Concept explainers
(a)
Interpretation:
Hybridization of the indicated atom in the given molecule is to be determined.
Concept introduction:
Atomic orbitals mix and form an equal number of hybrid orbitals. The number of hybrid orbitals required by an atom in a molecule or an ion is equal to the number of electron groups in its valence shell. In case of atoms from the second row, like carbon, these are formed by mixing of one s AO and the necessary number of p AO(s).
An electron group is a lone pair or a bond. The bond, whether single, double, or triple, counts as just one electron group.
(b)
Interpretation:
Hybridization of the indicated atom in the given molecule is to be determined.
Concept introduction:
Atomic orbitals mix and form an equal number of hybrid orbitals. The number of hybrid orbitals required by an atom in a molecule or an ion is equal to the number of electron groups in its valence shell. In case of atoms from the second row, like carbon, these are formed by mixing of one s AO and the necessary number of p AO(s).
An electron group is a lone pair or a bond. The bond, whether single, double, or triple, counts as just one electron group.
(c)
Interpretation:
Hybridization of the indicated atom in the given molecule is to be determined.
Concept introduction:
Atomic orbitals mix and form an equal number of hybrid orbitals. The number of hybrid orbitals required by an atom in a molecule or an ion is equal to the number of electron groups in its valence shell. In case of atoms from the second row, like carbon, these are formed by mixing of one s AO and the necessary number of p AO(s).
An electron group is a lone pair or a bond. The bond, whether single, double, or triple, counts as just one electron group.
(d)
Interpretation:
Hybridization of the indicated atom in the given molecule is to be determined.
Concept introduction:
Atomic orbitals mix and form an equal number of hybrid orbitals. The number of hybrid orbitals required by an atom in a molecule or an ion is equal to the number of electron groups in its valence shell. In case of atoms from the second row, like carbon, these are formed by mixing of one s AO and the necessary number of p AO(s).
An electron group is a lone pair or a bond. The bond, whether single, double, or triple, counts as just one electron group.
(e)
Interpretation:
Hybridization of the indicated atom in the given molecule is to be determined.
Concept introduction:
Atomic orbitals mix and form an equal number of hybrid orbitals. The number of hybrid orbitals required by an atom in a molecule or an ion is equal to the number of electron groups in its valence shell. In case of atoms from the second row, like carbon, these are formed by mixing of one s AO and the necessary number of p AO(s).
An electron group is a lone pair or a bond. The bond, whether single, double, or triple, counts as just one electron group.
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ORGANIC CHEMISTRY E-BOOK W/SMARTWORK5
- The molecule shown here has quite a large dipole, as indicated in its electrostatic potential map. Explain why.Hint: Consider various resonance structures.arrow_forwardWhat is the hybridizarion of the atom labeled with arrow in each of the following molecules?arrow_forwardDraw each of the species in Problem as a condensed formula.arrow_forward
- Please draw a more stable resonance structure for the following molecule. Use a curved arrow to show how to transform the original structure to the new one and please specify charges.arrow_forwardGive a clear handwritten answer with explanation....given below some compounds choose which compound is contains sp2 hybridized carbon atom...?arrow_forwardPlease answer this asap.. you can see the example on the other picture Instruction: Identify the hybrid orbitals used in the given moleculesarrow_forward
- Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning