Draw the Molecular Energy Level Diagrams of NO+, NO, and NO-, Calculate Their Bond Orders, and Determine Their Magnetism (Diamagnetic or Paramagnetic)

To understand the molecular energy level diagrams of NO⁺, NO, and NO^–, we need to consider their electronic configurations and molecular orbital theory.

Molecular Energy Level Diagrams

The molecular orbital (MO) diagram for NO can be constructed by combining the atomic orbitals of nitrogen (N) and oxygen (O). The atomic orbitals of N and O combine to form bonding and antibonding molecular orbitals. The order of these orbitals is as follows:

• σ_2s
• σ_2s*
• σ_2p
• π_2p (degenerate)
• π_2p* (degenerate)
• σ_2p*

For NO⁺, one electron is removed from the π_2p* orbital, while for NO^–, an electron is added to the π_2p* orbital.

Bond Order Calculation

The bond order (BO) is calculated using the formula:

BO = (Number of bonding electrons – Number of antibonding electrons) / 2

• NO⁺: BO = (10 – 4) / 2 = 3
• NO: BO = (10 – 5) / 2 = 2.5
• NO^–: BO = (10 – 6) / 2 = 2

Magnetism

Magnetism is determined by the presence of unpaired electrons:

• NO⁺: No unpaired electrons → Diamagnetic
• NO: One unpaired electron → Paramagnetic
• NO^–: No unpaired electrons → Diamagnetic

In summary, NO⁺ has a bond order of 3 and is diamagnetic, NO has a bond order of 2.5 and is paramagnetic, and NO^– has a bond order of 2 and is diamagnetic.