Textbook Question
Using Figures 9.39 and 9.43 as guides, draw the molecular-orbital electron configuration for (d) Ne22+. In each case indicate whether the addition of an electron to the ion would increase or decrease the bond order of the species.
Ch.9 - Molecular Geometry and Bonding Theories
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- 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: 9780137542970Not the one you use?Change textbook
Chapter 9, Problem 80b
If we assume that the energy-level diagrams for homonuclear diatomic molecules shown in Figure 9.43 can be applied to heteronuclear diatomic molecules and ions, predict the bond order and magnetic behavior of b. NO–
Verified step by step guidance1
Identify the total number of electrons in the molecule NO⁻. Nitrogen (N) has 7 electrons, oxygen (O) has 8 electrons, and the negative charge adds 1 more electron, totaling 16 electrons.
Use the molecular orbital (MO) theory to distribute these 16 electrons in the molecular orbitals. For NO⁻, the order of filling is: \( \sigma_{1s}^2, \sigma^*_{1s}^2, \sigma_{2s}^2, \sigma^*_{2s}^2, \sigma_{2p_z}^2, \pi_{2p_x}^2 = \pi_{2p_y}^2, \pi^*_{2p_x}^2 = \pi^*_{2p_y}^1 \).
Calculate the bond order using the formula: \( \text{Bond Order} = \frac{1}{2} (\text{Number of bonding electrons} - \text{Number of antibonding electrons}) \).
Determine the magnetic behavior by checking for unpaired electrons. If there are unpaired electrons, the molecule is paramagnetic; if all electrons are paired, it is diamagnetic.
Conclude the bond order and magnetic behavior based on the calculations and observations from the previous steps.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Bond Order
Bond order is a measure of the number of chemical bonds between a pair of atoms. It is calculated as the difference between the number of bonding and antibonding electrons divided by two. A higher bond order indicates a stronger bond and greater stability of the molecule. For example, a bond order of 1 corresponds to a single bond, while a bond order of 2 corresponds to a double bond.
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Average Bond Order
Magnetic Behavior
Magnetic behavior in molecules is determined by the presence of unpaired electrons. Molecules with unpaired electrons exhibit paramagnetism, meaning they are attracted to magnetic fields, while those with all electrons paired are diamagnetic and are repelled by magnetic fields. Understanding the electron configuration and the arrangement of electrons in molecular orbitals is crucial for predicting a molecule's magnetic properties.
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Molecular Orbital Theory
Molecular Orbital Theory describes the behavior of electrons in molecules by considering the combination of atomic orbitals to form molecular orbitals. These orbitals can be bonding, antibonding, or non-bonding, and they help explain the stability, bond order, and magnetic properties of molecules. This theory is particularly useful for analyzing diatomic molecules, including both homonuclear and heteronuclear types.
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Related Practice
Textbook Question
Determine whether each of the following statements about diamagnetism and paramagnetism is true or false:
a. A diamagnetic substance is weakly repelled from a magnetic field.
b. A substance with unpaired electrons will be diamagnetic.
c. A paramagnetic substance is attracted to a magnetic field.
d. The O2 molecule is paramagnetic.
Textbook Question
a. Which of the following is expected to be paramagnetic: Ne, Li2, Li2+, N2, N2+, N22−? b. For each of the substances in part (a) that is paramagnetic, determine the number of unpaired electrons it has.
Textbook Question
If we assume that the energy-level diagrams for homonuclear diatomic molecules shown in Figure 9.43 can be applied to heteronuclear diatomic molecules and ions, predict the bond order and magnetic behavior of d. NeF+
Textbook Question
Determine the electron configurations for CN+, CN, and CN-. (a) Which species has the strongest C¬N bond?
Textbook Question
Determine the electron configurations for CN+, CN, and CN-. b. Which species, if any, is paramagnetic?