Title 1.15th group elements exercise( 1-43 ).pdf ✅

NISHITH Multimedia India (Pvt.) Ltd., 1 JEE MAINS - CW - VOL - I VA GROUP ELEMENTS NISHITH Multimedia India (Pvt.) Ltd., JEE ADVANCED-VOL-VII VA GROUP ELEMENTS Preparation of dinitrogenN2  : 01. Nitrogen is prepared by treating sodium azide with hydrogen sulphide solution NaN H S H O N S NH NaOH 3 2 2 2 3        02. Nitrogen is prepared by treating hydrazene with iodine, oxygen or copper sulphate. N H 2I N 4HI 2 4 2 2    N H 2O N 2H O 2 4 2 2 2 2    N H 2CuSO N 2Cu 2H SO 2 4 4 2 2 4     03. (a) Nitrogen in the laboratory can be obtained by heating ammonium nitrite or ammonium dichromate or ammonium perchlorate NH NO N H O 4 2 2 2        4 2 7 2 2 3 2 2 green NH Cr O N Cr O 4H O     NH ClO N ClO 2H O 4 4 2 2 2     04. It can be obtained by the action of nitrous acid (or NaNO2 and dil. H2 SO4 ) on urea.   2 2 2 2 2 2 urea NH CONH 2HNO 2N CO 3H O     05. Nitrogen can be obtained by passing the ammonia vapours over heated CuO, Cl2 , Br2 , a hypochlorite, a hypobromite or bleaching powder. 3 2 2 2NH 3CuO N 3Cu 3H O     3 2 2 4 8NH 3Cl N 6NH Cl    3 2 2 4 8NH 3Br N 6NH Br    3 2 2 2NH 3NaOCl N 3NaCl 3H O     3 2 2 2 2 2NH 3CaOCl N 3CaCl 3H O     3 2 2 2 2 2NH 3CaOCl N 3CaCl 3H O     06. Nitrogen can be prepared by passing nitric oxide over red hot copper   2 , 2 2 2 red overheated Black NO Cu CuO N    07.   3 2 2 3 2 3 2 2 3             Ba N Ba N NaN Na N Purest N obtained by this method 2  08. From air: (a) Commercially nitrogen is obtained by liquefaction of air. The resultant liquid is fractionally distilled in CLAUDE’S apparatus. (b) By removing oxygen of the air with the use of chemical substances. Purified air Hot CuNitrogen 2 2 2 Cu O CuO   Purified air Hot coke 2 2 CO CO N , , CO2 and CO are removed by usual methods. Purified air P P O N 2 5 2  2 3 4 H O  H PO Properties of Nitrogen: 1. It is inert due to high bond energy. 2. It reacts with hot metals like Ca Mg Al , , ... 3. N2 can be absorbed by calcium carbide at the temperature around 0 1000 C   0 1000 2 2 C Nitrolim CaC N CaNCN C    Cynamide ion : N C N   2 N N C     4.   2 3 3 CaNCN C H O CaCO NH C      3 2 Slowlydecomposes NH2 2   CO NH Intermediate formed SYNOPSIS
VA GROUP ELEMENTS 2 NISHITH Multimedia India (Pvt.) Ltd., JEE ADVANCED-VOL-VII NISHITH Multimedia India (Pvt.) Ltd., Preparation and properties of oxides of nitrogen: I. N O2 : Preparations: 01. By the action of cold and dilute nitric acid on zinc metal. 3 2 3 2  2 d il 4 Zn 10H N O N O 4 Zn N O 5H O     02. By heating the mixture of hydroxylamine hydrochloride and sodium nitrite (1 : 1)   2 2 2 2 Hydroxylamine NH OH HNO N O 2H O    03. By reducing nitric acid with stannous chloride and hydrochloric acid. 04. By reducing nitric oxide with sulphur dioxide 2 2 2 4 2 2NO SO H O H SO N O     Properties: 01. The burning material decompose nitrous oxide into nitrogen and oxygen. 0 800 C 2N O 2N O 2 2 2   02. It supports combustion of sulphur, phosphorus, magnesium, sodium, candle and a splineter. S + 2N2O SO2 + 2N2 4P + 10N2O  2P2O5 + 10N2 Mg + N2O  MgO + N2 03. It is decomposed by red hot copper. Cu + N2O  CuO + N2 04. 2 2 3 3 N O NaNH NaN NH NaOH     2  H O2 N2  NH3  II. NO : Preparation: 01. By the action of dilute nitric acid on copper (Lab. Method). the nitric oxide liberated is collected over water.     3 d il 2 3 2 3 M C u / A g / P b 8 H N O 2 N O 4 H O 3 M N O     02. It can be preppared by treating nitrous acid with acidified iodide. 2HNO 2I 2H 2NO I 2H O 2 2 2        03. NO is obtained by the reduction of nitrates with acidified ferrous ions. 2 3 NO 3Fe 4H NO 3Fe 2H O 3 2          Properties: 01. It acts as a both oxidising and reducing agent 02. It oxidises H S2 to S, SO / H O 2 2 to H SO2 4 , SnCl / HCl 2 to SnCl4 etc. 2 4 2 2NO 3SnCl 6HCl 3SnCl 2NH OH     03. It reduces MnO / H 4   to 2 Mn  , 2 Cr O / H 2 7   to 3 Cr  etc 04. NO NO  nitrosonium ion  Bond order : Bond length : 2.5 3.0 0 1.15A 0 1.06A 05. It reacts with Cl2 and gives nitrosyl chloride NO Cl 2NOCl nitrosyl chloride  2   06. It readily form coordination complexes with transition metal ions. These complexes are called nitrosyls. Ex:     2 2 5 Fe H O NO      : Brown ring complex 2 2     5 Na Fe CN NO .2H O     : Sodium nitro prusside 07. NO often acts as a three electron donor, in contrast to most ligands which donate two electrons. Thus,three CO groups may be replaced by two NO groups.       5 2 2   Fe CO 2NO Fe CO NO 3CO              6 4   Cr CO 4NO Cr NO 6CO          III. N O2 3 : Preparation: 01. The mixture of NO and NO2 may be obntained by the action of 6N nitric acid on copper.
NISHITH Multimedia India (Pvt.) Ltd., 3 JEE MAINS - CW - VOL - I VA GROUP ELEMENTS NISHITH Multimedia India (Pvt.) Ltd., JEE ADVANCED-VOL-VII   3 2 3 2 2 2 6 Cu HNO      NO NO Cu NO H O 2 3 N2 3 O Condensation 02. It is obtained by the reduction of nitric acid with arsenious oxide. 3 2 2 3 2 3 2 5 2 5 2 3 4 2 2 2 3 2 HNO H O N O O As O O As O As O H O H AsO        As O HNO H O H AsO N O 2 3 3 2 3 4 2 3     2 2 2 Properties: 01. It condenses to a blue coloured liquid at –300C. The liquid when warmed at room temperature, decomposes to a mixture of NO and NO2 (Brown coloured) room temperature N O NO NO 2 3 2   02. N O NH OH NH NO H O 2 3 4 4 2 2     N H O 2 2  03. N O2 3 is a weakly acidic oxide. It form nitrosyl salts when reacts with strong acids like H SO2 4 , HClO4 . N O 2H SO 2NO HSO H O 2 3 2 4 4 2      N O 2HClO 2NO ClO H O 2 3 4 4 2      IV. NO2 : Preparation: 01. NO2 is obtained by heating heavy metals like M Cu, Ag, Zn, Pb, Hg   with concentrated nitric acid. 3 2 3 2   M conc HNO NO M NO H O 2     M Cu, Ag, Zn, Pb, Hg   02. Tin on treating with concentrated nitric acid nitrogen dioxide is liberated   3 2 3 2 2 metastannic acid Sn conc HNO H SnO H O NO     Properties: 01. It acts as a both oxidising and reducing agent. 02. It oxidises H S2 to S, SO / H O 2 2 to H SO2 4 , CO to CO2 , HCl to Cl2 etc 03. It oxidises P to 2 5 P O , S to 2 SO , C to CO2 04. It can oxidise metals like Na, K, Sn etc.. 05. It liberates iodine from KI and turns starch iodide papeer blue. 2 2 2 2 2 KI NO    2KNO I 06. It reduces MnO / H 4   to 2 Mn  , 2 Cr O / H 2 7   to 3 Cr  , O3 to O2 etc NO O O N O 2 3 2 2 5    07. It reacts with F2 and Cl2 , forming nitryl fluoride and nitryl chloride. 2 2 2 2NO F 2NO F   2 2 2 2NO Cl 2NO Cl   08. 2 2NO cool hot N O2 4 paramagnetic  brown gas diamagnetic  colourless solid  09. The N N bond in N O2 4 is longer than the N N bond in N H2 4 . 10. Solid N O : 2 4 planar molecule 11. Liquid N O2 4 is useful as a non - aqueous solvent. It self - ionizes :     2 4 3 acid base N O NO NO     12. In N O2 4 , substances containing NO are acids and those containing NO3  are bases. Ex:           4 3 4 2 4 acid base salt solvent NOCl NH NO NH Cl N O    acid base reaction  13. When obsorbed by Alkalies, Nitrites and nitrates are formed. 2 2 3 2 2NO     2NaOH NaNO NaNO H O
VA GROUP ELEMENTS 4 NISHITH Multimedia India (Pvt.) Ltd., JEE ADVANCED-VOL-VII NISHITH Multimedia India (Pvt.) Ltd., V. N O2 5 : Preparation: 01. It is also prepared by the action of dry chlorine on solid silver nitrate at 95oC. 4AgNO s 2Cl dry 2N O 4AgCl O 3 2 2 5 2         Properties: 01. In vapour phase, it is covalent 02. In solid phase , it is ionic 03. Solid N O2 5 : NO NO 2 3   (nitronium nitrate) 04. N O NaCl NaNO NO Cl 2 5 3 2    N O Na NaNO NO 2 5 3 2    05. In vapour phase, it decomposes to NO, NO ,O2 2 06. It acts as oxidising agent Ex: N O I I O NO 2 5 2 2 5 2    07. Nitrogen trioxide is obtained by treating N O2 5 with ozone. N O O NO O 2 5 3 3 2    08. N2 5 O is decomposed by alkalie metals N2 5 3 2 O Na NaNO NO    09. It forms nitrate salts with alkalies. 2 5 3 2 N O NaOH NaNO H O    2 2 Properties of oxides of phosphorus: I. P O4 6 : 01. It condenses at 0 5 C 02. In cold water it dissolves slowly forming phosphorus acid. P O 6H O 4H PO 4 6 2 3 3   hydrolysis 4 6 3 4 3 hot P O H PO PH   (disproportionation reaction) 03. When heated above 210oC, it forms red phosphorus and another oxide, P4O8 0 250 C 4P O 3P O P 4 6 4 8 4    04. It burns in chlorine forming oxy-chlorides. P O 4Cl 2POCl 2PO Cl 4 6 2 3 2    II. P O4 10 : 01. It condenses at 0 60 C 02. P O 6H O 4H PO 4 10 2 3 4   03. 4 10 3 4  2 P O 6CaO 2Ca PO   04.     4 10 2 3 4 strongly acidic behaves likea basic oxide P O 2 B O 4BPO   Structure of phosphorus trioxide Structure of phosphorus pentoxide Important reactions: 01. NCl 3H O NH 3HOCl 3 2 3    02. PCl 3H O H PO 3HCl 3 2 3 3    03. AsCl 3H O H AsO 3HCl 3 2 3 3    04.   3 2 white SbCl H O SbOCl 2HCl    05.   3 2 white BiCl H O BiOCl 2HCl    SbOCl: antimonyl chloride: SbO Cl      : contain oxocation BiOCl: bismuthyl chloride: BiO Cl      : contains oxocation