Periodic Trends: Atomic Radius and Ionization Energy

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What is the atomic radius?
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The atomic radius is the distance from the nucleus of an atom to the outermost electron cloud.
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How does atomic radius change across a period?
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Atomic radius decreases across a period from left to right.
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Why does atomic radius decrease across a period?
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Atomic radius decreases across a period due to increased nuclear charge pulling electrons closer to the nucleus.
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How does atomic radius change down a group?
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Atomic radius increases down a group.
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Why does atomic radius increase down a group?
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Atomic radius increases down a group because additional electron shells are added, which outweighs the increased nuclear charge effect.
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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 its gaseous state.
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How does ionization energy change across a period?
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Ionization energy generally increases across a period.
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Why does ionization energy increase across a period?
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Ionization energy increases across a period due to greater nuclear charge, making it harder to remove an electron.
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How does ionization energy change 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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Ionization energy decreases down a group because electrons are farther away from the nucleus, and the increased distance reduces nuclear attraction.
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What trend is observed in ionization energy for noble gases?
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Noble gases have high ionization energies because they have full valence shells, making electron removal more difficult.
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Explain the relationship between atomic radius and ionization energy.
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Generally, as atomic radius decreases, ionization energy increases due to the stronger attraction between the nucleus and electrons.
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Which element has the smallest atomic radius in the periodic table?
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Helium has the smallest atomic radius in the periodic table.
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How does shielding affect atomic radius?
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Increased shielding from inner electrons allows the outer electrons to be less attracted to the nucleus, increasing atomic radius.
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How does effective nuclear charge influence periodic trends?
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Effective nuclear charge increases across a period, reducing atomic radius and increasing ionization energy.
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