Electron six

Example the IE1 that Magnesium: Mg(g) -> Mg+(g) + e- I1 = 738 kJ/mol

IE1 represents the an initial ionization energy: the power the atom calls for to expel the very first electron native its orbital. Similarly, the second ionization energy, will be the power needed come expel the 2nd electron.

Mg+(g) -> Mg2+(g) + e- I2 = 1,451 kJ/mol

However, IE2 that Magnesium will be bigger than the of IE1 because it is no energetically favorable to separate an electron native a positively fee ion.

The basic pattern that the ionization power as they room in regard to the duration table is the the ie increases across a period, and also decreases under a group. Since it requires much more energy to eliminate an electron native a secure atom, the noble gases are usually linked with the greatest IE1. Because their valence shells are currently filled and stablized, castle will require much more energy to disrupt the stability. The an initial electron the is expelled is the most loosely organized to the atom.

You are watching: Relationship between ionization energy and electron affinity

On the other hand, the team 1 aspects are usually linked with the shortest IE1. Due to the fact that only one electron rectal the valence covering of this atoms, it will certainly be an ext energetically favorable for them to lose the electron in bespeak to achieve a full orbital shell.

However, over there are few exceptions. The IE1 decreases once crossing from aspect in group 15 to the element in group 16. The team 15 has actually half-filled electronic configuration ns2 np3. This kind of configuration is very stable; it’s difficult to eliminate electron native valence shell. Therefore, element in team 15 requires greater value that IE1 than group 16. One more exception is that going from be (group 2) come B (group 13), the IE1 decreases due to the fact that Be has the filled shell 2s2 i beg your pardon is an ext stable than the digital configuration the B 2s2 2p1. Hence, Be will require more IE1 than B. Similarly, the IE1 decreases once going from aspects in team 12 to group 13


Electron Affinities

Electron affinity, often abbreviated as EA, is the power released as soon as an electron is added to a valence shell of the atom.

F(g) + e- -> F-(g) EA = -328 kJ/mol

Atoms like the noble gases will certainly not gain an electron since they are currently in their many stable state through a full shell. Atoms like F will many likely gain an electron because when a cost-free electron is added to the outer shell that fluorine, it will certainly have acquired a full shell. Generally, atoms increasing across a period will rise in EA also.

See more: Long Division With Zero In The Quotient, Practice: Zeros In The Quotient (No Remainders)


Exothermic vs endothermic process

O(g) + e- -> O-(g) EA1= -141.0 kJ/mol

O-(g) + e- -> O2-(g) EA2 = +744kJ/mol

When an electron is added to one atom, the energy adjust is exothermic since of the attraction of the electron to the nucleus. However, in the instance of EA2 wherein the electron is included to an anion, the repulsion in between the anion and also this newly included electron will overwhelm the attraction the the electron to the nucleus. Therefore, this process will be endothermic, together opposed to EA1.


Periodic Trend

The basic trend the IE and also EA along a routine table.

IE and also EA.jpgrelationship between ionization energy and electron affinity