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notes_162_Exp_6_Notes_010308

notes_162_Exp_6_Notes_010308 - Experiment 6 The...

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Experiment 6 The Spectrochemical Series and Crystal Field Theory The report for this experiment will be due the following week in your Quiz section.
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Goal Understand Crystal Field Theory and how it predicts the following properties of complex ions: – Color – Magnetism (paramagnetic vs. diamagnetic) – Geometry Analyze various complex ions to establish a spectrochemical series of ligands.
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Definitions Coordination compound: – A compound consisting of a transition metal ion with its attached ligands and counter ions. – Example: [Co(NH 3 ) 5 Cl]Cl 2 Transition Metal Ion Ligands: molecule or ion having a lone pair of electrons that can be donated to the metal ion to form a covalent bond Counter Ions: positive or negative ions to produce a compound with zero net charge
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Definitions Complex Ion: – The transition metal with its ligands attached – Example: [Co(NH 3 ) 5 Cl] 2+ How do we know there is a 2+ charge on the ion? – There were 2 Cl - counter ions (don’t forget that halogens always form -1 ions!) What is the charge on Co? – NH 3 is a neutral compound. The Cl ligand, however, is an anion (see above). Therefore, the ligands have a net -1 charge. This means Co must have a 3+ charge in order for the complex to have an overall charge of 2+.
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Questions We Need Answered Question 1: Is CoF 6 3- diamagnetic or paramagnetic? Question 2: Why do complex ions tend to be highly colored?
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Questions We Need Answered Question 1: Is CoF 6 3- diamagnetic or paramagnetic?
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