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Why does ionization energy decrease from top to bottom?
The ionization energy of the elements within a group generally decreases from top to bottom. This is due to electron shielding. Click to see full answer. In this manner, why does ionization energy increase from left to right across a period?
What is the trend in ionization energy from left to right?
Ionization energies are dependent upon the atomic radius. Since going from right to left on the periodic table, the atomic radius increases, and the ionization energy increases from left to right in the periods and up the groups. Exceptions to this trend is observed for alkaline earth metals (group 2) and nitrogen group elements (group 15).
What happens to ionization energy as you move across a period?
Moving left to right across a period, atomic radius decreases, so electrons are more attracted to the (closer) nucleus. The general trend is for ionization energy to decrease moving from top to bottom down a periodic table group. Moving down a group, a valence shell is added.
What factors affect the ionisation energy of an element?
The second or another factor that decreases the ionisation energy is the shielding effect as we move down a group because of an increasing number of shells. While we move from the left to right across a period, the element’s ionisation energy increases. This happens because of the decrease in the size of atoms across a period.