Draw the Lewis structure of PF3 and Plg. Determine which statement best describes the Lewis acid or base properties of the compounds. O PF3 and Plg both have phosphorus sp hybridized with a lone pair in an sp orbital. Both can act as Lewis bases. The sp orbital with the lone pair on Plg is larger than on PF3. PF3 and Pl3 both have phosphorus sp2 hybridized with a lone pair in ap orbital. Both can act as Lewis bases. The p orbital with the lone pair on Pla is larger than on PF3. PF3 and Pl3 both have phosphorus sp2 hybridized with a lone pair in a p orbital. Both can act as Lewis bases. The p orbital with the lone pair on Pl3 is smaller than on PF3. PF3 and Pl3 both have phosphorus sp² hybridized with a lone pair in ap orbital. Both can act as Lewis acids. The p orbital with the lone pair on Pla is smaller than on PF3- O PF3 and Pl3 both have phosphorus sp hybridized with a lone pair in an sp orbital. Both can act as Lewis acids. The sp orbital with the lone pair on Pla is smaller than on PF3.
Draw the Lewis structure of PF3 and Plg. Determine which statement best describes the Lewis acid or base properties of the compounds. O PF3 and Plg both have phosphorus sp hybridized with a lone pair in an sp orbital. Both can act as Lewis bases. The sp orbital with the lone pair on Plg is larger than on PF3. PF3 and Pl3 both have phosphorus sp2 hybridized with a lone pair in ap orbital. Both can act as Lewis bases. The p orbital with the lone pair on Pla is larger than on PF3. PF3 and Pl3 both have phosphorus sp2 hybridized with a lone pair in a p orbital. Both can act as Lewis bases. The p orbital with the lone pair on Pl3 is smaller than on PF3. PF3 and Pl3 both have phosphorus sp² hybridized with a lone pair in ap orbital. Both can act as Lewis acids. The p orbital with the lone pair on Pla is smaller than on PF3- O PF3 and Pl3 both have phosphorus sp hybridized with a lone pair in an sp orbital. Both can act as Lewis acids. The sp orbital with the lone pair on Pla is smaller than on PF3.
Organic Chemistry
8th Edition
ISBN:9781305580350
Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote
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Chapter4: Acids And Bases
Section: Chapter Questions
Problem 4.35AP: The sec-butyl cation can react as both a Brnsted-Lowry acid (a proton donor) and a Lewis acid (an...
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Question
Transcribed Image Text:Draw the Lewis structure of PF3 and Plg. Determine which statement best describes
the Lewis acid or base properties of the compounds.
O PF3 and Plg both have phosphorus sp hybridized with a lone pair in an sp
orbital. Both can act as Lewis bases. The sp orbital with the lone pair on Plg is
larger than on PF3.
PF3 and Pl3 both have phosphorus sp² hybridized with a lone pair in ap orbital.
Both can act as Lewis bases. The p orbital with the lone pair on Pla is larger than
on PF3.
PF3 and Pl3 both have phosphorus sp2 hybridized with a lone pair in a p orbital.
Both can act as Lewis bases. The p orbital with the lone pair on Pl3 is smaller
than on PF3.
PF3 and Pl3 both have phosphorus sp² hybridized with a lone pair in ap orbital.
Both can act as Lewis acids. Thep orbital with the lone pair on Pla is smaller
than on PF3-
O PF3 and Pl3 both have phosphorus sp hybridized with a lone pair in an sp
orbital. Both can act as Lewis acids. The sp orbital with the lone pair on Pla is
smaller than on PF3.
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