Explore the patterns in the elements as you go across the rows and down the columns in the periodic table for the various ionization energies in the tables you are given. Discuss this with your partner. You will be asked to give the patterns you found, and the rationale you used to propose the pattern(s). Use the following tables to answer questions #9 and #10. Identify any patterns in the first energy as you go down a column (a family or group) and as you go across a row (a period) in the table. Give your rationale.
Generally speaking, as you go down a group in the periodic table, there is successively greater shielding of the outer-shell electrons by the inner-shell electrons.
Generally speaking, as you go across a period in the periodic table, the effective nuclear charge (Zeff) increases because each successive element contains more protons in the nucleus than the previous element and the outer electrons are all in the same shell as you go across a period.
Generally speaking, the lighter halogens can be predicted to exhibit greater shielding of the outer-shell electrons by the inner-shell electrons than heavier halogens.
Generally speaking, non-metallic elements have greater effective nuclear charge (Zeff) than metallic elements in the same period.