Consider the diatomic molecule Na2. For simplicity let the basis set consist of the orbitals: and . In the molecule the overlap integral between the 3s orbitals is 0.45. Answer the following questions using the orbital energies determined using the Revised Slater’s Rules found in Systematic Inorganic Chemistry.


The orbital energy of is ___________________________kJ/mole

The orbital energy of is ___________________________kJ/mole

The electronic energy of Na2 is ____________________kJ/mole.

To determine the orbital energy and electronic energy of Na2 using the Revised Slater's Rules, we need the orbital energies and the overlap integral between the 3s orbitals.

1. The orbital energy of is not provided in the question. However, we can find it using the Revised Slater's Rules. The orbital energy can be calculated by subtracting the effective nuclear charge from the ionization energy. The effective nuclear charge (Zeff) can be approximated by the screening constant (S). For sodium (Na), S is equal to 10.85. Therefore, to find the orbital energy of , we need the ionization energy of sodium. Unfortunately, it is not provided in the question. However, if you have that information, you can calculate the orbital energy using the Revised Slater's Rules.

2. Similarly, the orbital energy of is not provided in the question. You would need the ionization energy of sodium to calculate it using the Revised Slater's Rules.

3. The electronic energy of Na2 can be calculated using the molecular orbital theory and the overlap integral between the 3s orbitals. The electronic energy is given as the sum of the products of the molecular orbital coefficients and their respective orbital energies.

In this case, we have:

Electronic energy (Na2) = (coefficient of )*(orbital energy of ) + (coefficient of )*(orbital energy of )

However, the coefficients of the molecular orbitals are not provided in the question. Therefore, without this information, we cannot accurately determine the electronic energy of Na2.