How does electronegativity generally vary in the periodic table?
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A.
It increases down a group and increases across a period.
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B.
It decreases down a group and increases across a period.
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C.
It increases down a group and decreases across a period.
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D.
It decreases down a group and decreases across a period.
Correct Answer:
B. It decreases down a group and increases across a period.
Explanation:
Electronegativity is the measure of an atom's ability to attract shared electrons within a chemical bond. This property follows specific patterns across the periodic table based on atomic structure: - Across a Period: As you move from left to right, electronegativity increases. This occurs because the number of protons in the nucleus increases, creating a stronger positive charge (effective nuclear charge) that pulls more forcefully on electrons without the addition of new electron shells.
- Down a Group: As you move from top to bottom, electronegativity decreases. This is due to the addition of electron shells, which increases the distance between the nucleus and the valence electrons. Additionally, inner electrons provide a shielding effect that further weakens the nucleus's attraction to outside electrons.Consequently, the correct observation is that electronegativity decreases down a group and increases across a period. This makes the most electronegative elements, like fluorine, reside in the top right of the table, while the least electronegative elements, like francium, are found in the bottom left.
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