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  Factors governing ionization energy

Factors governing ionization energy:

The ionization energy depends on the factors shown below:

(A) Size of atom or ion:

The ionization energy reduces with the rising size of atom. The bigger the size of atom, lesser is the ionization energy. It is due to the fact that electrons are closely held in smaller atoms while in large atoms, electrons are held quite loose, that is, lesser energy is needed for elimination of electrons from larger atoms than the smaller one. Therefore ionization energy is smaller for bigger atoms and higher for lower atoms.

Example:

The I.E of Be (i.e., At. No.4) is bigger than that of Li (i.e., At. No.3) since the nuclear charge of Be (I.e., Z=4) is bigger than Li (i.e., Z=3). Bigger the nuclear charge, greater would be the force of attraction among nucleus and outermost electron.

Therefore, the first I.E. of Be is more than that of Li.

(b) Magnitude of nuclear charge:

The bigger the nuclear charge of protons in the nucleus, the bigger is the ionization energy. Since of the higher nuclear charge, the electrons are bound with much force and therefore higher energy will be needed for their elimination. For occasion, magnesium has high nuclear charge (i.e., 12 protons) as compared to sodium (i.e., 11 protons). Therefore ionization energy in case of magnesium is high as compared to sodium.

Likewise the I.E. of fluorine is more than that of oxygen. It can be demonstrated as follows:

F (Z = 9; 1s2 2s2 2px2 2py2 2pz1) is containing more nuclear charge than oxygen (Z = 8; 1s2 2s2 2px2 2py1 2pz1).  In both the situations the electron has to be eliminated from the similar 2p-subshell. Since fluorine contains more nuclear charge than oxygen, this means that the nucleus of fluorine will attract the outer 2p-electrons much firmly than oxygen. Therefore, first I.E. of fluorine would be greater than that of oxygen.

(c) Effect of number of electrons in the inner shells: (Screening or shielding effect):

The attractive force applied by the nucleus on the most loosely bound electron is at least partly counterbalanced by the repulsive forces applied by the electrons existed in the inner shells. The electron to be eliminated is therefore shielded from the nucleus by the electrons in inner shell. Therefore, the electron in the valence shell experiences less attraction from nucleus. Therefore the ionisation energy will be less. This is the other reason why ionization energy reduces in moving down a group.

(d) Effect of shape of orbital:

The shape of orbital too influences the ionization potential. Since s-electrons stay closer to the nucleus than p-, d-, and f-electrons of the identical valence shell, the ionization energy reduces in the order specified below:

s > p > d > f

For illustration, the first ionization energy of aluminium is lesser than that of magnesium. The electronic configuration of magnesium is [Ne] 3s2 and that of aluminium is [Ne] 3s2 3p1. Therefore, one has to eliminate 3p-electron in case of aluminium and 3s electron in the situation of magnesium. Though it is easier to eliminate the p electron as compare to the s-electron. Therefore, the first ionization energy of aluminium is lesser than that of magnesium.

(e) Effect of arrangement of electrons:

The more stable the electronic arrangement is the greater is the ionization energy. Since the noble gases have maximum stable electronic arrangements, they exhibit maximum ionization energy.

 

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