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Ch.9 - Molecular Geometry and Bonding Theories
Brown - Chemistry: The Central Science 14th Edition
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Tutti i libri di testoBrown 14th EditionCh.9 - Molecular Geometry and Bonding TheoriesProblema 87a
Capitolo 9, Problema 87a

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?

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Determine the number of valence electrons for each central atom: P, Br, Cl, and Al.
Add or subtract electrons based on the charge of the ion: add one electron for negative charges and subtract one for positive charges.
Calculate the total number of electrons around the central atom by adding the electrons from the fluorine atoms (each F contributes one electron to the central atom).
Check if the total number of electrons around the central atom exceeds 8, which would indicate more than an octet.
Identify which ions have central atoms with more than 8 electrons, indicating an expanded octet.

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Octet Rule

The octet rule is a chemical principle that states atoms tend to bond in such a way that they have eight electrons in their valence shell, achieving a stable electron configuration similar to that of noble gases. This rule is particularly relevant for main group elements, which typically form bonds to fulfill this requirement. However, some elements, especially those in the third period and beyond, can expand their octet due to available d-orbitals.
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Octet Rule

Expanded Octet

An expanded octet occurs when an atom has more than eight electrons in its valence shell. This phenomenon is common in elements from the third period of the periodic table and beyond, such as phosphorus, sulfur, and chlorine, which can utilize their d-orbitals to accommodate additional electrons. Understanding which elements can expand their octet is crucial for predicting the bonding and structure of certain molecules and ions.
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Octet Rule

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They are essential for visualizing the arrangement of electrons and determining whether an atom has achieved an octet or an expanded octet. By drawing Lewis structures for the given ions, one can easily identify the number of electrons surrounding the central atom and assess compliance with the octet rule.
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Lewis Dot Structures: Ions
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Domanda del libro di testo

An AB2 molecule is described as having a tetrahedral geometry. (a) How many nonbonding domains are on atom A?

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Domanda del libro di testo

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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Domanda del libro di testo

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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Domanda del libro di testo

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

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Domanda del libro di testo

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?