Multiple Choice
Which of the following statements correctly describes the molecular orbital diagram for N_2?
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12. Molecular Shapes & Valence Bond Theory
Molecular Orbital Theory
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Using molecular orbital theory, determine the magnetism of O2 and O2−.
A
O2 is paramagnetic; O2− is diamagnetic.
B
O2 is diamagnetic; O2− is paramagnetic.
C
Both O2 and O2− are diamagnetic.
D
Both O2 and O2− are paramagnetic.
Verified step by step guidance1
Identify the total number of electrons in each molecule. O2 has 16 electrons (8 from each oxygen atom), and O2⁻ has 17 electrons due to the extra electron.
Construct the molecular orbital (MO) diagram for O2. The order of orbitals for O2 is: σ(1s), σ*(1s), σ(2s), σ*(2s), σ(2p_z), π(2p_x) = π(2p_y), π*(2p_x) = π*(2p_y), σ*(2p_z).
Fill the molecular orbitals with the electrons for O2. Place 16 electrons in the MO diagram, following the Aufbau principle, Pauli exclusion principle, and Hund's rule.
Determine the magnetism of O2 by checking for unpaired electrons in the MO diagram. O2 has two unpaired electrons in the π*(2p_x) and π*(2p_y) orbitals, making it paramagnetic.
For O2⁻, add one more electron to the MO diagram of O2. This extra electron will pair with one of the unpaired electrons in the π*(2p_x) or π*(2p_y) orbitals, but one unpaired electron remains, making O2⁻ also paramagnetic.
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