What happens to ionic size across a period?

Question

Avery Adams · Accepted Answer

Radii of the anion (-ion) are generally greater than those of the original atom, and cation (+ion) are generally smaller than the atomic radius of the original atom. On the periodic table, the ions tend to get bigger as one moves from right to left. This pattern holds true for all the periods. For the Cations in period 2 (2nd row of the periodic table),
Boron #B^(+3)#  is smaller than Beryllium #Be^(+2)# which is smaller than Lithium #Li^(+1)# For the Anions in period 2 (2nd row of the periodic table),
Fluorine #F^(-1)#  is smaller than Oxygen #O^(-2)# which is smaller than Nitrogen #N^(-3)#. I hope this was useful to you, smartteacher.

Axel Alvarado · Answer

undefined Ionic size generally decreases across a period from left to right on the periodic table. This is due to increasing nuclear charge, which pulls the outermost electrons closer to the nucleus, resulting in a smaller ionic size.