\( \mathrm{Li}+\mathrm{Pb}\left(\mathrm{NO}_{3}\right) 2 \rightarrow 2 \mathrm{LiNO}_{3}+\mathrm{Pb} \) \( \begin{array}{ll}\sim & \text { 1. Oxidized, electron loss } \\ \square & \text { 2. Reduced, electron loss } \\ \square & \text { 3. Oxidized, electron gain } \\ \square & \text { 4. Reduced, electron gain } \\ \square & \text { 5. No change }\end{array} \)

Lithium (Li) is known to react with lead(II) nitrate (Pb(NO₃)₂) in a classic redox reaction. Here, lithium undergoes oxidation, meaning it loses electrons and increases its oxidation state from 0 to +1. On the other hand, lead (Pb) is reduced, which involves gaining electrons, as its oxidation state decreases from +2 to 0. This fascinating interplay of oxidation and reduction showcases the fundamental principles of redox chemistry in action! Understanding redox reactions is crucial not just in chemistry classrooms, but also in various real-world applications, from batteries powering our gadgets to processes in metallurgy. For instance, lithium-ion batteries utilize the principles of redox reactions to store and release energy efficiently. The ability of materials to either donate or accept electrons determines how well they perform in these essential technologies that keep our world buzzing!