Periodic Trends: Electronegativity and Electron Affinity
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What is electronegativity?
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Electronegativity is the tendency of an atom to attract electrons towards itself in a chemical bond.
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How does electronegativity change across a period?
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Electronegativity increases across a period from left to right.
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Why does electronegativity increase across a period?
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Electronegativity increases due to greater nuclear charge, attracting bonding electrons more strongly.
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How does electronegativity change down a group?
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Electronegativity decreases down a group.
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Why does electronegativity decrease down a group?
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The decrease is due to increased distance and shielding, reducing the nucleus' pull on bonding electrons.
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Which element is the most electronegative?
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Fluorine is the most electronegative element.
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What is electron affinity?
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Electron affinity is the energy change that occurs when an electron is added to an isolated atom.
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How does electron affinity change across a period?
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Electron affinity generally becomes more negative across a period.
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Why does electron affinity become more negative across a period?
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As nuclear charge increases, atoms more readily accept an additional electron, releasing energy.
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How does electron affinity change down a group?
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Electron affinity becomes less negative down a group.
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Explain the exception in the trend of electron affinity.
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Some elements like noble gases and certain second-period elements show less predictable electron affinity due to full or half-full subshells.
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Which group in the periodic table generally has the highest electron affinity?
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The halogens (Group 17) generally have the highest electron affinity.
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What is the relationship between electronegativity and electron affinity?
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Both electronegativity and electron affinity indicate an atom's tendency to attract electrons, but electronegativity applies to bonded atoms while electron affinity applies to isolated atoms.
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Why do noble gases have low electronegativity and electron affinity?
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Noble gases have complete valence shells, making them stable and not inclined to attract additional electrons.
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How does atomic size affect electronegativity?
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Larger atomic size generally leads to lower electronegativity as the valence electrons are farther from the nucleus' pull.
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