Using the molecular orbital model, write electron configurations for the following diatomic species and calculate the bond orders. Which ones are paramagnetic? Place the species in order of increasing bond length and bond energy. a. CN + b. CN c. CN −
Using the molecular orbital model, write electron configurations for the following diatomic species and calculate the bond orders. Which ones are paramagnetic? Place the species in order of increasing bond length and bond energy. a. CN + b. CN c. CN −
Using the molecular orbital model, write electron configurations for the following diatomic species and calculate the bond orders. Which ones are paramagnetic? Place the species in order of increasing bond length and bond energy.
a. CN+
b. CN
c. CN−
(a)
Expert Solution
Interpretation Introduction
Interpretation: The electronic configuration for the given diatomic species is to be determined and their bond orders have to be calculated. The paramagnetic species have to be identified. The given molecules have to be placed in the correct order of increasing bond length and bond energy.
Concept introduction: The electronic configuration for multi-electron diatomic is written using the molecular orbitals, derived from the
H2+ molecular ion. A molecule having an unpaired electron in the valence shell is termed as a paramagnetic in nature, while the one that has no unpaired electrons is termed as diamagnetic. The bond order is calculated by difference between the anti-bonding electrons and the bonding electrons by two. This can be stated as,
The bond order is directly proportional to the bond energy and inversely proportional to the bond length.
To determine: The electronic configuration of
CN+, its bond order and its paramagnetic or diamagnetic nature.
Answer to Problem 56E
Answer
The configuration of
CN+ is
(σ2s)2(σ2s∗)2(π2p)4 and its bond order is
2_. It is diamagnetic in nature.
Explanation of Solution
The electronic configuration of the involved atoms is,
C=1s22s22p2N=1s22s22p3
The number of valence electrons present in
CN+=4+5−1=8
The molecular orbital configuration of
CN+ is
(σ2s)2(σ2s∗)2(π2p)4
Number of bonding electrons
=6
Number of non-bonding electrons
=2
Hence,
Bond order
=12(6−2)=2_
No unpaired electron is present; hence it is a diamagnetic molecule.
(b)
Expert Solution
Interpretation Introduction
Interpretation: The electronic configuration for the given diatomic species is to be determined and their bond orders have to be calculated. The paramagnetic species have to be identified. The given molecules have to be placed in the correct order of increasing bond length and bond energy.
Concept introduction: The electronic configuration for multi-electron diatomic is written using the molecular orbitals, derived from the
H2+ molecular ion. A molecule having an unpaired electron in the valence shell is termed as a paramagnetic in nature, while the one that has no unpaired electrons is termed as diamagnetic. The bond order is calculated by difference between the anti-bonding electrons and the bonding electrons by two. This can be stated as,
The bond order is directly proportional to the bond energy and inversely proportional to the bond length.
To determine: The electronic configuration of
CN, its bond order and its paramagnetic or diamagnetic nature.
Answer to Problem 56E
Answer
The configuration of
CN is
(σ2s)2(σ2s∗)2(π2p)4(σ2p)1 and its bond order is
2.5_. It is paramagnetic in nature.
Explanation of Solution
The electronic configuration of the involved atoms is,
C=1s22s22p2N=1s22s22p3
The number of valence electrons present in
CN=4+5=9
The molecular orbital configuration of
CN is
(σ2s)2(σ2s∗)2(π2p)4(σ2p)1
Number of bonding electrons
=7
Number of non-bonding electrons
=2
Hence,
Bond order
=7−22=2.5_.
The
CN molecule contains one unpaired electron. Hence, it is a paramagnetic molecule.
(c)
Expert Solution
Interpretation Introduction
Interpretation: The electronic configuration for the given diatomic species is to be determined and their bond orders have to be calculated. The paramagnetic species have to be identified. The given molecules have to be placed in the correct order of increasing bond length and bond energy.
Concept introduction: The electronic configuration for multi-electron diatomic is written using the molecular orbitals, derived from the
H2+ molecular ion. A molecule having an unpaired electron in the valence shell is termed as a paramagnetic in nature, while the one that has no unpaired electrons is termed as diamagnetic. The bond order is calculated by difference between the anti-bonding electrons and the bonding electrons by two. This can be stated as,
The bond order is directly proportional to the bond energy and inversely proportional to the bond length.
To determine: The electronic configuration of
CN−, its bond order and its paramagnetic or diamagnetic nature.
Answer to Problem 56E
Answer
The configuration of
CN− is
(σ2s)2(σ2s∗)2(π2p)4(σ2p)2 and its bond order is
3_. It is diamagnetic in nature. The required order is,
CN−<CN<CN+
Explanation of Solution
The electronic configuration of the involved atoms is,
C=1s22s22p2N=1s22s22p3
The number of valence electrons present in
CN−=4+5+1=10
The molecular orbital configuration of
CN− is
(σ2s)2(σ2s∗)2(π2p)4(σ2p)2
Number of bonding electrons
=8
Number of non-bonding electrons
=2
Hence,
Bond order
=8−22=3_.
No unpaired electron is present; hence it is a diamagnetic molecule.
Conclusion
The diatomic configuration of a diatomic species can be determined using the molecular orbital diagram. The difference between the bonding electrons and the non-bonding electrons divided by two gives the bond order of the molecule.
The bond order is inversely proportional to bond length. The molecule having the least bond order value has the greatest bond length.
The bond order is directly proportional to bond energy. The molecule having the least bond order value has the least bond energy.
The bond order is directly proportional to the bond energy and inversely proportional to the bond length.
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How would doubling the concentration of reactant
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