Determine the shape of each of the following species. (a) P O 4 3 , (b) PCl
Question:
Determine the shape of each of the following species.
(a) P O 4 3–,
(b) PCl5
Strategy Draw the Lewis structures. Each of these molecules has only single bonds around its central atom. So we can count the number of bonding pairs around the central atom and assign the geometry by consulting Table 7.3 as needed.
Table 7.3
Transcribed Image Text:
Each of the geometrical arrangements shown in the table minimizes the electron pair repulsions for the indicated number of electron pairs. To visualize the shapes of molecules, it is essential that you have a sound mental picture of each of these geometries. Number of Electron Pairs 2 3 5 6 Geometric Name Linear Trigonal planar Tetrahedral Bond Angles Octahedral 180° 120° 109.5⁰ Trigonal bipyramidal 120°, 90° 90⁰, 180° Diagram 180° 90° 2: Linear 3: Trigonal planar 120⁰ 4: Tetrahedral 90% 109.5° 5: Trigonal bipyramidal 6: Octahedral -120° -90°
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a The Lewis structure of P O 4 3 which we drew in Example Problem 75 is The central phosphorus atom has a complete octet of electrons contributed by f...View the full answer
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Related Book For
Chemistry For Engineering Students
ISBN: 9780357026991
4th Edition
Authors: Lawrence S. Brown, Tom Holme
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