1. Chem. 1B – 11/17 Lecture

2. Announcements I Mastering Chemistry Lab Exam 3:
Chapter 18 Assignment is due today
Lab
Completing Experiment 10; Starting Experiment 12
Exam 3:
Next Tuesday (11/24)
On Electrochemistry and Transition Metals
Electrochemistry part will be similar to exams 1 and 2, while Transition Metals part will be more focused on qualitative/conceptual understanding

3. Announcements II Today’s Lecture - Transition Elements (Ch. 24)
Coordination Compounds
Ligand types (last time)
Geometries
Naming
Isomers

4. Chapter 18 Electrochemistry Electrolytic Cells
Error in Previous lecture
Electrolysis forces reactions to occur that don’t normally occur (e.g. if Ecell <0)
For this reason, reduction reactions typically have negative standard reduction potentials and oxidation reactions typically have positive standard reduction potentials
I may have said potential closest to zero will occur (NOT TRUE)
However, the reduction reaction that occurs will have the highest reduction potential (not always negative) and the oxidation reaction will have the lowest reduction potential (reactions must be possible)

5. Chapter 18 Electrochemistry Electrolytic Cells
Example:
a solution contains M CuCl2 and M SnCl2. A potential is applied to two inert electrodes. What happens at each electrode? - +
Power Supply
Reaction
E° (V)
Cu2+(aq) + 2e- ↔ Cu(s)
0.34
Sn2+(aq) + 2e- ↔ Sn(s)
-0.14
O2(g) + 4H+(aq) + 4e- ↔ 2H2O(l)
1.23
2H2O(l) + 2e- ↔ 2H2(g) + 2OH-(aq)
-0.83 V
Cl2 (g) + 2e- ↔ 2Cl-(aq)
1.36 V

6. Chapter 24 Transition Metals
Coordination Complex - Geometries and numbers of ligands
Most Common Geometries:
Linear (with two ligands)
example: H3N-Ag-NH3
Square Planar (4 ligand bonds)
example: [PtCl4]2-
Tetrahedral (4 ligand bonds)
example: [Zn(OH)4]2- Zn HO OH

7. Chapter 24 Transition Metals
Coordination Complex - Geometries and numbers of ligands
Most Common Geometries:
Octahedral (with six ligand bonds – note octahedral refers to 8 sides, even though 6 corners)
example: [Co(H2O)6]2+ Co
H2O
OH2

8. Chapter 24 Transition Metals
Coordination Complex - Geometries and numbers of ligands – Example Questions
Cobalt(II) forms a complex with three bidentate oxalate ligands. What is the geometry?
Mercury reacts with 4 I- ligands. What geometries are possible?
1 EDTA ligand forms an octahedral complex with Ni2+. EDTA is a _____ dentate ligand

9. Chapter 24 Transition Metals
Coordination Complex - Geometries and numbers of ligands – More Questions
What is the metal oxidation state and number of ligands + ligand bonds for the following compounds:
1. Mg[HgCl4]
2. [Co(NH3)5Cl]NO3
3. Na2[Cu(ox)2] (ox = C2O42-)

10. Chapter 24 Transition Metals
Coordination Complex – Naming Compounds
Naming ligands:
Neutral ligands are given molecule names (e.g. ethylenediamine) except for:
H2O = aqua
NH3 = ammine
CO = carbonyl
Anionic ligands are changed from anion:
-ide becomes -o
-ate becomes -ato
-ite becomes -ito

11. Chapter 24 Transition Metals
Coordination Complex – Naming Compounds
Naming ligands:
List names of ligands in alphabetical order before cation name
Prefixes used to indicate number of ligands (di-, tri-, tetra-, penta-, hexa-) or bis- , tris- if ligand name already has prefix
Metal names (Depends on complex charge):
Cations (metal name same as in ionic compounds)
Anions (metal – or Latin root – ending in ate)

12. Chapter 24 Transition Metals
Coordination Complex – Naming Compounds
Naming ligands – information for exam:
Too much to expect you to know all naming rules listed
Should know all 4th row elements plus d8 to d10 5th and 6th row elements
Focus on main rules: ligands names plus 3 exceptions at top of guidelines, di- to hexa- prefixes, will give table of Latin roots (e.g. ferrate) if needed

13. Chapter 24 Transition Metals
Coordination Complex – Naming Compounds – Examples:
[Ag(NH3)2]+ =
[Pt(ox)2]2- =
[Fe(NH3)4Br2]Cl =
Tetracyanozincate =
Pentaaquabromonickel(II) =
Sodium diaquatetrachlorovanadate(III) =

14. Chapter 24 Transition Metals
Coordination Complex – Isomers
What are isomers?
Have same formula but are somehow different
Structural isomers
Have different connections between atoms
Examples:
- [Fe(NH3)5Br]Cl vs. [Fe(NH3)5Cl]Br (switch of counter ion with binding ion)
- :CΞN: ligands can bind at C (cyano) or N (isocyano) side

15. Chapter 24 Transition Metals
Coordination Complex – Isomers
Stereoisomers
Due to different neighboring ligands
Examples: [Pt(Cl)2(Br)2]2- (square planar)
Trans isomer – like ligands apart
Cis isomer – like ligands together Br Br Cl Pt Br Pt Cl Cl Br Cl
These will have slight differences in properties (cis has slight net dipole moment while trans does not)

16. Chapter 24 Transition Metals
Coordination Complex – Isomers
Stereoisomers – cont.
For tetrahedral compounds, MX2Y2 have only one isomer (X is same distance to other X and other Ys)
For octahedral compounds, MX4Y2, also has cis- trans- isomers (guess which is trans) X M X Y Y M Y X X X M Y X

17. Chapter 24 Transition Metals
Coordination Complex – Isomers
Stereoisomers – cont.
For octahedral compounds, MX3Y3, also has fac- (for face) and mer- isomers (for meridinal)
mer
fac X Y Y Y Y M Y X M X Y X X X

18. Chapter 24 Transition Metals
Coordination Complex – Isomers
Stereoisomers – cont.
The stereoisomers mentioned so are geometric isomers that will have different properties (even if only slight differences)
Another class is optical isomers, which have (mostly) identical properties; except that each isomer will rotate light differently (and can interact differently with other “chiral” molecules)
A test for an optical isomer is if its mirror image is non-superimposeable (unique)

19. Chapter 24 Transition Metals
Coordination Complex – Isomers
Optical Isomers (examples)
MX2Y2 – two or one optical isomer?
MABCD – two or one optical isomer?
Not the same – if we line up A-M-D, B and C are reversed
120 rotation about Z axis gives back original structure
mirror
mirror M Y X M B C A D M B C A D M Y X

20. Chapter 24 Transition Metals
Coordination Complex – Isomers
Questions
Which of the following ligands will have linkage isomers?
NH3 b) CN- c) H2O d) SCN-
e) C2O42-
In what way is [Cr(NH3)5Br]Cl2 different from [Cr(NH3)5Cl]BrCl?
How many different isomers are present for the square planar compound [Pt(NH3)2ClBr]?