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S  6D$ <K   P*    6$) v K  R*  H  0g彖 ? ̙3380___PPT10.Z=_ 0X(   $+ X X 0(Q <7   X*  X 0$U v 7  Z*  X 6lZ <K   X*  X 6pF v K  Z* H X 0g彖 ? ̙3380___PPT10.Zٌ_ 0L0 ( $(    0/ 0SHAPES OF MOLECULES A guide for A level studentsB1(26f<f  0P5 OKNOCKHARDY PUBLISHING(2fJ  C "A KTRE]  (  ( 0H:"`>B 2008 SPECIFICATIONS<G$G   B  s *޽h ? ̙33}  0L0   P  (  I  0p 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,   0@ OSHAPES OF MOLECULES (2$fjB  BD)@0A  6Pp@ 0 0jB @ BD)@X@  6X0@ 0 0dB  <D?    0T`  OKNOCKHARDY PUBLISHING(2___B  s *޽h ? ̙33  0L0 Z R `!  (    0@  O CONTENTS Prior knowledge Electron pair repulsion theory The regular molecular shapes Shapes of molecules with lone pairs Shapes of ions Molecules with double bonds Other examples Test questions Check listJ0}2 ( jB   BD)@0A   6Pp@ 0 0jB  @ BD)@X@   6X0@ 0 0  6?_P@ 0 0  <?_@ 0 0  <?_ 0@ 0 0  <?_  @ 0 0  <?X /m @  0 0  <?0 O @  0 0  <? _h @  0 0  <?(_/ @} 0 0  0 OSHAPES OF MOLECULES (2$f   <?0  @u 0 0 ! <? ww r @  0 0B  s *޽h ? ̙33 0L0 _Wp p(  p p 0H ` ~Before you start it would be helpful to& know the definition of a covalent bond know what a lone pair is know that like charges repelH*(2d 2)ddB p <D)@0A p 0Pp@ 0 0dB p@ <D)@X@ p 0X0@ 0 0  p 0Ñ OSHAPES OF MOLECULES (2$fB p s *޽h ? ̙33 0L0  DT ( T T  T 0 XELECTRON PAIR REPULSION THEORY(2fjB T BD)@0A T 6Pp@ 0 0jB T@ BD)@X@ T 6X0@ 0 0j T s *?f/V  THE SHAPE ADOPTED BY A SIMPLE MOLECULE OR ION IS THAT WHICH KEEPS REPULSIVE FORCES TO A MINIMUM 2b(2a T s *?m  uMolecules contain covalent bonds. As covalent bonds consist of a pair of electrons, each bond will repel other bonds.v 2v<L H_  8T# Y _ "T <F?  DAl&(2 2 #TB c ƃC`mENGĄH.xJ~NQfԔ? `TޢN`m`TޢN`m~NN`m~N-jB $T  `?DԔ?B %T TDԔ?H3 b B -T TDԔ?|& U  2 .T c ƃC`mENGĄH.xJ~NQfԔ? `TޢN`m`TޢN`m~NN`m~N7 2 4T c μB.vCסENGaH"BI!QfjJ? n.v>Cסn.v>Cס!`T>Cס!`T _ pB 6T HDjJ?Bbc 7T 6 F?`h  4Bonds are further apart so repulsive forces are lessZ5 2  9T 6F? 9Bonds are closer together so repulsive forces are greater\: 2 pB :T HDjJ?\ll<L   5T#    'T < F?>%  DAl&(2 2 (T c ƃC xENGZYHGJ^QQjJ? `TUJ x`TUJ x^QUJ x^QsB )T  `?DԔ?QQYB *T TDԔ?| B +T TDԔ?t  2 0TB c ƃC xENGZYHGJ^QQjJ? `TUJ x`TUJ x^QUJ x^Q1 2 1T c μC xENGZYHGJ^QQjJ? `TUJ x`TUJ x^QUJ x^Q9  ;T 6F?6   9All bonds are equally spaced out as far apart as possible:: 2pB ?X     6F?4U hu ZCl"(2   6 F?8U lu ZCl"(2   6F?U u @Be"(2rB   BD>? H 2   BwENGPITQfo? wnMw`TwnMw`TT`TnMw`TT`T@ (   <\Ff? t  L180,(2ff  6xF?c $N  QBOND PAIRS 2 LONE PAIRS 0 2  <TFo?  `BOND ANGLE... SHAPE....82______  6F?6 | O 180 LINEAR( 02 F 0h  Pf2  6o?P=  6F? X? \Cl$(2x2  H?33?Px2  H?33?Hx2  H?33?0x2  H?33?Hhx2  H?33?`x2  H?33?0xx2  H?33?XPF Oxx  AA  6F? BBe$(2f2  6o?{xkxf2   6f?O<f2 ! 6f?'D F  ` "  I # 6D?C BBe$(2f2 $ 6o? ==f2 % 6o?XE & 68?TX \Cl$(2x2 ' H?33?`x2 ( H?33?j/x2 ) H?33?lXx2 * H?33?]ux2 + H?33?`x2 , H?33?@x2 - H?33?sf2 . 6o?,  / 6F?( ,  \Cl$(2x2 0 H?33? 0 x2 1 H?33? o| x2 2 H?33? d$x2 3 H?33? Td x2 4 H?33? N8 x2 5 H?33? | x2 6 H?33? T f2 7 6f??yf2 8 6f? !D 9 0? V Beryllium - has two electrons to pair up Chlorine - needs 1 electron for  octet (Q 2P : 0@? V {ETwo covalent bonds are formed Beryllium still has an incomplete shellF 2FB  s *޽h ? ̙33 0L0 0(  dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0X  C 0A shapetpyrag#   60*? ADDING ANOTHER ATOM - ANIMATION2 (2ffB  s *޽h ? ̙33y___PPT10Y+D=' = @B +h 0L0 7wx( ^(  x^2 Ax 6o?dB x <D)@0A x 0Pp@ 0 0dB x@ <D)@X@ x 0X0@ 0 0d2 x <?KEd2 x <?lf x < H?   BAl$(2 1x 6M? ZALUMINIUM CHLORIDE,(2f^2 @x 6?E8 0h Qxx8f2 Bx 6o?P= Ix 6|Q? X? \Cl$(2~2 x N?33?Px2 Kx H?33?Hx2 Lx H?33?0x2 Mx H?33?Hhx2 Nx H?33?`x2 Ox H?33?0xx2 Px H?33?X8  P qx Pl2 Dx <o? PP Gx <0Y?   BAl$(2l2 Sx <o? 0 Tx <<^? ,0 \Cl$(2~2 Ux N?33? `@~2 Vx N?33? Ph~2 Wx N?33? HP~2 Xx N?33? X(~2 Yx N?33? xX~2 Zx N?33? `P~2 [x N?33? X8l2 ]x <o? 0 ^x <e? ,0 \Cl$(2~2 _x N?33? hH~2 `x N?33? p~2 ax N?33? P~2 bx N?33? X~2 cx N?33? 8@~2 dx N?33? x8~2 ex N?33?  l2 gx <o?   hx <l?  \Cl$(2~2 ix N?33? X@~2 jx N?33?  PP ~2 kx N?33? @ H ~2 lx N?33? P(~2 mx N?33? hH~2 nx N?33? 8 8 ~2 ox N?33? `Hl2 Hx <? L<l2 Fx <? /El2 Ex <? [T wx 0dw?|m  TAluminium - has three electrons to pair up Chlorine - needs 1 electron to complete  octet Three covalent bonds are formed; aluminium still has an incomplete outer shell. 2$ s &B x s *޽h ? ̙33 ' 0L0 &&CC&(  ^2  6o?dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0^2  6?KE^2  6?lf   6`?   BAl$(2   6? ZALUMINIUM CHLORIDE,(2fjB   BD>?% / %    6? 4  ZCl"(2   6̕? | ZCl"(2  6? 1  @Al"(22   BENGPH!ITQfo? wnMwnMT`TnMT`T3 P# jB  BD>?    <4f? ;  L120,(2ffpB  HD>? O   6h?3 S  ZCl"(2^2  6?EF 0h  x8f2  6o?P=  6ĥ? X? \Cl$(2x2  H?33?Px2  H?33?Hx2  H?33?0x2  H?33?Hhx2  H?33?`x2  H?33?0xx2  H?33?XF  P   Pf2   6o?PP ! 6`?  BAl$(2f2 " 6o?0 # 6?,0 \Cl$(2x2 $ H?33?`@x2 % H?33?Phx2 & H?33?HPx2 ' H?33?X(x2 ( H?33?xXx2 ) H?33?`Px2 * H?33?X8f2 + 6o?0 , 6ȹ?,0 \Cl$(2x2 - H?33?hHx2 . H?33?px2 / H?33?Px2 0 H?33?Xx2 1 H?33?8@x2 2 H?33?x8x2 3 H?33? f2 4 6o?  5 6? \Cl$(2x2 6 H?33?X@x2 7 H?33? PP x2 8 H?33?@ H x2 9 H?33?P(x2 : H?33?hHx2 ; H?33?8 8 x2 < H?33?`Hf2 = 6?L<f2 > 6?/Ef2 ? 6?[T @ 6H?c $N  QBOND PAIRS 3 LONE PAIRS 0 2 A <o?  `BOND ANGLE... SHAPE....82______ B 6?6 4  X120 TRIGONAL PLANAR(02 C 0T?|m  TAluminium - has three electrons to pair up Chlorine - needs 1 electron to complete  octet Three covalent bonds are formed; aluminium still has an incomplete outer shell. 2$ s &B  s *޽h ? ̙33' 0L0 &&CC&(  ^2  6o?dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0^2  6?KE^2  6?lf   6x?   BAl$(2   6? ZALUMINIUM CHLORIDE,(2fjB   BD>?% / %    6X? 4  ZCl"(2   6? | ZCl"(2  6 ? 1  @Al"(22   BENGPH!ITQfo? wnMwnMT`TnMT`T3 P# jB  BD>?    <\f? ;  L120,(2ffpB  HD>? O   6?3 S  ZCl"(2^2  6?EF 0h  x8f2  6o?P=  6 ? X? \Cl$(2x2  H?33?Px2  H?33?Hx2  H?33?0x2  H?33?Hhx2  H?33?`x2  H?33?0xx2  H?33?XF  P   Pf2   6o?PP ! 60?  BAl$(2f2 " 6o?0 # 6T?,0 \Cl$(2x2 $ H?33?`@x2 % H?33?Phx2 & H?33?HPx2 ' H?33?X(x2 ( H?33?xXx2 ) H?33?`Px2 * H?33?X8f2 + 6o?0 , 6 ?,0 \Cl$(2x2 - H?33?hHx2 . H?33?px2 / H?33?Px2 0 H?33?Xx2 1 H?33?8@x2 2 H?33?x8x2 3 H?33? f2 4 6o?  5 6T'? \Cl$(2x2 6 H?33?X@x2 7 H?33? PP x2 8 H?33?@ H x2 9 H?33?P(x2 : H?33?hHx2 ; H?33?8 8 x2 < H?33?`Hf2 = 6?L<f2 > 6?/Ef2 ? 6?[T @ 60?c $N  QBOND PAIRS 3 LONE PAIRS 0 2 A <4o?  `BOND ANGLE... SHAPE....82______ B 6|8?6 4  X120 TRIGONAL PLANAR(02 C 0<?|m  TAluminium - has three electrons to pair up Chlorine - needs 1 electron to complete  octet Three covalent bonds are formed; aluminium still has an incomplete outer shell. 2$ s &B  s *޽h ? ̙33y___PPT10Y+D=' = @B + 0L0 E(  dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0X D C 0A shapetetrag]J  E 6XH? mADDING ANOTHER ATOM - ANIMATION2 (2ffB  s *޽h ? ̙33y___PPT10Y+D=' = @B + 0L0 ia&$ (  dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0   6X?  OMETHANE,(2f+F 8  x n ,hf2 o 6?p 4  p 6^?   AC$(2f2 q 6o?8  xf2 r 6?`  Mf2 s 6? \ Ef2 t 6? ,T F  H ( u  v 6b?   AH$(2f2 w 6o? H (x2 x H?? 0 ^2 y 6o?;=Q F X z 3 pf2 { 6?M5 | 6h?i AC$(2f2 } 6o?-Xf2 ~ 6?lf2  6?`uf2  6?|A  6\p? AH$(2f2  6o?Xx2  H??X  6r?hxO AH$(2f2  6o?Px2  H??Hx  6}?4 AH$(2f2  6o?eXx2  H??EH  64t?r AH$(2x2  H??J=  0u?D  NCarbon - has four electrons to pair up Hydrogen - 1 electron to complete shellO 2O  0?  u?Four covalent bonds are formed C and H now have complete shells@ 2@B  s *޽h ? ̙33 0L0 '55(  dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0  6X?  OMETHANE,(2f  6?c $N  QBOND PAIRS 4 LONE PAIRS 0 2  <o?  `BOND ANGLE... SHAPE....82______   6$?6   V109.5 TETRAHEDRAL(02+F 8  x   ,hf2   6?p 4    6?   AC$(2f2   6o?8  xf2  6?`  Mf2  6? \ Ef2  6? ,T F  H (    6Ԭ?   AH$(2f2  6o? H (x2  H?? 0 ^2  6o?;=Q F X  3 pf2  6?M5  6?i AC$(2f2  6o?-Xf2  6?lf2  6?`uf2  6?|A  6? AH$(2f2  6o?Xx2  H??X   6@?hxO AH$(2f2 ! 6o?Px2 " H??Hx # 6 ă?4 AH$(2f2 $ 6o?eXx2 % H??EH & 6X?r AH$(2x2 ' H??J={F 2 E (  2E2 ) # BsC>E$GCՃHڻI`TQfo? >s>s`T`T>s`T`T   * < f?2   N109.5,(2ffrB + BD>?   , 6ʃ?   ?H"(2 - 6؃?& % ?H"(2 . 6d݃?~ }  ?C"(2xB / HD>?b XH xB 0 HxRD>?`   1 6,?   ?H"(2 2 6L?F E  ?H"(2lb 3 <? U&  4 0t?D  NCarbon - has four electrons to pair up Hydrogen - 1 electron to complete shellO 2O 5 0?  u?Four covalent bonds are formed C and H now have complete shells@ 2@B  s *޽h ?) ̙33` 0L0 P*6(  dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0  6?  OMETHANE,(2f  6?c $N  QBOND PAIRS 4 LONE PAIRS 0 2  <|o?  `BOND ANGLE... SHAPE....82______   6?6   V109.5 TETRAHEDRAL(02+F 8  x   ,hf2   6?p 4    6 ?   AC$(2f2   6o?8  xf2  6?`  Mf2  6? \ Ef2  6? ,T F  H (    6,?   AH$(2f2  6o? H (x2  H?? 0 ^2  6o?;=Q F X  3 pf2  6?M5  6?i AC$(2f2  6o?-Xf2  6?lf2  6?`uf2  6?|A  6? AH$(2f2  6o?Xx2  H??X   6#?hxO AH$(2f2 ! 6o?Px2 " H??Hx # 6$)?4 AH$(2f2 $ 6o?eXx2 % H??EH & 60,?r AH$(2x2 ' H??J= 4 0D1?D  NCarbon - has four electrons to pair up Hydrogen - 1 electron to complete shellO 2O 5 0L6?  u?Four covalent bonds are formed C and H now have complete shells@ 2@\ 6 C 4A tetrahedral3dm <B  s *޽h ? ̙33+ 0L0 t+l+M|4  *(  |dB | <D)@0A | 0Pp@ 0 0dB |@ <D)@X@ | 0X0@ 0 0 1| 6>?$` ^PHOSPHORUS(V) FLUORIDE,(2f8 s5 ||< f2 >| 6o?l2 ?| <?c=~2 @| N??fE A| 6E?@  AF$(2~2 B| N??s5~2 x| N??,w~2 y| N??,~2 z| N??f5~2 {| N??d2 D| <o?  p]  E| <0K? (X AP$(2v2 F| N??  Pv2 G| N?? PPv2 I| N?? x v2 J| N?? xv2 }| N?? xX8 P y | 'Ql2 | <o? XXl2 | <o? 0 | <HR? D AP$(2l2 | <o? ((r2 | B? M2 | T?? U | <W? }I AF$(22 | T?? E2 | T?? S<2 | T?? <T2 | T?? E2 | T?? Dl2 | <o? } CmCr2 | B? `2 | T?? p | <^?   AF$(22 | T?? P  02 | T?? |2 | T??  /2 | T??  TP2 | T?? k  l2 | <o? pxpr2 | B? TU2 | T?? D | <Xe? 0 AF$(22 | T?? t2 | T?? >L2 | T?? LO2 | T?? N42 | T?? Ml2 | <o? XHr2 | B?   lm2 | T?? % | <Hl? X? AF$(22 | T?? [ m2 | T?? To2 | T?? G2 | T?? 2 | T?? &%~2 | N?? p~2 | N?? 8~2 | N??  ~2 | N?? ~2 | N?? X0r2 | B? 8$2 | T?? vA | <@t? d AF$(22 | T?? @42 | T?? 2 | T?? W2 | T?? 'y2 | T?? &A( | 0z?|  pPhosphorus - has five electrons to pair up Fluorine - needs one electron to complete  octet Five covalent bonds are formed; phosphorus can make use of d orbitals to expand its  octet  2B | s *޽h ? ̙337 0L0 `7X7bb6(  dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0  6?$` ^PHOSPHORUS(V) FLUORIDE,(2f F s5  < f2  6o?l2   <?c=~2   N??fE   6?@  AF$(2~2   N??s5~2   N??,w~2  N??,~2  N??f5~2  N??^2  6o? p]   6 ?(X AP$(2p2  H?? Pp2  H??PPp2  H??x p2  H??xp2  H??xXF P y   'Qf2  6o?XXf2  6o?0  68?D AP$(2f2  6o?((l2  <?M~2  N??U  6?}I AF$(2~2   N??E~2 ! N??S<~2 " N??<T~2 # N??E~2 $ N??Df2 % 6o?} CmCl2 & <?`~2 ' N??p ( 6?  AF$(2~2 ) N??P  0~2 * N??|~2 + N?? /~2 , N?? TP~2 - N??k  f2 . 6o?pxpl2 / <?TU~2 0 N??D 1 6H?0 AF$(2~2 2 N??t~2 3 N??>L~2 4 N??LO~2 5 N??N4~2 6 N??Mf2 7 6o?XHl2 8 <?  lm~2 9 N??% : 68?X? AF$(2~2 ; N??[ m~2 < N??To~2 = N??G~2 > N??~2 ? N??&%x2 @ H??px2 A H??8x2 B H?? x2 C H??x2 D H??X0l2 E <?8$~2 F N??vA G 60?d AF$(2~2 H N??@4~2 I N??~2 J N??W~2 K N??'y~2 L N??&A M 6? $s  QBOND PAIRS 5 LONE PAIRS 0 2 N <(Èo?-  `BOND ANGLE... SHAPE....82______ O 6Ȉ?[   ^"120 & 90 TRIGONAL BIPYRAMIDAL #02# F &h  P  &2 Q # CmENGCՃH6mI`TJ8.Qfo? m m `T8.m `T8.g z]  R <8ƈf?& p  L120,(2ff S 6ш?   ?F"(2 T 6Ո?  ?F"(2 U 6ڈ?   ?P"(2xB V HD>?   W 6$?h   ?F"(2 X 6?j   ?F"(2rB Y BD>?0 0 rB Z BD>?0x 0  [ 6l?5 U  ?F"(2\T    \# @  xB ] HDo?  xB ^ HDo?   _ <f? 2h  K90,(2ffxB ` HD>?  lb a < ?x x ( b 0?|  pPhosphorus - has five electrons to pair up Fluorine - needs one electron to complete  octet Five covalent bonds are formed; phosphorus can make use of d orbitals to expand its  octet  2B  s *޽h ?Q ̙3393 0L0 22Y@O2(  dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0  6@? \SULPHUR(VI) FLUORIDE,(2f%F DM   fo   6?m/ CF&(2l2   <o?x0~2   N??D~2   N??'}~2  N??n m~2  N??g~2  N??|~2  N??6 ~2  N??M8 7 z :l2  <o?   < ?+' AS$(2~2  N??OO~2  N??~2  N??~2  N??O7~2  N??"~2  N??#8  +m ,-r2  Bo?|Kl2   <o?`M ! <?tH AS$(2r2 & Bo?L ' <?s5 CF&(22 ( T??q'2 ) Z??52 * Z??$+2 + Z??d2 , Z??k52 - Z??t!~2 . N??F02 / Z??+Ur2 0 Bo?6G 1 <?e CF&(22 2 T??2 3 Z??ne2 4 Z??u?2 5 Z??4v2 6 Z??\G2 7 Z??]o2 8 Z??vr2 : Bo?h  ; <&?M CF&(22 < T??<2 = Z??CH2 > Z??gW2 ? Z??_^2 @ Z??w(2 A Z??v?~2 B N??V2 C T??3~2 D N??{t2 E T??j2 F T??;+2 G T??B2 H T??Br2 I T??[K2 J T??j k K <\/?I/  CF&(22 L T??23l2  <o?.?  6X4?] CF&(2~2  N??D{2  T?? 6U2  T??$2  T??g2  T??42  T?? _2  T??V~2 # N??_l2  <o?\  6`;?u7 CF&(2~2  N??s2  T???\2  T??F{2  T??fD2  T??72  T??> l2  T?? tm~2 % N??wPx2  H??4  0B?{  `Sulphur - has six electrons to pair up Fluorine - needs one electron to complete  octet Six covalent bonds are formed; sulphur can make use of d orbitals to expand its  octet  26qB  s *޽h ? ̙33> 0L0 !>>nn=(  dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0  6M? \SULPHUR(VI) FLUORIDE,(2f%F DM  fo  6|R?m/ CF&(2l2   <o?x0~2   N??D~2   N??'}~2   N??n m~2   N??g~2  N??|~2  N??6 ~2  N??MsF 7   :f2  6o?   6Y?+' AS$(2x2  H??OOx2  H??x2  H??x2  H??O7x2  H??"x2  H??  6_?[ $F  QBOND PAIRS 6 LONE PAIRS 0 2  <ao?  `BOND ANGLE... SHAPE....82______  6h?.   K90 OCTAHEDRAL 02+"F  +m  ,-l2  <o?|Kf2  6o?`M   6@m?tH AS$(2l2 ! <o?L " 6p?s5 CF&(2~2 # N??q'2 $ T??52 % T??$+2 & T??d2 ' T??k52 ( T??t!x2 ) H??F02 * T??+Ul2 + <o?6G , 6`x?e CF&(2~2 - N??2 . T??ne2 / T??u?2 0 T??4v2 1 T??\G2 2 T??]o2 3 T??vl2 4 <o?h  5 6?M CF&(2~2 6 N??<2 7 T??CH2 8 T??gW2 9 T??_^2 : T??w(2 ; T??v?x2 < H??V~2 = N??3x2 > H??{t~2 ? N??j~2 @ N??;+~2 A N??B~2 B N??Br~2 C N??[K~2 D N??j k E 6䇋?I/  CF&(2~2 F N??23l2 G <o?.? H 6H?] CF&(2~2 I N??D{2 J T?? 6U2 K T??$2 L T??g2 M T??42 N T?? _2 O T??Vx2 P H??_l2 Q <o?\ R 6ē?u7 CF&(2~2 S N??s2 T T???\2 U T??F{2 V T??fD2 W T??72 X T??> l2 Y T?? tmx2 Z H??wPx2 [ H??4 \ 0?{  `Sulphur - has six electrons to pair up Fluorine - needs one electron to complete  octet Six covalent bonds are formed; sulphur can make use of d orbitals to expand its  octet  26qk F V  ] < VN V ^ V  _ 6?J   9F(2 ` 6Ԧ?V6 "  AF$(2 a 6?w w^  9F(2 b 6x? }  AF$(2lb c <P?  [ lb dB <e?: r  e 64?\ C  CS&(2xB fB HDԔ?l = xB g HDԔ?K  rB h BDԔ?# #Z rB i BDԔ?#C #  j 6̹?  9F(2 k 6?  9F(2xB l HDo?1 # xB m HDo?   n <f?n .  K90,(2ffB  s *޽h ? ̙334 0L0 Q4I4`]o 3(   dB   <D)@0A   0Pp@ 0 0dB  @ <D)@X@   0X0@ 0 0   6dˋ? \SULPHUR(VI) FLUORIDE,(2f%F DM   fo   6Ћ?m/ CF&(2l2   <o?x0~2   N??D~2   N??'}~2   N??n m~2   N??g~2   N??|~2   N??6 ~2   N??MsF 7    :f2   6o?    6d؋?+' AS$(2x2   H??OOx2   H??x2   H??x2   H??O7x2   H??"x2   H??   6?[ $F  QBOND PAIRS 6 LONE PAIRS 0 2   <݋o?  `BOND ANGLE... SHAPE....82______   6 ?.   K90 OCTAHEDRAL 02+"F  +m   ,-l2   <o?|Kf2   6o?`M   6?tH AS$(2l2 !  <o?L "  6?s5 CF&(2~2 #  N??q'2 $  T??52 %  T??$+2 &  T??d2 '  T??k52 (  T??t!x2 )  H??F02 *  T??+Ul2 +  <o?6G ,  6܋?e CF&(2~2 -  N??2 .  T??ne2 /  T??u?2 0  T??4v2 1  T??\G2 2  T??]o2 3  T??vl2 4  <o?h  5  64?M CF&(2~2 6  N??<2 7  T??CH2 8  T??gW2 9  T??_^2 :  T??w(2 ;  T??v?x2 <  H??V~2 =  N??3x2 >  H??{t~2 ?  N??j~2 @  N??;+~2 A  N??B~2 B  N??Br~2 C  N??[K~2 D  N??j k E  6 ?I/  CF&(2~2 F  N??23l2 G  <o?.? H  6?] CF&(2~2 I  N??D{2 J  T?? 6U2 K  T??$2 L  T??g2 M  T??42 N  T?? _2 O  T??Vx2 P  H??_l2 Q  <o?\ R  6?u7 CF&(2~2 S  N??s2 T  T???\2 U  T??F{2 V  T??fD2 W  T??72 X  T??> l2 Y  T?? tmx2 Z  H??wPx2 [  H??4 \  0#?{  `Sulphur - has six electrons to pair up Fluorine - needs one electron to complete  octet Six covalent bonds are formed; sulphur can make use of d orbitals to expand its  octet  26qZ o  C 2Aoctahedral3d` #B   s *޽h ? ̙33w 0L0 1`M(    0+ JIRREGULAR SHAPES(2fdB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0L   s */?9 If a molecule, or ion, has lone pairs on the central atom, the shapes are slightly distorted away from the regular shapes. This is because of the extra repulsion caused by the lone pairs.  2   6L5?)7 "NBOND PAIR - BOND PAIR < LONE PAIR - BOND PAIR < LONE PAIR - LONE PAIR O 2 8 i 6p  . { \  S ,Alpairp 64 tB  TDԔ?P  p   <,B?i Y {  CO&(22 B C ƃC {ENHGQ|? `TJ {`TJ {`TJ {`T _ E8 N  -{   <G?{  CO&(2 2 B c ƃC xENGZYHGJ^QQjJ? `TUJ x`TUJ x^QUJ x^QL B   `?DԔ?fNf~B   NDԔ?  8 N  /Lp ^  S .Alpairp2S  \ ' S ,AlpairpN ) <R?  CO&(2 2 *B c ƃC xENGZYHGJ^QQ;? `TUJ x`TUJ x^QUJ x^Q[  0 s *U?   lAs a result of the extra repulsion, bond angles tend to be slightly less as the bonds are squeezed together.m(2mB  s *޽h ??0* ̙33 0L0 z'0 (  dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0  6_?|  OAMMONIA,(2fF  H (    6a?   AH$(2f2  6o? H (x2  H?? 0 8 8 N  <g?hO AN$(2l2  <o?Xx2 E H??x2 F H??Hx2 G H??@Hx2 H H??P8x2 I H??P 8 %0 K-x   < NxRDԔ?( h  ? 6?'  AH$(2jb @ Bu? E N A C &Alpairp6 ] t  2 B@ C C xENGZYHGJ^QQԔ? `TUJ x`TUJ x^QUJ x^Q x 2 C@ c dkC xENGZYHGJ^QQo? `TUJ x`TUJ x^QUJ x^Q + ]@F    D  l-G 2 E # <BsCME$GsHڻI`TQfo? /Ms/Ms`T`T/Ms`T`Tu   F <f?1   L107,(2fff2 G 6?; j@  H 6(? y  AH$(2 I 6@ ? N  AH$(2 J 6?/   AN$(2~B K NDԔ? @ ~B L NxRDԔ? C  M 6 ?A   AH$(2rb N Bu?V<  f2 O 6?} @  P s *?h4]   The shape is based on a tetrahedron but not all the repulsions are the same LP-BP REPULSIONS > BP-BP REPULSIONS The N-H bonds are pushed closer together Lone pairs are not included in the shape 2L<  B  s *޽h ??0EBC ̙33P 0L0 @(Pv(  dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0  6,?|  OAMMONIA,(2fF  H (     6P?   AH$(2f2   6o? H (x2   H?? 0 F 8      6\?hO AN$(2f2  6o?Xx2  H??x2  H??Hx2  H??@Hx2  H??P8x2  H??PF %0  -x   6?i AN$(2f2  6o?0-  6 ? AH$(2f2  6o?0x2  H??0x2  H??H  6`? AH$(2f2  6o?0 x2  H??H  6?]jD AH$(2f2  6o?B%x2   H??2x2 ! H??`@x2 " H??"x2 # H??H(x2 $ H??P F < n_ % %4fw & 6?< n_ {'BOND PAIRS 3 LONE PAIRS 1 TOTAL PAIRS 48( 2 rB ' BDo?pHX O C 0A pyramid3d1g X P C 0A pyramid3d2g# -B  s *޽h ? ̙33j 0L0 0&$ d( w dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0  62?  MWATER,(2fF  H ( X  Y 67?   AH$(2f2 Z 6o? H (x2 [ H?? 0 8 x ]  z-x   e <<?A (%  AO$(2l2 f <o? h  g <A?   AH$(2l2 h <o?x  8~2 i N??x  8~2 j N?f? 8 ~2 m N?f?  } n <,G?F " | AH$(2l2 o <o? ]j ~2 p N?f? MZ ~2 q N?f?(  ~2 r N?f?j  M~2 s N?f?  ~2 t N?? Xx F < n_ u %4fw v 6\M?< n_ {'BOND PAIRS 2 LONE PAIRS 2 TOTAL PAIRS 48( 2 rB w BDo?pH8   y  ] <S? AO$(2l2 ^ <o?(H~2 _ N?f?( ~2 ` N?f?~2 a N?f? y%~2 b N?f? `~2 c N?f?(Hx2 x H?f? zG  s *\?h4D  K Oxygen has six electrons in its outer shell It cannot pair up all six - it is restricted to eight electrons in its outer shell It pairs up only two of its six electrons 2 covalent bonds are formed and 2 pairs of non-bonded electrons are left As the total number of electron pairs is 4, the shape is BASED on a tetrahedron*L 2KB  s *޽h ? ̙33R+ 0L0 **@IM8*(  H  k  < ho? 1c #ANGLE... 104.5 SHAPE... ANGULAR$082___  ___  dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0|B   TDjJ? g   6t? 0 AH$(2   6y?   AO$(2vB   NxRDԔ?m UC  6?lS, AH$(2jb  Bu? h&N  C &Alpairp B P  C (Alpairp2C # pB @ HDjJ?p tvB @ NiO7DjJ? QvB @ NiO7DjJ?5  pB  HDjJ?|vB  NDjJ? F  H (    6?   AH$(2f2  6o? H (x2  H?? 0 F x ]   -x    6t?A (%  AO$(2f2  6o? h   6p?   AH$(2f2  6o?x  8x2   H??x  8x2 ! H?f? 8 x2 " H?f?  } # 6?F " | AH$(2f2 $ 6o? ]j x2 % H?f? MZ x2 & H?f?(  x2 ' H?f?j  Mx2 ( H?f?  x2 ) H?? Xx F < n_ * %4fw + 6?< n_ {'BOND PAIRS 2 LONE PAIRS 2 TOTAL PAIRS 48( 2 rB , BDo?pHsF   -   . 6? AO$(2f2 / 6o?(Hx2 0 H?f?( x2 1 H?f?x2 2 H?f? y%x2 3 H?f? `x2 4 H?f?(Hx2 5 H?f? zG 6 6?   AH$(2 7 6H? { m  AO$(2vB 8 NxRDԔ?M h # 9 6\?L  AH$(2jb : Bu? E N ; C &Alpairp[ ]  2 <@ C C xENGZYHGJ^QQԔ? `TUJ x`TUJ x^QUJ x^Q 2 =@ S dkC xENGZYHGJ^QQo? `TUJ x`TUJ x^QUJ x^Q + 2 > # <BsCME$GsHڻI`TQfo? /Ms/Ms`T`T/Ms`T`T Z  ? <@f? c  N104.5,(2ff^2 @ 6?   A 68“?\ l1  AH$(2 B 6Ǔ? \'  AO$(2vB C NxRDԔ? s  D 6̓? T\  AH$(2jb E Bu? V ^2 F 6?  P G C (Alpairp2 f 2 H@ S C xENGZYHGJ^QQ33Ԕ? `TUJ x`TUJ x^QUJ x^Q G ~  ^2 I 6? 2N ^2 J 6?_ 2  K 0ғf?h4]   The shape is based on a tetrahedron but not all the repulsions are the same LP-LP REPULSIONS > LP-BP REPULSIONS > BP-BP REPULSIONS The O-H bonds are pushed even closer together Lone pairs are not included in the shape 2Pf[ L 6?  MWATER,(2fB  s *޽h ?O@><=H ̙33, 0L0 ++PNS, +( w dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0 1 6H? [XENON TETRAFLUORIDE,(2f%F DM  W6?`  6 ?m/ CF&(2l2  <o?x0~2  N??D~2  N??'}~2  N??n m~2  N??g~2  N??|~2  N??6 ~2  N??M8  _  ' _ l2 I <o?@- J <?,P \Xe$(2~2 K N??x8~2 L N??`P~2 M N?? Ez~2 N N??6_~2 O N??Hx2  H??x x2  H??c7x2  H??/ 8  hC h r2  Bo? c |f2  6o?  6? \Xe$(2x2  H??Wx2  H??x2  H??gx2   H??r2  Bo?  ~g  <? K#  CF&(22 [ T?? *s2  Z??  F 2  Z??  5'2  Z?? E2  Z??  %?2  Z?? 4&x2  H??02   T??T~l2   <o?    6h ?bT$( CF&(2~2   N??XL2  T?? 4P2  T?? O$2  T??SO2  T??CG2  T??_D2  T??#8x2  H??T(l2  <o?wY  6? CF&(2~2  N??R$2  T?? C2  T??2  T??2  T??q2  T??hvx2  H??8~2  N??3%~2  N?? ,2  T?? Q2 € T?? YL2 Ā T?? )[2 ŀ T?? :2 ƀ T?? |2 ǀ T?? ;: ̀ <0? @ CF&(2~2  N??L O s *?|h  ; Xenon has eight electrons in its outer shell It pairs up four of its eight electrons 4 covalent bonds are formed and 2 pairs of non-bonded electrons are left As the total number of electron pairs is 6, the shape is BASED on an octahedron* 2F < n_ P %4fw Q 6P#?< n_ {'BOND PAIRS 4 LONE PAIRS 2 TOTAL PAIRS 68( 2 rB R BDo?pHB  s *޽h ? ̙33= 0L0 <<`nuP<(  dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0  6-? [XENON TETRAFLUORIDE,(2f%F DM   W6?`   62?m/ CF&(2l2   <o?x0~2   N??D~2   N??'}~2  N??n m~2  N??g~2  N??|~2  N??6 ~2  N??MF  _    _ f2  6o?@-  6:?,P \Xe$(2x2  H??x8x2  H??`Px2  H?? Ezx2  H??6_x2  H??Hx2  H??x x2  H??c7x2  H??/ PF  hC  h l2  <o?c |f2   6o? ! 6@? \Xe$(2x2 " H??Wx2 # H??x2 $ H??gx2 % H??l2 & <o? ~g ' 6|G?K#  CF&(2~2 ( N??*s2 ) T?? F 2 * T?? 5'2 + T??E2 , T?? %?2 - T??4&x2 . H??02 / T??T~l2 0 <o?  1 6N?bT$( CF&(2~2 2 N??XL2 3 T?? 4P2 4 T?? O$2 5 T??SO2 6 T??CG2 7 T??_D2 8 T??#8x2 9 H??T(l2 : <o?wY ; 6U? CF&(2~2 < N??R$2 = T?? C2 > T??2 ? T??2 @ T??q2 A T??hvx2 B H??8~2 C N??3%x2 D H??,~2 E N??Q~2 F N??YL~2 G N??)[~2 H N??:~2 I N??|~2 J N??;: K 6^?@ CF&(2~2 L N??L Q < d? Y  9F(2 R <4h?- e AF$(2 S <`l?n U 9F(2 T <p? ['t  AF$(2jb U BP? L R jb V@ Be?1  i  W <u?S :  ^Xe&(2vB X@ NDԔ?c  vB Y NDԔ?B ! b Z S ,Alpairp"` #6 V [ S .Alpairp3h @ F    \ } t4E N K  ] ^  xr ^ HjJ?K B _ TDjJ?K B ` TDjJ? k  a 6}?   9F(2 b 6D? j Q  AF$(2 c 6?b .  9F(2 d 6?   AF$(2lb e <P? T  lb fB <e?@n ~  g 6Ў?Q uw  ^Xe&(2xB hB HDԔ?n  xB i HDԔ? ` 2N {   j l % f2 k 6?{  f2 l 6?{  2N {   m   f2 n 6?{  f2 o 6?{  J p <o?[ ,r &ANGLE... 90 SHAPE... SQUARE PLANAR'082 ___  ___   s q s *?|   As the total number of electron pairs is 6, the shape is BASED on an octahedron There are two possible spatial arrangements for the lone pairs The preferred shape has the two lone pairs opposite each other* 2F < n_ r %4fw s 6?< n_ {'BOND PAIRS 4 LONE PAIRS 2 TOTAL PAIRS 68( 2 rB t BDo?pHB  s *޽h ? ̙33y___PPT10Y+D=' = @B +P  0L0 _Wp(  dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0  6?v eCALCULATING THE SHAPE OF IONS,(2f  s *?jY hThe shape of a complex ion is calculated in the same way a molecule by... calculating the number of electrons in the outer shell of the central species * pairing up electrons, making sure the outer shell maximum is not exceeded calculating the number of bond pairs and lone pairs using ELECTRON PAIR REPULSION THEORY to calculate shape and bond angle(s) the number of electrons in the outer shell depends on the charge on the ion if the ion is positive you remove as many electrons as there are positive charges if the ion is negative you add as many electrons as there are negative charges e..g. for PF6- add one electron to the outer shell of P for PCl4+ remove one electron from the outer shell of P pJ 2!! 2 2 *2{ *2.)B  s *޽h ? ̙33y___PPT10Y+D=' = @B +  0L0 , $ {(  dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0  6Օ?  ZSHAPES OF IONS0(2 p s *D?\p  z,Draw outer shell electrons of central atom 2- 2+ F l < q n. r 6?9g AN$(2f2 s 6o?  x2 t H??xx2 u H??*x2 v H??lx2 w H??^<x2 x H??X  z H̙?%y KEXAMPLE((2B  s *޽h ? ̙33 0L0 &"Q(  dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0  6X?  ZSHAPES OF IONS0(2~F lD    "5    0?1. RN+4(2 f2   6o?tt x2   H??fDx2   H??l>x2  H??^4  x2  H??XFF x 0 ' "< ( 0\? ]  AN$(2f2 ) 6o? x2 * H??f @ x2 + H??xB  x2 , H??^ 0x2 - H??L2  rB . BDo?  x2 / H??H  x2 0 H??>6   C 6? z `NH4+@(2   D 0?n dNH2-D(2    G s *?\p  Draw outer shell electrons of central atom For every positive charge on the ion, remove an electron from the outer shell... For every negative charge add an electron to the outer shell... for NH4+ remove 1 electron for NH2- add 1 electron  2+     I <"?Y EN((2j2 J Bo?@@v2 K N??tv2 L N??`xv2 M N??v2 N N??t.v2 O N??n P H)̙?%y KEXAMPLE((2B  s *޽h ? ̙33) 0L0 W)O)KX(( w dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0  6;?  ZSHAPES OF IONS0(2~F lD    "5    0H??1. RN+4(2 f2   6o?tt x2   H??fDx2   H??l>x2  H??^4  x2  H??XF F D P   MP \, T Br #  P A   6F?y> AH$(2l2  <o?Brf2  6o?F F x2  H?? "x x2  H?? t ( T Br #     6 O?y> AH$(2l2  <o?Brx2  H??  x2  H??z  T Br #  X   6XR?y> AH$(2l2  <o?Brx2  H?? R x2   H?? R T Br !# D t G  " 6Y?y> AH$(2l2 # <o?Brx2 $ H??  > x2 % H??  ~ & 0@`? A   RN+4(2 F x 0 ' "< ( 0Ld? ]  AN$(2f2 ) 6o? x2 * H??f @ x2 + H??xB  x2 , H??^ 0x2 - H??L2  rB . BDo?  x2 / H??H  x2 0 H??>6  Q F D 8 z ] 1 X_} f2 2 6o?F 0 F 0x2 3 H?? x ! 2 4 Nk?? ; z  > T Br 5#  8 k  6 6n?y> AH$(2l2 7 <o?Brx2 8 H??   x2 9 H??z  x2 : H??] Zx2 ; H?? 3 ]T Br <# D t  = 6s?y> AH$(2l2 > <o?Brx2 ? H?? Z x2 @ H??  A 0y?  AN$(2rB B BDo?s  C 6}? z `NH4+@(2   D 0$?n dNH2-D(2  Y G s *?\p  Draw outer shell electrons of central atom For every positive charge on the ion, remove an electron from the outer shell For every negative charge add an electron to the outer shell.. for NH4+ remove 1 electron for NH2- add 1 electron Pair up electrons in the usual way  202# P H̙?%y KEXAMPLE((2 Q 6L?Y EN((2d2 R <o?@@p2 S H??tp2 T H??`xp2 U H??p2 V H??t.p2 W H??nB  s *޽h ? ̙33+ 0L0 `+X+MX*( w dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0  6P?  ZSHAPES OF IONS0(2~F lD    "5    0 ?1. RN+4(2 f2   6o?tt x2   H??fDx2   H??l>x2  H??^4  x2  H??XF F D P   MP \, T Br #  P A   6в?y> AH$(2l2  <o?Brf2  6o?F F x2  H?? "x x2  H?? t ( T Br #     6P?y> AH$(2l2  <o?Brx2  H??  x2  H??z  T Br #  X   6U?y> AH$(2l2  <o?Brx2  H?? R x2   H?? R T Br !# D t G  " 6×?y> AH$(2l2 # <o?Brx2 $ H??  > x2 % H??  ~ & 0\Η? A   RN+4(2 F x 0 ' "< ( 0,З? ]  AN$(2f2 ) 6o? x2 * H??f @ x2 + H??xB  x2 , H??^ 0x2 - H??L2  rB . BDo?  x2 / H??H  x2 0 H??>6  Q F D 8 z ] 1 X_} f2 2 6o?F 0 F 0x2 3 H?? x ! 2 4 Nؗ?? ; z  > T Br 5#  8 k  6 6ܗ?y> AH$(2l2 7 <o?Brx2 8 H??   x2 9 H??z  x2 : H??] Zx2 ; H?? 3 ]T Br <# D t  = 6?y> AH$(2l2 > <o?Brx2 ? H?? Z x2 @ H??  A 0?  AN$(2rB B BDo?s  C 6? z `NH4+@(2   D 0p?n dNH2-D(2   E 6? m r >BOND PAIRS 4 LONE PAIRS 0 TETRADHEDRAL H-N-H 109.5, 2.0P2? F <4? tr 9BOND PAIRS 2 LONE PAIRS 2 ANGULAR H-N-H 104.5, 2)0P2:y G s *4 ?\p  cDraw outer shell electrons of central atom For every positive charge on the ion, remove an electron from the outer shell For every negative charge add an electron to the outer shell.. for NH4+ remove 1 electron for NH2- add 1 electron Pair up electrons in the usual way Work out shape and bond angle(s) from number of bond pairs and lone pairs.d 25L P Hl̙?%y KEXAMPLE((2 Q 6?Y EN((2d2 R <o?@@p2 S H??tp2 T H??`xp2 U H??p2 V H??t.p2 W H??nB  s *޽h ? ̙336 0L0 ~6v6c԰0 5(   & dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0  6?  ZSHAPES OF IONS0(28 l < ˰$^T  <!?9g AN$(2l2  <o?  ~2  N??x~2  N??*~2  N??l~2  N??^<~2  N??X  ' <t+?   9BOND PAIRS 3 PYRAMIDAL LONE PAIRS 1 H-N-H 107Z: 2    ` 64?Pc  >BOND PAIRS 4 TETRAHEDRAL LONE PAIRS 0 H-N-H 109.5L? 2  8 D Dx # ѰDD x # b 6T:?   AN$(2f2 c 6o?F <F <x2 d H?? x *x2 h H?? Pt N Br s  D w t 6`A?y> AH$(2l2 u <o?Brx2 v H??  x2 w H??z  N Br x   # y 6F?y> AH$(2l2 z <o?Brx2 { H??  Zx2 | H??  ZN Br } D t  ~ 68L?y> AH$(2l2  <o?Brx2  H?? f x2  H??  8 lD  ͰDT  Y 6DR? 1. RN+4(2 l2  <o? tt ~2  N?? fD~2  N?? l>~2  N?? ^4  ~2  N?? XF 8 D P  аD P T Br m#   P A  n 6Y?y> AH$(2l2 o <o?Brl2  <o? F F ~2  N??  "x ~2  N??  t ( T Br #      6_?y> AH$(2l2  <o?Br~2  N??   ~2  N?? z  T Br #   X   6`e?y> AH$(2l2  <o?Br~2  N??  R ~2  N??  R T Br #  D t G   6 k?y> AH$(2l2  <o?Br~2  N??   > ~2  N??   ~  6p?  A   RN+4(2   S <u? _   9BOND PAIRS 2 ANGULAR LONE PAIRS 2 H-N-H 104.5L: 28 x 0 ΰ `0  6|?  ]  AN$(2l2  <o?  ~2  N?? f @ ~2  N?? xB  ~2  N?? ^ 0~2  N?? L2  xB  HDo?   ~2 ° N?? H  ~2 ð N?? >6   8 D 8 z ] ϰ8 D z ]l2  <o? F 0 F 0~2  N??  x ! 2  T??  ; z  > T Br #   8 k   6?y> AH$(2l2  <o?Br~2  N??    ~2  N?? z  ~2  N?? ] Z~2  N??  3 ]T Br #  D t   67?y> AH$(2l2  <o?Br~2  N??  Z ~2  N??    6?   AN$(2xB İ HDo? s  ǰ 6? ^NH4+>(2    Ȱ 6?j   `NH2-@(2  $ Ұ 6 ? ONH30(2  Ӱ H̙?Vy JREVIEW((2B  s *޽h ? ̙33F 0L0 /Bl(  dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0  6ȸ? WMOLECULES WITH DOUBLE BONDS (2f+F 8  x   y>f2   6?p 4    6h?   AC$(2f2   6o?8  xf2  6?`  Mf2  6? \ Ef2  6? ,T sF     W  6™? AO$(2f2  6o?(Hx2  H?f?( x2  H?f?x2  H?f? y%x2  H?f? `x2  H?f?(Hx2  H?f? zG^2  6?Lc  6ș? AC$(2^2  6o?D>^2  6?D ^2  6?'^2  6?xc   6xЙ?v AO$(2^2 ! 6o? l/p2 " H?f?7 |p2 # H?f?hp2 $ H?f?p2 % H?f?tWp2 & H?f?_ |p2 ' H?f? ( 6י? v AO$(2^2 ) 6o?d /p2 * H?f?7L p2 + H?f?Pp2 , H?f?Mp2 - H?f?\Wp2 . H?f?_L p2 / H?f?F  0 0 ? d  fCarbon - needs four electrons to complete its shell Oxygen - needs two electron to complete its shell(g 2f 1 0?3 'd  q;The atoms share two electrons each to form two double bonds< 2<7 B s *8?^ The shape of a compound with a double bond is calculated in the same way. A double bond repels other bonds as if it was single e.g. carbon dioxide.(2B  s *޽h ? ̙33# 0L0 J#B#>@"(  dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0  6(? WMOLECULES WITH DOUBLE BONDS (2f+F 8  x  y>f2   6?p 4    6$?   AC$(2f2   6o?8  xf2   6?`  Mf2   6? \ Ef2  6? ,T sF     W  6 ? AO$(2f2  6o?(Hx2  H?f?( x2  H?f?x2  H?f? y%x2  H?f? `x2  H?f?(Hx2  H?f? zG^2  6?Lc  6? AC$(2^2  6o?D>^2  6?D ^2  6?'^2  6?xc  6l?v AO$(2^2  6o? l/p2   H?f?7 |p2 ! H?f?hp2 " H?f?p2 # H?f?tWp2 $ H?f?_ |p2 % H?f? & 6? v AO$(2^2 ' 6o?d /p2 ( H?f?7L p2 ) H?f?Pp2 * H?f?Mp2 + H?f?\Wp2 , H?f?_L p2 - H?f?F  . 0 ? d  fCarbon - needs four electrons to complete its shell Oxygen - needs two electron to complete its shell(g 2f / 08*?3 'd  q;The atoms share two electrons each to form two double bonds< 2< 0 6(%? _ ~  c!DOUBLE BOND PAIRS 2 LONE PAIRS 0&" 2!F }k  1  > 2 <t3o?}k  bBOND ANGLE... SHAPE...08 2______ 3 6$(?  s 180 LINEARL 0@2!F    4  o | rB 5 BDԔ?   6 64??   ?O"(2 7 6D?   ?O"(2 8 6I?/ .  ?C"(2rB 9 BDԔ?D  2 :  BwENGPITQfo? wnMw`TwnMw`TT`TnMw`TT`T@ (  ; <Lf? t  L180,(2ffrB < BDԔ?0 0 rB = BDԔ?D0 0 = > 0,S? p Y Double bonds behave exactly as single bonds for repulsion purposes so the shape will be the same as a molecule with two single bonds and no lone pairs.* 27 @ s *TX?^ The shape of a compound with a double bond is calculated in the same way. A double bond repels other bonds as if it was single e.g. carbon dioxide.(2B  s *޽h ?: ̙338 0L0 77^( 6(  dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0  6f?R JOTHER EXAMPLES (2f  <`  2 f  ZBrF5&    t  Bk?  h  BOND PAIRS 5 LONE PAIRS 1  UMBRELLA ANGLES 90 <90 b 220P2-  <y? ] @ D  9F(2  <|?  o AF$(2  <l?  =  9F(2  <To? 6   AF$(2jb  BP? t d\ jb @ Be?  !1   <(?  <P  DBr&(2vB @ NDԔ?  P1D vB  NDԔ?  S5 pB  HDԔ?    <t? T  9F(2b  S ,A lpairp"` l 7L  ! #  ; 8T {   # { ! Pf2  6?{  f2  6?{    6ȏ? 9F(2  6|? ,  AF$(2  68? T; 9F(2  6?  k AF$(2lb  <4;?q i Hlb B <?  B  6?B 9V  DBr&(2~B B N2RDԔ?/ ~B  N-q8DԔ? u) rB  BDԔ?    6?Z &  9F(28 8 1q X  C (Alpairp40n B <4 ZBrF3&    B T <?1 'J tBOND PAIRS 3 LONE PAIRS 2  T SHAPED ANGLE <90> 2*0P2: W <Է?U]< AF$(2 Y <`?/ AF$(2 \ <Կ?]&D DBr&(2xB ` HDԔ?,  a <Ĝ?2 9F(2X  C (Alpairp2NxB  HYDԔ?E%rB  BDԔ?t@ 1   88T {   r# '9 | f2 s 6?{  f2 t 6?{    6ʜ?1 ~ e AF$(2  6Ϝ?o ;  AF$(2  6 Ԝ?  m DBr&(2  6@ٜ?f 2  9F(2xB  HYDԔ?  xB  HDԔ?  xB B HDԔ? M -8T {   # ht  }f2  6?{  f2  6?{  8  ) jS G 6  C  uSO42-@     @    B  ZDjJ?w C1~B B NDjJ? P0B B TiO7DjJ?~ - B B TiO7DjJ?  ~B  NDjJ?4X\B  TDjJ?C @     ~B Q NDԔ? 5 xB  HDԔ?Pu P|   <L?  AO$(2  <œ?o C  AS$(2B  TxRDԔ? 1   <?P S PO-2(2 xb  Hu?D  rB  BDԔ?xu x| ~B  NxRDԔ?! Q   6@?   PO-2(2   6?   AO$(2xB  HDԔ?` `   <?S~ +R  AO$(2  < ? \  AS$(2  <?   ) PO-2(2 xB  HDԔ?    <?_   PO-2(2   <?   AO$(2xB  HDԔ?  xB  HDԔ?  rB  BDԔ?s= sDxB  HDԔ?    <"?1 N J =BOND PAIRS 4 LONE PAIRS 0 TETRAHEDRAL ANGLE 109.5, 2-0P2>B  s *޽h ? ̙33y___PPT10Y+D=' = @B +  0L0   Lh`i (  hjB -h BD)@0A .h 6Pp@ 0 0jB 0h@ BD)@X@ 1h 6X0@ 0 0 7h 60?/ TANSWERS ON NEXT PAGE$(2 8h 0 @ 0 0 :h 086"` JTEST QUESTIONS (2f Ch 0: +For each of the following ions/molecules, state the number of bond pairs state the number of lone pairs state the bond angle(s) state, or draw, the shape P@     Gh HC? ?u gSiCl42     Hh 0K   PCl6- L      Ih 009 F  qH2S>     Jh 0lS   wSiCl62-@      Kh 0YpW  PCl4+ N       Lh 6_I0 YBF3&    B h s *޽h ? ̙33y___PPT10Y+D=' = @B + 0L0 !( `@`@   0i"` JTEST QUESTIONS (2fdB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0X   08sy  ^3 bp 0 lp 120 trigonal planar boron pairs up all 3 electrons in its outer shell 4 bp 0 lp 109.5 tetrahedral silicon pairs up all 4 electrons in its outer shell 4 bp 0 lp 109.5 tetrahedral as ion is +, remove an electron in the outer shell then pair up 6 bp 0 lp 90 octahedral as the ion is - , add one electron to the 5 in the outer shell then pair up 6 bp 0 lp 90 octahedral as the ion is 2-, add two electrons to the outer shell then pair up 2 bp 2 lp 92 angular sulphur pairs up 2 of its 6 electrons in its outer shell - 2 lone pairs are left__^      E    S    ^    f    ^    k   <I0 YBF3&      N? ?u gSiCl42      6   PCl6- L       6D9 F  qH2S>      6   wSiCl62-@       6pW  PCl4+ N        6h̙? HANSWER&(2  0$ +For each of the following ions/molecules, state the number of bond pairs state the number of lone pairs state the bond angle(s) state, or draw, the shape P@    B  s *޽h ? ̙33  0L0 { (    0 JREVISION CHECK (2  0 ZWhat should you be able to do? (21   0| Recall the theory of Electron Pair Repulsion Understand why repulsion between electron pairs affects the shape Recall and explain the shapes and bond angles of molecules with 2,3,4,5 and 6 bond pairs Recall the relative strengths of bond pair and lone pair repulsions Recall and explain the shapes and bond angles of water and ammonia Apply the above concepts to other molecules and ions, including those with double bonds   2f*f f8ffGff=fff f0ffQff   0̝   ~,CAN YOU DO ALL OF THESE? 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