How would you relate periodicity to electronic configuration?
Periodicity occurs where there are visible trends between different periods in the periodic table. There are many trends we can relate to the electronic configuration. Those elements that have fewer electrons on their outer shell tend to have lower ionisation energies (there are some exceptions, for instance, oxygen actually has a lower ionisation energy than nitrogen) . For instance, in period three Sodium (Na) has the lowest ionisation energy. In group four Potassium (K) has the lowest ionisation energy, and so on. Both of these elements have only one electron on their outer shell. Another trend that is visible is the increase and decrease of boiling point. As we go across a period from groups one to four, the boiling point will increase. After group four, the boiling point will decrease. This is true across all periods of the periodic table, and again directly relates to the electronic configuration of the elements found in the periods. Another trend is that the atomic radii of elem
Periodicity is a regular periodic variation. From the Periodic Table, across a period, there are certain trends which can be found out. As you go across a period, the number of electrons increases, filling each orbital so that it remains more closely identical to that of the noble gas on that period. Because electrons are increasing, this explains why there is a change from metallic to a nonmetallic character as you move along the period, because the number of electrons determines the chemical properties of an element.
