COLOR OF THE TRANSITION ELEMENTS

1. COLOR OF THE TRANSITION ELEMENTS Presenter: MS SAMIA SAADIA (Vice Principal) Subject: CHEMISTRY Class: XII Defence Authority College for Women - Phase VIII ColourinTansition Metal Complexes Application of Crystal Field Theory

2. CONTENTS • Introduction of Transition Metal Complex • Explanation of the subject by Crystal Field Theory (C F T) • Distinction Between the d-orbitals splitting in Octahedral and Tetrahedral complexes • Visible Region of the Spectrum • Examples • References

3. TRANSITION ELEMENTS Introduction Transition elements are known by this name because they show their properties which are transitional between highly reactive and strong electropositive elements of s-block which form ionic bonds and highly electronegative elements of p-block elements which form largely covalent compounds. B-group elements are transition elements Transition elements consists of following :- d- block elements f- block elements d- block elements are placed in the middle (in between the s & p- block elements) & f- block elements are placed at the bottom of the periodic table separately.

4. TransitionElementsd-block elements • The elements in which d-orbitals are progressively filled up with electrons are called d-block elements. • The elements in which the last electron (differentiating) electron enters (n-1)d orbitals i.e d-orbitals of the penultimate shell. • d- block elements also called outer transition elements. f- block elements • Transition elements in which f-orbitals are partially filled are called f-block elements. • These are named as Inner Transition Elements or Rare Earth elements.

6. d-Block covered in XII Syllabus

7. Color of the Transition Elements Complex or Coordination Compounds: Metal atom or ion surrounded by oppositely charged ions or neutral molecules. Polyatomic ion or molecule in which number of ions or molecules are bonded to a transition metal ion or atom through coordination bonds. Tendency of Transition metals to form complex compounds: Due to small size of the metal atoms or their cations, have a high charge density on them. Makes the atom or cation to attract(accept) the lone pair of electrons from the ligands. Have vacant d-orbitals [(n-1)d orbitals] to accommodate the lone pairs of electrons donated by ligands to form coordinate bonds (L→M).

8. Color of the Transition Elements Complex ion: When one or more neutral molecules or negatively charged ions become attached to central atom by coordination bond. It is charged positively or negatively. Ligand or Coordination group: An ion or neutral molecules surrounding a centre atom A part of complex compound which is directly attached with the central transition atom by coordination bonds. Transition metals accept electrons from negatively charged Ions and acts as Lewis acid or electrophile. Legands are electron donors and are called Lewis Base or Nucleophile. Coordination Number “n”: The number of ligands attached to a centre atom or the number of coordination bonds formed with in a single central atom in a complex compounds. It is usaully fixed for a metal.

9. Color of the Transition Elements • A Complex compound or Complex ion consists of • A Cation (+ve) • A coordination Sphere is: • Positively charged & Negatively charged • A coordination Sphere consists of: • Metal atom or Central metal ion • Ligand (Neutral molecules & Anion which can donate pair of electrons) • Strength of Ligands in magnetic field for a common metal ion: increasing_∆ Cl <F <H2O <NH3 <en < NO2 (N-bonded) <CN • This list is known as Spectrochemical Series • Ligands lie on the low end of series are termed as weak field ligands & on the high end are called strong ligands

10. Color of the Transition Elements CRYSTAL FIELD THEORY • A model for bonding in transition- metals complexes • The interaction between metal ion & ligand is viewed as electrostatic • The ligands produce an electric field that causes a splitting in the energies • In a six coordinate octahedral complex, when the ligand approach the metal ion along x, y, z axis the overall energy of the metal ion plus ligand is lowered (more stability) • When the ligands are drawn towards the metal centre, there is a repulsive interaction between the outermost electrons on the metal & the negative charges on the ligands.This interaction is called crystal field • The crystal field causes the energies of the d-electrons on the metal ion to increase • The repulsive interaction give rise to the splitting of the d-orbitals

11. Color of the Transition Elements FIGURE : CRYSTAL FIELD THEORY Separated Metal and Ligands Electrostatic Attraction Energy Splitting of Outer D-orbital in octahedral field Ligands-d Electrostatic Repulsion Metal Ion Plus Coordinated Ligands

12. Color of the Transition Elements Central transition atom in complex ion contain partially filled d-orbital The color is due to the bonding between transition metal and ligand i.e electrostatic and is most successfully explained by Crystal Field Theory The electrostatic field splits the five degenerated d- orbitals into two sets of energy levels namely t2g (triply degenerate) & engerade or eg (doubly degenerate) T2g includes orbitals lie in between the axis (non-axial) eg includes orbitals lie on the axis (axial) This splitting causes unpaired electrons to transit triply degenerate from one set to another The ∆E0 i.e. energy difference is too small and equivalent to the wavelength that electron jump from an orbital to the other

13. dxy dyz A high energy pair, dx2-y2 and dz2 designated as “eg” (Doubly degenerate) dx2-y2 dz2 eg dzx dx2-y2 dz2 Td t2g dxy dyz dzx A lower energy trio, dxy, dyz and dzx designated as “t2g” (Triply degenerate) Color of the Transition Element

14. Splitting of d orbitals in an Octahedral Field

15. Splitting of d orbitals in an Octahedral Field Example: [Co(NH3)6]2+

16. Splitting of d-orbitals in an Octahedral Field • According to C F T, the interaction between metal ion ligands in a complex is electrostatic • In free metal ions, all five d-orbitals have equal energies & are called degenerate orbitals • Lone pairs present on the ligands attract the positively charge metal ion • When six ligands (strong field ligand) approach the set d-orbitals along x, y, z axis (dx2-dy2 ,dz2), this directionof approach produces an octahedral complex • Stronger repulsion occur between the two orbitals & approaching ligands • This raises the energies of these d-orbitals than their energies in free ion • The energies of other d-orbitals which are between the axis i.e dxy, dyz & dxz are not raised • As a result the d-orbitals of central metal ion split into two sets eg (higher energy) & t2g (lower energy) • Strong field ligand, create a splitting of d-orbitals energies i.e large enough to overcome the spin-pairing energy • The d-electrons then preferentially pair up in the lower energy orbitals producing a low- spin complex

17. Splitting of d orbitals in a Octahedral Complex Example: [Co(NH3)6]2+ • The strongest repulsion occurs between these two d-orbitals and approaching ligands. • In free metal ions all five d-orbitals have equal energies and are called degenerate orbitals. • When six ligands (NH3) approach the set of d-orbitals along x, y & z axis (dx2- y,2 dz2) the direction of approach produces an octahedral complex. • This raises the energies of these d-orbitals more than the energies in free ions. • The energies of the other d-orbitals which are between the axis i.e dxy, dyz & dxz are not raised. • As a result the d-orbitals of central metal ions split into two sets eg (higher energy) and t2g(lower energy). As NH3 is strong field ligand, so low spin complex is formed.

18. Splitting of d orbitals in a Tetrahedral Field Example:[Co(NH3)4]2+

19. Splitting of d orbitals in a Tetrahedral Field • Example:[Co(NH3)4]2+ • In free metal ions, all five d- orbitals have equal energies and are called degenerate orbitals • When four ligands(eg NH3) approach the set of d-orbitals along x, y, and z axis dxy, dyz & dxz. This approach produces tetrahedral complex • Stronger repulsion occur between these three d- orbitals and approaching ligands • This raises the energies of these d- orbitals which are on the axis • As a result the d- orbitals of central metal ion split into two sets t2g (higher energy) & eg (lower energy) • When the ligand exert a weak crystal field, the splitting of the d- orbital is small • The electrons then occupy the higher energy d-orbitals in preference to pairing up in the lower energy set, producing a high- spin complex

20. Color of the Transition Elements • d-Orbital Splitting • The magnitude of the splitting of the d-orbitals in a transition • metal complex depends on three things: • The geometry of the complex • The oxidation state of the metal • The nature of the ligands • The Nature of the Ligands • Some ligands only produce a small energy separation among • the d-orbitals while others cause a wider band gap. • Ligands that cause a small separation are called weak field • ligands and those that cause a large separation are called • strong field ligands. • The ordering of their splitting ability is called the spectrochemical • series. • Increasing • Cl < F< H2O < NH3 < en < NO2(N-bonded) < CN

21. Colour and Variation in Color • Oxidation State of the metal atom/ion. eg Cu1+(White), Cu2+(Blue) • Geometry of the complex. eg [Zn(NH3)4]2+(White), [Fe(CN)]63-(Violet) • Nature and approach of the ligand. eg [Cu(H2O)6]2+(Blue), [Cu(NH3)2]2+(Deep Blue)

22. Colour and Variation in Color eg [Ti(H2O)6]3+ absorbs blue green color at 4900A-5000A & transmits Red-Purple color but [Ti(F)6]3- absorbs yellow color at 5750A- 5900A& transmits violet color. Reason: changes weaker ligand smaller crystal field splitting at range of longer wave length.

23. Effect of the nature of ligand when metal shows same oxidation state Examples: A comparison of the visible absorption maxima for a number of cobalt (III) complexes shows the effects of ligands on the d-orbital band gap.

24. Color of the Transition Elements VISIBLE REGION OF THE SPECTRUM: This excitation involves absorption of light (photons) of certain wave length in the region of visible light(3800A0-7800A0) and release of energy is observed in the form of colors ‘VIBGYOR’ This is called d-d transition which is responsible for the color

25. Color of the Transition Elements If we add the colors on opposite sides of the wheel together, white light is obtained. We only detect colors when one or more of the wavelengths in the visible spectrum have been absorbed, and thus removed, by interaction with some chemical species. When the wavelengths of one or more colors is absorbed, it is the colors on the opposite side of the color wheel that are transmitted.

26. Why go Green? • If red, yellow, orange, blue and violet are absorbed... only one color is transmitted: GREEN. • If violet, red, and orangeare absorbed… then blue, green and yellow are transmitted ... And the middle color which is perceived... GREEN

27. Pictorial Presentation of the concept

28. Pictorial Presentation of the concept a) Sample absorbs all , black color perceived White Light Black Only Sample does not absorb any color of light. White light is perceived White light White light Sample

29. Everyday Life Examples Chlorophyll (Green matter of leaves) Grass and leaves appear green because chlorophyll absorbs wavelengths in the red and blue portion of the visible spectrum. The wavelengths in between (green) are transmitted.

30. Everyday Life Examples • Vitamin B12 (Cobalamin) contains Co (III) : • The antipernicious anemia vitamin owning to its curative effect in anemia • Isolated from liver & the compound is usaully referred to as Cyanocobalamin • Presence of Cobalt atom in the trivalent state • The only organic compound which contains cobalt • It appears as a red crystalline compound containing nitrogen, phosphorus & cobalt

31. Everyday Life Examples

32. Color of the Transition Elements Examples of Transition Metal Complexes: • When light passes through a solution containing transition metal complexes, we see those wavelengths of light that are transmitted. • The color of the transmitted light is called complementry color of the absorbed light • The solutions of most octahedral Cu (II) complexes are blue. The visible spectrum for an aqueous solution of Cu (II), [Cu(H2O6]2+, shows that the absorption band spans the red-orange-yellow portion of the spectrum and green, blue and violet are transmitted.

33. The absorption band corresponds to the energy required to excite an electron from the t2g level to the eg level. The energy possessed by a light wave is inversely proportional to its wavelength. The Cu(II) solution transmits relatively high energy waves and absorbs the low energy wavelengths. This indicates that the band gap between the two levels is relatively small for this ion in aqueous solution. Excitation of d electron in Cu(II) Complex

34. Color of the Transition Elements Examples: Anhydrous Cobalt Compounds: They absorbs light for the excitation of their d-electrons. When red color is absorbed from light, then the transmitted light consists of wavelengths corresponding to other colors of white light in which the blue color predominates and the cobalt compounds thus appear blue green. Hydrated Cobaltic Compounds: absorbs light of a different wavelength blue green and therefore appears red in color. Co, [Co(NH3)6]2+  appears blue because the incoming ligand interacts with the d-orbital of transition metal ion. Thus interaction results in the  splitting of the energies of d-orbital. It causes the unpaired electrons to transit from one set to another. This excitation involves absorption & release of energy is observed in the form of blue color in the visible region of spectrum.

35. ColourChange Physical state:Anhydrous and hydrated species of a metal atom or ion absorb at different wavelengths that is why exhibit different colors. Examples: • Anhydrous Cobalt Compounds absorb (6250A-7500A) red color from the light& appear blue green. • Hydrated Cobalt Compounds are peach red in colour. They absorb (4900A-5000A) blue green color from the light & transmit red color • Approach of ligand:In a solution, if ligand is Ammine, then it appears blue. • Oxidation state: Cu(I) is white but Cu(II) are blue-green. • Fe(II) is light green but Fe(III) shows rust colour. • Cr(III) is deep green but Cr(VI) appear orange yellow.

36. References • Chemistry of Transition Elements by Dr M. S Yadav • College Chemistry by M.M.Baig • Inorganic Chemistry & Advance Inorganic Chemistry by Satya • Parkash, G.D Tuli, S.K Basu, R.D Madan • Essentials of Teaching Skills by Chris Kyriacon • British Education Research Association Conference, Manchester- • 2004by David Hall • Andy Ash and Carlo Raffo Research Proposal presented at Africa- • Asia Dialogue Seminar held at the United Nations University Tokyo • 10th of March 2006 • General Chemistry by Hill and Petrucci; • Chemistry by Mc. Murrey and Fay (c) 1995 by Prentice-Hall, Inc. A • Sinmon and Schuster Company. Engle Wood Clif New Jersey 07632 • Kroschwitz / Winokur / Lees, Chemistry; A first course, 3c (c) 1995 • Wn.C. Round Communications. Inc, Dubuque I.A • Computers, IT, Multimedia, Periodic tables etc. • www.wou.edu ,Net googling • Chemistry The Central Science Brown LeMay Burslen, 7th edition • Chemistry (6th Edition) Steven S. Zumdahl & Susan A . Zumdahl • A text book of animal physiology, R.Nagabhushanam, M.S.Kodarkar, • R. Sarojini