2. The ionization energy of Mg is 7.6 eV and Cl is 13.0 eV. 1) Construct an MO diagram for MgCl+. 2)Predict the bond order. 3) Using your diagram explain the property of the bond (i.e. polar or non -polar, co-valent or ionic)

1. Constructing an MO diagram for MgCl+:

The MO diagram for MgCl+ would be constructed based on the atomic orbitals of the individual atoms.

• Magnesium (Mg) has the electron configuration [Ne] 3s2. In its ionized state (Mg+), it loses one electron and thus has the configuration [Ne] 3s1.
• Chlorine (Cl) has the electron configuration [Ne] 3s2 3p5.

In the MO diagram, the 3s orbitals of Mg and Cl would overlap to form bonding (σ) and antibonding (σ*) molecular orbitals. The 3p orbitals of Cl would remain non-bonding as they do not have corresponding orbitals in Mg to form bonds with.

2. Predicting the bond order:

The bond order can be calculated using the formula: Bond Order = 0.5 * (Number of electrons in bonding orbitals - Number of electrons in antibonding orbitals)

In this case, there are 2 electrons in the bonding orbital (one from Mg and one from Cl) and none in the antibonding orbital. So, the bond order would be 0.5 * (2 - 0) = 1. This indicates a single bond between Mg and Cl in MgCl+.

3. Explaining the property of the bond:

The bond in MgCl+ is likely to be polar covalent. This is because there is a significant difference in electronegativity between Mg and Cl, which leads to an uneven distribution of electron density and thus a polar bond. However, the bond is not completely ionic despite the difference in electronegativity because there is some sharing of electrons (as indicated by the presence of a bonding molecular orbital in the MO diagram). Therefore, the bond has characteristics of both covalent (electron sharing) and ionic (electron transfer) bonds, but is best described as polar covalent.