Homonuclear diatomic molecules Bond Order=0.5* bonding e-# antibonding e) Larger bond order More stable molecule When bond order =0. it means this molecule cannot exist Example: 1st period elements 01s H H H He He He Q: EXplain(1)why H2, He2 t ions can exist?(2) What is the bond order of these ionsHomonuclear Diatomic Molecules  Bond Order = 0.5 * (# bonding e – # antibonding e)  Larger bond order ↔ More stable molecule  When bond order = 0, it means this molecule cannot exist. Example: 1st period elements  Q: Explain (1) why H2 - , He2 + ions can exist? (2) What is the bond order of these ions? 4 H H2 H He He2 He