OH–<\/sup>(aq) + l2<\/sub>(s) + O2<\/sub>(g)<\/p>\n

          Uses:
          \nAs a germicide, disinfectant and for sterilising water; for bleaching oils, ivory, starch etc. as oxidising agent in the manufacture of KMnO4<\/sub>.<\/p>\n

          Sulfur-allotropic Forms:<\/span>
          \nRhombic Sulphur (\u03b1 – Sulphur):
          \nyellow, insoluble in water, dissolve to some extent in benzene and alcohol, readily soluble in CS2<\/sub>.<\/p>\n

          Monoclinic Sulphur (\u03b2 – Sulphur):
          \nSoluble in CS2<\/sub>, needle shaped crystals.<\/p>\n

          Structure:
          \nThey exists as S8<\/sub> molecules, the S8<\/sub> ring is puckered and has a crown shape. The cylco-S6<\/sub> ring adopts a chair form.
          \n\"Plus<\/p>\n

          Sulphur Dioxide (SO2<\/sub>):<\/span>
          \nPreparation:
          \n1. Burning of S in air
          \nS(s) + O2<\/sub>(g) \u2192 SO2<\/sub>(g)<\/p>\n

          2. Treating sulphite with diluted H2<\/sub>SO4<\/sub>.
          \nSO3<\/sub>2-<\/sup> + 2H+<\/sup> \u2192 H2<\/sub>O + SO2<\/sub><\/p>\n

          Properties:
          \nColourless gas with pungent smell, highly soluble water, when passed through water forms sulphurous acid.
          \nSO2<\/sub>(g) + H2<\/sub>O(l) \u2192 H2<\/sub>SO3<\/sub>(aq)<\/p>\n

          React with NaOH:
          \n2NaOH + SO2<\/sub> \u2192 Na2<\/sub>SO3<\/sub> + H2<\/sub>O<\/p>\n

          Other reactions:
          \n3SO2<\/sub> + Cl2<\/sub> \u2192 SO2<\/sub>Cl2<\/sub>
          \n\"Plus<\/p>\n

          Users:
          \nIn pertroleum refining and sugar industry, in bleaching wool and silk, in manufacturing H2<\/sub>SO4<\/sub>.<\/p>\n

          Oxoacids of Sulphur:<\/span>
          \nSulphur forms a number of oxoacids such as H2<\/sub>SO3<\/sub>, H2<\/sub>SO4<\/sub>, H2<\/sub>S2<\/sub>O3<\/sub>, H2<\/sub>S2<\/sub>O7<\/sub><\/p>\n

          Manufacture of Sulphuric Acid:<\/span>
          \nSulphuricacid is known as king of chemicals. It is manufactured by Contact Process.<\/p>\n

          Steps Involved:
          \n(i) Burning of S or Sulphide ores in air to form SO2<\/sub><\/p>\n

          (ii) Conversion of SO2<\/sub> to SO3<\/sub> by the reaction with O2<\/sub> in presence of V2<\/sub>O5<\/sub> catalyst.
          \n\"Plus
          \n\u0394H = -196.6 KJ mol-1<\/sup>
          \nLow temperature (720 K) and high pressure (2 bar) are the favourable conditions for maximum yield.<\/p>\n

          (iii) Absorption of SO3<\/sub> in H2<\/sub>SO4<\/sub> to give oleum (H2<\/sub>S2<\/sub>O7<\/sub>)
          \nSO3<\/sub> + H2<\/sub>SO4<\/sub> \u2192 H2<\/sub>S2<\/sub>O8<\/sub>
          \nDilution of oleum with water gives H2<\/sub>SO4<\/sub> of desired concentration. H2<\/sub>S2<\/sub>O7<\/sub> + H2<\/sub>O \u2192 2 H2<\/sub>SO4<\/sub><\/p>\n

          Properties:
          \nColourless, oily liquid, dissolves in water with the evolution of large quantity of heat, dibasic acid, in aqueous solution, it ionises in two steps:
          \nH2<\/sub>SO4<\/sub>(aq) + H2<\/sub>O(l) \u2192 H3<\/sub>O+<\/sup>(aq) + HSO4<\/sub>–<\/sup> (aq)
          \nHSO4<\/sub>–<\/sup>(aq) + H2<\/sub>O(l) \u2192 H3<\/sub>O+<\/sup>(aq) + SO4<\/sub>2-<\/sup>(aq)
          \nConcentrated H2<\/sub>SO4<\/sub> is a strong dehydrating agent.<\/p>\n

          Uses:
          \nManufacture of fertilisers; petroleum refining; manufacture of pigments, paints, dyestuff; detergent industry; storage batteries; laboratory reagent<\/p>\n

          Group 17 Elements (Halogens):<\/span> F, Cl, Br, I and At (radioactive), highly reactive non-metallic elements.<\/p>\n

          1-6 Occurrence:
          \nF-in fluorides (CaF2<\/sub>, Na3<\/sub>AIF6<\/sub>). Seawater contains chlorides, bromides and iodides of Na & K, electronic configuration – ns\u00b2np5<\/sup>, in a group from top to bottom atomic and ionic radii increases, ionisation enthalpy decreases.<\/p>\n

          Electron gain enthalpy – halogen have maximum negative electron gain enethalpy. Cl has highest electron gain enthalpy. Electronegativity decreases down the group. F is the most electronegative element in the periodic table.<\/p>\n

          Physical Properties:
          \nF2<\/sub>, Cl2 <\/sub>– gases, Br2<\/sub> – liquid and l2 <\/sub>– solid. F2<\/sub> and Cl2<\/sub> react with water Br2<\/sub> and l2<\/sub> sparingly soluble in water.<\/p>\n

          Oxidation States and Trends in Chemical Reactivity:
          \nAll the halogens exhibit-1 oxdn. state. But, Cl, Br and I exhibit +1, +3, +5 and +7 also. They react with metals and non-metals to form halides. The reactivity of the halogens decreases down the group.<\/p>\n

          Anomalous Behaviour of Fluorine:
          \nIt is due to smaller in size, high electronegativity, low F-F bond dissociation enthalpy and non-availability of d-orbitals, due to which it cannot expand its octet. It exhibits only-1 oxidation state.<\/p>\n

          (i) Reactivity Towards Hydrogen:
          \nAll form hydrogen halides (HX) which dissolve in water to form hydrohalic acids. The acidic strength of acids:
          \nHF < HCl < HBr < Hl .The stability of halides decreases down the group due to decrease in (H-X) dissociation enthalpy in the order: H-F > H-Cl > H-Br > H-l.<\/p>\n

          (ii) Reactivity Towards Oxygen:
          \nThey form many oxides but most of them are unstable. Fluorine form OF2<\/sub> and O2<\/sub>F2<\/sub>. Chlorine form oxides Cl2<\/sub>O, ClO2<\/sub>, Cl2<\/sub>O6<\/sub> and Cl2<\/sub>O7<\/sub>, which are highly reactive oxidising agents, ClO2<\/sub> is used as a bleaching agent for paper pulp, textiles.<\/p>\n

          (iii) Reactivity Towards Metals:
          \nMetal halides are formed,
          \ne.g. Mg(s) + Br2<\/sub>(l) \u2192 MgBr2<\/sub>(s)<\/p>\n

          (iv) Reactivity of Halogens Towards Other Halogens:
          \nHalogens combine amongst themselves to form a number of compounds known as interhalogens. Five types: XX\u2019, XX3, XX\u20195, XX\u20197 where X is a halogen of larger size and X\u2019 of smaller size.<\/p>\n

          Chlorine:<\/span>
          \nPreparation:
          \n(i) By heating manganese dioxide with concentrated HCl.
          \nMnO2<\/sub> + 4HCl \u2192 MnCl2<\/sub> + 2H2<\/sub>O + Cl2<\/sub><\/p>\n

          (ii) By the action of HCl on KMnO4<\/sub>.
          \n2KMnO4<\/sub> + 16HCl \u2192 2KCl + 2MnCl2<\/sub> + 8H2<\/sub>O + 5Cl2<\/sub><\/p>\n

          Manufacture:
          \n(i) Deacon\u2019s Process – By oxidation of HCl gas by atm oxygen in the presence of CuCl2<\/sub> at 723K.
          \n\"Plus<\/p>\n

          (ii) Electrolytic process
          \n\"Plus\u00a0(liberated at anode)<\/p>\n

          Properties:
          \nGreenish yellow gas with pungent and suffocating odour, reacts with metal, and non metals
          \n\"Plus
          \nWith excess NH3<\/sub>, Cl2<\/sub> gives N2<\/sub> and NH4<\/sub>Cl whereas with excess Cl2<\/sub>, NH3<\/sub> gives NCl3<\/sub> (explosive) and HCl.
          \n\"Plus
          \nWith cold and dilute alkalies chlorine produces a mixture of chloride and hypochlorite but with hot and concentrated alkalies it gives chloride and chlorate.
          \n\"Plus
          \nWith dry slaked lime, it gives bleaching powder.
          \n2Ca(OH)2<\/sub> + 2Cl2<\/sub> \u2192 Ca(OCl)2<\/sub> + CaCl2<\/sub> + 2H2<\/sub>OCl2<\/sub> is a powerful bleaching agent.
          \nCl2<\/sub> + H2<\/sub>O \u2192 2HCl + [O]
          \nColoured substance + [0] \u2192 colourless substance<\/p>\n

          Uses:
          \nFor bleaching wood pulp, cotton and textiles; for the preparation of insectiside, pesticides and other organic solvents, e.g. CHCl3<\/sub>, DDT, BHC etc.<\/p>\n

          Hydrogen Chloride (HCl):<\/span>
          \nPreparation:
          \n\"Plus
          \nHCl gas is dried by passing through a cone. H2<\/sub>SO4<\/sub>.
          \nProperties :
          \nColourless and pungent-smelling gas, soluble in water and ionises as follows:
          \nHCl + H2<\/sub>O \u2192 H3<\/sub>O+<\/sup> + Cl–<\/sup>
          \nIt reacts with NH3<\/sub> to give white fumes of NH4<\/sub>Cl.
          \nNH3<\/sub> + HCl \u2192 NH4<\/sub>Cl
          \nIt decomposes salt of weaker acids.
          \nNa2<\/sub>CO3<\/sub> + 2HCl \u2192 2NaCl + H2<\/sub>O + CO2<\/sub>
          \nNaHCO3<\/sub> + HCl \u2192 NaCl + H2<\/sub>O + CO2<\/sub><\/p>\n

          Uses: manufacture of Cl2<\/sub>, NH4<\/sub>Cl and glucose; for extracting glue.<\/p>\n

          Oxoacids of Halogen:<\/span>
          \nDue to high electronegativity and smaller in size fluorine forms only one oxoacid, HOF known as fluoric acid or hypofluorous acid.<\/p>\n

          Some oxoacids of Chlorine:<\/p>\n

            \n
          • Hypochlorous acid: HOCl (Cl in +1 state)<\/li>\n
          • Chlorous acid: HClO2<\/sub> (Cl in +3 state)<\/li>\n
          • Chloricacid: HClO3<\/sub> (Cl in +5 state)<\/li>\n
          • Perchloric acid: HClO4<\/sub>(Cl in +7 state).<\/li>\n<\/ul>\n

            Interhalogen Compounds:<\/span>
            \nTwo different halogens react to form interhalogen compounds, e.g. ClF, ClF3<\/sub>, BrF5<\/sub>, IF7<\/sub><\/p>\n

            Preparation:
            \nBy the direct combination of halogens.
            \n\"Plus<\/p>\n

            Properties:
            \nCovalent molecules, diamagnetic, volatile solids or liquids at 25\u00b0C except ClF which is a gas. They are more reactive than halogens because X-X bond is weaker than X-X bond. Due to electronegativity difference the X – X bond is polarised, hence it is reactive.<\/p>\n

            Their stability increases as the size difference of the halogens increases due to increase in the polarity of the bond. e.g. IF3<\/sub> is more stable than ClF3<\/sub>.<\/p>\n

            Group 18 Elements (Noble Gases):<\/span>
            \nHe, Ne, Ar, Kr, Xe and Rn (radioactive). Except He all other noble gas have 8 electrons in the valence shell. Due stable electronic configuration all these are gases and chemically unreactive, (exeption – Kr, Xe, Rn)<\/p>\n

            Occurrence:
            \nAll except Rn occur in the atmosphere. The main source of He-natural gas. Rn- obtained as a decay of product of Radium.<\/p>\n

            Electronic Configuration-ns\u00b2np6<\/sup> (except He-1s\u00b2 ), ionisation enthalpy-high due to stable electronic configuration-it decreases down the group, atomic radii-increases down the group, electron gain enthalpy-almost zero since no tendency to accept an electron.<\/p>\n

            Physical Properties:
            \nMonoatomic, colourless, odourless and tasteless gases, sparingly soluble in water, very low melting and boiling points because the only type of interatomic interaction in these elements is weak dispersion forces.<\/p>\n

            Chemical Properties:
            \nLeast reactive due to stable electronic configuration, high ionisation enthalpy and more positive electron gain enthalpy.<\/p>\n

            N. Bartlett prepared Xe+<\/sup>PtF6<\/sub> by mixing PtF6<\/sub> and Xe.<\/p>\n

            (a) Xenon – Fluorine Compounds:
            \nXe forms three binary fluorides XeF2<\/sub>, XeF4<\/sub> and XeF6<\/sub> by the direct reaction of Xe with F2<\/sub>.
            \n\"Plus<\/p>\n

            XeF4<\/sub>–<\/sup> also prepared by reaction with O2<\/sub>F2<\/sub> and XeF4<\/sub>. XeF4<\/sub> + O2<\/sub>F2<\/sub> \u2192 XeF6<\/sub> + O2<\/sub><\/p>\n

            Structure:
            \n(a) XeF2<\/sub> – sp3<\/sup>d hybridisation -linear
            \nXeF4<\/sub> – sp3<\/sup>d2<\/sup> hybridisation – square planar
            \nXeF6<\/sub> – sp3<\/sup>d3<\/sup> hybridisation – distorted octahedral
            \n\"Plus<\/p>\n

            (b) Xenon-Oxygen Compounds:
            \nXeO3<\/sub>: Prepared by hydrolysis of XeF4<\/sub> and XeF6<\/sub>.
            \n6XeF4<\/sub> + 12H2<\/sub>O \u2192 4Xe + 2XeO3<\/sub> + 24HF + 3O2<\/sub>
            \nXeF6<\/sub> + 3H2<\/sub>O \u2192 XeO3<\/sub> + 6HF.
            \nXeOF4–<\/sup><\/sub>prepared by partial hydrolysis of XeF6<\/sub>.
            \nXeF6<\/sub> + H2<\/sub>O \u2192 XeOF4<\/sub> + 2HCl<\/p>\n

            Structure:
            \nXeO3<\/sub> – sp3<\/sup> hybridisation – Pyramidal
            \nXeOF3<\/sub> – sp3<\/sup>d2<\/sup> hybridisation – Square pyramidal
            \n\"Plus<\/p>\n

            Uses of Noble Gases:
            \n1. He – for filling airships, aeroplane tyres, in gas-cooled nuclear reactors, for providing an inert atmosphere in the welding of metals and alloys.<\/p>\n

            2. Ne – for filling discharge tubes and fluorescent bulb for advertisement purpose, in botanical gardens and greenhouses.<\/p>\n

            3. Ar – to provide inert atmosphere in high-temperature metallurgical processes, for filling electric bulbs, for handling air-sensitive substances in laboratory.<\/p>\n

            4. Xe and Kr – in light bulbs designed for special purposes.<\/p>\n

            We hope the Plus Two Chemistry Notes Chapter 7 The p Block Elements help you. If you have any query regarding Plus Two Chemistry Notes Chapter 7 The p Block Elements, drop a comment below and we will get back to you at the earliest.<\/p>\n","protected":false},"excerpt":{"rendered":"

            Plus Two Chemistry Notes Chapter 7 The p Block Elements is part of Plus Two Chemistry Notes. Here we have given Plus Two Chemistry Notes Chapter 7 The p Block Elements. Board SCERT, Kerala Text Book NCERT Based Class Plus Two Subject Chemistry Notes Chapter Chapter 7 Chapter Name The p Block Elements Category Plus […]<\/p>\n","protected":false},"author":7,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_genesis_hide_title":false,"_genesis_hide_breadcrumbs":false,"_genesis_hide_singular_image":false,"_genesis_hide_footer_widgets":false,"_genesis_custom_body_class":"","_genesis_custom_post_class":"","_genesis_layout":"","footnotes":""},"categories":[42728],"tags":[],"yoast_head":"\nPlus Two Chemistry Notes Chapter 7 The p Block Elements - A Plus Topper<\/title>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/www.aplustopper.com\/plus-two-chemistry-notes-chapter-7\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Plus Two Chemistry Notes Chapter 7 The p Block Elements\" \/>\n<meta property=\"og:description\" content=\"Plus Two Chemistry Notes Chapter 7 The p Block Elements is part of Plus Two Chemistry Notes. 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Here we have given Plus Two Chemistry Notes Chapter 7 The p Block Elements. Board SCERT, Kerala Text Book NCERT Based Class Plus Two Subject Chemistry Notes Chapter Chapter 7 Chapter Name The p Block Elements Category Plus […]","og_url":"https:\/\/www.aplustopper.com\/plus-two-chemistry-notes-chapter-7\/","og_site_name":"A Plus Topper","article_publisher":"https:\/\/www.facebook.com\/aplustopper\/","article_published_time":"2023-01-12T04:30:26+00:00","article_modified_time":"2023-01-13T04:48:53+00:00","og_image":[{"url":"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2019\/02\/Plus-Two-Chemistry-Notes-Chapter-7-The-p-Block-Elements-1.png"}],"twitter_card":"summary","twitter_misc":{"Written by":"Kalyan","Est. reading time":"18 minutes"},"schema":{"@context":"https:\/\/schema.org","@graph":[{"@type":"Organization","@id":"https:\/\/www.aplustopper.com\/#organization","name":"Aplus Topper","url":"https:\/\/www.aplustopper.com\/","sameAs":["https:\/\/www.facebook.com\/aplustopper\/"],"logo":{"@type":"ImageObject","@id":"https:\/\/www.aplustopper.com\/#logo","inLanguage":"en-US","url":"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2018\/12\/Aplus_380x90-logo.jpg","contentUrl":"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2018\/12\/Aplus_380x90-logo.jpg","width":1585,"height":375,"caption":"Aplus Topper"},"image":{"@id":"https:\/\/www.aplustopper.com\/#logo"}},{"@type":"WebSite","@id":"https:\/\/www.aplustopper.com\/#website","url":"https:\/\/www.aplustopper.com\/","name":"A Plus Topper","description":"Improve your Grades","publisher":{"@id":"https:\/\/www.aplustopper.com\/#organization"},"potentialAction":[{"@type":"SearchAction","target":{"@type":"EntryPoint","urlTemplate":"https:\/\/www.aplustopper.com\/?s={search_term_string}"},"query-input":"required name=search_term_string"}],"inLanguage":"en-US"},{"@type":"ImageObject","@id":"https:\/\/www.aplustopper.com\/plus-two-chemistry-notes-chapter-7\/#primaryimage","inLanguage":"en-US","url":"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2019\/02\/Plus-Two-Chemistry-Notes-Chapter-7-The-p-Block-Elements-1.png","contentUrl":"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2019\/02\/Plus-Two-Chemistry-Notes-Chapter-7-The-p-Block-Elements-1.png","width":318,"height":33,"caption":"Plus Two Chemistry Notes Chapter 7 The p Block Elements 1"},{"@type":"WebPage","@id":"https:\/\/www.aplustopper.com\/plus-two-chemistry-notes-chapter-7\/#webpage","url":"https:\/\/www.aplustopper.com\/plus-two-chemistry-notes-chapter-7\/","name":"Plus Two Chemistry Notes Chapter 7 The p Block Elements - 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