Periodic Trends: Electronegativity and Metallic Character
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What is electronegativity?
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Electronegativity is the ability of an atom to attract electrons toward itself in a chemical bond.
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What is the trend in electronegativity 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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As atoms have more positive nuclear charge but smaller radii, they exert greater pull on shared electrons.
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What is the trend in electronegativity 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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Increased distance from the nucleus and greater electron shielding reduce the pull on bonding electrons.
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How is electronegativity different from electron affinity?
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Electronegativity is an atom's ability to attract electrons in a bond, while electron affinity refers to the energy change when an atom gains an electron.
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What is metallic character?
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Metallic character refers to an element’s tendency to lose electrons and form positive ions.
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What is the trend in metallic character across a period?
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Metallic character decreases across a period from left to right.
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Why does metallic character decrease across a period?
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Due to increasing electronegativity and ionization energy, elements are less likely to lose electrons.
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What is the trend in metallic character down a group?
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Metallic character increases down a group.
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Why does metallic character increase down a group?
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As atomic radius increases, outer electrons are more easily lost, enhancing metallic properties.
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How does electronegativity correlate with metallic properties?
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Low electronegativity is associated with high metallic character as metals tend to lose electrons.
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Which element has the highest electronegativity?
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Fluorine has the highest electronegativity of all elements.
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How do trends in electronegativity and ionization energy compare?
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Both increase across a period and decrease down a group, indicating a relation in attraction to electrons.
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Why is fluorine more electronegative than chlorine?
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Despite being in the same group, fluorine's smaller atomic radius allows it to exert a stronger pull on electrons.
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