The difference in bond enthalpies of F 2 and F 2 − is to be determined using the molecular orbital theory. Concept introduction: According to the molecular orbital theory: Two atomic orbitals undergo a combination process in order to form a bonding and an antibonding molecular orbital. Orbitals that lie on internuclear axis combine to form sigma σ molecular orbital, and orbitals parallel to each other combine to form π molecular orbitals. The molecular orbital formed by the combination of 1s orbital forms bonding molecular orbital designated as σ 1 s and antibonding molecular orbital σ ∗ 1 s . The 2s orbital forms corresponding molecular orbitals. Molecular orbital formed by the combination of 2p x orbital forms a bonding molecular orbital designated as σ 2 p x and an antibonding molecular orbital designated as σ ∗ 2 p x . Molecular orbitals formed by combining 2p y and 2p z orbital forms bonding molecular orbitals designated as π 2p y and π 2p z , and antibonding molecular orbitals designated as π ∗ 2p y and π ∗ 2p z . Electrons are filled in the molecular orbitals in increasing order of their energy. Bond order is determined by subtracting the number of electrons in antibonding orbitals from the number of electrons in bonding, divided by two. The higher the bond order, the more stable is the molecule and thus higher is the bond enthalpy.
The difference in bond enthalpies of F 2 and F 2 − is to be determined using the molecular orbital theory. Concept introduction: According to the molecular orbital theory: Two atomic orbitals undergo a combination process in order to form a bonding and an antibonding molecular orbital. Orbitals that lie on internuclear axis combine to form sigma σ molecular orbital, and orbitals parallel to each other combine to form π molecular orbitals. The molecular orbital formed by the combination of 1s orbital forms bonding molecular orbital designated as σ 1 s and antibonding molecular orbital σ ∗ 1 s . The 2s orbital forms corresponding molecular orbitals. Molecular orbital formed by the combination of 2p x orbital forms a bonding molecular orbital designated as σ 2 p x and an antibonding molecular orbital designated as σ ∗ 2 p x . Molecular orbitals formed by combining 2p y and 2p z orbital forms bonding molecular orbitals designated as π 2p y and π 2p z , and antibonding molecular orbitals designated as π ∗ 2p y and π ∗ 2p z . Electrons are filled in the molecular orbitals in increasing order of their energy. Bond order is determined by subtracting the number of electrons in antibonding orbitals from the number of electrons in bonding, divided by two. The higher the bond order, the more stable is the molecule and thus higher is the bond enthalpy.
Solution Summary: The author explains how the molecular orbital theory determines the difference in bond enthalpies between two atomic orbitals. Orbitals that lie on internuclear axis combine to form sigma
is to be determined using the molecular orbital theory.
Concept introduction:
According to the molecular orbital theory:
Two atomic orbitals undergo a combination process in order to form a bonding and an antibonding molecular orbital. Orbitals that lie on internuclear axis combine to form sigma σ molecular orbital, and orbitals parallel to each other combine to form π
molecular orbitals.
The molecular orbital formed by the combination of 1s
orbital forms bonding molecular orbital designated as σ1s and antibonding molecular orbital σ∗1s. The 2s orbital forms corresponding molecular orbitals.
Molecular orbital formed by the combination of 2px orbital forms a bonding molecular orbital designated as σ2px
and an antibonding molecular orbital designated as σ∗2px.
Molecular orbitals formed by combining 2py and 2pz orbital forms bonding molecular orbitals designated as π2py
and π2pz, and antibonding molecular orbitals designated as π∗2py
and π∗2pz.
Electrons are filled in the molecular orbitals in increasing order of their energy.
Bond order is determined by subtracting the number of electrons in antibonding orbitals from the number of electrons in bonding, divided by two.
The higher the bond order, the more stable is the molecule and thus higher is the bond enthalpy.
Benzimidazole E. State its formula. sState the differences in the formula with other benzimidazoles.
Draw product A, indicating what type of reaction occurs.
F3C
CN
CF3
K2CO3, DMSO, H₂O2
A
19) Which metal is most commonly used in galvanization to protect steel structures from oxidation?
Lead
a.
b. Tin
C. Nickel
d. Zinc
20) The following molecule is an example of a:
R₁
R2-
-N-R3
a. Secondary amine
b. Secondary amide
c. Tertiary amine
d. Tertiary amide
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INTRODUCTION TO MOLECULAR QUANTUM MECHANICS -Valence bond theory - 1; Author: AGK Chemistry;https://www.youtube.com/watch?v=U8kPBPqDIwM;License: Standard YouTube License, CC-BY