Using the molecular orbital energy ordering for second-row homonuclear diatomic molecules in which the π_2p orbitals lie at higher energy than the σ_2p, draw MO energy diagrams and predict the bond order in a molecule or ion with each number of total valence electrons. Will the molecule or ion be diamagnetic or paramagnetic? c. 13

Verified step by step guidance

1. Identify the second-row homonuclear diatomic molecule or ion with 13 valence electrons. This could be a molecule like \( \text{N}_2^+ \).
2. Draw the molecular orbital (MO) energy diagram for second-row homonuclear diatomic molecules, noting that the \( \pi_{2p} \) orbitals are higher in energy than the \( \sigma_{2p} \) orbital.
3. Fill the MO diagram with 13 electrons, starting from the lowest energy orbital and following Hund's rule and the Pauli exclusion principle.
4. Calculate the bond order using the formula: \( \text{Bond Order} = \frac{1}{2} (\text{Number of bonding electrons} - \text{Number of antibonding electrons}) \).
5. Determine if the molecule or ion is diamagnetic or paramagnetic by checking if all electrons are paired (diamagnetic) or if there are unpaired electrons (paramagnetic).

Key Concepts

Molecular Orbital Theory

Molecular Orbital Theory describes how atomic orbitals combine to form molecular orbitals, which can be occupied by electrons. In this theory, electrons are delocalized over the entire molecule rather than being confined to individual atoms. The energy levels of these molecular orbitals are determined by the energies of the atomic orbitals involved and their interactions, leading to bonding and antibonding orbitals.

Bond Order

Bond order is a measure of the number of chemical bonds between a pair of atoms, calculated as the difference between the number of bonding and antibonding electrons divided by two. A higher bond order indicates a stronger bond and greater stability of the molecule. For example, a bond order of 1 corresponds to a single bond, while a bond order of 2 corresponds to a double bond.

Magnetism in Molecules

The magnetic properties of a molecule, whether it is diamagnetic or paramagnetic, depend on the presence of unpaired electrons in its molecular orbitals. Diamagnetic molecules have all electrons paired and are not attracted to a magnetic field, while paramagnetic molecules contain unpaired electrons and are attracted to magnetic fields. This property can be predicted by analyzing the electron configuration derived from the molecular orbital diagram.