Textbook Question
(a) An AB6 molecule has no lone pairs of electrons on the A atom. What is its molecular geometry? (c) For the AB4 molecule in part (b), predict the molecular geometry.
12. Molecular Shapes & Valence Bond Theory
Molecular Geometry
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Determine the molecular geometry for the following molecule:FSSF.
A
Tetrahedral
B
Bent
C
Trigonal Planar
D
Trigonal Pyramidal
Verified step by step guidance1
Identify the central atom in the molecule FSSF. In this case, the central atom is sulfur (S).
Determine the number of valence electrons for each atom. Fluorine (F) has 7 valence electrons, and sulfur (S) has 6 valence electrons.
Count the total number of valence electrons in the molecule. There are two sulfur atoms and two fluorine atoms, so the total is: \(2 \times 6 + 2 \times 7 = 26\) valence electrons.
Draw the Lewis structure for the molecule, ensuring that each atom satisfies the octet rule where possible. Connect the atoms with single bonds initially and distribute the remaining electrons to satisfy the octet rule.
Determine the molecular geometry using VSEPR theory. Consider the number of bonding pairs and lone pairs around the central sulfur atom to predict the shape. In this case, the presence of lone pairs on the central sulfur atom leads to a bent geometry.
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