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Explore TopicChoose the Best Answer
A
Fluorine will attract the shared electrons more strongly than Phosphorus, leading to a polar covalent bond.
B
Phosphorus will attract the shared electrons more strongly than Fluorine, resulting in a non-polar covalent bond.
C
Both elements will share electrons equally, resulting in an ionic bond.
D
The bond will be purely metallic, as Fluorine does not have a significant electronegativity.
Understanding the Answer
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Answer
Fluorine’s electronegativity (about 4. 0) is much higher than phosphorus’s (around 2. 1), so when they bond the electron pair is pulled strongly toward fluorine, giving a highly polar covalent bond with a partial negative charge on F and a partial positive charge on P. The large electronegativity difference (≈1. 9) is close to the threshold for ionic character, so the bond can display significant ionic traits, especially in a solid or ionic complex.
Detailed Explanation
Fluorine is much more electronegative than phosphorus, so it pulls the shared electrons closer to itself. Other options are incorrect because The idea that phosphorus can attract the electrons more is wrong because phosphorus has a lower electronegativity than fluorine; Sharing electrons equally does not create an ionic bond; ionic bonds form when electrons are almost completely transferred from one atom to another.
Key Concepts
Electronegativity
Chemical Bonding
Periodic Trends
Topic
Electronegativity
Difficulty
medium level question
Cognitive Level
understand
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