The table below shows first ionization energies of some of the elements in the periodic table.Based on the information in the table, what can you conclude about the ability of noble gases to undergo ionization? a
Noble gases give up first electrons easily compared to elements in other groups.
b
Noble gases cannot be forced to give up electrons.
c
The willingness of a noble gas to give up electrons decreases from top to bottom within the group.
d
It is more difficult to remove electrons from a noble gas than it is to remove electrons from elements in other groups.

It is more difficult to remove electrons from a noble gas than it is to remove electrons from elements in other groups.

Explanation:

Let me restate here that in the noble gases, the outermost shell is filled. Owing to this full shell, noble gases has the outermost eight electrons required  for any specie to attain stability.

It is very difficult to remove an electron from a closed shell. This is why the first ionization energy of noble gases is usually far higher than that of elements from other groups.

Relative crystal field splitting of the ligands

Explanation:

The formation constant of a complex is the equilibrium constant that shows the stability of the complex. This equilibrium constant is found to depend on the identity of the central metal atom/ion and the identity of the ligands.

Some ligands are called strong field ligands while others are known as weak field ligands. Other ligands lie somewhere in between the two extremes in the spectrochemical series. The spectrochemical series arranges ligands in order of their relative magnitude of crystal field splitting. The greater the magnitude of crystal field splitting, the greater the formation constant or equilibrium constant of the complex.

Strong field ligands are able to participate in ligand to metal charge transfer or metal to ligand charge transfer as the case may be. Hence strong field ligands possess pi-orbitals which interact with metal pi orbitals.

The order of decreasing formation constant in the question reflects the relative positions of the ligands in the spectrochemical series. Ammonia is lower than ethylene diammine in the series which is also lower than a diene. A diene has pi orbitals capable of interaction with metal pi orbitals hence the highest crystal field splitting and equilibrium constant.