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General properties Transition Metals The transition metals lie between groups 2A and 3A of the periodic table. They are malleable and ductile They are good conductors of heat and electricity Transition metals are less reactive but melting and boiling points are higher than 1A and 2A group elements

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I R O N Its density is 7.87 g/cm3 Melting point is 1538 oC Boiling point is 2861 oC Pure iron is a silvery white colored, lustrous, soft metal with important magnetic properties. It is malleable and ductile.

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Occurrence of iron Iron is second most abundant metal (6%) in the earth’s crust. But it is not found in elemental form in nature. Iron is found in most clays, sandstones and granites. Hematite Fe2O3 Pyrite FeS2 Magnetite Fe3O4 Siderite FeCO3 are common ores of iron

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Preparation of Iron In the laboratory 1. H2 gas is added to iron oxide Fe2O3 + 3H2 2Fe + 3H2O 2. Iron oxides are reduced by more active metals 3FeO + 2Al 3Fe + Al2O3 Fe2O3 + 2Al 2Fe + Al2O3 By the electrolysis of solutions of iron salts FeCl2 Fe + Cl2

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Chemical Properties of Iron Iron has 26Fe: [18Ar]4s23d6 electron configuration In compounds, iron takes +2 and +3 0xidation states (charges)

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Reactions of Iron 1) Iron reacts with dilute solutions of strong acids. Fe + 2HCl → FeCl2 + H2 Fe(s) + H2SO4(dil.) → FeSO4(aq) + H2(g) The reactions of iron with oxidizing acids form its salts, containing Fe3+ ions 2Fe(s) + 6H2SO4(conc) → Fe2(SO4)3(aq) + 3SO2 + 6H2O Fe(s) + 4HNO3(dil.) → Fe(NO3)3(aq) + NO(g) + 2H2O(l)

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2) Iron produces mixed oxides by water 2) Iron produces mixed oxides by water 3Fe + 4 H2O →Fe3O4 + 4H2 3) When iron is heated with sulfur iron sulfide, FeS forms Fe(s) + S(s) t FeS(s)

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4) At high temperature, it reacts with halogens. 4) At high temperature, it reacts with halogens. 2Fe(s) + 3Cl2(g) 1200°C 2FeCl3(s) Moisture and oxygen cause the formation of crystal hydrate of iron (III) oxide (corrosion) 4 Fe + 3 O2 + nH2O → 2Fe2O3 . nH2O red-brown

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Uses Iron is useful in our society today because iron is virtually used in everything : building ( bridge , highway , rail road ,etc.), transportation (car , train , boats ,plane, etc.) , tools (knife , machines , etc.)

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IMPORTANT COMPOUNDS OF IRON Iron has +2 and +3 oxidation states in its compounds. Fe2+ ion is called ferrous and compounds that contain Fe2+ ion are called ferrous compounds, Fe3+ ion is called ferric and Fe3+ compounds are called ferric compounds

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Iron (II) compounds (Ferro Compounds) 1. Iron (II) chloride, FeCl2 It is obtained by passing hydrogen chloride gas over heated iron. FeCl2 is a white colored crystal. Fe (s) + 2HCl (g) → FeCl2 (s) + H2 (g)

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2. Iron (II) oxide, FeO This compound is produced by decomposition of iron (II) oxalate. FeC2O4 (s) heat FeO (s) + CO (g) + CO2(g) FeO is also unstable in air. 4FeO (s) + O2 (g) → 2Fe2O3 (s)

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Iron (III) Compounds (Ferric Compounds) 1. Iron(III) chloride, FeCl3 When iron is reacted with chlorine gas, it produces iron(III) chloride. 2Fe(s) + 3Cl2(g) heat 2FeCl3(s)

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2. Iron (III) hydroxide, Fe(OH)3 It is obtained by the reaction of Fe3+ with a base or carbonates. It is similar to gelatin. Fe(OH)3 is a reddish-brown colored precipitate which shows amphoteric property. Fe3+(aq) + 3KOH(aq) → Fe(OH)3(s) + 3K+(aq)

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3. Iron (III) oxide, Fe2O3 3. Iron (III) oxide, Fe2O3 In nature Fe2O3 is found in hematite and limonite minerals. It can be obtained by several methods. 2FeCl3 + 3H2O heat Fe2O3 + 6HCl 4FeO + O2 → 2Fe2O3 2Fe(OH)3 → Fe2O3 + 3H2O 4Fe(OH)2 + O2 → 2Fe2O3 + 4H2O The most common preparation method of Fe2O3 is the burning of pyrite, FeS2 mineral. 4FeS2 + 11O2 → 2Fe2O3 + 8SO2

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Iron(II, III) oxide, Fe3O4 Iron(II, III) oxide, Fe3O4 Fe3O4, mixed oxide, is obtained by passing heated steam over iron metal or heating Fe2O3 3Fe + 4H2O heat Fe3O4 + 4H2 6Fe2O3 heat 4Fe3O4 + O2 Fe3O4 is found in nature as black colored magnetite.

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Compounds of Iron Ferro Compounds; Iron(II) compounds 1.Iron (II) chloride, FeCl2 2.Iron (II) sulfate ; FeSO4 . 7H2O 3.Iron (II) oxide; FeO Ferric Compounds; Iron (III) compounds 1.Iron (III) chloride; FeCl3 2.Iron (III) oxide; Fe2O3 3.Iron (III) hydroxide Fe(OH)3 Iron (II, III) oxide, Fe3O4