Final answer:
The CN⁻ ion has a triple bond with a bond order of 3 and is diamagnetic, meaning it has no unpaired electrons and is not attracted to magnetic fields.
Step-by-step explanation:
The bond order and magnetic characteristics of CN⁻ can be determined using molecular orbital theory. Based on the valence electron configuration, the CN⁻ ion has a total of 10 valence electrons: 4 from the carbon atom (C), 5 from the nitrogen atom (N), and 1 additional electron due to the negative charge. The bond order can be calculated as (8 - 2) ÷ 2 = 3, which means that CN⁻ has a triple bond similar to that in dinitrogen (N₂).
Magnetic characteristics depend on the presence of unpaired electrons. Since all the electrons in CN⁻ are paired, the ion is diamagnetic, which means it has no unpaired electrons and will not be attracted to magnetic fields, unlike paramagnetic species which contain unpaired electrons and are attracted to magnetic fields.