Textbook Question
Consider the following hydrocarbon:
d. Identify all the 120° bond angles in the molecule.
12. Molecular Shapes & Valence Bond Theory
Bond Angles
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In the PCl3F2 molecule the chlorine atoms exist in the equatorial positions and the fluorine atoms exist in the axial positions. Based on this information, predict the Cl–P–Cl bond angle.
A
90°
B
180°
C
109.5°
D
120°
Verified step by step guidance1
Identify the molecular geometry of PCl3F2. The molecule has five regions of electron density around the central phosphorus atom, which corresponds to a trigonal bipyramidal geometry.
Understand the arrangement of atoms in a trigonal bipyramidal geometry. It consists of two axial positions and three equatorial positions.
Recognize that in PCl3F2, the chlorine atoms occupy the equatorial positions while the fluorine atoms occupy the axial positions.
Recall that in a trigonal bipyramidal geometry, the bond angles between equatorial positions are 120 degrees.
Conclude that the Cl–P–Cl bond angle, with both chlorine atoms in equatorial positions, is 120 degrees.
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