Domanda del libro di testo
Determine the electron configurations for CN+, CN, and CN-. (a) Which species has the strongest C¬N bond?
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Ch.9 - Molecular Geometry and Bonding Theories
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Capitolo 9, Problema 80d
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) ClF.
Guida verificata passo dopo passo1
Identify the valence electrons for each atom in the molecule. Chlorine (Cl) has 7 valence electrons and Fluorine (F) also has 7 valence electrons.
Combine the total number of valence electrons from both atoms. Since both Cl and F contribute 7 electrons each, the total number of valence electrons for ClF is 14.
Draw the molecular orbital diagram for ClF. Since Cl and F are in the same period, you can use a simplified diagram similar to that of homonuclear diatomic molecules, but adjust for differences in electronegativity and orbital energies.
Fill the molecular orbitals with the 14 electrons, starting from the lowest energy orbital. Follow the Pauli exclusion principle and Hund's rule while filling the orbitals.
Calculate the bond order using the formula: Bond Order = (number of electrons in bonding orbitals - number of electrons in antibonding orbitals) / 2. Determine the magnetic behavior by checking if there are unpaired electrons (paramagnetic if unpaired, diamagnetic if all are paired).
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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 diatomic molecules, bond order can help predict the bond length and strength.
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Percorso guidato
00:36
Average Bond Order
Molecular Orbital Theory
Molecular Orbital Theory describes the behavior of electrons in molecules using molecular orbitals, which are formed by the combination of atomic orbitals. Electrons occupy these orbitals according to the Aufbau principle, and the arrangement of electrons in bonding and antibonding orbitals determines the stability and properties of the molecule. This theory is essential for predicting the magnetic behavior of molecules.
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Percorso guidato
03:06Molecular Orbital Theory
Magnetic Behavior
Magnetic behavior in molecules is determined by the presence of unpaired electrons in molecular orbitals. If a molecule has unpaired electrons, it exhibits paramagnetism, meaning it is attracted to magnetic fields. Conversely, if all electrons are paired, the molecule is diamagnetic and is not attracted to magnetic fields. Understanding the electron configuration of ClF is crucial for predicting its magnetic properties.
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Percorso guidato
00:59Magnetic Quantum Example
Pratica correlata
Domanda del libro di testo
(a) The nitric oxide molecule, NO, readily loses one electron to form the NO+ ion. Which of the following is the best explanation of why this happens: (i) Oxygen is more electronegative than nitrogen, (ii) The highest energy electron in NO lies in a π2p* molecular orbital, or (iii) The π2p* MO in NO is completely filled.
Domanda del libro di testo
Using Figures 9.35 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.
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Domanda del libro di testo
How would we describe a substance that contains only paired
electrons and is weakly repelled by a magnetic field? Which
of the following ions would you expect to possess similar
characteristics: H2-, Ne2+, F2, O22 +?
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Domanda del libro di testo
Determine the electron configurations for CN+, CN, and CN-. (b) Which species, if any, has unpaired electrons?
2116
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Domanda del libro di testo
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+.
669
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