Concept explainers
(a)
Interpretation:
The hybridization of each carbon and oxygen atom in aspirin is to be determined.
Concept introduction:
Hybridization is the process of intermixing of atomic orbital of slightly different energies to form hybrid orbitals that have similar energy. These orbital have lower energy and more stability than the atomic orbital.
Hybridization of the central atom can be determined from the number of electron groups around the central atom in the Lewis structure of the molecule. Single bond, double bond, triple bond and lone pair all are considered as single electron group.
(b)
Interpretation:
The number of localized pi bonds in aspirin is to be determined.
Concept introduction:
The sigma bond is the covalent bond that is formed by the axial overlap of orbitals. The pi bond is formed by the lateral overlap of orbitals. Both types of bonds can be bonding or anti-bonding interaction. Bonding interaction takes place when there is an overlap of orbitals in the same phase and antibonding interaction occurs when the orbital overlap in opposite phase. Sigma bond is stronger than the pi bond.
All single bonds are sigma bonds. One double bond is made up of one sigma bond and one pi bond. One triple bond is made up of one sigma bond and two pi bonds.
(c)
Interpretation:
The number of carbon atoms that have a trigonal planar shape and a tetrahedral shape is to be determined.
Concept introduction:
Hybridization is the process of intermixing of atomic orbital of slightly different energies to form hybrid orbitals that have similar energy. These orbital have lower energy and more stability than the atomic orbital.
Hybridization of the central atom can be determined from the number of electron groups around the central atom in the Lewis structure of the molecule. Single bond, double bond, triple bond and lone pair all are considered as single electron group.
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Loose Leaf for Chemistry: The Molecular Nature of Matter and Change
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