A student mixes aqueous bromine, Br2(aq)\text{Br}_2(\text{aq})Br2(aq), with aqueous potassium iodide, KI(aq)\text{KI}(\text{aq})KI(aq).
Which statement correctly predicts whether a reaction occurs and provides the correct explanation based on periodic trends?
No reaction occurs because bromide ions (Br−\text{Br}^-Br−) are stronger oxidizing agents than iodide ions (I−\text{I}^-I−) due to their smaller ionic radius and lower shielding.
A reaction occurs to form iodine (I2\text{I}_2I2), because bromine (Br2\text{Br}_2Br2) is a stronger oxidizing agent than iodine; its outer shell is closer to the nucleus with less shielding, allowing it to gain electrons more readily.
A reaction occurs to form iodine (I2\text{I}_2I2), because bromine (Br2\text{Br}_2Br2) is a stronger reducing agent than iodine; its outer shell is closer to the nucleus with less shielding, allowing it to lose electrons more readily.
No reaction occurs because iodine (I2\text{I}_2I2) is a stronger oxidizing agent than bromine (Br2\text{Br}_2Br2), as the outer shell of iodine is further from the nucleus and experiences more shielding.