Question

Do the calculated IE values match the trend we predicted in class? Discuss how close they are to the tabulated values. Are the charges on H2, F2, and HF what you would have predicted?

Answer 1

The ionization energy (IE) values decrease down the group.

Explanation: Down the group, one more valence shell is added to the atom, as a result, the nuclear attraction of the valence electron decreases. So, the energy to remove the valence electron decreases.

The ionization energy (IE) values increase across the period.

Explanation: Across the period, one more electron is added to the same valence shell, as a result, the nuclear attraction of the valence electron increases. So, the energy to remove the valence electron increases.

2. The molecules H2, F2, and HF are neutral molecules, hence the charge on them is zero.

Note: You can cross-check whether the above concepts are obeying in the given data or no!