Textbook Question
Determine the electron configurations for CN+, CN, and CN-. (a) Which species has the strongest C¬N bond?
1822
views
Ch.9 - Molecular Geometry and Bonding Theories
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
Not the one you use?Change textbookSelect a different textbook
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 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.
Verified step by step guidance1
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).
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
5mWas this helpful?
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 diatomic molecules, bond order can help predict the bond length and strength.
Recommended video:
Guided course
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.
Recommended video:
Guided course
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.
Recommended video:
Guided course
00:59Magnetic Quantum Example
Related Practice
Textbook Question
(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.
Textbook Question
Explain the following: (c) The O22 + ion has a stronger O—O bond than O2 itself.
885
views
1
rank
Textbook Question
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.
823
views
Textbook Question
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 +?
354
views
Textbook Question
Determine the electron configurations for CN+, CN, and CN-. (b) Which species, if any, has unpaired electrons?
2115
views