Exam 6 Ch 21-23 CHEMISTRY 1B 100 Points
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1. Supply the correct name or formula for each compound below and determine the number of moles of
ions per mole of compound in aqueous solution for b and d. (10)
a. [Fe (en)2 I2]2CO3
b. triammine triaqua cobalt(III) sulfate
c. K4[Ni Br2 Cl2 I2]
d. aluminum tetrabromo platinate(II)
2. Draw all the isomers for each of the following and identify each isomer. (10)
a. [Cr(NH3)3Br3]
b. [Pd I2 (NH3)2]
c. [Pt I2 (H2O)2 F2]
3. Construct complete valence bond (molecular orbital) and crystal field diagrams for each ion. Include:
geometry, "d" configuration, hybridization, magnetic properties, spin states, and labels as appropriate.(36)
a. [CoCl4]-2
b. [Fe I6]-3
c. [Pt(CO)4]+2
d. [Os(CN)6]-4
4. Explain and predict the order of ligand strength for: (9)
(CH3)2NH, Br-, CN-, and F-.
If one octahedral metal ion complex has a yellow color and one a green color, and if these represent the
extremes for this series, which ligand is associated with the yellow complex and which ligand is
associated with the green complex? Explain your answer.
5. Write the balanced equations for the half-reaction occurring at the anode and at the cathode for the
electrolysis of molten AlH3. Also write the balanced net-ionic equation for the process. (9)
6. Write balanced equations, including physical states, for the following laboratory procedure for the
behavior of barium metal when burned in air.
When burned in air, barium metal produces a mixture of two solids, both binary compounds. The mixture
is treated with water and heated. A strong smell of ammonia is noted. The result is a single pure product
which was one of the original products. There are four equations. (8)
7. Write the balanced equations for the reaction of aluminum solid with selenium solid, hydrogen gas, and
chlorine gas. (9)
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