Ch.9 - Molecular Geometry and Bonding Theories

Brown - Chemistry: The Central Science 14th Edition

Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook

Brown 14th Edition

Ch.9 - Molecular Geometry and Bonding Theories

Problem 87c

Chapter 9, Problem 87c

Consider the following XF4 ions: PF4-, BrF4-, ClF4+, and AlF4-. (c) Which of the ions will have an octahedral electron-domain geometry?

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Identify the central atom in each ion: P in PF4-, Br in BrF4-, Cl in ClF4+, and Al in AlF4-.

Determine the number of valence electrons for each central atom and add or subtract electrons based on the ion's charge.

Add one electron for each fluorine atom bonded to the central atom, as each F forms a single bond.

Calculate the total number of electron domains (regions of electron density) around the central atom, including both bonding pairs and lone pairs.

Identify the electron-domain geometry based on the total number of electron domains: 6 domains correspond to an octahedral geometry.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Electron-Domain Geometry

Electron-domain geometry refers to the spatial arrangement of electron pairs around a central atom, which can include bonding pairs and lone pairs. The VSEPR (Valence Shell Electron Pair Repulsion) theory is used to predict this geometry, where electron pairs repel each other and adopt an arrangement that minimizes repulsion. Common geometries include linear, trigonal planar, tetrahedral, and octahedral.

Octahedral Geometry

An octahedral geometry occurs when a central atom is surrounded by six electron domains, resulting in a symmetrical arrangement of atoms or groups at the corners of an octahedron. This geometry typically arises in molecules with six bonding pairs and no lone pairs, or in cases where lone pairs are present but do not alter the overall shape significantly.

Formal Charge and Stability

Formal charge is a theoretical charge assigned to an atom in a molecule, calculated based on the number of valence electrons, the number of non-bonding electrons, and half the number of bonding electrons. Understanding formal charge helps predict the most stable structure of a molecule, as lower formal charges on atoms generally indicate greater stability. This concept is crucial when determining the most likely electron-domain geometry for ions.

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Formal Charge

Related Practice

Textbook Question

Consider the following XF₄ ions: PF₄^-, BrF₄^-, ClF₄⁺, and AlF₄^-. (a) Which of the ions have more than an octet of electrons around the central atom?

Textbook Question

Consider the molecule PF4Cl. (c) Predict the molecular geometry of PF₄Cl. How did your answer for part (b) influence your answer here in part (c)?

Textbook Question

Consider the molecule PF₄Cl. (d) Would you expect the molecule to distort from its ideal electron-domain geometry? If so, how would it distort?

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Textbook Question

An AB2 molecule is described as having a tetrahedral geometry. (b) Based on the information given, which of the following is the molecular geometry of the molecule: (i) linear, (ii) bent, (iii) trigonal planar, or (iv) tetrahedral?

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Textbook Question

Consider the molecule PF₄Cl. (a) Draw a Lewis structure for the molecule, and predict its electron-domain geometry.

Textbook Question

Consider the following XF₄ ions: PF₄^-, BrF₄^-, ClF₄⁺, and AlF₄^-. (b) For which of the ions will the electron-domain and molecular geometries be the same?