Periodic Trends: Atomic Radius and Ionization Energy

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What is the trend in atomic radius across a period in the periodic table?
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Atomic radius decreases across a period from left to right due to increasing nuclear charge.
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Why does atomic radius decrease across a period?
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As you move across a period, protons are added to the nucleus, increasing nuclear charge, which pulls electrons closer, decreasing atomic radius.
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What is the trend in atomic radius down a group in the periodic table?
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Atomic radius increases down a group due to the addition of electron shells.
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Why does atomic radius increase down a group?
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As you move down a group, additional electron shells are added, increasing the distance between the outer electrons and the nucleus.
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What is ionization energy?
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Ionization energy is the energy required to remove an electron from an atom in the gaseous state.
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What is the trend in ionization energy across a period?
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Ionization energy increases across a period from left to right.
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Why does ionization energy increase across a period?
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This is due to increasing nuclear charge, which holds electrons more tightly, requiring more energy to remove an electron.
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What is the trend in ionization energy down a group?
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Ionization energy decreases down a group.
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Why does ionization energy decrease down a group?
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Despite the increasing nuclear charge, the added electron shells reduce the effective nuclear attraction, making electrons easier to remove.
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How do atomic radius and ionization energy compare across a period?
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As atomic radius decreases, ionization energy increases across a period.
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How does a greater atomic radius affect ionization energy?
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A greater atomic radius often leads to lower ionization energy because outer electrons are further from the nucleus.
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What is electron shielding?
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Electron shielding is the phenomenon where inner electrons block attraction between the nucleus and outer electrons.
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How does electron shielding affect periodic trends?
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It causes the effective nuclear charge felt by outer electrons to decrease, influencing trends such as atomic radius and ionization energy.
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What is effective nuclear charge?
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Effective nuclear charge is the net positive charge experienced by an electron in an atom, influenced by shielding.
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How is effective nuclear charge related to periodic trends?
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Higher effective nuclear charge leads to a decrease in atomic radius and an increase in ionization energy across a period.
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