1. by : Mrs.Shashi Jit Virdi ASSOCIATE PROFESSOR Chemistry Department PGGCG, Sector 11 Chandigarh NOBLE GASES

2. Where are the noble gases? The elements in group 0, on the right of the periodic table, are called the noble gases. He Rn Xe Kr Ar Ne helium neon argon krypton xenon radon

3. NOBLE GASES  The group of noble gases is regarded as zero group of the periodic table.  These are gases at ordinary temperature and do not have chemical reactivity.  Due to chemical inertness, these were called inter gases.  The elements Helium (He), Neon (Ne), Argon (Ar), Krypton (Kr), Xenon (Xe) and Radon (Rn) comprise noble gases.

4. Atomic World: Fast and Furious 3,000 miles per hour 1 mile/sec Air (oxygen + nitrogen 1,000 miles per hour 7,000,000,000 collisions per second Helium

5. Now-a-days, as number of compounds of these gases, particularly of xenon and krypton have been prepared, this shows that these gases are not completely inert. They are called noble gases instead of inert gases which signifies that these gases have some reactivity. Because of the low abundance of these gases on earth, they have also been called rare gases.

6.  Mendeleef had not left any space for the noble gases in the periodic Table  Obviously, he could not imagine the existence of elements which have almost no chemical reactivity.

7.  Ramsay, discoverer of these gases, proposed a new group for these elements on the basis of their atomic masses and lack of chemical reactivity.  This group is called zero group of the periodic table. The zero group also suggests chemical inertness or zero valency.

8. Before the discovery of noble gases, there was a sudden change from the most electronegative halogens (on right hand side) to most electropositive alkali metals (left hand side) in the periodic table. The addition of zero group between VII A group and IA group has solved this anomaly.

9. The position of noble gases in the periodic table was later on confirmed by Moseley who constructed the periodic table on the basis of atomic numbers. The values of atomic number of noble gases strongly suggest that they should be placed after halogens and before alkali metals

10. ElementOuter electronic configuration Vander Wall's radius (Å) First IE (kj mol -1 ) m.pt. (K) b.pt. (K) ∆H fux (kj mol -1 ) ∆H vap (kj mol -1 ) He Ne Ar Kr Xe Rn 1s2 2s 2 2p 6 3s 2 3p 6 4s 2 4p 6 5s 2 5p 6 6s 2 6p 6 - 1.31 1.74 1.89 2.10 2.15 2372 2080 1519 1351 1170 1037 - 24.4 83.6 116 161 200 4.2 27.1 87.3 120 166 211 0.02 0.33 1.18 1.64 2.3 2.9 0.08 1.77 6.5 9.0 12.6 16.4 Physical Properties Noble gases

11. CHEMICAL INERTNESS OF NOBLE GASE S Chemical Inertness of these gases is supported by the reasons: i)The atoms have stable completely field electronic shells ii)They have high ionisation energies iii)The noble have almost zero electron affinities. Therefore, they do not have any tendency to gain, lose or share electrons with other atoms.

12. Chemical properties of Nobel Gases  The atoms of inert gases have saturated shells, therefore they are chemically inert.  Recent studies have shown that under certain specific condition, they enter into chemical combinations and form some rare chemical compounds.  The specific conditions and the types of compounds formed by these gases are disused below-

13.  Under excited condition:- Sparking Helium at low pressure in presence of mercury, tungsten etc. forms compounds like HgHe 2, HgHe 10, WHe 2..  Helium compounds are also fromed in discharge tubes like BiHe 2, FeHe, Pt 3 He, PdHe. These compounds are not considered as true chemical compounds as He is absorbed on the surface.

14. Compounds formed through co-ordination- Argon forms a number of unstable compound with varying no. of BF 3 molecules e.g. Ar.BF 3, Ar.6BF 3 In these compounds, argon atoms donates a pair of electrons to Boron atom of BF 3. In case of higher compounds fluorine atoms of BF 3 also donate pair of electrons.

15. c)Hydrates of noble gases:The hydrates of these gases are formed by compressing the gases with water e.g., Xe.6 H 2 O. d)Compounds formed by physical trapping (Clathrates) The inert gases Argon, Krypton and Xenon form solid compounds with certain organic molecules such as phenol and hydroquinone under pressure In such compounds the inert gas are enclosed in the crystal lattice of organic compounds known as clathrates or cage compounds.

16. Xenon forms a large no. of compounds with oxygen and fluorine in different oxidation states. These are xenon fluorides, xenon oxides and xenon oxifluorides. 1. XeF 2 Preparation. 1.Xenon di fluoride is best prepared by heating a mixture of xenon and fluorine in molecular ratio of 2:1 at 400 0 C in a sealed nickel tube. On cooling quickly, a colourless solid XeF 2 is obtained. Ni Xe+F 2 XeF 2 400 0 C Compounds of noble gases-

17. Properties 1.Xenon difluoride is a colourless, crystalline solid which melts at 129 0 C. 2.It reacts with hydrogen to give hydrogen fluoride and xenon. XeF 2 + H 2 Xe+2HF

18. 3. 3.It gives substitution reactions with strong protonic acids. XeF 2 + HX FXeX + HF FXeX + HXXeX 2 + HF Where X= CIO - 4 CF 3 COO -, SO 3 F - etc.

19. 4. It hydrolyses slowly but completely in acidic, neutral or alkaline solutions. 2 XeF 2 +2H 2 O 2 Xe+4HF+O 2 2 XeF 2 +4NaOH 2Xe+4NaF+O 2 +2H 2 O 5.It oxidizes iodine in the presence of BF 3 to give IF.

20. 2.XeF 4 Preparation.  It is prepared by heating a mixture of xenon and fluorine, in a nickel vassal, at 400 0 C under pressure of 5-6 atm.  It can also be synthesized by passing an electric discharge through a mixture of xenon and fluorine at -78 O C. Properties of XeF 4 are:  It is a colorless, crystalline solid, with m.pt. 117. 1 0 c, sublimes readily.  Oxidized by hydrogen to HF at 30 0 C.  A stronger fluorinating agent than XeF 2

21. 3. XeF 6 Preparation. 1.It is prepared by heating xenon with excess of fluorine (in the molar ratio of 1:20) in a nickel vessel at 250-300 0 C under pressure of 50-60 atm. Xe + 3F 2 XeF 6 2.It can also be obtained by the oxidation of XeF 4 with O 2 F 2 under pressure. XeF 4 + O 2 F 2 -130 0 c XeF 6 + O 2

22. 2XeF 6 +SiO 2 2XeOF 4 +SiF 4 2XeOF 4 +SiO 2 2XeO 2 F 2 +SiF 4 2XeO 2 F 2 +SiO 2 2XeO 3 +SiF 4 (explosive) Properties:- Crystalline substance, m.pt. 49.5 0 C, Mostly volatile, all the fluorides of xenon are greenish yellow colour vapour. It is extremely reactive. Therefore, it cannot be stored in glass or quartz vessels because of the following reactions which finally give the dangerously explosive xenon trioxide.

23. 2It reacts with fluoride ion acceptors to form adducts. XeF 6 +PtF 5 XeOF 4 +PtF 5 [XeF 5 ] + [PtF 6 ] - XeF 6 +SbF 5 XeF 6.SbF 5 [XeF 5 ] + [SbF 6 ] - XeF 6 +AsF 5 XeF 6.AsF 5 [XeF 5 ] + [AsF 6 ] -

24. 4.XeOF 4 Preparation : (i) Xenon Oxytetraflouride is prepared by partial hydrolysis of Xenon hexa flouride XeF 6 + H 2 O XeOF 4 + 2 HF (ii ) by the action of XeF 6 on silicon dioxide 2XeF 6 + SiO 2 XeOF 4 + SiF 4

25. Soon as the yellow colour of XeF 6 disappears, the contents are immediately quenched with solid CO 2. It is done to avoid the formation of XeO 3 (explosive) as: XeOF 4 +SiO 2 XeO 3 +SiF 4

26. Properties. 1.It is a colourless compound melting at -46 o C. 2 It is reduced by hydrogen to xenon. XeOF 4 +3H 2 Xe+H 2 O+4HF 3 It reacts with water or silica to form another oxyfluoride, XeO 2 F 2, in ;which xenon remains in the same oxidation state. Further reaction gives explosive compound XeO 3

27. 4 XeOF 4 + H 2 O XeO 2 F 2 + 2HF XeO 2 F 2 + H 2 O XeO 3 + 2HF 2XeOF 4 + SiO 2 2 XeO 2 F 2 + SiF 4 2XeO 2 F 2 + SiO 2 2 XeO 3 + SiF 4

28. 5. XeO 2 F 2 Preparation ; 1. by mixing XeO 3 and XeOF 4 at temperature close to - 78 O C. XeO 3 +XeOF 4 2XeO 2 F 2 The compound is purified by fractional distillation. 2. It is also formed when XeOF 4 is hydrolyzed or reacted with silica. 2XeOF 4 +SiO 2 2XeO 2 F 2 +SiF 4 XeOF 4 +H 2 O XeO 2 F 2 + 2HF

29. Properties. 1. It is a colourless solid. 2. Its melting point is 30.8 O C. 3. It is easily hydrolyzed to give xenon trioxide. XeO 2 F 2 + H 2 O XeO 3 + 2HF.

30. 6.XeO 3 Preparation. Xenon trioxide is prepared by the hydrolysis of XeF 6 or XeF 4 6XeF 4 + 12H 2 O 2XeO 3 + 4Xe +24HF+3O 2 XeF 6 + 3H 2 O XeO 3 + 6HF It acts as a powerful oxidizing agent in acidic medium. For instance, it oxidizes Pu 3+ to Pu 4+ in the presence of H + ions. 6Pu +3 + XeO 3 + 6H + 6Pu +4 + Xe + 3H 2 O

31. 7. Xe O 4 Preparation :- It is prepared by action of conc. H 2 SO 4 on sodium or barium xenate (Na 4 XeO 6 or Ba 2 Xe O 6 ) at room temp. Na 4 XeO 6 + 2H 2 SO 4 XeO 4 + 2Na 2 SO 4 +2H 2 O Properties: It is very unstable and decomposes to xenon and oxygen.

32. Structure of Some Xenon Compounds FormulaName Oxid n state m.pt. ( m.pt. ( o C)Structure XeF 2 Xenon difluoride +2129Linear XeF 4 Xenon tetra fluoride +4117Square Planner XeF 6 Xenon hexafluoride +649.6Distorted octahedron XeO 3 Xenon trioxide +6Explodes Pyramidal tetrahedral with one corner un occupied

33. XeO 2 F 2 Xenon dioxy difluoride +630.8Trigonal lipyramid (with one position unoccupied) XeOF 4 Xenon oxy tetrafluoride +6-46Square pyramidal (octahedral with one position un occupied XeO 4 Xenon tetra oxide +8-35.9Tetrahedral XeO 3 F 2 Xenon trioxy difluoride +8-54.1Trigonal bipyramidal Ba 2 [XeO 6 ]-4Barium perxenate +8octahedral

34. Structure and Bonding in Xenon Compounds FormulaStructure No. of e pairs No. of lone pairs VSEPR (Explanation of structure) XeF 2 Linear53Five electron pairs form trigonal bipyramidal with three lone pairs at equatorial positions XeF 4 Square Planner 62Six electron pairs form octahedron with two positions occupied by lone pairs XeF 6 Distorted octahedron 71Pentagonal bipyramidal or capped octahedron with one lone pair XeO 3 Pyramidal71Three π bonds so that the remaining four electron pairs form a tetrahedron with one corner occupied by a lone pairs.

35. FormulaStructureNo. of e pairs No. of lone pairs VSEPR (Explanation of structure) XeO 2 F 2 Trigonal lipyramid 71 Two π bonds so remaining five electron pair form trigonal bipyramid with one equatorial position occupied by a lone pair XeOF 4 Square pyramidal 71 One π bond so remaining six electron pairs form an octahedron with one position occupied by a lone pair. XeO 4 Tetrahedra l 80 Four π bonds so remaining four electron pair form a tetrahedron XeO 3 F 2 Trigonal bipyramid 80 Three π bonds so remaining five electron pairs form trigonal bipyramid Ba 2 [XeO 6 ]Octahedral 80 Two π bonds so remaining six electron pair form an octahedron.

36. . Xe. XeF 4 sp 3 d 2 Xe F.. F. Molecule Type of Hybridization Geometrical Shape XeF 2 F F F F

37. XeF 6 sp 3 d 3. Xe xe XeO 3 sp 3 F F F F F F. Geometrical Shape Molecules & Type of hybridization

38. xe O F O XeOF 4 sp 3 d 2 Xe F XeO 2 F 2 sp 3 d O FF F F. F XeO 2 F 4 Sp 3 d 2 Xe O FF F F O

39. XeOF 4 Sp 3 d 2 Xe O FF F O XeO 6 Sp 3 d 2 Xe OO O F O -4 O.

40. Significance of Noble gases in development of theoretical chemistry. 1. In Elucidation of distribution of electrons in atom 2. In periodic classification 3. In the development of electronic theory of valency 4. In radioactivity.

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