Textbook Question
For each molecule (a)–(f), indicate how many different electron-domain geometries are consistent with the molecular geometry shown. a.
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Ch.9 - Molecular Geometry and Bonding Theories
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement140
- Ch.2 - Atoms, Molecules, and Ions192
- Ch.3 - Chemical Reactions and Reaction Stoichiometry172
- Ch.4 - Reactions in Aqueous Solution156
- Ch.5 - Thermochemistry151
- Ch.6 - Electronic Structure of Atoms137
- Ch.7 - Periodic Properties of the Elements127
- Ch.8 - Basic Concepts of Chemical Bonding143
- Ch.9 - Molecular Geometry and Bonding Theories167
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces97
- Ch.12 - Solids and Modern Materials129
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics175
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Acid-Base Equilibria127
- Ch.17 - Additional Aspects of Aqueous Equilibria133
- Ch.18 - Chemistry of the Environment88
- Ch.19 - Chemical Thermodynamics140
- Ch.20 - Electrochemistry137
- Ch.21 - Nuclear Chemistry99
- Ch.22 - Chemistry of the Nonmetals66
- Ch.23 - Transition Metals and Coordination Chemistry69
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry11
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 9, Problem 6b
The orbital diagram that follows presents the final step in the formation of hybrid orbitals by a silicon atom. (b) What type of hybrid orbital is produced in this hybridization?
Verified step by step guidance1
Step 1: Look at the orbital diagram provided. The orbital diagram should show the distribution of electrons in the atomic orbitals of the silicon atom after hybridization.
Step 2: Count the number of orbitals that are involved in the hybridization. The number of atomic orbitals that are involved in the hybridization process will determine the type of hybrid orbitals formed.
Step 3: Identify the type of hybridization. If there are four orbitals involved (one 2s and three 2p), the hybridization is sp3. If there are three orbitals involved (one 2s and two 2p), the hybridization is sp2. If there are two orbitals involved (one 2s and one 2p), the hybridization is sp.
Step 4: The type of hybrid orbital produced corresponds to the type of hybridization. For example, sp3 hybridization produces sp3 hybrid orbitals, sp2 hybridization produces sp2 hybrid orbitals, and sp hybridization produces sp hybrid orbitals.
Step 5: Remember that the type of hybridization can also give you information about the geometry of the molecule. For example, sp3 hybridization corresponds to a tetrahedral geometry, sp2 hybridization corresponds to a trigonal planar geometry, and sp hybridization corresponds to a linear geometry.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Hybridization
Hybridization is a concept in chemistry that describes the mixing of atomic orbitals to form new hybrid orbitals. These hybrid orbitals have different energies and shapes compared to the original atomic orbitals, allowing for the formation of more stable molecular structures. In the case of silicon, hybridization typically involves the combination of its 3s and 3p orbitals.
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Hybridization
Types of Hybrid Orbitals
There are several types of hybrid orbitals, including sp, sp2, and sp3, which correspond to the number of atomic orbitals mixed. For example, sp hybridization involves one s and one p orbital, resulting in two equivalent sp orbitals, while sp3 hybridization involves one s and three p orbitals, resulting in four equivalent sp3 orbitals. The type of hybridization affects the geometry and bonding properties of the molecule.
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Silicon's Hybridization
Silicon typically undergoes sp3 hybridization when forming four equivalent bonds, as seen in compounds like silicon tetrafluoride (SiF4). In this process, one 3s and three 3p orbitals combine to create four sp3 hybrid orbitals, which are oriented tetrahedrally. Understanding this hybridization is crucial for predicting the molecular geometry and reactivity of silicon-containing compounds.
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Related Practice
Textbook Question
In the hydrocarbon
(d) Identify all the 120° bond angles in the molecule.
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Textbook Question
In the hydrocarbon (b) How many s bonds are there in the molecule?
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Textbook Question
The orbital diagram that follows presents the final step in the formation of hybrid orbitals by a silicon atom. (a) Which of the following best describes what took place before the step pictured in the diagram: (i) Two 3p electrons became unpaired, (ii) An electron was promoted from the 2p orbital to the 3s orbital, or (iii) An electron was promoted from the 3s orbital to the 3p orbital?
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Textbook Question
The following plot shows the potential energy of two Cl atoms as a function of the distance between them. (c) If the Cl2 molecule is compressed under higher and higher pressure, does the Cl–Cl bond become stronger or weaker?
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Textbook Question
In the hydrocarbon
(a) What is the hybridization at each carbon atom in the molecule?
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