Question

question 2 (2 points)
effective nuclear charge _______________________.
has no effect on atomic radius
decreases as you move from left to right on the periodic table
increases as you move from left to right on the periodic table
increases as you move from right to left on the periodic table

Explanation:

Effective nuclear charge \(Z_{eff}\) is calculated as \(Z_{eff}=Z - S\) (where \(Z\) is the atomic number and \(S\) is the shielding constant). As we move from left to right across a period in the periodic table, the number of protons (\(Z\)) increases while the shielding (\(S\)) remains relatively constant (since electrons are added to the same principal energy level). So, \(Z_{eff}\) increases. Atomic radius is inversely related to \(Z_{eff}\) (higher \(Z_{eff}\) pulls electrons closer, decreasing atomic radius).

Answer:

C. increases as you move from left to right on the periodic table