What is the total count of lone electron pairs present in a molecule of XeOF4_________?
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Answer: B. 1
Explanation
Xenon possesses eight valence electrons in its outermost shell before forming chemical bonds. Four fluorine atoms utilize four single covalent bonds while oxygen uses a double bond. Subtracting these bonding electrons leaves exactly one unshared lone electron pair on xenon. Noble gases can form stable compounds under extreme conditions despite their traditionally inert chemical reputation. VSEPR theory explains molecular geometries by accounting for repulsive forces between bonding and lone pairs. Xenon oxyfluorides are powerful fluorinating and oxidizing agents used in specialized advanced chemical research.
Understanding lone electron pairs helps chemists predict three-dimensional molecular shapes and overall dipole moments accurately. Inorganic fluorine chemistry requires rigorous safety protocols due to the extreme reactivity of heavy noble gas compounds. Advanced structural studies confirm that lone pairs exert greater electrostatic repulsion than shared bonding pairs. Zero lone pairs would imply that all eight valence electrons are fully tied up in bonding arrangements. Two lone pairs would contradict the precise electron counting required for the square pyramidal geometry. Three lone pairs would leave too few electrons to account for all five attached peripheral atoms.
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