Study guide
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Instructional
Offering:
Code:
Lecturer:
Prescribed
Textbook:
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Inorganic Chemistry III
Module 3
Practical Coordination
Chemistry
CHI32P1
Dr
N Vorster
None |
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Recommended
reading:
G.Pass and H. Sutcliffe,
"Practical Inorganic Chemistry", 2nd Ed. |
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Practical Coordination Chemistry
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The goal of this practical module is to provide you with
practical applications of the bonding theories developed during the theory
modules, and to provide you with the ability to correlate the observed data with
theoretical predictions and interpret experimental observations in terms
of chemical bonding theories.
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To assist you in the
interpretation of the practical module |
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To break down the practical
module into smaller units |
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To highlight essential
learning material |
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To enable you to evaluate
your own progress |
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3. GENERAL INFORMATION AND REGULATIONS
The practical module is divided into nine experiments
performed during approximately fourteen practical sessions.
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You are required to attend all the practical sessions and
must sign a log book at the beginning of each practical session. You may not
miss more than two practicals for medical or other reasons, otherwise
you will not obtain a class mark for the module. Any absence from a practical
session must be validated by a medical certificate or letter explaining the
reason for absence.
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You will write two (2) major class tests, each of 1 hour
duration, to evaluate your understanding of the practical course content. In
addition to these tests, you may write a number of short practical tests just
before a practical session. Dates for the class tests and minor practical
tests will be announced during the lectures.
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You must hand in a practical report one week after completion of each
experiment. The class mark will be determined as a weighted average of the
marks obtained for each practical report as well as the minitests and class
tests. See calculation of
class marks. Note that in order to obtain examination entrance, you must
achieve a minimum of 50% for your class mark. See exam
admission requirements. Also note the rules and regulations regarding
writing and missing class tests in the Department’s Rules and Regulations
Brochure.
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The final examination for this module will consist of one
one and a half (11/2) hour written examination based on the theory of the
practicals done during the semester.
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3.6.1 Modules
You will obtain a pass for a module if the combined class
and examination mark is 50%, or more, provided that a subminimum of 40% has
been obtained in the final examination. The combined mark for each module is
computed as follows:
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Class mark :
Exam mark :
Final mark : |
60%
40%
100% |
3.6.2 Course
The final course mark for Inorganic Chemistry III is
calculated as a weighted average of the marks obtained for the individual
modules, "Introduction to Coordination Chemistry", "Descriptive
Chemistry of the Transition Elements" and "Practical Coordination
Chemistry". Should you fail one of the modules, you retain your
pass mark for other modules passed. You will pass the course Inorganic
Chemistry III only if a final mark of at least 50% is obtained for each
module. See Calculating the
final mark.
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4. PRACTICAL COORDINATION CHEMISTRY
14 × 3 hrs = 42 hrs
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Exp1: Ir Spectroscopy and Nickel(II) Hexammines
Exp 2: Aqueous Chemistry of the 3d Transition Metals
Exp 3: Complex Ions Formed by Some Transition Metal Ions
Exp 4: Oxidation State Determinations for Some Reduction Products
of Vanadium(V)
Exp 5: The Chemistry of Manganese(III)
Exp 6: Determination of )0
for the Ion Ti(H2O)63+
Exp 7: Influence of Ligand Field Strength on The Spectra of Cu(II)
Complexes
Exp 8: Complex Ion Composition by Job’s Method
Exp 9: A Comparative Study of Co2+ And Ni2+
Complexes
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After completion of this unit you should be able to:
P be familiar with the principle of
infrared spectrophotometry;
P interpret IR spectra;
P know which factors affect the
vibration of a ligand upon coordination to a metal species;
P know the typical aqueous chemistry
of individual transition metal ions;
P know which metal hydroxides are
amphoteric or basic;
P interpret UV/visible spectra;
P know which transition metal ions
form ammine complexes;
P be familiar with the chloride
complexes of cobalt(II) ;
P be familiar with the basic acetate
complex of chromium(III);
P be familiar with the typical
chemistry of iron(III);
P know the formulas and colours of
the complexes of vanadium in its typical oxidation states;
P calculate the oxidation state
changes for three oxidation reactions of vanadium;
P determine the stoichiometry of the
reaction of manganese(II) with potassium permanganate;
P perform a spectroscopic titration
by the mole ratio method;
P prepare some complexes of
manganese(III);
P calculate )o
for Ti(H2O)63+ from a UV/vis spectrum scan;
P correlate the position, width and
intensity of a spectral band with certain properties of a metal complex;
P determine the influence of ligand-field
strength on the spectra of metal complexes;
P calculate the value of n in the
reaction M + nL ºMLn using Job’s
method;
P prepare some octahedral and
tetrahedral pyridine complexes of cobalt(II) and nickel(II) and determine the
percentage purity;
P determine, spectrophotometrically,
the stability constant for the tetrahedral/octahedral equilibrium of cobalt(II).
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