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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 17a,c
Capitolo 9, Problema 17a,c

(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.

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Step 1: Understand the concept of molecular geometry. Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is determined by the number of bonding pairs and lone pairs of electrons around the central atom.
Step 2: Analyze the AB6 molecule. Since the A atom has no lone pairs and is surrounded by six B atoms, the electron pairs are arranged to minimize repulsion. This arrangement is typically octahedral, where the bond angles are 90 degrees.
Step 3: Consider the AB4 molecule. If the A atom has no lone pairs and is surrounded by four B atoms, the electron pairs will arrange themselves in a way that minimizes repulsion, typically resulting in a tetrahedral geometry with bond angles of approximately 109.5 degrees.
Step 4: Apply VSEPR theory. VSEPR (Valence Shell Electron Pair Repulsion) theory helps predict the geometry of molecules based on the repulsion between electron pairs. For AB6, the octahedral shape is predicted, and for AB4, the tetrahedral shape is predicted.
Step 5: Visualize the molecular geometries. For AB6, imagine a central atom with six surrounding atoms forming an octahedron. For AB4, visualize a central atom with four surrounding atoms forming a tetrahedron.

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VSEPR Theory

Valence Shell Electron Pair Repulsion (VSEPR) Theory is a model used to predict the geometry of molecules based on the repulsion between electron pairs surrounding a central atom. According to this theory, electron pairs, whether bonding or lone pairs, will arrange themselves to minimize repulsion, leading to specific molecular shapes.
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Molecular Shapes and VSEPR

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule. It is determined by the number of bonding pairs and lone pairs of electrons around the central atom, which influences the overall shape, such as linear, trigonal planar, tetrahedral, octahedral, etc.
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Molecular Geometry with Two Electron Groups

Coordination Number

The coordination number is the number of atoms, ions, or molecules that a central atom can bond with in a molecule. In the case of AB<sub>6</sub>, the coordination number is six, indicating that the central atom A is bonded to six B atoms, which typically results in an octahedral geometry.
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Coordination Numbers
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(b) An AB4 molecule has two lone pairs of electrons on the A atom (in addition to the four B atoms). What is the electron-domain geometry around the A atom?

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