Textbook Question
(b) How many of the MOs from part (a) would be occupied by electrons?
12. Molecular Shapes & Valence Bond Theory
MO Theory: Homonuclear Diatomic Molecules
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Which of the following molecules is nonpolar?
A
PH3
B
SCN−
C
SF4
D
XeBr2
E
BrF5
Verified step by step guidance1
Identify the molecular geometry of each molecule. This involves determining the number of bonding pairs and lone pairs around the central atom using VSEPR theory.
For PH3, recognize that it has a trigonal pyramidal shape due to the lone pair on phosphorus, which makes it polar.
For SCN-, note that it is a linear molecule, but the difference in electronegativity between sulfur, carbon, and nitrogen can lead to a polar molecule.
For SF4, understand that it has a seesaw shape due to the lone pair on sulfur, which results in a polar molecule.
For XeBr2, determine that it has a linear shape with symmetric distribution of electron pairs, making it nonpolar despite the presence of polar bonds.
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