Notes
Observation 4: Heat Change Associated with a reaction
Many chemical reactions occur with large amounts of heat being consumed or
produced. We can sense these changes by determining if the temperatures of the
materials change when they are mixed together. Simply holding a beaker in your
hands will allow for the detection of these changes.
Oxidation-Reduction Reactions: Movement of
electrons
Oxidation-reduction reactions involve the transfer of electrons from one atom to
a different atom. Many types of chemical reactions are oxidation-reduction
reactions; combination reactions, many decomposition reactions, combustion
reactions, and single-displacement reactions are all classified as oxidation-
reduction reactions. The key feature to identify is the changing oxidation
numbers of different atoms when these reactions occur. When transition metals
are involved, we will typically see color changes occurring when the transition
metal undergoes a change in oxidation state.
Red-Ox Reaction 1: Oxidation States of Manganese
Here we will look at the reaction of potassium permanganate (KMnO4) with
iron(II) chloride (FeCl2) under acidic conditions.
In a medium test-tube, mix about 3 mL of the potassium permanganate solution
with 2 mL of HCl solution and 1 mL of iron(II) chloride solution. Record your
observations. Manganese compounds in aqueous solutions tend to have different
colors based on the oxidation state of the manganese. When manganese is in the
+2 oxidation state, aqueous solutions are a pale pink color. When manganese is
in the +4 oxidation state, it tends to form insoluble brown compounds. When
manganese is in the +7 oxidation state, aqueous solutions have a rich purple
color.
Oxidation-reduction reactions involve the transfer of electrons. Is
manganese losing or gaining electrons in this process? Some other atom
in the reaction must have the opposite behavior with its oxidation state.
What other atom do you think is changing its oxidation state? Is it being
oxidized or reduced?
Write the reduction half-reaction, oxidation half-reaction, and the
balanced Red-Ox reaction for this process.
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