Complete the table below, which lists information about some diatomic molecules or molecular ions.
In particular:
- Decide whether each molecule is stable or not.
- Decide whether each molecule would be diamagnetic or paramagnetic.
- Calculate each molecule’s bond order.
The Correct Answer and Explanation is :
To analyze the stability, magnetic properties, and bond order of diatomic molecules or molecular ions, we employ Molecular Orbital (MO) theory. This theory provides a framework for understanding how atomic orbitals combine to form molecular orbitals, which dictate the bonding characteristics of a molecule.
Stability: molecule is considered stable if it has a positive bond order, meaning there are more electrons in bonding orbitals than in antibonding orbitals. bond order of zero indicates instability, as the bonding and antibonding interactions cancel each other out.
Magnetic Properties: molecule is paramagnetic if it has unpaired electrons, causing it to be attracted to a magnetic field.onversely, it is diamagnetic if all electrons are paired, resulting in a slight repulsion from a magnetic field.
Bond Order Calculation: he bond order is calculated using the formula:
[
\text{Bond Order} = \frac{(N_b – N_a)}{2}
]
here ( N_b ) is the number of electrons in bonding molecular orbitals, and ( N_a ) is the number of electrons in antibonding molecular orbitals.
Let’s apply this analysis to several diatomic species:
- Dihydrogen (H₂):
- Total Electrons: – MO Configuration: ( (σ_{1s})^2 ) – Bond Order: ( \frac{2 – 0}{2} = 1 ) – Stability: table – Magnetic Properties: iamagnetic (all electrons paired)
- Helium Dimer (He₂):
- Total Electrons: – MO Configuration: ( (σ{1s})^2(σ{1s}^*)^2 ) – Bond Order: ( \frac{2 – 2}{2} = 0 ) – Stability: ot stable (bond order of zero) – Magnetic Properties: iamagnetic (all electrons paired)
- Dioxygen (O₂):
- Total Electrons: 6 – MO Configuration: ( (σ{2s})^2(σ{2s}^)^2(σ{2p_z})^2(π{2p_x})^2(π{2p_y})^2(π{2p_x}^)^1(π_{2p_y}^*)^1 ) – Bond Order: ( \frac{10 – 6}{2} = 2 ) – Stability: table – Magnetic Properties: aramagnetic (two unpaired electrons)
- Dinitrogen (N₂):
- Total Electrons: 4 – MO Configuration: ( (σ{2s})^2(σ{2s}^*)^2(π{2p_x})^2(π{2p_y})^2(σ_{2p_z})^2 ) – Bond Order: ( \frac{10 – 4}{2} = 3 ) – Stability: table – Magnetic Properties: iamagnetic (all electrons paired)
- Fluorine Molecule (F₂):
- Total Electrons: 8 – MO Configuration: ( (σ{2s})^2(σ{2s}^)^2(σ{2p_z})^2(π{2p_x})^2(π{2p_y})^2(π{2p_x}^)^2(π_{2p_y}^*)^2 ) – Bond Order: ( \frac{10 – 8}{2} = 1 ) – Stability: table – Magnetic Properties: iamagnetic (all electrons paired)
- Nitric Oxide (NO):
- Total Electrons: 1 – MO Configuration: ( (σ{2s})^2(σ{2s}^)^2(π{2p_x})^2(π{2p_y})^2(σ{2p_z})^2(π{2p_x}^)^1 ) – Bond Order: ( \frac{8 – 3}{2} = 2.5 ) – Stability: table – Magnetic Properties: aramagnetic (one unpaired electron)
n summary, the bond order provides insight into the strength and stability of a bond: higher bond orders correspond to stronger, more stable bonds.he magnetic properties are determined by the presence or absence of unpaired electrons, with paramagnetic species having unpaired electrons and diamagnetic species having all electrons paired.