Given below are two statements : Statement (I) : The correct sequence of bond lengths in the following species is : O₂^+ Statement (II) : The correct sequence of number of unpaired electrons in the following species is : O₂ > O₂^+ > O₂^- > O₂²⁻ In the light of the above statements, choose the correct answer from the options given below :

Step-by-step solution

The bond order of the given oxygen species can be calculated using molecular orbital theory: For O₂ (16 electrons), the configuration is _ 1s ^2 ^ * _ 1s ^2 _ 2s ^2 ^ * _ 2s ^2 _ 2p_z ^2 _ 2p_x ^2 = _ 2p_y ^2 ^ * _ 2p_x ^1 = ^ * _ 2p_y ^1 . Bond order = 10 - 6 2 = 2 . Number of unpaired electrons = 2 . For O₂^+ (15 electrons), one electron is removed from a ^ * orbital. Bond order = 10 - 5 2 = 2.5 . Number of unpaired electrons = 1 . For O₂^- (17 electrons), one electron is added to a ^ * orbital. Bond order = 10 -