Open Question
In which of the following AFn molecules or ions is there more than one F-A-F bond angle: PF6⁻, SbF5, SF4?
Ch.9 - Molecular Geometry and Bonding Theories
Chapter 9, Problem 34
Name the proper three-dimensional molecular shapes for each of the following molecules or ions, showing lone pairs as needed: (a) ClO2- (b) SO4 2- (c) NF3 (d) CCl2Br2 (e) SF4 2+
Verified step by step guidance1
Step 1: Determine the total number of valence electrons for each molecule or ion. For example, for ClO2-, count the valence electrons from Cl and O, and add one more for the negative charge.
Step 2: Draw the Lewis structure for each molecule or ion. Arrange the atoms to satisfy the octet rule, and place any extra electrons as lone pairs on the central atom.
Step 3: Use the VSEPR (Valence Shell Electron Pair Repulsion) theory to determine the electron pair geometry around the central atom. Consider both bonding pairs and lone pairs of electrons.
Step 4: Identify the molecular geometry by considering only the positions of the atoms (ignoring lone pairs). For example, if there are four electron pairs and one is a lone pair, the molecular shape is trigonal pyramidal.
Step 5: Name the molecular shape for each molecule or ion based on the arrangement of atoms. For example, a molecule with four bonding pairs and no lone pairs is tetrahedral.
Related Practice
Textbook Question
(a) Explain why BrF4- is square planar, whereas BF4- is tetrahedral.
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Textbook Question
(b) How would you expect the H¬X¬H bond angle to vary in the series H2O, H2S, H2Se? Explain. (Hint: The size of an electron pair domain depends in part on the electronegativity of the central atom.)
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Open Question
What is the distinction between a bond dipole and a molecular dipole moment?
Open Question
Consider a molecule with the formula AX2. Supposing the A-X bond is polar, how would you expect the dipole moment of the AX2 molecule to change as the X-A-X bond angle decreases from 180° to 100°?
Textbook Question
(a) Does CS2 have a dipole moment? If so, in which direction does the net dipole point?
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