Which of the following is a correct stoichiometric reaction of lead (Pb2+) with chlorine ion?
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Correct Answer: E. Pb2+ + 2Cl– → PbCl2
The correct reaction should have a net charge of zero, and must be stoichiometrically correct (no extra electrons or elements). Pb has a charge of 2+, and the chlorine ion has a charge of 1-. Although chlorine’s charge is not stated directly, it should be obvious from the periodic table that chlorine has a charge of 1-. Thus, the resulting compound must be PbCl2, with no charge, which is answer E.
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Photo attributed to Rudolf_Schuba.
