Domanda del libro di testo
(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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Ch.9 - Molecular Geometry and Bonding Theories
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Capitolo 9, Problema 18
Describe the bond angles to be found in each of the following molecular structures: (a) trigonal planar, (b) tetrahedral, (c) octahedral, (d) linear.
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Identify the molecular geometry for each structure: (a) trigonal planar, (b) tetrahedral, (c) octahedral, (d) linear.
Recall that the bond angles are determined by the electron pair geometry around the central atom.
For (a) trigonal planar, the bond angles are typically 120° due to the arrangement of three electron pairs around the central atom.
For (b) tetrahedral, the bond angles are typically 109.5° as four electron pairs are arranged in a three-dimensional space.
For (c) octahedral, the bond angles are typically 90° because six electron pairs are symmetrically arranged around the central atom, and for (d) linear, the bond angles are 180° as two electron pairs are directly opposite each other.
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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, which influences the shape and angles between bonds. Understanding molecular geometry is crucial for predicting bond angles and the overall structure of molecules.
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Percorso guidato
01:33
Molecular Geometry with Two Electron Groups
VSEPR Theory
Valence Shell Electron Pair Repulsion (VSEPR) theory is a model used to predict the geometry of individual molecules based on the repulsion between electron pairs in the valence shell of the central atom. According to VSEPR, electron pairs will arrange themselves to minimize repulsion, leading to specific bond angles characteristic of different molecular shapes, such as trigonal planar or tetrahedral.
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02:13Molecular Shapes and VSEPR
Bond Angles
Bond angles are the angles formed between adjacent bonds in a molecule, which are influenced by the molecular geometry. For example, in a trigonal planar structure, bond angles are approximately 120 degrees, while in a tetrahedral structure, they are about 109.5 degrees. Understanding these angles is essential for predicting the behavior and reactivity of molecules.
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01:53Bond Angles
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b. The NH3 molecule is trigonal pyramidal, while BF3 is trigonal planar. Which of these molecules is flat?
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For each of these contour representations of molecular orbitals, identify (c) whether the MO is bonding or antibonding (i)
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a. Methane (CH4) and the perchlorate ion (ClO4−) are both described as tetrahedral. What does this indicate about their bond angles?
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Would you expect the nonbonding electron-pair domain in NH3 to be greater or less in size than the corresponding one in PH3?
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