The relative stabilities of F 2 and F 2 + is to be compared using molecular orbital theory. Concept introduction: The combination of two atomic orbitals results in the formation of 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 anti-bonding molecular orbital as σ ∗ 1 s . The 2s orbital forms corresponding molecular orbitals. Bond order is determined by subtracting the total number of antibonding electrons and the total number of bonding electrons and dividing the obtained number by two. Stability of molecules increases with increase in bond order.
The relative stabilities of F 2 and F 2 + is to be compared using molecular orbital theory. Concept introduction: The combination of two atomic orbitals results in the formation of 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 anti-bonding molecular orbital as σ ∗ 1 s . The 2s orbital forms corresponding molecular orbitals. Bond order is determined by subtracting the total number of antibonding electrons and the total number of bonding electrons and dividing the obtained number by two. Stability of molecules increases with increase in bond order.
Solution Summary: The author explains that the relative stabilities of F_ 2 and > are to be compared using molecular orbital theory.
The relative stabilities of F2 and F2+ is to be compared using molecular orbital theory.
Concept introduction:
The combination of two atomic orbitals results in the formation of 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 anti-bonding molecular orbital as σ∗1s. The 2s orbital forms corresponding molecular orbitals.
Bond order is determined by subtracting the total number of antibonding electrons and the total number of bonding electrons and dividing the obtained number by two.
Stability of molecules increases with increase in bond order.
identify which spectrum is for acetaminophen and which is for phenacetin
The Concept of Aromaticity
21.15 State the number of 2p orbital electrons in each molecule or ion.
(a)
(b)
(e)
(f)
(c)
(d)
(h)
(i)
DA
(k)
21.16 Which of the molecules and ions given in Problem 21.15 are aromatic according to the
Hückel criteria? Which, if planar, would be antiaromatic?
21.17 Which of the following structures are considered aromatic according to the Hückel
criteria?
---0-0
(a)
(b)
(c)
(d)
(e)
(h)
H
-H
.8.0-
21.18 Which of the molecules and ions from Problem 21.17 have electrons donated by a
heteroatom?
1. Show the steps necessary to make 2-methyl-4-nonene using a
Wittig reaction. Start with triphenylphosphine and an alkyl
halide. After that you may use any other organic or inorganic
reagents.
2. Write in the product of this reaction:
CH3
CH₂
(C6H5)₂CuLi
H₂O+
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Quantum Molecular Orbital Theory (PChem Lecture: LCAO and gerade ungerade orbitals); Author: Prof Melko;https://www.youtube.com/watch?v=l59CGEstSGU;License: Standard YouTube License, CC-BY