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Why Fluorine Can't Form FH? or FCl?: Unpacking VSEPR Theory & Electron
Chapter 6, Problem 6.46(choose chapter or problem)
Because fluorine has seven valence electrons \(\left(2 s^{2} 2 p^{5}\right)\), in principle, seven covalent bonds could form around the atom as in \(\rm{FH}_7\) or \(\rm{FCl}_7\). Explain why these compounds have never been prepared.
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QUESTION:
Because fluorine has seven valence electrons \(\left(2 s^{2} 2 p^{5}\right)\), in principle, seven covalent bonds could form around the atom as in \(\rm{FH}_7\) or \(\rm{FCl}_7\). Explain why these compounds have never been prepared.
ANSWER:Step 1 of 3
Geometric Constraints. One of the primary reasons compounds like \(\mathrm{FH}_{7}\) or \(\mathrm{FCl}_{7}\) cannot be formed is due to geometric limitations. Fluorine has seven valence electrons, but it becomes geometrically impossible to fit seven other atoms closely enough to form stable covalent bonds. The Valence Shell Electron Pair Repulsion (VSEPR) theory shows that electron pairs around fluorine will strongly repel each other, making it difficult to bring other atoms close enough for stable bonding.
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Why Fluorine Can't Form FH? or FCl?: Unpacking VSEPR Theory & Electron
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Explore why fluorine, with its seven valence electrons, doesn't form compounds like FH? or FCl?. Understand the role of VSEPR theory, atomic size, and electronegativity in limiting bond formation. Grasp the interplay of geometric challenges and electron repulsion in compound stability.