How can you use the periodic table and electron configurations to predict relative atomic radii and ionization energies for two atoms?

Answer 1

in a periodic table

1>from left to right across a periodic table

ionization energy increases & atomic radii decreases

2>from top to bottom along a group

ionization energy decreases and atomic radii increases

when considering the Periodic Table from left to right the main energy level is the same,but the number of electrons and protons increases.so the nuclear attraction increases and thus the electrons are pulled closer towards the nucleus.this decreases the atomic radii and increases the amount of energy needed to remove the electron in the outer most shell from the strong attraction.that is the ionization energy increases and atomic radii decreases when going from left to right across the period

when going down the group in a periodic table the electronic configuration of elements increases by 1 shell.that is the number of main energy levels increases.so the nuclear attraction between the atomic nuclei and the last electron decreases due to the increase in the distance.therefore it is more easier to remove the electron in the outer most shell of an element than that of the element immediately above it.therefore the ionization energy increases down the group.and since number of energy levels increases the atomic radius increases.

Answer 2

For predicting relative atomic radii, look at the atomic number and period on the periodic table - atoms with higher atomic numbers have smaller radii. For ionization energies, atoms with higher ionization energies are further up and to the right on the periodic table due to increasing effective nuclear charge and higher electron affinity. Additionally, electron configurations can help determine the number of valence electrons and their ease of removal, affecting ionization energy.