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.

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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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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.

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.

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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