Textbook Question
Draw a molecular orbital energy diagram for ClF. (Assume that the sp orbitals are lower in energy than the p orbitals.) What is the bond order in ClF?
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Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving107
- Ch.2 - Atoms & Elements100
- Ch.3 - Molecules, Compounds & Chemical Equations127
- Ch.4 - Chemical Quantities & Aqueous Reactions114
- Ch.5 - Gases103
- Ch.6 - Thermochemistry92
- Ch.7 - Quantum-Mechanical Model of the Atom50
- Ch.8 - Periodic Properties of the Elements89
- Ch.9 - Chemical Bonding I: The Lewis Model84
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory74
- Ch.11 - Liquids, Solids & Intermolecular Forces60
- Ch.12 - Solids and Modern Material50
- Ch.13 - Solutions90
- Ch.14 - Chemical Kinetics111
- Ch.15 - Chemical Equilibrium65
- Ch.16 - Acids and Bases135
- Ch.17 - Aqueous Ionic Equilibrium145
- Ch.18 - Free Energy and Thermodynamics92
- Ch.19 - Electrochemistry100
- Ch.20 - Radioactivity and Nuclear Chemistry68
- Ch.21 - Organic Chemistry121
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Tro 4th EditionCh.10 - Chemical Bonding II: Molecular Shapes & Valence Bond TheoryProblem 95
Tro 4th EditionCh.10 - Chemical Bonding II: Molecular Shapes & Valence Bond TheoryProblem 95Chapter 10, Problem 95
Draw the structure of a molecule with the formula C4H6Cl2 that has a dipole moment of 0.
Verified step by step guidance1
Identify the molecular formula and the requirement of zero dipole moment. The formula given is C4H6Cl2, and a zero dipole moment suggests a symmetrical structure.
Consider possible structures for C4H6Cl2. The molecule could be a chain or a ring. Given the need for symmetry, a ring might be more plausible.
Place the chlorine atoms in positions that would maintain symmetry. For a zero dipole moment, the chlorines should be placed opposite each other in the ring structure.
Fill in the hydrogen atoms while maintaining the general rules of valency for carbon, which makes four bonds. Each carbon in the ring should end up with appropriate hydrogen atoms to satisfy its valency.
Verify the structure by ensuring all valencies are satisfied and the structure is symmetrical, thus supporting the zero dipole moment. A possible structure could be 1,4-dichlorocyclobutane, where the chlorine atoms are on opposite carbons in a four-membered ring.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Molecular Structure
Molecular structure refers to the three-dimensional arrangement of atoms within a molecule. It determines the molecule's shape, bond angles, and the spatial orientation of its functional groups. Understanding how atoms are connected and their spatial distribution is crucial for predicting the molecule's properties, including polarity.
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Molecular Formula
Dipole Moment
A dipole moment is a measure of the separation of positive and negative charges in a molecule, indicating its polarity. Molecules with a dipole moment have uneven charge distribution, while those with a dipole moment of zero are nonpolar. The dipole moment is influenced by the electronegativity of atoms and the symmetry of the molecular structure.
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Isomerism
Isomerism is the phenomenon where two or more compounds have the same molecular formula but different structures or arrangements of atoms. In the case of C4H6Cl2, various structural isomers can exist, and some may have a symmetrical arrangement that results in a net dipole moment of zero. Understanding isomerism is essential for identifying the correct structure that meets the given criteria.
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2:14Isomerism in Coordination Complexes Example
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How many types of hybrid orbitals do we use to describe each molecule? a. N2O5 c. BrCN (no formal charges)
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How many types of hybrid orbitals do we use to describe each molecule? b. C2H5NO (four C-H bonds and one O-H bond)
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The compound C3H4 has two double bonds. Describe its bonding and geometry, using a valence bond approach.
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Draw the structures of two compounds that have the composition CH3NO2 and have all three H atoms bonded to the C. Predict which compound has the larger ONO bond angle.
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