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: Principles and Mechanisms (Second Edition)
- Which of the molecules are polar in attached problem?arrow_forwardTo preview the image Click Here t A) For the indicated Carbon atom, give its hybridization and a list of all hybridized and unhybridized atomic orbitals and how each orbital is used for this atom. B) REDRAW the structure on your paper. Directly ON TOP of the structure, draw pictorial representation of the T for the localized bonding molecular orbitals for the bond that is indicated in the following structure. State the atomic orbitals that are used to build the molecular orbitals. Part B CEC-H Part A pointing to this carbonarrow_forwardPlease answer this asap.. you can see the example on the other picture Instruction: Identify the hybrid orbitals used in the given moleculesarrow_forward
- Would each end of the bond line structure be carbon? Is problem (a) correct?arrow_forwardIn the spaces provided, indicate the type of bond, and the hybridized orbitals that overlap to form the bond.arrow_forwardX Answered - Incorrect • 1 attempt left In the given reactions is the starting material being oxidized, reduced or is there no change in the oxidation state? O Drag and drop options on the right- hand side to reorder and match with items on the left. Reordering may cause items on the right-hand side to swap positions. 1. Oxidized Reduced Oxidized Reduced No change in oxidation state X Your answer OH 1) H. он 2) 3) II 2. 3.arrow_forward
- Below are two sets of resonance structures. Where applicable provide the missing curved arrow notation, lone pair electrons, and nonzero formal charge. Do not delete or add any bonds or atoms.arrow_forwardDraw each of the species in Problem as a condensed formula.arrow_forwardFor the molecule shown, what orbital is the lone pair in?arrow_forward
- The instructions are to draw the resonance hybrid structure of the molecule on the left. My answer is circled , which is wrong. Can someone explain why?arrow_forward( find pount group of each of the molecule with detail explanationarrow_forward• Show all significant resonance contributors and a resonance hybrid for the following molecule.arrow_forward
- Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning