Standard reduction potentials of the half reactions are given below array ll F ₂(g)+2 e⁻ 2 ~F ⁻(a q) ; & E^ =+2.85 ~V Cl ₂(g)+2 e⁻ 2 Cl ⁻(a q) ; & E^ =+1.36 ~V Br ₂(l)+2 e⁻ 2 Br ⁻(a q) ; & E^ =+1.06 ~V I ₂(s)+2 e⁻ 2 I ⁻(a q) ; & E^ =+0.53 ~V array The strongest oxidising and reducing agents respectively are

Step-by-step solution

Higher the value of standard reduction potential, stronger will be the oxidising agent. Therefore, F ₂ will act as strongest oxidising agent. Similarly lower the value of standard reduction potential, stronger will be the reducing agent. Therefore, I ⁻ will act as strongest reducing agent.