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Chapter 17: Problem 17

Is the reaction below a redox reaction? Explain your answer. $$\mathrm{Ca}(s)+\mathrm{Cl}_{2}(g) \rightarrow \mathrm{CaCl}_{2}(s)$$

Short Answer

Expert verified
Yes, the reaction given \(Ca(s) + Cl_{2}(g) \rightarrow CaCl_{2}(s)\) is a redox reaction because it involves oxidation (loss of electrons) and reduction (gain of electrons). Calcium is oxidized and chlorine is reduced.

Step by step solution

01

Identification of elements in the reaction

First, identify the different elements involved in the reaction. The reaction provided includes calcium (Ca), chlorine (Cl), and the compound calcium chloride (CaCl2).
02

Determine the oxidation state of each element in the reaction

Second, determine the oxidation state of each element in the reaction. The oxidation state of pure elements or in their natural state is always zero. Hence, for Ca and Cl2 - it is zero. In the compound CaCl2, calcium has an oxidation state of +2 and chlorine has an oxidation state of -1.
03

Evaluate Change in Oxidation State

Finally, compare the initial and final oxidation states of each element. Calcium (from 0 to +2) has lost electrons, indicating that it has been oxidized. Chlorine (from 0 to -1) has gained electrons, indicating that it has been reduced.

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