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In this lesson, we will learn how to identify transition metal complexes based on their flame tests and interactions with sodium hydroxide and ammonia.
When dissolved in water, the chloride of a first-row transition metal
reacts with dilute ammonia to form a pale green solid and with concentrated ammonia to form a blue solution.
What is the identity of the element
When dissolved in water, which of the following transition metal chlorides does not react with sodium carbonate to produce a blue or green precipitate?
When a reagent
is added to a strongly basic solution of chromium(III) nitrate, a yellow solution is produced.
What color is the original solution?
Which species produces the yellow color of the final solution?
Which of the following is a possible molecular formula for the reagent
What is the oxidation state of chromium in the final yellow solution?
At pH 3, a dilute aqueous solution of iron(III) chloride is yellow in color.
Which species is mostly responsible for the color of this solution?
What change is observed if concentrated acid is added to this solution?
If added to this solution, which of the following reagents would not react to form a solid material?
As the pH of the solution increases, what happens to the geometry of the transition metal complex and the frequency of the light absorbed?
When a complex of vanadium reacts with zinc under acidic aqueous conditions, the color of the solution changes from blue to purple.
What is the structure of the original complex?
What is the oxidation state of vanadium in the final complex?
If the original vanadium complex is instead oxidized, what is the color of the resulting solution?
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