(b)2.(C) Assign the hybridization, number of p orbitals remaining following hybridization, andHybridization and MOSformal charge for nitrogen and carbon 1 in the molecule below.H₂-CH₂NHHAtomHybridization(sp, sp², or sp³)Carbon 1Nitrogen# p orbitalsremaining(0, 1, 2, or 3)Formal charge(0, -1, or +1)σCircle all types of molecular orbitals that are present in this moleculeπ(c) (1) Circle the HOMO of the molecule in (a):σπ(d) ) Circle the LUMO of the molecule in (a):σπσ'ποnonbondingποnonbondingπ"HO

Part (a): Hybridization, Number of p Orbitals Remaining, and Formal ChargeIn the molecule, you have…

Answered: (b) 2. (C) Assign the hybridization,…

Organic Chemistry

9th Edition

ISBN:9781305080485

Author:John E. McMurry

Publisher:John E. McMurry

Chapter24: Amines And Heterocycles

Section24.9: Heterocyclic Amines

Problem 20P: Draw an orbital picture of thiazole. Assume that both the nitrogen and sulfur atoms are...

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H genistein HO, H H : ОН HO, H (a) Is the hybridization of each C in the right-most ring the same? Explain. (b) Is the hybridization of the O atoms in/on the center ring the same as that of the O atoms in the OH groups? Explain. (c) How many carbon-oxygen o-bonds are there in genistein? How many carbon-oxygen n-bonds? (d) Do all the lone pairs on the oxygens occupy the same type of hybrid orbital? Explain by labeling the hybridization of each oxygen atom in genistein.
For each of the following structures, determine the hybridization requested and whether the electrons will be delocalized: (a) Hybridization of each carbon н :0: Н | || | Н—с—с——н H. (b) Hybridization of sulfur (c) All atoms EN: H.
3) Which statement best describe the structure of a carbonate anion C02- ? A) The electron geometry of carbon in a carbonate anion is trigonal planar with a sp2 hybridization and bond angles are 120°. There is a n-bond formed between a non-hybridized "C" p-orbital overlapping with an "O" p-orbital. C) The electron geometry of carbon in a carbonate anion is trigonal planar with a sp2 hybridization and bond angles are 120°. There is a 7-bond formed between a non-hybridized “C" p-orbital overlapping with an “O" p-orbital.
The unmistakable odor of a freshly cut cucumber is largely due to cucumber aldehyde.(a) How many sp2 hybridized carbon atoms does cucumber aldehyde contain? (b) What is the hybridization of the O atom? (c) What orbitals are used to form the carbon–oxygen double bond? (d) How many σ bonds does cucumber aldehyde contain? (e) How many πbonds does it contain?
Use an MO diagram and the bond order you obtain from it to answer: (a) Is O2- stable? (b) Is O2- paramagnetic? (c) What is the outer (valence) electron configuration of O2-?
The unmistakable odor of a freshly cut cucumber is largely due to cucumber aldehyde. (a) How many sp2 hybridized carbon atoms does cucumber aldehyde contain? (b) What is the hybridization of the O atom? (c) What orbitals are used to form the carbon–oxygen double bond? (d) How many σ bonds does cucumber aldehyde contain? (e) How many π bonds does it contain?
The unmistakable odor of a freshly cut cucumber is largely due to cucumber aldehyde. (a) How many sp2 hybridized carbon atoms does cucumber aldehyde contain? (b) What is the hybridization of the O atom? (c) What orbitals are used to form the carbon–oxygen double bond? (d) How many σ bonds does cucumber aldehyde contain? (e) How many π bonds does it contain?
(a) Identify which atomic orbitals are used to construct the specified o bonds: Bond a is: b Bond a is: OH bond b is: Identify which orbital is used to construct the л-bond at the marked atom. (b) Identify which atomic orbitals are used to construct the specified & bonds: a and bond c is: OH bond b is: and bond c is: Identify which orbital is used to construct the л-bond at the marked atom.
The ground-state electron configuration of the H; molec- ular ion is (og15)'. (a) A molecule of H absorbs a photon, promoting the electron to the os molecular orbital. Predict what happens to the molecule. (b) Another molecule of H absorbs even more energy promoting the electron to the o,2, molecular orbital. Predict what happens to this molecule.
Use MO diagrams and the bond orders you obtain fromthem to answer: (a) Is O₂⁻ stable? (b) Is O₂⁻ paramagnetic? (c) What is the outer (valence) electron configuration of O₂⁻?
Estimate whether the compound will have a large, small, or zero dipole moment. (a) CF4(b) CH3CHO(c) CH2“CHCl
(a) What is the difference between a localized p bond and adelocalized one? (b) How can you determine whether a moleculeor ion will exhibit delocalized p bonding? (c) Is the pbond in NO2- localized or delocalized?

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