PROPERTIES OF PERIODIC TABLE ELECTRON AFFINITY
It is the energy change accompanied in addition of an electron to an isolated atom. It decreases across the period then increases down the group.
ATOMIC RADII It is the half the distance of the outermost electron from the nucleus. It decreases across the period then increase down the group.
IONIZATION ENERGY It is the minimum energy required to remove an electron FROM an isolated gaseous atom. e.g the I.E of Hydrogen is 13.6ev.
FACTORS THAT AFFECT I.E
I. Screening effect of the inner electrons.
II. Size of the nuclear charge
III. Atomic radius( as the atomic radius decreases the I.E increases). I.E decreases down the group then increase across the period.
FORMS OF I.E
First, Second and Third
NB: First is less than and Second is less than Third. To be continued…..