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According to MO theory, which molecule or ion has the highest bond energy? O2, O2- , O22-
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Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving118
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds131
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions82
- Ch.6 - Gases114
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements90
- Ch.10 - Chemical Bonding I: The Lewis Model89
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials47
- Ch.14 - Solutions90
- Ch.15 - Chemical Kinetics115
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases136
- Ch.18 - Aqueous Ionic Equilibrium153
- Ch.19 - Free Energy & Thermodynamics93
- Ch.20 - Electrochemistry106
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry140
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
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Tro 6th EditionCh.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO TheoryProblema 82a
Tro 6th EditionCh.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO TheoryProblema 82aCapitolo 11, Problema 82a
Use molecular orbital theory to predict if each molecule or ion exists in a relatively stable form. a. F22–
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Identify the total number of electrons in the molecule or ion. For F2^{2-}, each fluorine atom has 9 electrons, and the 2- charge adds 2 more electrons, giving a total of 20 electrons.
Write the electron configuration for the molecule using molecular orbitals. For diatomic molecules like F2^{2-}, use the order: \( \sigma_{1s}^2, \sigma^*_{1s}^2, \sigma_{2s}^2, \sigma^*_{2s}^2, \sigma_{2p_z}^2, \pi_{2p_x}^2, \pi_{2p_y}^2, \pi^*_{2p_x}^2, \pi^*_{2p_y}^2, \sigma^*_{2p_z}^2 \).
Fill the molecular orbitals with the 20 electrons according to the Aufbau principle, Pauli exclusion principle, and Hund's rule.
Calculate the bond order using the formula: \( \text{Bond Order} = \frac{(\text{Number of bonding electrons} - \text{Number of antibonding electrons})}{2} \).
Determine the stability of the molecule. A positive bond order indicates a stable molecule, while a bond order of zero or negative suggests instability.
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Molecular Orbital Theory
Molecular Orbital Theory (MOT) describes the behavior of electrons in molecules by combining atomic orbitals to form molecular orbitals. These orbitals can be bonding, antibonding, or non-bonding, and the distribution of electrons among them determines the stability and properties of the molecule. Understanding MOT is essential for predicting molecular stability and reactivity.
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03:06
Molecular Orbital Theory
Bond Order
Bond order is a measure of the number of chemical bonds between a pair of atoms, calculated as the difference between the number of bonding and antibonding electrons divided by two. A higher bond order indicates a more stable molecule, while a bond order of zero suggests that the molecule is unstable and unlikely to exist. This concept is crucial for assessing the stability of the F22– ion.
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00:36Average Bond Order
Electron Configuration in Ions
The electron configuration of ions reflects the distribution of electrons in molecular orbitals after accounting for the gain or loss of electrons. For the F22– ion, two additional electrons must be considered, which will occupy the available molecular orbitals. Analyzing the resulting electron configuration helps determine the overall stability and existence of the ion.
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00:35Anion Electron Configuration
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According to MO theory, which molecule or ion has the shortest bond length? O2, O2- , O22-
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Using the molecular orbital energy ordering for second-row homonuclear diatomic molecules in which the π2p orbitals lie at higher energy than the σ2p, draw MO energy diagrams and predict the bond order in a molecule or ion with each number of total valence electrons. Will the molecule or ion be diamagnetic or paramagnetic? c. 13
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Using the molecular orbital energy ordering for second-row homonuclear diatomic molecules in which the π2p orbitals lie at higher energy than the σ2p, draw MO energy diagrams and predict the bond order in a molecule or ion with each number of total valence electrons. Will the molecule or ion be diamagnetic or paramagnetic? d. 14
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Use molecular orbital theory to predict if each molecule or ion exists in a relatively stable form. a. Li22+ b. Li2 c. Be22+ d. C22+
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According to MO theory, which molecule or ion has the highest bond order? O2, O2- , O22-
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