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Do Now – Complete the table

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1 Do Now – Complete the table
Count number of electron pairs on central atom Pairs of e- repel each other so that they are as far apart as possible Keeps repulsive forces to a minimum Gives each molecule a characteristic shape No of e- pairs around central metal ion Name of shape Bond angle(s) (°) Example 2 3 4 5 6

2 No of e- pairs around central metal ion
Shapes of Molecules Shapes of complexes can be predicted in a similar way ... Count number of electron pairs on central atom Pairs of e- repel each other so that they are as far apart as possible Keeps repulsive forces to a minimum Gives each molecule a characteristic shape No of e- pairs around central metal ion Name of shape Bond angle(s) (°) Example 2 Linear 180 BCl2 3 Trigonal planar 120 BCl3 4 Tetrahedral 109.5 CH4 5 Trigonal pyramidal 90 and 120 PF5 6 Octahedral 90 SF6

3 Cheat method ... In general for monodentate ligands ...
2 ligands = linear (most silver complexes) 4 ligands = tetrahedral (large charged ligands (Cl-) (exception: some are square planar [cis-platin] – see later) 6 ligands = octahedral (small uncharged ligands, H2O, NH3)

4 Shapes of Complex Ions Co-ordination number 2 4 6 Shape linear
tetrahedral square planar octahedral Bond angles Occurrence e.g.

5 Shapes of Complex Ions Co-ordination number 2 4 6 Shape linear
tetrahedral square planar octahedral Bond angles 180º 109½º 90º Occurrence e.g.

6 Shapes of Complex Ions Co-ordination number 2 4 6 Shape linear
tetrahedral square planar octahedral Bond angles 180º 109½º 90º Occurrence Ag+ complexes e.g. [Ag(NH3)2]+

7 Shapes of Complex Ions Co-ordination number 2 4 6 Shape linear
tetrahedral square planar octahedral Bond angles 180º 109½º 90º Occurrence Ag+ complexes Large ligands (e.g. Cl-) e.g. [Ag(NH3)2]+ [CuCl4]2-

8 Shapes of Complex Ions Co-ordination number 2 4 6 Shape linear
tetrahedral square planar octahedral Bond angles 180º 109½º 90º Occurrence Ag+ complexes Large ligands (e.g. Cl-) Pt2+ complexes e.g. [Ag(NH3)2]+ [CuCl4]2- [PtCl4]2-

9 Shapes of Complex Ions Co-ordination number 2 4 6 Shape linear
tetrahedral square planar octahedral Bond angles 180º 109½º 90º Occurrence Ag+ complexes Large ligands (e.g. Cl-) Pt2+ complexes Commonest e.g. [Ag(NH3)2]+ [CuCl4]2- [PtCl4]2- [Cu(H2O)6]2+

10 Shapes of Complex Ions

11 Octahedral Complexes Most common ligands – water, ammonia and hydroxide ion Only uses one lone pair to form a coordinate bond Six ligands – six-fold coordination Electron pair donor in each ligand is an element from Period 2 (N and O) This means the ligands are approximately equal size Name the following: [Mn(H2O)6]2+ [Fe(H2O)4(OH)2] [Al(OH)6]3- What is unusual about the final complex? Draw the shape of each complex once named

12 Tetrahedral Complexes
Less common Chloride ions act as ligands Chlorine is a Period 3 element  therefore ions are bigger than water, ammonia and hydroxide Cannot fix 6 chloride ions around the central metal ion Can fit 4 [CuCl4]2-

13 Reactive ion present in Tollen’s reagent (ammoniacal silver nitrate)
Linear Complexes Less common Reactive ion present in Tollen’s reagent (ammoniacal silver nitrate) Silver behaves differently to the other transition metals looked at Due to being in Period 5, not Period 4 [Ag(NH3)2]+

14 Shapes of Complex Ions Task 1 from booklet (p5) ...
For each of the following complexes: Draw the complex Name the shape Show bond angles Give the metal oxidation state Give the co-ordination number [Ag(CN)2]- [Cr(NH3)6]3+ [Ni(en)3]2+ [Co(en)2Cl2 ]+ [Pt(NH3)2Cl2] [Fe(C2O4)3]4- Chemsheets booklet P5 Task 1

15 Shapes of Complex Ions Linear 180º Ag +1 Co-ordination number = 2 1 2
Octahedral 90º Cr +3 Co-ordination number = 6

16 Shapes of Complex Ions Octahedral 90º Ni +2 Co-ordination number = 6 3
2+ Octahedral 90º Ni +2 Co-ordination number = 6 3 Ni 4 Octahedral 90º Co +3 Co-ordination number = 6

17 Shapes of Complex Ions Tetrahedral 90º Pt +2 Co-ordination number = 4
5 6 Octahedral 90º Fe +2 Co-ordination number = 6 4- Fe

18 Summary Questions A complex that forms between cobalt ions and nitrate ions (NO2-) has the abbreviated formula [Co(NO2)6]3+. Predict its shape and the oxidation number of the transition metal ion. A complex forms between nickel (II) ions and chloride ions. Predict its shape, name and formula.

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