1 / 30

Lecture 16. The Halogens

Lecture 16. The Halogens. PhD Halina Falfushynska. Group 17 elements properties. The Group 17 elements are known as the halogens. All are non-metals. • The elements exist as diatomic molecules, X2.

phinney
Download Presentation

Lecture 16. The Halogens

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Lecture 16. The Halogens PhD Halina Falfushynska

  2. Group 17 elements properties • The Group 17 elements are known as the halogens. All are non-metals. • • The elements exist as diatomic molecules, X2. • • Fluorine is the most electronegative element, and forms compounds only in the –1 oxidation state. For the other halogens the oxidation states up to +7 are also observed. • Their melting and boiling points steadily increase with atomic number. • • Going down the group, the elements become less oxidizing.

  3. • Astatine is radioactive, with the longest lived isotope having a half life of only several hours. • Fluorine and chlorine react with water. Bromine and iodine are only sparingly soluble in water but are soluble in various organic solvents such as chloroform, carbon tetrachloride, carbon disulphide and hydrocarbons to give coloured solutions. • • The X2 bond dissociation enthalpies generally decrease going down the group, but the value for F2 is anomalously low due to a high degree of electron–electron repulsion.

  4. Preparation of Chlorine and other halogens • By heating manganese dioxide with concentrated hydrochloric acid. • MnO2 + 4HCl → MnCl2 + Cl2 + 2H2O 4NaCl + MnO2 + 4H2SO4 → MnCl2 + 4NaHSO4 + 2H2O + Cl2 • By the action of HCl on potassium permanganate.2KMnO4 + 16HCl → 2KCl + 2MnCl2 + 8H2O + 5Cl2 • Deacon’s process: By oxidation of hydrogen chloride gas by atmospheric oxygen in the presence of CuCl2 (catalyst) at 723 K.

  5. Preparation of Chlorine

  6. Electrolytic process: Chlorine is obtained by the electrolysis of brine (concentrated NaCl solution). • 2 NaCl + 2 H2O → Cl2 + H2 + 2 NaOH Cathode: 2 H+ (aq) + 2 e− → H2 (g) Anode: 2 Cl− (aq) → Cl2 (g) + 2 e−

  7. Preparation of Chlorine and other halogens • K2Cr2O7 + 6KJ +7H2SO4  4K2SO4+ Cr2(SO4)3 +3J2+ 7H2O • 2NaCl + 4H2SO4 + PbO2 Cl2 + Pb(HSO4)2 + 2NaHSO4 + 2H2O • 4HCl + CaOCl2  CaCl2 + 2Cl2  + 2H2O • 4HCl + O2 2H2O + 2Cl2  • HJO + H+ + e  1/2J2 + H2O

  8. Preparation of Bromine 2NaBr + H2SO4 + H2O2 = Br2 + Na2SO4 + 2H2O

  9. Reactivity towards metals They react with metals to form halides. The reactivity of the halogens decreases down the group. Mg (s) + Br2 (l) → MgBr2 (s) 2Al + 3Cl2 → 2AlCl3 The ionic character of the halides decreases in the order MF > MCl > MBr > MI where M is a monovalent metal. 2Na + Cl2 2NaCl

  10. Reactivity towards oxygen Halogensformmanyoxideswithoxygenbutmostofthemareunstable. Fluorineformstwooxides OF2and O2F2. Botharestrongfluorinatingagents. O2F2oxidisesplutoniumto PuF6andthereactionisusedinremovingplutoniumas PuF6fromspentnuclearfuel. Chlorine, bromineandiodineformoxidesinwhichtheoxidationstatesofthesehalogensrangefrom +1 to +7. Orderofstabilityofoxidesformedbyhalogens, I > Cl > Br. Thehigheroxidesofhalogenstendtobemorestablethanthelowerones.

  11. H H Cl Cl Halogen + metal ionic salt Na + - Cl Na Cl Halogen + non-metal covalent molecule The halogens – some reactions 1) Halogen + metal: + 2) Halogen + non-metal: +

  12. Reactivity of halogens towards other halogens Reactivity of halogens towards other non-metals Halogens combine amongst themselves to form a number of compounds known as interhalogens of the types XX ′ , XX3′, XX5′ and XX7′ where X is a larger size halogen and X’ is smaller size halogen Halogensreactwith a numberof non-metalstoformhalides P4 + 6Cl2 → 4PCl3 S8 + 4Cl2 → 4S2Cl2 H2 + Cl2 → 2HCl

  13. Reaction of Aluminium with Bromine. Aluminium is oxidized by liquid bromine. Reaction of read Phosphorus with Bromine. The oxidation of red phosphorus with bromine proceeds under combustion.

  14. Reactivity towards water Reactivity of halogens towards alkalies 2NaOH + Cl2 → NaCl + NaOCl + H2O(cold and dilute)6 NaOH + 3Cl2 → 5NaCl + NaClO3 + 3H2O(hot and conc.)With dry slaked lime it gives bleaching powder.2Ca(OH)2 + 2Cl2 → Ca(OCl)2 + CaCl2 + 2H2O Ca(OH)2 + Cl2 → CaOCl2 + H2O When chlorine is inhaled at concentrations above 30 ppm, it begins to react with water and cells, which change it into hydrochloric acid (HCl) and hypochlorous acid (HClO) - Chlorine water. Cl2 + H2O → HCl + HClO

  15. Disproportionation and Comproportionation of Bromine and Iodine. Aqueous solutions of bromine and iodine are disproportionated under the influence of NaOH. Oxidation of Iodide with Halogenates. The formation of iodine by oxidation of iodide with halogenates is dependent on the pH value.

  16. A halogen oxidises halide ions of higher atomic number.F2 + 2X– → 2F– + X2 (X = Cl, Br or I)Cl2 + 2X– → 2Cl– + X2 (X = Br or I)Br2 + 2I– → 2Br– + I2 • The relative oxidising power of halogens can be illustrated by their reactions with water 2F2 (g) + 2H2O (l) → 4H+ (aq) + 4F− (aq) + O2 (g)X2 (g) + H2O (l) → HX (aq) + HOX (aq)( where X = Cl or Br )4I− (aq) + 4H+ (aq) + O2 (g) → 2I2 (s) + 2H2O (l)

  17. Chlorinewaterhas strong oxidisingandbleachingproperties • Itoxidisesferroustoferric, sulphitetosulphate, sulphurdioxidetosulphuricacidandiodinetoiodicacid.2FeSO4 + H2SO4 + Cl2 → Fe2(SO4)3 + 2HClNa2SO3 + Cl2 + H2O → Na2SO4 + 2HClSO2 + 2H2O + Cl2 → H2SO4 + 2HClI2 + 6H2O + 5Cl2 → 2HIO3 + 10HCl • Itis a powerfulbleachingagent; bleachingactionisduetooxidation.Cl2 + H2O → 2HCl + OColouredsubstance + O → Colourlesssubstance

  18. Hydrogen Halides • In laboratory, HCl is prepared by heating sodium chloride with concentrated sulphuric acid NaCl + H2SO4 → NaHSO4 + HCl (420K) • Hydrogen Halides can also be prepared by the hydrolysis of certain reactive halide compounds. PCl5 + H2O → POCl3 + 2 HCl 2PBr3 + 6H2O → 2H3PO3 + 6HBr • 2P + 3Br2 + 6H2O → 2H3PO3 + 6HBr • S + 3Br2 + 4H2O → 6HBr + H2SO4

  19. Hydrogen Chloride • When three parts of concentrated HCl and one part of concentrated HNO3 are mixed, aqua regia is formed which is used for dissolving noble metals.Au + 4H+ + NO3− + 4Cl− → AuCl−4 + NO + 2H2O3Pt + 16H+ + 4NO3 + 18Cl− → 3PtCl6− + 4NO + 8H2O • Hydrogen chloride is a monoprotic acid. In aqueous hydrochloric acid, the H+ joins a water molecule to form a hydronium ion, H3O+:HCl + H2O → H3O+ + Cl−

  20. Hydrochloric acid decomposes salts of weaker acids, e.g., carbonates, hydrogencarbonates, sulphites, etc.Na2CO3 + 2HCl → 2NaCl + H2O + CO2NaHCO3 + HCl → NaCl + H2O + CO2Na2SO3 + 2HCl → 2NaCl + H2O + SO2 • Hydrochloric acid is the preferred acid in titration for determining the amount of bases. Azeotropic or "constant-boiling" hydrochloric acid (roughly 20.2%) can be used as a primary standard in quantitative analysis. • It is use in the pickling of steel, to remove rust or iron oxide scale from iron or steel before subsequent processing: Fe2O3 + Fe + 6 HCl → 3 FeCl2 + 3 H2O

  21. Hydrochloric acid application • Regeneration of ion exchangers. Cation exchange is widely used to remove ions such as Na+ and Ca2+ from aqueous solutions, producing demineralized water. The acid is used to rinse the cations from the resins. • Hydrogen chloride is used to produce the hydrochloride salt of methamphetamine. • Hydrochloric acid is used in veterinary medicine as a gastric acidifier.

  22. Oxoacids of Halogens

  23. The structures ofoxoacids of chlorine

  24. TESTING FOR HALIDES

  25. Uses of Fluorine Uses of Bromine The main use of fluorine is toothpaste even though it isn’t as fluorine itself but instead as fluoride, a compound of fluorine. Bromine is one of the main ingredients in camera films (as silver bromide).

  26. Uses of Chlorine ---for bleaching woodpulp (required for the manufacture of paper and rayon), cotton and textiles --in the extraction of gold and platinum --in the manufacture of dyes, drugs and organic compounds such as CCl4, CHCl3, DDT, refrigerants, etc. --in sterilising drinking water ---preparation of poisonous gases such as phosgene (COCl2), tear gas (CCl3NO2), mustard gas (ClCH2CH2SCH2CH2Cl). Chlorine gas has also been used by insurgents against the local population and coalition forces in the Iraq War in the form of chlorine bombs. On March 17, 2007, for example, three chlorine filled trucks were detonated in the Anbar province killing two and sickening over 350.

  27. Uses of Iodine When dissolved in water, iodine can be used as a strong antiseptic or as a test for starch.

More Related