Multiple Choice
From left to right across a period for main-group elements, how does the effective nuclear charge (Z_{eff}) change?
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10. Periodic Properties of the Elements
Periodic Trend: Effective Nuclear Charge
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Which of the following periodic trends is inversely proportional to the effective nuclear charge, Z_ext{eff}?
A
Electron affinity
B
Ionization energy
C
Electronegativity
D
Atomic radius
Verified step by step guidance1
Understand the concept of effective nuclear charge (\(Z_{\text{eff}}\)), which is the net positive charge experienced by an electron in an atom. It accounts for the actual nuclear charge minus the shielding effect of inner electrons.
Recall that as \(Z_{\text{eff}}\) increases, the attraction between the nucleus and the valence electrons becomes stronger, pulling electrons closer to the nucleus.
Analyze how each periodic trend relates to \(Z_{\text{eff}}\): Ionization energy, electron affinity, and electronegativity generally increase with increasing \(Z_{\text{eff}}\) because electrons are held more tightly.
Recognize that atomic radius behaves oppositely: as \(Z_{\text{eff}}\) increases, the atomic radius decreases because electrons are drawn closer to the nucleus, making the atom smaller.
Conclude that atomic radius is inversely proportional to \(Z_{\text{eff}}\), meaning when \(Z_{\text{eff}}\) goes up, atomic radius goes down.
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