Redox Reaction: Detecting Blood Traces Experiment.
Give an example of a free radical discussed in this experiment
The Kastle–Meyer test is a presumptive blood test, in which the chemical indicator phenolphthalein is used to detect the possible presence of hemoglobin. The Kastle-Meyer test relies on the peroxidase-like activity of hemoglobin , which is the iron-containing portion of a red blood cell, to promote the oxidation of phenolphthalin to phenolphthalein. Phenolphthalin is colorless, but in the presence of blood and hydrogen peroxide, it changes to phenolphthalein, which makes the solution pink.
Equation given below describes how phenolphthalin (colorless) is oxidized by hydrogen peroxide and heme (which comes from the blood cells) to form phenolphthalein (pink) and water.
Equation :
heme iron Fe4+ + phenolphthalin (colorless) + H2O2 → phenolphthalein (pink) + H2O + heme iron Fe3+
The Kastle-Meyer test “is all about transfer of electrons through reduction and oxidation (called redox for short). If something gains electrons, it is reduced, if something loses electrons, it is oxidized.” Oxygen free radicals which are produced in this experiment are cleaved from peroxide group to oxidize phenolphthalin (colorless) to phenolphthalein (pink).
Step 1:
Heme has peroxidase activity as a result of which oxygen free radicals are cleaved from peroxide group.
Step 2:
Oxygen free radicals generated above react with phenolphthalin (colorless) and oxidise it to form phenolphthalein (pink).
This test is very sensitive. One drop of blood diluted in 10,000 drops of water can still be detected by the Kastle-Meyer test.
Redox Reaction: Detecting Blood Traces Experiment. Give an example of a free radical discussed in this...
Give the structures of the free-radical intermediates in the peroxide-initiated reaction of HBr with the following alkene. Include all lone-pair electrons and unpaired electrons. Hint: the radicals do not coexist in the same mechanistic step. CH2 Hint: One organic radical and one inorganic radical.
Give an example of a redox reaction. Include the balanced chemical equation.
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Give the structures of the free-radical intermediates in the peroxide-initiated reaction of HBr with the following alkene. Include all lone-pair electrons and unpaired electrons. Hint: the radicals do not coexist in the same mechanistic step.
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