Greater the atomic size of the atom, smaller the ionization energy value and vice versa. The ionization energy of an atom depends upon the following factors. Factors affecting the ionization energy values. Addition of another electron does not result in a fractional decrease in the electrostatic attraction to any given electron, but it does increase the electron-electron repulsion, so an overall decrease in Net attractive force. Atomic radii decrease in a period from left to the right in the periodic table. The internal energy levels “shield” and reduce electrostatic attraction of the valence electrons to the protons.
(2) Number of energy levels: The greater the number of energy levels, the larger the atomic radii. (1) Nuclear charge (number of protons) : The stronger the ‘pull’ the protons have to the electrons with electrostatic attraction, then the smaller the size of the atom radii Because positive charge binds electrons more strongly, the second ionization energy of an element is always higher than the first. The same trend of atomic radius applies once you divide the table into metal and. An elements second ionization energy is the energy required to remove the outermost, or least bound, electron from a 1+ ion of the element. In basic chemistry, we may see several patterns in the characteristics (physical and chemical) of elements as we move down a group. Atomic Radii is affected by two main factors : A higher effective nuclear charge causes greater attractions to the. In other words, size of the iso-electronic ions decreases with the increase in the magnitude of nuclear charge.
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