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Interpretation:
Charge and bond order of the ion Cn−2 has to be determined.
Concept Introduction:
Molecular orbital diagram is a linear combination of atomic orbitals of similar energy and similar symmetry. It is formed by the proper overlap of the atomic orbitals.
There are 3 types of molecular orbitals as follows:
1. Bonding molecular orbital: They are formed by the constructive interference of atomic orbitals and electrons in it stabilize the molecule and are of lesser in energy.
2. Antibonding molecular orbital: This type of orbitals increases the energy of molecule and destabilizes it and weakens the bond between the atoms.
3. Non-bonding molecular orbital: These types of orbitals have energy similar to atomic orbitals that is addition or removal of electron does not change the energy of molecule.
The order of energy in molecular orbital follows two rules as follows:
1. For
σ1s<σ∗1s<σ2s<σ∗2s<(π2px=π2py)<σ2pz<(π∗2px=π∗2py)<σ∗2pz
2. For atomic number more than 14 order of energy is,
σ1s<σ∗1s<σ2s<σ∗2s<σ2pz<(π2px=π2py)<(π∗2px=π∗2py)<σ∗2pz
Bond order (b) is defined as total number of bonds between the atoms. It is calculated as follows:
b=12[number of elctrons in bonding orbitals−number of electrons in antibonding orbitals] (1)
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Chapter 2 Solutions
Chemical Principles: The Quest for Insight
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