The hybridisation of central O atom in O3 has to be given; also, the bonding in O 3 in terms of delocalized molecular orbitals has to be described. Concept Introduction: Molecular orbitals are formed by the combination of the atomic orbitals of the atoms in the molecule. The properties of the newly formed molecular orbital will be different from their individual atomic orbitals. In molecular orbital theory, electrons shared by atoms in a molecule reside in the molecular orbitals. Delocalized molecular orbitals are extended over two or more atoms, these are not confined to adjacent bonding atoms. Therefore, the electrons are free to move around the entire molecule. The structures that arise due to delocalization of electrons or charges is called as resonance structures or canonical structures. If a species can be represented in resonance structures, the π bonds of the species are delocalized. To Discuss: The hybridisation of central O atom in O 3 and also the bonding in O 3 in terms of delocalized molecular orbitals.
The hybridisation of central O atom in O3 has to be given; also, the bonding in O 3 in terms of delocalized molecular orbitals has to be described. Concept Introduction: Molecular orbitals are formed by the combination of the atomic orbitals of the atoms in the molecule. The properties of the newly formed molecular orbital will be different from their individual atomic orbitals. In molecular orbital theory, electrons shared by atoms in a molecule reside in the molecular orbitals. Delocalized molecular orbitals are extended over two or more atoms, these are not confined to adjacent bonding atoms. Therefore, the electrons are free to move around the entire molecule. The structures that arise due to delocalization of electrons or charges is called as resonance structures or canonical structures. If a species can be represented in resonance structures, the π bonds of the species are delocalized. To Discuss: The hybridisation of central O atom in O 3 and also the bonding in O 3 in terms of delocalized molecular orbitals.
Solution Summary: The author describes the hybridisation of central O atom in O3 and the bonding in O_ 3 in terms of delocalized molecular orbitals.
Interpretation: The hybridisation of central O atom in O3 has to be given; also, the bonding in O3 in terms of delocalized molecular orbitals has to be described.
Concept Introduction: Molecular orbitals are formed by the combination of the atomic orbitals of the atoms in the molecule. The properties of the newly formed molecular orbital will be different from their individual atomic orbitals. In molecular orbital theory, electrons shared by atoms in a molecule reside in the molecular orbitals.
Delocalized molecular orbitals are extended over two or more atoms, these are not confined to adjacent bonding atoms. Therefore, the electrons are free to move around the entire molecule.
The structures that arise due to delocalization of electrons or charges is called as resonance structures or canonical structures. If a species can be represented in resonance structures, the π bonds of the species are delocalized.
To Discuss: The hybridisation of central O atom in O3 and also the bonding in O3 in terms of delocalized molecular orbitals.
Draw a Lewis diagram(s) for the ozone molecule (O3). Determine the steric number and hybridization of the central oxygen atom, and identify the molecular geometry. Describe the nature of the p bonds and give the bondorder of the O-O bonds in ozone.
Acetic acid can be made by the oxidation of acetaldehyde(CH3CHO). Molecules of acetaldehyde have a-CH3 group, an oxygen atom, and a hydrogen atom attached to a carbon atom. Draw the Lewis diagram for this molecule, give the hybridization of each carbon atom, and describethe p orbitals and the number of electrons that occupy each one. Draw the three-dimensional structure of the molecule, showing all angles.
Use valence bond theory to explain the bonding in O2. Sketch the overlap of the atomic orbitals involved in the bonds in O2
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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