The standard reduction potentials for four hypothetical metals A, B, C, and D are given below: E^ _ A ²⁺/ A = +0.80 V E^ _ B ²⁺/ B = -0.76 V E^ _ C ²⁺/ C = +0.34 V E^ _ D ²⁺/ D = -2.36 V Which of the following metals acts as the strongest reducing agent?

Step-by-step solution

The strength of a reducing agent depends on its tendency to lose electrons (undergo oxidation). A lower (more negative) standard reduction potential indicates a higher tendency to get oxidized, making the metal a stronger reducing agent. Comparing the given E^ values: -2.36 V (D) Since metal D has the most negative standard reduction potential, it is the strongest reducing agent among the given options. Answer: D