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S  08ߕ ``  X*  0 `   Z*  0 `   Z*z  bA޽h @ ?Parchment ̙33 Default Design 0 zr@ ( )   0h8 P    P*    0`=     R*  d  c $ ?    0<  @  RClick to edit Master text styles Second level Third level Fourth level Fifth level!     S  6xD `P   P*    6XI `   R*  H  0޽h ? ̙3380___PPT10. 0X(   $+ X X 0\X P    X*  X 0X\     Z*  X 6a `P   X*  X 6$f `   Z* H X 0޽h ? ̙3380___PPT10.1 0L0 P-(    0X? -AN INTRODUCTION TO TRANSITION METAL CHEMISTRYT$(2 82 f0f<f " <̙? x @ 0 0 ( <̙? x @L 0 0 ) 0XCx m OKNOCKHARDY PUBLISHING(2 fJ + C "A KTRE  , 0@H"`>B 2008 SPECIFICATIONS<G$G   B  s *޽h ? ̙33y___PPT10Y+D=' = @B +  0L0   ` (  dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0W   0\ INTRODUCTION This Powerpoint show is one of several produced to help students understand selected topics at AS and A2 level Chemistry. It is based on the requirements of the AQA and OCR specifications but is suitable for other examination boards. Individual students may use the material at home for revision purposes or it may be used for classroom teaching if an interactive white board is available. Accompanying notes on this, and the full range of AS and A2 topics, are available from the KNOCKHARDY SCIENCE WEBSITE at... www.knockhardy.org.uk/sci.htm Navigation is achieved by... either clicking on the grey arrows at the foot of each page or using the left and right arrow keys on the keyboard (2 2(2 2  75, dB   <D?` `    0){0P( OKNOCKHARDY PUBLISHING(2    0X _TRANSITION METALS2(2$f<fB  s *޽h ? ̙33y___PPT10Y+D=' = @B +`  0L0 o g  (    0G  f CONTENTS Definition Metallic properties Electronic configurations Variable oxidation state Coloured ions Complex ion formation Shapes of complexes Isomerism in complexes Catalytic propertiesF 2 2wddB  <D)P0Q  0Pp@ 0 0dB  @ <D)PXP   0X0@ 0 0  0[eP @o  0 0  6Fm @ 0 0  6(]x @ 0 0  6 mx @ 0 0  6]A @ 0 0  6 ]> @ 0 0  0X _TRANSITION METALS2(2$f<f  6 e> O @ 0 0  6 e@ / @ 0 0  6 e g @ 0 0B  s *޽h ? ̙33y___PPT10Y+D=' = @B + 0L0 p=(    0X˚Hx RBefore you start it would be helpful to& Recall the definition of a co-ordinate (dative covalent) bond Recall how to predict the shapes of simple molecules and ionsH*(2 2)dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0  0՚X _TRANSITION METALS2(2$f<fB  s *޽h ? ̙33y___PPT10Y+D=' = @B +y 0L0 0(   0dB 0 <D)P0Q 0 0Pp@ 0 0dB 0@ <D)PXP 0 0X0@ 0 0 0 0Kq~ p"THE FIRST ROW TRANSITION ELEMENTS 2#(2"ff 0 0 K60 Definition D-block elements forming one or more stable ions with partially filled (incomplete) d-sub shells. The first row runs from scandium to zinc filling the 3d orbitals. Properties arise from an incomplete d sub-shell in atoms or ions 8@ &  K B 0 s *޽h ? ̙33y___PPT10Y+D=' = @B +@  0L0 O G  ( w dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0  0Kq~ p"THE FIRST ROW TRANSITION ELEMENTS 2#(2"ff   0K60s M!Definition D-block elements forming one or more stable ions with partially filled (incomplete) d-sub shells. The first row runs from scandium to zinc filling the 3d orbitals. Properties arise from an incomplete d sub-shell in atoms or ions Metallic properties all the transition elements are metals strong metallic bonds due to small ionic size and close packing higher melting, boiling points and densities than s-block metals K Ca Sc Ti V Cr Mn Fe Co m. pt / C 63 850 1400 1677 1917 1903 1244 1539 1495 density / g cm-3 0.86 1.55 3 4.5 6.1 7.2 7.4 7.9 8.9@2PP@lPPx @nPF !2,3Pf G P@  f   B  s *޽h ? ̙33y___PPT10Y+D=' = @B +% 0L0 l%d%EH$(  dB  <D>+   0?K p D4s&(2  0DKW  A3$(2L k 7 # 7y~  N??kw 7~  N??k7~  N??k)7~   N??)k7~   N??w k 7^B   6Df>L  P x   # @4a ~   N?? P + ~  N??+P  ~  N??P x dB  <DK dB  <D ^B  6DoK ^B  6DoC9 C  0hBK a  D3p&(2  0QK  D3d&(2L NT - # 4yfB  6Df>WWN  P x   ` sT ?~  N?? P + ~  N??+P  ~  N??P x lB  <D>PlB  <D>WlB  <D>WlB  <D=P~   N??M a -fB ! 6Doj  " 0YK A4$(2fB # 6Doj  $ 0^Ks)G D4p&(2 % 0bK|)P D4d&(2 & 0gKN)" D4f&(20L Zo (# R j VfB ) 6DooofB *B 6DoZo0L Zo +# Zr> fB , 6DooofB -B 6DoZo0L Zo .# > fB / 6DooofB 0B 6DoZo0L Zo 1#  "> fB 2 6DooofB 3B 6DoZo0L Zo 4# Yq> fB 5 6DooofB 6B 6DoZo0L Zo 7# > fB 8 6DooofB 9B 6DoZo0L Zo :# > fB ; 6DooofB <B 6DoZo = 0pK y=ELECTRONIC CONFIGURATIONS OF THE FIRST ROW TRANSITION METALS  >(2>f > 0uKf0 S POTASSIUM. (2 U ? 0Kf   1s2 2s2 2p6 3s2 3p6 4s1(2      dB @ <D)@0A A 0Pp@ 0 0dB B@ <D)@X@ C 0X0@ 0 0V F 0Kr 0a ,In numerical terms one would expect the 3d orbitals to be filled next. However, because the principal energy levels get closer together as you go further from the nucleus coupled with the splitting into sub energy levels, the 4s orbital is of a LOWER ENERGY than the 3d orbitals so gets filled first.z- 2\N 4,+ G 6K? y  $ Aufbau Principle,8K<  H 6K2U  e)INCREASING ENERGY / DISTANCE FROM NUCLEUS *(2*z  bA޽h @ ?Parchment ̙33% 0L0 Z%R%GJ$( ޽h dB  <D>+   0K p D4s&(2  0pKW  A3$(2L k 7 # 7y~  N??kw 7~  N??k7~  N??k)7~   N??)k7~   N??w k 7^B   6Df>L  P x   # @4a ~   N?? P + ~  N??+P  ~  N??P x dB  <DK dB  <D ^B  6DoK ^B  6DoC9 C  0K a  D3p&(2  0еK  D3d&(2L NT - # 4yfB  6Df>WWN  P x   ` sT ?~  N?? P + ~  N??+P  ~  N??P x lB  <D>PlB  <D>WlB  <D>WlB  <D=P~   N??M a -fB ! 6Doj  " 0K A4$(2fB # 6Doj  $ 0dKs)G D4p&(2 % 0lK|)P D4d&(2 & 0KN)" D4f&(20L Zo (# R j VfB ) 6DooofB *B 6DoZo0L Zo +#  VfB , 6DooofB -B 6DoZo0L Zo .# Zr> fB / 6DooofB 0B 6DoZo0L Zo 1# > fB 2 6DooofB 3B 6DoZo0L Zo 4#  "> fB 5 6DooofB 6B 6DoZo0L Zo 7# Yq> fB 8 6DooofB 9B 6DoZo0L Zo :# > fB ; 6DooofB <B 6DoZo0L Zo =# > fB > 6DooofB ?B 6DoZo @ 0K y=ELECTRONIC CONFIGURATIONS OF THE FIRST ROW TRANSITION METALS  >(2>f A 0Kf0 QCALCIUM.(2U B 0Kf   1s2 2s2 2p6 3s2 3p6 4s2(2      dB C <D)@0A D 0Pp@ 0 0dB E@ <D)@X@ F 0X0@ 0 0  I 0p 0P_ ,As expected, the next electron in pairs up to complete a filled 4s orbital. This explanation, using sub levels fits in with the position of potassium and calcium in the Periodic Table. All elements with an -s1 electronic configuration are in Group I and all with an -s2 configuration are in Group II.b- 2 ;  J 62U  e)INCREASING ENERGY / DISTANCE FROM NUCLEUS *(2*z  bA޽h @ ?Parchment ̙33' 0L0 1')'JM&(  dB  <D>+   0 p D4s&(2  0W  A3$(2L k 7 # 7y~  N??kw 7~  N??k7~  N??k)7~   N??)k7~   N??w k 7^B   6Df>L  P x   # @4a ~   N?? P + ~  N??+P  ~  N??P x dB  <DK dB  <D ^B  6DoK ^B  6DoC9 C  0(! a  D3p&(2  0(  D3d&(2L NT - # 4yfB  6Df>WWN  P x   ` sT ?~  N?? P + ~  N??+P  ~  N??P x lB  <D>PlB  <D>WlB  <D>WlB  <D=P~   N??M a -fB ! 6Doj  " 0/ A4$(2fB # 6Doj  $ 0<3s)G D4p&(2 % 0;|)P D4d&(2 & 0%N)" D4f&(20L Zo (# R j VfB ) 6DooofB *B 6DoZo0L Zo +#  VfB , 6DooofB -B 6DoZo0L Zo .# Zr> fB / 6DooofB 0B 6DoZo0L Zo 1# > fB 2 6DooofB 3B 6DoZo0L Zo 4#  "> fB 5 6DooofB 6B 6DoZo0L Zo 7# Yq> fB 8 6DooofB 9B 6DoZo0L Zo :# > fB ; 6DooofB <B 6DoZo0L Zo =# > fB > 6DooofB ?B 6DoZo0L Zo @# ZrfB A 6DooofB BB 6DoZo C 0F y=ELECTRONIC CONFIGURATIONS OF THE FIRST ROW TRANSITION METALS  >(2>f D 0If0 RSCANDIUM. (2w E 0Mf   1s2 2s2 2p6 3s2 3p6 4s2 3d1(2       dB F <D)@0A G 0Pp@ 0 0dB H@ <D)@X@ I 0X0@ 0 0 L 0D\p 0P &With the lower energy 4s orbital filled, the next electrons can now fill p the 3d orbitals. There are five d orbitals. They are filled according to Hund s Rule. BUT WATCH OUT FOR TWO SPECIAL CASES.: 2'>R, M 6e2U  e)INCREASING ENERGY / DISTANCE FROM NUCLEUS *(2*z  bA޽h @ ?Parchment ̙33+) 0L0 ((NQ!((  dB  <D>+   0l p D4s&(2  0 rW  A3$(2L k 7 # 7y~  N??kw 7~  N??k7~  N??k)7~   N??)k7~   N??w k 7^B   6Df>L  P x   # @4a ~   N?? P + ~  N??+P  ~  N??P x dB  <DK dB  <D ^B  6DoK ^B  6DoC9 C  0} a  D3p&(2  0  D3d&(2L NT - # 4yfB  6Df>WWN  P x   ` sT ?~  N?? P + ~  N??+P  ~  N??P x lB  <D>PlB  <D>WlB  <D>WlB  <D=P~   N??M a -fB ! 6Doj  " 0 A4$(2fB # 6Doj  $ 0s)G D4p&(2 % 0`|)P D4d&(2 & 0얃N)" D4f&(20L Zo (# R j VfB ) 6DooofB *B 6DoZo0L Zo +#  VfB , 6DooofB -B 6DoZo0L Zo .# Zr> fB / 6DooofB 0B 6DoZo0L Zo 1# > fB 2 6DooofB 3B 6DoZo0L Zo 4#  "> fB 5 6DooofB 6B 6DoZo0L Zo 7# Yq> fB 8 6DooofB 9B 6DoZo0L Zo :# > fB ; 6DooofB <B 6DoZo0L Zo =# > fB > 6DooofB ?B 6DoZo0L Zo @# ZrfB A 6DooofB BB 6DoZo0L Zo C#  "fB D 6DooofB EB 6DoZo F 0 y=ELECTRONIC CONFIGURATIONS OF THE FIRST ROW TRANSITION METALS  >(2>f G 0f0 RTITANIUM. (2w H 0Df   1s2 2s2 2p6 3s2 3p6 4s2 3d2(2       dB I <D)@0A J 0Pp@ 0 0dB K@ <D)@X@ L 0X0@ 0 0 O 0Hp 0P  The 3d orbitals are filled according to Hund s rule so the next electron doesn t pair up but goes into an empty orbital in the same sub level. 2,a P 6d? FHUND S RULE OF MAXIMUM MULTIPLICITY*$P# Q 6ȃ2U  e)INCREASING ENERGY / DISTANCE FROM NUCLEUS *(2*z  bA޽h @ ?Parchment ̙33c* 0L0 ))QUY)( ޽h dB  <D>+   0΃ p D4s&(2  0ӃW  A3$(2L k 7 # 7y~  N??kw 7~  N??k7~  N??k)7~   N??)k7~   N??w k 7^B   6Df>L  P x   # @4a ~   N?? P + ~  N??+P  ~  N??P x dB  <DK dB  <D ^B  6DoK ^B  6DoC9 C  0 ܃ a  D3p&(2  0  D3d&(2L NT - # 4yfB  6Df>WWN  P x   ` sT ?~  N?? P + ~  N??+P  ~  N??P x lB  <D>PlB  <D>WlB  <D>WlB  <D=P~   N??M a -fB ! 6Doj  " 0 A4$(2fB # 6Doj  $ 0s)G D4p&(2 % 0x|)P D4d&(2 & 0N)" D4f&(20L Zo (# R j VfB ) 6DooofB *B 6DoZo0L Zo +#  VfB , 6DooofB -B 6DoZo0L Zo .# Zr> fB / 6DooofB 0B 6DoZo0L Zo 1# > fB 2 6DooofB 3B 6DoZo0L Zo 4#  "> fB 5 6DooofB 6B 6DoZo0L Zo 7# Yq> fB 8 6DooofB 9B 6DoZo0L Zo :# > fB ; 6DooofB <B 6DoZo0L Zo =# > fB > 6DooofB ?B 6DoZo0L Zo @# ZrfB A 6DooofB BB 6DoZo0L Zo C#  "fB D 6DooofB EB 6DoZo0L Zo F# fB G 6DooofB HB 6DoZo I 0D y=ELECTRONIC CONFIGURATIONS OF THE FIRST ROW TRANSITION METALS  >(2>f J 0 f0 RVANADIUM. (2w K 00f   1s2 2s2 2p6 3s2 3p6 4s2 3d3(2       dB L <D)@0A M 0Pp@ 0 0dB N@ <D)@X@ O 0X0@ 0 0 S 0L!p 0P  The 3d orbitals are filled according to Hund s rule so the next electron doesn t pair up but goes into an empty orbital in the same sub level. 2,a T 60'? FHUND S RULE OF MAXIMUM MULTIPLICITY*$P# U 6l-2U  e)INCREASING ENERGY / DISTANCE FROM NUCLEUS *(2*z  bA޽h @ ?Parchment ̙33* 0L0 S*K*SU)(  dB  <D>+   07 p D4s&(2  0:W  A3$(2L k 7 # 7y~  N??kw 7~  N??k7~  N??k)7~   N??)k7~   N??w k 7^B   6Df>L  P x   # @4a ~   N?? P + ~  N??+P  ~  N??P x dB  <DK dB  <D ^B  6DoK ^B  6DoC9 C  0A a  D3p&(2  0tF  D3d&(2L NT - # 4yfB  6Df>WWN  P x   ` sT ?~  N?? P + ~  N??+P  ~  N??P x lB  <D>PlB  <D>WlB  <D>WlB  <D=P~   N??M a -fB ! 6Doj  " 0N A4$(2fB # 6Doj  $ 0Rs)G D4p&(2 % 0X|)P D4d&(2 & 0 ^N)" D4f&(2 ' 6Ha2U  e)INCREASING ENERGY / DISTANCE FROM NUCLEUS *(2*0L Zo (# R j VfB ) 6DooofB *B 6DoZo0L Zo +# Zr> fB , 6DooofB -B 6DoZo0L Zo .# > fB / 6DooofB 0B 6DoZo0L Zo 1#  "> fB 2 6DooofB 3B 6DoZo0L Zo 4# Yq> fB 5 6DooofB 6B 6DoZo0L Zo 7# > fB 8 6DooofB 9B 6DoZo0L Zo :# > fB ; 6DooofB <B 6DoZo0L Zo =# ZrfB > 6DooofB ?B 6DoZo0L Zo @#  "fB A 6DooofB BB 6DoZo0L Zo C# fB D 6DooofB EB 6DoZo0L Zo F# JbfB G 6DooofB HB 6DoZo0L Zo I#  fB J 6DooofB KB 6DoZo L 0o y=ELECTRONIC CONFIGURATIONS OF THE FIRST ROW TRANSITION METALS  >(2>f M 0 uf0 RCHROMIUM. (2w N 0tyf   1s2 2s2 2p6 3s2 3p6 4s1 3d5(2       dB O <D)@0A P 0Pp@ 0 0dB Q@ <D)@X@ R 0X0@ 0 0 U 0`p 0P One would expect the configuration of chromium atoms to end in 4s2 3d4. To achieve a more stable arrangement of lower energy, one of the 4s electrons is promoted into the 3d to give six unpaired electrons with lower repulsion. 2A  ':+z  bA޽h @ ?Parchment ̙33* 0L0 `*X*V\ )(   dB   <D>+    0p p D4s&(2   0HW  A3$(2L k 7  # 7y~   N??kw 7~   N??k7~   N??k)7~   N??)k7~   N??w k 7^B   6Df>L  P x   # @4a ~   N?? P + ~   N??+P  ~   N??P x dB   <DK dB   <D ^B   6DoK ^B   6DoC9 C   0 a  D3p&(2   0Ȭ  D3d&(2L NT -  # 4yfB   6Df>WWN  P x    ` sT ?~   N?? P + ~   N??+P  ~   N??P x lB   <D>PlB   <D>WlB   <D>WlB   <D=P~   N??M a -fB !  6Doj  "  0 A4$(2fB #  6Doj  $  00s)G D4p&(2 %  0|)P D4d&(2 &  0ƄN)" D4f&(20L Zo ( # R j VfB )  6DooofB * B 6DoZo0L Zo + # Zr> fB ,  6DooofB - B 6DoZo0L Zo . # > fB /  6DooofB 0 B 6DoZo0L Zo 1 #  "> fB 2  6DooofB 3 B 6DoZo0L Zo 4 # Yq> fB 5  6DooofB 6 B 6DoZo0L Zo 7 # > fB 8  6DooofB 9 B 6DoZo0L Zo : # > fB ;  6DooofB < B 6DoZo0L Zo = # ZrfB >  6DooofB ? B 6DoZo0L Zo C #  "fB D  6DooofB E B 6DoZo0L Zo F # fB G  6DooofB H B 6DoZo0L Zo I # JbfB J  6DooofB K B 6DoZo0L Zo L #  fB M  6DooofB N B 6DoZo O  0dԄ y=ELECTRONIC CONFIGURATIONS OF THE FIRST ROW TRANSITION METALS  >(2>f P  0لf0 S MANGANESE. (2 w Q  0ބf   1s2 2s2 2p6 3s2 3p6 4s2 3d5(2       dB R  <D)@0A S  0Pp@ 0 0dB T @ <D)@X@ U  0X0@ 0 0 X  0p 1PD  t>The new electron goes into the 4s to restore its filled state.? 2? Y  6H2U  e)INCREASING ENERGY / DISTANCE FROM NUCLEUS *(2*0L Zo Z #  VfB [  6DooofB \ B 6DoZoz   bA޽h @ ?Parchment ̙33q- 0L0  --Z]g,( ޽h dB  <D>+   0 p D4s&(2  0$W  A3$(2L k 7 # 7y~  N??kw 7~  N??k7~  N??k)7~   N??)k7~   N??w k 7^B   6Df>L  P x   # @4a ~   N?? P + ~  N??+P  ~  N??P x dB  <DK dB  <D ^B  6DoK ^B  6DoC9 C  0  a  D3p&(2  0  D3d&(2L NT - # 4yfB  6Df>WWN  P x   ` sT ?~  N?? P + ~  N??+P  ~  N??P x lB  <D>PlB  <D>WlB  <D>WlB  <D=P~   N??M a -fB ! 6Doj  " 0( A4$(2fB # 6Doj  $ 0Hs)G D4p&(2 % 0)|)P D4d&(2 & 0"N)" D4f&(20L Zo (# R j VfB ) 6DooofB *B 6DoZo0L Zo +#  VfB , 6DooofB -B 6DoZo0L Zo .# Zr> fB / 6DooofB 0B 6DoZo0L Zo 1# > fB 2 6DooofB 3B 6DoZo0L Zo 4#  "> fB 5 6DooofB 6B 6DoZo0L Zo 7# Yq> fB 8 6DooofB 9B 6DoZo0L Zo :# > fB ; 6DooofB <B 6DoZo0L Zo =# > fB > 6DooofB ?B 6DoZo0L Zo @# ZrfB A 6DooofB BB 6DoZo0L Zo C# fB D 6DooofB EB 6DoZo0L Zo F#  "fB G 6DooofB HB 6DoZo0L Zo I# fB J 6DooofB KB 6DoZo0L Zo L# JbfB M 6DooofB NB 6DoZo0L Zo O#  fB P 6DooofB QB 6DoZo R 0 8 y=ELECTRONIC CONFIGURATIONS OF THE FIRST ROW TRANSITION METALS  >(2>f S 0T=f0 NIRON.(2w T 08 f   1s2 2s2 2p6 3s2 3p6 4s2 3d6(2       dB U <D)@0A V 0Pp@ 0 0dB W@ <D)@X@ X 0X0@ 0 0P [ 0Lp 0>D  Orbitals are filled according to Hund s Rule. They continue to pair up.H 2H$! \ 60X? FHUND S RULE OF MAXIMUM MULTIPLICITY*$P# ] 6\2U  e)INCREASING ENERGY / DISTANCE FROM NUCLEUS *(2*z  bA޽h @ ?Parchment ̙33. 0L0 C.;. ]a-(  dB  <D>+   0HW p D4s&(2  0eW  A3$(2L k 7 # 7y~  N??kw 7~  N??k7~  N??k)7~   N??)k7~   N??w k 7^B   6Df>L  P x   # @4a ~   N?? P + ~  N??+P  ~  N??P x dB  <DK dB  <D ^B  6DoK ^B  6DoC9 C  0o a  D3p&(2  0s  D3d&(2L NT - # 4yfB  6Df>WWN  P x   ` sT ?~  N?? P + ~  N??+P  ~  N??P x lB  <D>PlB  <D>WlB  <D>WlB  <D=P~   N??M a -fB ! 6Doj  " 0|~ A4$(2fB # 6Doj  $ 0s)G D4p&(2 % 0؆|)P D4d&(2 & 0N)" D4f&(20L Zo (# R j VfB ) 6DooofB *B 6DoZo0L Zo +#  VfB , 6DooofB -B 6DoZo0L Zo .# Zr> fB / 6DooofB 0B 6DoZo0L Zo 1# > fB 2 6DooofB 3B 6DoZo0L Zo 4#  "> fB 5 6DooofB 6B 6DoZo0L Zo 7# Yq> fB 8 6DooofB 9B 6DoZo0L Zo :# > fB ; 6DooofB <B 6DoZo0L Zo =# > fB > 6DooofB ?B 6DoZo0L Zo @# ZrfB A 6DooofB BB 6DoZo0L Zo C# fB D 6DooofB EB 6DoZo0L Zo F#  "fB G 6DooofB HB 6DoZo0L Zo I# YqfB J 6DooofB KB 6DoZo0L Zo L# fB M 6DooofB NB 6DoZo0L Zo O# JbfB P 6DooofB QB 6DoZo0L Zo R#  fB S 6DooofB TB 6DoZo U 0 y=ELECTRONIC CONFIGURATIONS OF THE FIRST ROW TRANSITION METALS  >(2>f V 0f0 PCOBALT.(2w W 0f   1s2 2s2 2p6 3s2 3p6 4s2 3d7(2       dB X <D)@0A Y 0Pp@ 0 0dB Z@ <D)@X@ [ 0X0@ 0 0P _ 0dp 0>D  Orbitals are filled according to Hund s Rule. They continue to pair up.H 2H$! ` 6? FHUND S RULE OF MAXIMUM MULTIPLICITY*$P# a 62U  e)INCREASING ENERGY / DISTANCE FROM NUCLEUS *(2*z  bA޽h @ ?Parchment ̙33/ 0L0 {/s/0`e.(  dB  <D>+   0 Ȉ p D4s&(2  0HW  A3$(2L k 7 # 7y~  N??kw 7~  N??k7~  N??k)7~   N??)k7~   N??w k 7^B   6Df>L  P x   # @4a ~   N?? P + ~  N??+P  ~  N??P x dB  <DK dB  <D ^B  6DoK ^B  6DoC9 C  0׈ a  D3p&(2  0و  D3d&(2L NT - # 4yfB  6Df>WWN  P x   ` sT ?~  N?? P + ~  N??+P  ~  N??P x lB  <D>PlB  <D>WlB  <D>WlB  <D=P~   N??M a -fB ! 6Doj  " 0|߈ A4$(2fB # 6Doj  $ 0s)G D4p&(2 % 0|)P D4d&(2 & 0N)" D4f&(20L Zo (# R j VfB ) 6DooofB *B 6DoZo0L Zo +#  VfB , 6DooofB -B 6DoZo0L Zo .# Zr> fB / 6DooofB 0B 6DoZo0L Zo 1# > fB 2 6DooofB 3B 6DoZo0L Zo 4#  "> fB 5 6DooofB 6B 6DoZo0L Zo 7# Yq> fB 8 6DooofB 9B 6DoZo0L Zo :# > fB ; 6DooofB <B 6DoZo0L Zo =# > fB > 6DooofB ?B 6DoZo0L Zo @# ZrfB A 6DooofB BB 6DoZo0L Zo C# fB D 6DooofB EB 6DoZo0L Zo F#  "fB G 6DooofB HB 6DoZo0L Zo I# YqfB J 6DooofB KB 6DoZo0L Zo L# fB M 6DooofB NB 6DoZo0L Zo O# fB P 6DooofB QB 6DoZo0L Zo R# JbfB S 6DooofB TB 6DoZo0L Zo U#  fB V 6DooofB WB 6DoZo X 0 y=ELECTRONIC CONFIGURATIONS OF THE FIRST ROW TRANSITION METALS  >(2>f Y 0@f0 PNICKEL.(2w Z 0 f   1s2 2s2 2p6 3s2 3p6 4s2 3d8(2       dB [ <D)@0A \ 0Pp@ 0 0dB ]@ <D)@X@ ^ 0X0@ 0 0P b 0p 0>D  Orbitals are filled according to Hund s Rule. They continue to pair up.H 2H$! d 6l? FHUND S RULE OF MAXIMUM MULTIPLICITY*$P# e 6#2U  e)INCREASING ENERGY / DISTANCE FROM NUCLEUS *(2*z  bA޽h @ ?Parchment ̙33j1 0L0 10@cg`0( ޽h dB  <D>+   0) p D4s&(2  0,W  A3$(2L k 7 # 7y~  N??kw 7~  N??k7~  N??k)7~   N??)k7~   N??w k 7^B   6Df>L  P x   # @4a ~   N?? P + ~  N??+P  ~  N??P x dB  <DK dB  <D ^B  6DoK ^B  6DoC9 C  087 a  D3p&(2  0<  D3d&(2L NT - # 4yfB  6Df>WWN  P x   ` sT ?~  N?? P + ~  N??+P  ~  N??P x lB  <D>PlB  <D>WlB  <D>WlB  <D=P~   N??M a -fB ! 6Doj  " 0pF A4$(2fB # 6Doj  $ 0hKs)G D4p&(2 % 0P|)P D4d&(2 & 0@UN)" D4f&(20L Zo (# R j VfB ) 6DooofB *B 6DoZo0L Zo +# Zr> fB , 6DooofB -B 6DoZo0L Zo .# > fB / 6DooofB 0B 6DoZo0L Zo 1#  "> fB 2 6DooofB 3B 6DoZo0L Zo 4# Yq> fB 5 6DooofB 6B 6DoZo0L Zo 7# > fB 8 6DooofB 9B 6DoZo0L Zo :# > fB ; 6DooofB <B 6DoZo0L Zo =# ZrfB > 6DooofB ?B 6DoZo0L Zo @# fB A 6DooofB BB 6DoZo0L Zo C#  "fB D 6DooofB EB 6DoZo0L Zo F# YqfB G 6DooofB HB 6DoZo0L Zo I# fB J 6DooofB KB 6DoZo0L Zo L# fB M 6DooofB NB 6DoZo0L Zo O# JbfB P 6DooofB QB 6DoZo0L Zo R# fB S 6DooofB TB 6DoZo0L Zo U#  fB V 6DooofB WB 6DoZo0L Zo X# AYfB Y 6DooofB ZB 6DoZo [ 0dl y=ELECTRONIC CONFIGURATIONS OF THE FIRST ROW TRANSITION METALS  >(2>f \ 0qf0 PCOPPER.(2x ] 0nf   1s2 2s2 2p6 3s2 3p6 4s1 3d10(2       dB ^ <D)@0A _ 0Pp@ 0 0dB `@ <D)@X@ a 0X0@ 0 0 d 0p 0P >One would expect the configuration of copper atoms to end in 4s2 3d9. To achieve a more stable arrangement of lower energy, one of the 4s electrons is promoted into the 3d.v 2?  '3 f 6D? FHUND S RULE OF MAXIMUM MULTIPLICITY*$P# g 6P2U  e)INCREASING ENERGY / DISTANCE FROM NUCLEUS *(2*z  bA޽h @ ?Parchment ̙33K1 0L0 00Pei 50(   jB   BD>+    6, p D4s&(2   6ܙW  A3$(2L k 7  # 7y~   N??kw 7~   N??k7~   N??k)7~   N??)k7~   N??w k 7dB   <Df>L  P x   # @4a ~   N?? P + ~   N??+P  ~   N??P x jB   BDK jB   BD dB   <DoK dB   <DoC9 C   6L a  D3p&(2   6ܳ  D3d&(2L NT -  # 4yfB   6Df>WWN  P x    ` sT ?~   N?? P + ~   N??+P  ~   N??P x lB   <D>PlB   <D>WlB   <D>WlB   <D=P~ !  N??M a -fB "  6Doj  #  0` A4$(2fB $  6Doj  %  0Xs)G D4p&(2 &  00|)P D4d&(2 '  0ƊN)" D4f&(20L Zo ) # R j VfB *  6DooofB + B 6DoZo0L Zo , #  VfB -  6DooofB . B 6DoZo0L Zo / # Zr> fB 0  6DooofB 1 B 6DoZo0L Zo 2 # > fB 3  6DooofB 4 B 6DoZo0L Zo 5 #  "> fB 6  6DooofB 7 B 6DoZo0L Zo 8 # Yq> fB 9  6DooofB : B 6DoZo0L Zo ; # > fB <  6DooofB = B 6DoZo0L Zo > # > fB ?  6DooofB @ B 6DoZo0L Zo A # ZrfB B  6DooofB C B 6DoZo0L Zo D # fB E  6DooofB F B 6DoZo0L Zo G #  "fB H  6DooofB I B 6DoZo0L Zo J # YqfB K  6DooofB L B 6DoZo0L Zo M # fB N  6DooofB O B 6DoZo0L Zo P # fB Q  6DooofB R B 6DoZo0L Zo S # JbfB T  6DooofB U B 6DoZo0L Zo V # fB W  6DooofB X B 6DoZo0L Zo Y #  fB Z  6DooofB [ B 6DoZo0L Zo \ # AYfB ]  6DooofB ^ B 6DoZo _  0 y=ELECTRONIC CONFIGURATIONS OF THE FIRST ROW TRANSITION METALS  >(2>f `  0Df0 NZINC.(2x a  0f   1s2 2s2 2p6 3s2 3p6 4s2 3d10(2       dB b  <D)@0A c  0Pp@ 0 0dB d @ <D)@X@ e  0X0@ 0 0 h  0@p 0  eThe electron goes into the 4s to restore its filled state and complete the 3d and 4s orbital filling.f 2f i  62U  e)INCREASING ENERGY / DISTANCE FROM NUCLEUS *(2*z   bA޽h @ ?Parchment ̙33y 0L0  `{(  ^  0(]{#  xK 1s2 2s2 2p6 3s2 3p6 4s1 Ca 1s2 2s2 2p6 3s2 3p6 4s2 Sc 1s2 2s2 2p6 3s2 3p6 4s2 3d1 Ti 1s2 2s2 2p6 3s2 3p6 4s2 3d2 V 1s2 2s2 2p6 3s2 3p6 4s2 3d3 Cr 1s2 2s2 2p6 3s2 3p6 4s1 3d5 Mn 1s2 2s2 2p6 3s2 3p6 4s2 3d5 Fe 1s2 2s2 2p6 3s2 3p6 4s2 3d6 Co 1s2 2s2 2p6 3s2 3p6 4s2 3d7 Ni 1s2 2s2 2p6 3s2 3p6 4s2 3d8 Cu 1s2 2s2 2p6 3s2 3p6 4s1 3d10 Zn 1s2 2s2 2p6 3s2 3p6 4s2 3d10H y@                                                                     dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0  0Tqk UELECTRONIC CONFIGURATIONS (2fn  VA޽h ?Parchment ̙33f 0L0  eep d( w dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0  0q~ gVARIABLE OXIDATION STATES2(2ff    0L"` LArises from the similar energies required for removal of 4s and 3d electrons MHM M I  0ءl x When electrons are removed they come from the 4s orbitals first Cu 1s2 2s2 2p6 3s2 3p6 3d10 4s1 Ti 1s2 2s2 2p6 3s2 3p6 3d2 4s2 Cu+ 1s2 2s2 2p6 3s2 3p6 3d10 Ti2+ 1s2 2s2 2p6 3s2 3p6 3d2 Cu2+ 1s2 2s2 2p6 3s2 3p6 3d9 Ti3+ 1s2 2s 2p6 3s2 3p6 3d1 Ti4+ 1s2 2s2 2p6 3s2 3p6@H@@                                           &1     0K   maximum rises across row to manganese maximum falls as the energy required to remove more electrons becomes very high all (except scandium) have an M2+ ion stability of +2 state increases across the row due to increase in the 3rd Ionisation Energy THE MOST IMPORTANT STATES ARE IN REDd!@ a $  ! U8 K   K J |0T @ |  # K  T k 7  # @ N  ~   N??kw 7~   N??k7~   N??k)7~  N??)k7~  N??w k 7T k 7 # N  ~  N??kw 7~  N??k7~  N??k)7~  N??)k7~  N??w k 7T k 7 # @  ~  N??kw 7~  N??k7~  N??k)7~  N??)k7~  N??w k 7T k 7 #   ~  N??kw 7~  N??k7~  N??k)7~   N??)k7~ ! N??w k 7T k 7 "# @  ~ # N??kw 7~ $ N??k7~ % N??k)7~ & N??)k7~ ' N??w k 7T k 7 (#   ~ ) N??kw 7~ * N??k7~ + N??k)7~ , N??)k7~ - N??w k 7T k 7 .# @  ~ / N??kw 7~ 0 N??k7~ 1 N??k)7~ 2 N??)k7~ 3 N??w k 7T k 7 4#   ~ 5 N??kw 7~ 6 N??k7~ 7 N??k)7~ 8 N??)k7~ 9 N??w k 7T k 7 :# @ h ~ ; N??kw 7~ < N??k7~ = N??k)7~ > N??)k7~ ? N??w k 7T k 7 @#  h ~ A N??kw 7~ B N??k7~ C N??k)7~ D N??)k7~ E N??w k 7T k 7 F# @ h :~ G N??kw 7~ H N??k7~ I N??k)7~ J N??)k7~ K N??w k 7T k 7 L# h :~ M N??kw 7~ N N??k7~ O N??k)7~ P N??)k7~ Q N??w k 7T k 7 R# @ : ~ S N??kw 7~ T N??k7~ U N??k)7~ V N??)k7~ W N??w k 7T k 7 X# : ~ Y N??kw 7~ Z N??k7~ [ N??k)7~ \ N??)k7~ ] N??w k 7T k 7 v# @ |N ~ w N??kw 7~ x N??k7~ y N??k)7~ z N??)k7~ { N??w k 7T k 7 |# |N ~ } N??kw 7~ ~ N??k7~  N??k)7~  N??)k7~  N??w k 7 k N H 8 ITi *(2 l NhX 0 8 HSc*(2 n N@8 GV*(2 o NP'08 HCr*(2 p N+8 bMn*(2 q N)8 HFe*(2 r N8 HCo*(2 s N8 HNi*(2 t N=8 HCu*(2 u NA8 HZn*(2  NFt   P+12(2  NKB 4  H+2*(2  NPTb : ^ P+32(2  NY P+42(2  N]0* P+52(2  Na Z P+62(2  Nl84  H+2*(2  NP04  H+2*(2  Nhs4  P+22(2  Nw4  P+22(2  N0|4  P+22(2  Npz4  P+22(2  N 4  P+22(2  N4  P+22(2  NHZ H+6*(2  Ne P+72(2  N^ H+3*(2  NxH  ^ L+3.(2  N^ P+32(2  NlH   P+42(2  N졏@^ L+3.(2  Nx8 H+4*(2  N'^ P+32(2  N^ P+32(2  N8^ H+3*(2  Hx  H+4*(2  H H+4*(2  H H+4*(2  H8ď H+4*(2  Hxȏ * H+5*(2  H̏* H+5*(2  HЏ* H+5*(2  H8Տ* H+5*(2  HxُZ H+6*(2B  s *޽h ? ̙33y___PPT10Y+D=' = @B ++  0L0 : 2   ( w dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0  0q~ [ COLOURED IONS2(2 ff   0"`cF VTheory ions with a d10 (full) or d0 (empty) configuration are colourless ions with partially filled d-orbitals tend to be coloured it is caused by the ease of transition of electrons between energy levels energy is absorbed when an electron is promoted to a higher level the frequency of light is proportional to the energy difference ions with d10 (full) Cu+,Ag+ Zn2+ or d0 (empty) Sc3+ configuration are colourless e.g. titanium(IV) oxide TiO2 is white colour depends on ... transition element oxidation state ligand coordination numberHb@@ < ff ffffffff ff=fffZk        L   C $A rbowg <    0T8H QA characteristic of transition metals is their ability to form coloured compounds RHR R    0 0 ^ ,@f  B  s *޽h ? ̙33y___PPT10Y+D=' = @B +  0L0   a(  (  `dB ` <D)P0Q ` 0Pp@ 0 0dB `@ <D)PXP ` 0X0@ 0 0 ` 0tq~ Y 3d ORBITALS2 (2 ff  ` 0"`x /There are 5 different orbitals of the d variety0H0&   P  a C (A2dorbsg wP  a C (A3dorbsgEa$ a 0($ ~ xz2FH   a 0) ~ x2-y2lH   a 0/$  `xy H   a 03$A 1   `xz H   a 08$@0  `yz H  B ` s *޽h ? ̙33y___PPT10Y+D=' = @B +I 0L0 HH|H(  dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0  0\Fq~ fSPLITTING OF 3d ORBITALS2(2ff   00W ; q' Placing ligands around a central ion causes the energies of the d orbitals to change Some of the d orbitals gain energy and some lose energy In an octahedral complex, two (z2 and x2-y2) go higher and three go lower In a tetrahedral complex, three (xy, xz and yz) go higher and two go lower Degree of splitting depends on the CENTRAL ION and the LIGAND The energy difference between the levels affects how much energy is absorbed when an electron is promoted. The amount of energy governs the colour of light absorbed.~(@B   #        3           L   B   # 1 # ZB   s *Do X ZB   s *Do<  ZB   s *DoX A bN A ^    A ~ ~  N??A ^ ~  N?? ^ ZB  s *DoE  T  P x  # v B ~  N?? P + ~  N??+P  ~  N??P x ZB  s *DoX L T k 7 # ,, n ~  N??kw 7~  N??k7~  N??k)7~  N??)k7~  N??w k 7L   B  # ; ZB  s *Do X ZB  s *Do<  ZB   s *DoX A bN A ^  !  A ~ ~ " N??A ^ ~ # N?? ^ ZB $ s *DoE  T  P x  %# v B ~ & N?? P + ~ ' N??+P  ~ ( N??P x ZB ) s *DoX L T k 7 *# ,, n ~ + N??kw 7~ , N??k7~ - N??k)7~ . N??)k7~ / N??w k 7XB 0 0Do`u u   F . 1  N  k  2 .8T Zo 3#  k " fB 4 6DooofB 5B 6DoZo8T Zo 6# Y k q fB 7 6DooofB 8B 6DoZo8T Zo 9#  k fB : 6DooofB ;B 6DoZo8T Zo <#  k ! fB = 6DooofB >B 6DoZo8T Zo ?# b k z fB @ 6DooofB AB 6DoZo8T Zo B#  k fB C 6DooofB DB 6DoZo8T Zo E# "/:fB F 6DooofB GB 6DoZo8T Zo H# /fB I 6DooofB JB 6DoZo F . K X  N  k  L .8T Zo M#  k " fB N 6DooofB OB 6DoZo8T Zo P# Y k q fB Q 6DooofB RB 6DoZo8T Zo S#  k fB T 6DooofB UB 6DoZo8T Zo V#  k ! fB W 6DooofB XB 6DoZo8T Zo Y# b k z fB Z 6DooofB [B 6DoZo8T Zo \#  k fB ] 6DooofB ^B 6DoZo8T Zo _# "/:fB ` 6DooofB aB 6DoZo8T Zo b# /fB c 6DooofB dB 6DoZo,F  G e  :g VN  T  f  C8T Zo g#  T fB h 6DooofB iB 6DoZo8T Zo j# 1 IT fB k 6DooofB lB 6DoZo8T Zo m#  T fB n 6DooofB oB 6DoZo8T Zo p#  T fB q 6DooofB rB 6DoZo8T Zo s# I a GfB t 6DooofB uB 6DoZo8T Zo v#   GfB w 6DooofB xB 6DoZoTL  T  y# ) )@ 8T Zo z#  T fB { 6DooofB |B 6DoZo8T Zo }# 1 IT fB ~ 6DooofB B 6DoZo8T Zo #  T fB  6DooofB B 6DoZo8T Zo #  T fB  6DooofB B 6DoZo0L Zo # afB  6DooofB B 6DoZo0L Zo # a5fB  6DooofB B 6DoZo0L Zo # a~fB  6DooofB B 6DoZo0L Zo # e%=fB  6DooofB B 6DoZo0L Zo # 1fB  6DooofB B 6DoZo0L Zo # 1>VfB  6DooofB B 6DoZoXB  0Do\   0{u D3d&(2  0`{A u D3d&(2  0ԣv$ N OCTAHEDRAL( (2   0<  O TETRAHEDRAL( (2 P  C (A3dorbsg " P  C (A2dorbsg_ P  C (A3dorbsg1P  C (A2dorbsg  B  s *޽h ? ̙33y___PPT10Y+D=' = @B +  0L0   01 ( pJ dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0  0q~ [ COLOURED IONS2(2 ff   0ط 0 I Absorbed colour nm Observed colour nm VIOLET 400 GREEN-YELLOW 560 BLUE 450 YELLOW 600 BLUE-GREEN 490 RED 620 YELLOW-GREEN 570 VIOLET 410 YELLOW 580 DARK BLUE 430 ORANGE 600 BLUE 450 RED 650 GREEN 5208@'  P   C (AbeakergH 0T  C ,Aspectrevg@dB  <Do8~8dB  <Do8 08R  s *3T  C ,AspechalfgP@ p   0vJ ^The observed colour of a solution depends on the wavelengths absorbed Copper sulphate solution appears blue because the energy absorbed corresponds to red and yellow wavelengths. Wavelengths corresponding to blue light aren t absorbed.TFHP<@F    0h͐9& WWHITE LIGHT GOES IN((2  0\ѐ9  YSOLUTION APPEARS BLUE((2  0Ԑ0 & P  u1ENERGY CORRESPONDING TO THESE COLOURS IS ABSORBED(2(21  B  s *޽h ? ̙33y___PPT10Y+D=' = @B +~ 0L0  #(  dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0  0q~ [ COLOURED IONS2(2 ff   00 Xa solution of copper(II)sulphate is blue because red and yellow wavelengths are absorbed2YHX Y P  C (A'absorbg.Q`   0, X  W white light H     0   gblue and green not absorbedH  B  s *޽h ? ̙33y___PPT10Y+D=' = @B + 0L0 4( $NJ 4dB 4 <D)P0Q 4 0Pp@ 0 0dB 4@ <D)PXP 4 0X0@ 0 0 4 0p q~ [ COLOURED IONS2(2 ff 4 0p0 Xa solution of copper(II)sulphate is blue because red and yellow wavelengths are absorbed2YHX Y R 4 C *Acompcolg& B 4 s *޽h ? ̙33y___PPT10Y+D=' = @B + 0L0  ( w N   C &ACucolg& dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0  00q~ [ COLOURED IONS2(2 ff   0'0 Xa solution of copper(II)sulphate is blue because red and yellow wavelengths are absorbed2YHX Y B  s *޽h ? ̙33y___PPT10Y+D=' = @B + 0L0  ( X  N   C &ANicolg& dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0  01q~ [ COLOURED IONS2(2 ff!   060 _a solution of nickel(II)sulphate is green because violet, blue and red wavelengths are absorbed2`H_ ` B  s *޽h ? ̙33y___PPT10Y+D=' = @B +  0L0    2 (  dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0T   C ,A&photometgx    0 <   M WHITE LIGHT& (2   0`@ a  M BLUE FILTER& (2   0DHHC  K RED LIGHT& (2   0,Ik  +  JSOLUTION& (2  0lM P  M COLORIMETER& (2   0Qq0 .FINDING COMPLEX ION FORMULAE USING COLORIMETRY/@/f.   0V " a change of ligand can change the colour of a complex " this property can be used to find the formula of a complex ion " ight of a certain wavelength is passed through a solution " the greater the colour intensity, the greater the absorbance " the concentration of each species in the complex is altered " the mixture with the greatest absorbance identifies ratio of ligands and ions@Z  i      B  s *޽h ? ̙33y___PPT10Y+D=' = @B +\  0L0 k c   ( w dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0  0cq0 .FINDING COMPLEX ION FORMULAE USING COLORIMETRY/@/f.   0h " a change of ligand can change the colour of a complex " this property can be used to find the formula of a complex ion " ight of a certain wavelength is passed through a solution " the greater the colour intensity, the greater the absorbance " the concentration of each species in the complex is altered " the mixture with the greatest absorbance identifies ratio of ligands and ions@Z  i      R  C *A%photscngB    0l {+Finding the formula of an iron(III) complex ,H, , j   0w0R White light is passed through a blue filter. The resulting red light is passed through mixtures of an aqueous iron(III) and potassium thiocyanate solution. Maximum absorbance occurs first when the ratio of Fe3+ and SCN is 1:1. This shows the complex has the formula [Fe(H2O)5SCN]2+@ff?ffffff&    B  s *޽h ? ̙33y___PPT10Y+D=' = @B +  0L0     (  T   C ,A photedtagBv XdB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0  0Ԇq0 .FINDING COMPLEX ION FORMULAE USING COLORIMETRY/@/f.   0 " a change of ligand can change the colour of a complex " this property can be used to find the formula of a complex ion " ight of a certain wavelength is passed through a solution " the greater the colour intensity, the greater the absorbance " the concentration of each species in the complex is altered " the mixture with the greatest absorbance identifies ratio of ligands and ions@Z  i         0Ԗp 1Finding the formula of an nickel(II) edta complex 2H2&%       0<0RL  uFiltered light is passed through various mixtures of an aqueous solution of nickel(II) sulphate and edta solution. The maximum absorbance occurs when the ratio of Ni2+ and edta is 1:1.X@ffff@d  E    B  s *޽h ? ̙33y___PPT10Y+D=' = @B +@  0L0 O G 0 (  dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0  0䪗q~ vCOMPLEX IONS - LIGANDSD(2ff   00ʗ 9 GoFormation ligands form co-ordinate bonds to a central transition metal ion Ligands atoms, or ions, which possess lone pairs of electrons form co-ordinate bonds to the central ion donate a lone pair into vacant orbitals on the central species Ligand Formula Name of ligand chloride Cl chloro cyanide NC cyano hydroxide HO hydroxo oxide O2- oxo water H2O aqua ammonia NH3 ammine some ligands attach themselves using two or more lone pairs classified by the number of lone pairs they use multidentate and bidentate ligands lead to more stable complexes<p@ @ l?Q    x   ;      2             3  b         B  s *޽h ? ̙33y___PPT10Y+D=' = @B +  0L0   @7 ( w dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0  0֗q~ vCOMPLEX IONS - LIGANDSD(2ff   0ܗ"`   ? some ligands attach themselves using two or more lone pairs classified by the number of lone pairs they use multidentate and bidentate ligands lead to more stable complexes Unidentate form one co-ordinate bond Cl, OH, CN, NH3, and H2O Bidentate form two co-ordinate bonds H2NCH2CH2NH2 , C2O42-r@@ 1   "         b        !      !   8 L   C $A  lig1axR   C *A"ligand2a; )<R   C *A#ligand2c9  2pB   HDf3Ԕp d pB  HDf3Ԕp d vB  NDf3Ԕ_ S vB  NDf3Ԕg [ B  s *޽h ? ̙33y___PPT10Y+D=' = @B +- 0L0 <4 (  dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0  0Hq~ vCOMPLEX IONS - LIGANDSD(2ffA   0\  A  some ligands attach themselves using two or more lone pairs classified by the number of lone pairs they use multidentate and bidentate ligands lead to more stable complexes Multidentate form several co-ordinate bondsR@    b        !     L  C $A$ edtag_   0 _o ( #EDTA An important complexing agent*$f &    B  s *޽h ? ̙33y___PPT10Y+D=' = @B + 0L0 ` Z( w dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0  0 q~ vCOMPLEX IONS - LIGANDSD(2ffA   0& A  some ligands attach themselves using two or more lone pairs classified by the number of lone pairs they use multidentate and bidentate ligands lead to more stable complexes Multidentate form several co-ordinate bondsR@    b        !     L   C $A hemeg9    0h40@  HAEM A complex containing iron(II) which is responsible for the red colour in blood and for the transport of oxygen by red blood cells. Co-ordination of CO molecules interferes with the process*f  B  s *޽h ? ̙33y___PPT10Y+D=' = @B + 0L0 p /( Ow@ dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0  0Eq~ vCOMPLEX IONS - LIGANDSD(2ffA   0G A  some ligands attach themselves using two or more lone pairs classified by the number of lone pairs they use multidentate and bidentate ligands lead to more stable complexes Multidentate form several co-ordinate bondsR@    b        !     P   C (Acphyllgnx 0P   C (A!monastgTGB  s *޽h ? ̙33y___PPT10Y+D=' = @B +.  0L0 = 5  ( w dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0  0@Yq~ jCO-ORDINATION NUMBER & SHAPE2(2ffC   0Ti"`  the shape of a complex is governed by the number of ligands around the central ion the co-ordination number gives the number of ligands around the central ion a change of ligand can affect the co-ordination number Co-ordination No. Shape Example(s) 6 Octahedral [Cu(H2O)6]2+ 4 Tetrahedral [CuCl4]2- Square planar Pt(NH3)2Cl2 2 Linear [Ag(NH3)2]+@PF)@P`@#           Z7  H  '   P   C (A cltetraK f L   C $A 6aqua{N   C &A cplatg R T  C ,AsilvcompgSnB  s *޽h ? ̙33y___PPT10Y+D=' = @B +  0L0   T (  TdB T <D)P0Q T 0Pp@ 0 0dB T@ <D)PXP T 0X0@ 0 0 T 0q~ hISOMERISATION IN COMPLEXES2(2ff  T 0$"`~ 9Some octahedral complexes can exist in more than one form :H: : ` T C *A clcomp2b"`"@ ` T C *A clcomp3a"` "H ` T C *Aclcomp3b"` ` T C *Aclcomp2a"` T 000  [MA4B2]n+ @f ff ff f   T 0     [MA3B3]n+ @f ff ff ff   T 0(>   cTRANS.H   T 0 (&  aCIS.H  B T s *޽h ? ̙33y___PPT10Y+D=' = @B + 0L0  X V(  XdB X <D)P0Q X 0Pp@ 0 0dB X@ <D)PXP X 0X0@ 0 0 X 0q~ hISOMERISATION IN COMPLEXES2(2ffG  X 0"` 0Y GEOMETRICAL (CIS-TRANS) ISOMERISM Square planar complexes of the form [MA2B2]n+ exist in two forms trans platin cis platin"HAX)@"'    Zx       d  X S .Atplatin"`E> b  X S ,A cplatg"`E?   X 0dơ >   YAn important anti-cancer drug. It is a square planar, 4 co-ordinate complex of platinum.ZZ Z B X s *޽h ? ̙33y___PPT10Y+D=' = @B +5 0L0 D< \(  \dB \ <D)P0Q \ 0Pp@ 0 0dB \@ <D)PXP \ 0X0@ 0 0 \ 0 ϡq~ hISOMERISATION IN COMPLEXES2(2ffl  \ 0ԡ"`wj `Octahedral complexes with bidentate ligands can exist as a pair of enantiomers (optical isomers) aHaZ         `  \ C *Aoptcompb"` `  \ C *Aoptcompa"`|   \ 0ۡ 0 >OPTICAL ISOMERISM Some octahedral complexes exist in two forms>H-X- ? R \ C *Acoen2cl2  B \ s *޽h ? ̙33y___PPT10Y+D=' = @B +N 0L0 ]U@ <(  <dB < <D)P0Q < 0Pp@ 0 0dB <@ <D)PXP < 0X0@ 0 0 < 0q~ hISOMERISATION IN COMPLEXES2(2ff < 0@"`x aOPTICAL ISOMERISM Hf    < 0 0o 2jOPTICAL ISOMERISM AND GEOMETRICAL ISOMERSIM The complex ion [Co(en)2Cl2]+ exhibits both types of isomerism,H?X,   " k R  < C *Acoen2cl2 B < s *޽h ? ̙33y___PPT10Y+D=' = @B +  0L0 , $ P @(  @dB @ <D)P0Q @ 0Pp@ 0 0dB @@ <D)PXP @ 0X0@ 0 0 @ 0q~ hISOMERISATION IN COMPLEXES2(2ff @ 0"`x aOPTICAL ISOMERISM Hf   @ 0  0o 2jOPTICAL ISOMERISM AND GEOMETRICAL ISOMERSIM The complex ion [Co(en)2Cl2]+ exhibits both types of isomerism,H?X,   " k   @ 0D"`l   eGEOMETRICAL ISOMERISM Hf  R  @ C *Acoen2cl2 X  @ C 0Acoen2cl2geoZ qV  @ 0T"`_ ` SCIS Hf    @ 0l"`a~ UTRANS Hf  B @ s *޽h ? ̙33y___PPT10Y+D=' = @B + 0L0 )! ( w dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0  0q~ bCATALYTIC PROPERTIES2(2ff   0x kTransition metals and their compounds show great catalytic activity It is due to partly filled d-orbitals which can be used to form bonds with adsorbed reactants which helps reactions take place more easilyRDH@D&`   f    0T)&  bExamples of catalysts IRON Manufacture of ammonia - Haber Process NICKEL Hydrogenation reactions - margarine manufacture RHODIUM Catalytic converters VANADIUM(V) OXIDE Manufacture of sulphuric acid - Contact Process8H@f&7   B  s *޽h ? ̙33y___PPT10Y+D=' = @B + 0L0 % @(   X @ @ <̙? x @D 0 0 @ 08#x m i/ 2009 JONATHAN HOPTON & KNOCKHARDY PUBLISHING0(20 f @ 0\(fM  ATHE END(2f @ 0, -AN INTRODUCTION TO TRANSITION METAL CHEMISTRYT$(2 82 f0f<fJ  @ C "A KTRE  p H @ 0޽h ? ̙33y___PPT10Y+D=' = @B +r@f1&,OM hAd7`Z'86@nv?ZGPuUhbGQ@ғV@pn}{\9e߰,V* :?j pT\m |7nOh+'0T hp   No Slide TitleHOPTONJONATHAN HOPTON879Microsoft PowerPoint@PH\@@hNx@E. 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