The p orbitals present in given allyl cation should be sketched and the bonding should be described using the valence bond model for σ bonding and delocalized M O model for π bonding. Concept Introduction: Sigma (σ) bonds : The bonds in which shared hybrid orbital’s electron density are concentrated along the internuclear axis and it is represented as the single bond between atoms in molecules. Pi (π) bonds: the bonds in which shared unhybridized orbital’s (p, d, etc) electron density are concentrated in above and below of the plane of the molecule. Double bonds : One sigma bond and one pi bond are together known as a double bond. Molecular orbital theory: The atomic orbitals of the atoms constituted in a molecule are combined to produce new orbitals are called Molecular Orbitals. Like atomic orbitals, a molecular orbital can accommodate maximum two electrons and the two electrons must have opposite spins (Pauli Exclusion Principle). The numbers of MO’s are equals to the number of atomic orbitals are combined in such a way that the linear combination of similar atomic orbitals to form one bonding and one anti-bonding MO’s. The bonding MO’s are lower in energy than the anti-bonding MO’s. HOMO is the highest energized occupied orbital in the MO’s. Relative energy levels of molecules are according to the energy levels of atomic orbitals. LUMO is the lowest energized orbital in the MO’s.

Question

Want to see the full answer?

Answer 1

Question

Chapter 5, Problem 5.60SP

Interpretation Introduction

Interpretation:

The p orbitals present in given allyl cation should be sketched and the bonding should be described using the valence bond model for σ bonding and delocalized MO model for π bonding.

Concept Introduction:

Sigma (σ) bonds: The bonds in which shared hybrid orbital’s electron density are concentrated along the internuclear axis and it is represented as the single bond between atoms in molecules.

Pi (π) bonds: the bonds in which shared unhybridized orbital’s (p, d, etc) electron density are concentrated in above and below of the plane of the molecule.

Double bonds: One sigma bond and one pi bond are together known as a double bond.

Molecular orbital theory:

The atomic orbitals of the atoms constituted in a molecule are combined to produce new orbitals are called Molecular Orbitals.

Like atomic orbitals, a molecular orbital can accommodate maximum two electrons and the two electrons must have opposite spins (Pauli Exclusion Principle).

The numbers of MO’s are equals to the number of atomic orbitals are combined in such a way that the linear combination of similar atomic orbitals to form one bonding and one anti-bonding MO’s.

The bonding MO’s are lower in energy than the anti-bonding MO’s.

HOMO is the highest energized occupied orbital in the MO’s.

Relative energy levels of molecules are according to the energy levels of atomic orbitals.

LUMO is the lowest energized orbital in the MO’s.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

1)Using molecular orbital theory, determine the electronic structure of the first excited electronic state of N2. What differences are expected in the properties of the excited state of N2 compared with the same properties of the ground state? 2)Describe the bonding (including σ and п bonds) on an N atom in dinitrogen difluoride, N2F2, using valence bond theory. 3)Magic numbers are associated with protons and neutrons in a nucleus. State the magic numbers for protons and neutrons, and give two evidences to support the existence of these magic numbers

Draw Lewis structure for OPF, (P is the central atom). Write down all possible resonance structures, including formal charges. Draw the geometry of the ion. Indicate the hybridization of the central atom and type of orbitals involved in x bonding on both bonded atoms.

Use the molecular orbital model to fully describe the bonding in O2+, O2, O2-, and O22-.Determine which of the following statements are true and which are false. True or false? : Bond length increases with increasing bond order while bond energy decreases.The number of unpaired electrons in O2- and O2 is, respectively, 1 and 2. The electron configuration of O2 is (σ2s)2(σ2s*)2(σ2p)2(π2p)4(π2p*)1. The electron configuration of O2- is (σ2s)2(σ2s*)2(σ2p)2(π2p)4(π2p*)3. The bond order in O2- and O22- is, respectively, 2.5 and 1. The bond lengths increase in the order: O22- < O2- < O2 < O2+.