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 shell.
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How does atomic radius change across a period?
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The atomic radius decreases across a period from left to right due to increased nuclear charge.
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Why does the atomic radius decrease across a period?
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Increasing nuclear charge pulls electrons closer to the nucleus, reducing the atomic radius.
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How does atomic radius change down a group?
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The atomic radius increases down a group because additional electron shells are added.
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What is ionization energy?
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Ionization energy is the amount of energy required to remove an electron from an atom in the 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 as nuclear charge increases, making it harder to remove an electron.
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Why does ionization energy increase across a period?
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Increased nuclear charge holds electrons more tightly, requiring more energy for removal.
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How does ionization energy change down a group?
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Ionization energy decreases down a group as electrons are further from the nucleus and are more easily removed.
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What is the effect of shielding on atomic radius?
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Increased electron shielding down a group reduces effective nuclear charge, increasing atomic radius.
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What is successive ionization energy?
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Successive ionization energy refers to the energy required to remove additional electrons after the first one.
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Why is the second ionization energy generally higher than the first?
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The second ionization energy is higher because it requires removing an electron from a positively charged ion, which is harder.
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How do cations and anions affect atomic radius?
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Cations decrease in atomic radius due to loss of electrons, while anions increase in radius due to gaining electrons.
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Why do transition metals have similar atomic radii?
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Transition metals have similar atomic radii due to the filling of the d-subshell, which approximates nuclear charge.
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What is the trend in ionic radius down a group?
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Ionic radius increases down a group as atoms have more electron shells.
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Why is ionization energy important in chemical reactions?
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Ionization energy indicates how readily an atom can lose an electron, influencing its reactivity and bonding.
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