Indicate whether the following balanced equations involve oxidation–reduction. If they do, identify the elements that undergo changes in oxidation number. (a) 2 AgNO₃(aq) + CoCl₂(aq) → 2 AgCl(s) + Co(NO₃)₂(aq)

Verified step by step guidance

1. Determine the oxidation states of each element in the reactants and products.
2. For AgNO_3, Ag is +1, N is +5, and O is -2.
3. For CoCl_2, Co is +2, and Cl is -1.
4. For AgCl, Ag is +1, and Cl is -1.
5. For Co(NO_3)_2, Co is +2, N is +5, and O is -2.

Key Concepts

Oxidation-Reduction Reactions

Oxidation-reduction (redox) reactions involve the transfer of electrons between substances, leading to changes in oxidation states. In these reactions, oxidation refers to the loss of electrons (increase in oxidation state), while reduction refers to the gain of electrons (decrease in oxidation state). Identifying whether a reaction is a redox process requires analyzing the oxidation states of the elements involved before and after the reaction.

Oxidation States

Oxidation states (or oxidation numbers) are assigned to atoms in a compound to indicate their degree of oxidation or reduction. The rules for determining oxidation states include that the oxidation state of an element in its elemental form is zero, and for monoatomic ions, it equals the charge of the ion. Understanding how to assign oxidation states is crucial for identifying which elements are oxidized or reduced in a chemical reaction.

Balancing Chemical Equations

Balancing chemical equations ensures that the number of atoms for each element is the same on both sides of the equation, reflecting the law of conservation of mass. In redox reactions, balancing also involves ensuring that the total charge is the same on both sides. This process may require adjusting coefficients and can help in identifying the changes in oxidation states of the elements involved.