Organic Chemistry: A Guided Inquiry
2nd Edition
ISBN: 9780618974122
Author: Andrei Straumanis
Publisher: Cengage Learning
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Chapter 7, Problem 13CTQ
Interpretation Introduction
Interpretation: The cyclic alkane which is most commonly found in nature needs to be determined and explained.
Concept Introduction: The stability of the cyclic alkane depends on the ring strain energy. For cyclic
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So I cant see any of the answers on section 4.41 D, F, G In the
Organic Chemistry: Principles And Mechanisms (second Edition)
2nd Edition
Textbook. Would you be able to just send me the answers and images. I have already done them and I am practicing for class but I dont know if I am correct.
1) In this problem, you will compare Lewis/VSEPR theory and Covalent Bond theory to
experimental data. The experimental photoelectron data for Ne, HF, H.O, NH,, and CH. are
shown below. Photoelectron spectroscopy measures the filled Orbitals of a molecule. For
each molecule, draw the structure using Lewis formalisms and give the geometry using
VSEPR structure. Answer questions regarding Lewis/VSEPR prediction using this structure
combined with your assigned point group for the structure.
10
18
NH3
CH₂
H₂O
Ne
26
HF
34
Ionisation energy (eV)
Neon
a) Draw the Lewis/VSEPR structure for Ne.
42
b) How many separate electron energy levels does the Lewis/VSEPR structure predict?
c) Write down the electron configuration for Neon.
d) For each major feature observed in the spectrum, give the energy of the transition and
assign the orbital(s) from which the electron comes.
To preview the image
Part 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.
Part B-1) REDRAW the structure on your paper. Directly ON TOP of
the structure, draw a picture of the for electrons for both 7-
bonding and m*-anti-bonding orbitals.
Part B-2) Clearly indicate positions of any nodes.
Part A
Pointing to this carbon
Part B
Pointing to these electrons
л-bonding and *-antibonding
Chapter 7 Solutions
Organic Chemistry: A Guided Inquiry
Ch. 7 - Prob. 1CTQCh. 7 - Prob. 2CTQCh. 7 - Prob. 3CTQCh. 7 - Draw wedge and dash skeletal representations of...Ch. 7 - Label each ring in Figure 7.2 cis or trans.Ch. 7 - Prob. 6CTQCh. 7 - Prob. 7CTQCh. 7 - Prob. 8CTQCh. 7 - a model of cyclohexane in a chair conformation,...Ch. 7 - Prob. 10CTQ
Ch. 7 - Prob. 11CTQCh. 7 - Fill in the blanks: cis-1,3-Dimethylcyclohexane...Ch. 7 - Prob. 13CTQCh. 7 - Prob. 14CTQCh. 7 - Prob. 15CTQCh. 7 - Prob. 16CTQCh. 7 - Prob. 17CTQCh. 7 - Prob. 18CTQCh. 7 - Draw chair representations of...Ch. 7 - Which stereoisomer in the previous question is...Ch. 7 - Prob. 21CTQCh. 7 - Prob. 1ECh. 7 - Label each of the following as cis, trans or...Ch. 7 - Which pair has more in common with one another?Ch. 7 - Prob. 4ECh. 7 - Prob. 5ECh. 7 - Prob. 6ECh. 7 - Fill in the table by drawing a representation of a...Ch. 7 - Prob. 9ECh. 7 - True or False: If you perform a chair flip on...Ch. 7 - Prob. 11ECh. 7 - Prob. 12ECh. 7 - Prob. 13ECh. 7 - Prob. 14ECh. 7 - Prob. 15ECh. 7 - Draw trans-1-tert-butyl-3-methylcyclohexane in its...Ch. 7 - Build a model of methylcyclohexane, and use the...
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- a) Draw Lewis structures for each of the compounds below. Be sure to show all bonding and non-bonding valence electrons. Also, clearly indicate any formal charges on atoms. b) Consider the molecular geometry information given for each compound below: based on this information, specify the orbitals that each atom could use in σ- and à-bonding (sp², sp³, p, etc.) and for holding non-bonding electron pairs. Explain how your orbital assignments are consistent with the observed geometries. H₂CO (formaldehyde) HCO-angle 120⁰ CH3CO₂ (acetate anion) HCC-angle ≈ 109⁰ CCO-angle OCO≈ 120° DCH=CHBr(1-bromo-2-deuterioethylene) (two isomers) (all atoms are coplanar) (CH3)2SO (dimethylsulfoxide, DMSO) HCS-angle CSO CSC≈ 109⁰ ≈arrow_forward2.State the two main experiments that were used to establish the extra stability of the benzene moleculearrow_forwardFor this molecule complete the following: a. Use Valence Bond theory to write the atomic energy level or orbital diagrams for the Nitrogen atom and for this Carbon atom before hybridization and after hybridization. b. Use Valence Bond theory to draw a diagram of this molecule. Show and label all orbitals involved in bonding and identify each bond type. You may want to use a separate sheet of paper and draw in landscape mode. Be sure that your drawing is something I can easily read and interpret.arrow_forward
- A. Classify the following molecules as polar or non-polar (write below the chemical formula in the first column. Explain your answer in terms of the (a) Lewis structure (b) molecular geometry and (c) bond polarity. (You can add rows if you need more spaces for your explanation.) Hint: Although I am not asking you to give the no. of bonding and non-bonding pairs, you have to do it to be able to identify the electron pair geometry and molecular geometry. Note: Items #1 to #4 are hypothetical molecules. The number of valence electron/s of the hypothetical atoms are given in parenthesis.) There is no need to give actual molecules to represent them. Polar or Non-polar Explanation 1. .arrow_forwardA. Classify the following molecules as polar or non-polar (write below the chemical formula in the first column. Explain your answer in terms of the (a) Lewis structure (b) molecular geometry and (c) bond polarity. (You can add rows if you need more spaces for your explanation.) Hint: Although I am not asking you to give the no. of bonding and non-bonding pairs, you have to do it to be able to identify the electron pair geometry and molecular geometry. Note: Items #1 to #4 are hypothetical molecules. The number of valence electron/s of the hypothetical atoms are given in parenthesis.) There is no need to give actual molecules to represent them. Polar or Non-polar Explanation 1. nodarrow_forwardA. Classify the following molecules as polar or non-polar (write below the chemical formula in the first column. Explain your answer in terms of the (a) Lewis structure (b) molecular geometry and (c) bond polarity. (You can add rows if you need more spaces for your explanation.) Hint: Although I am not asking you to give the no. of bonding and non-bonding pairs, you have to do it to be able to identify the electron pair geometry and molecular geometry. Note: Items #1 to #4 are hypothetical molecules. The number of valence electron/s of the hypothetical atoms are given in parenthesis.) There is no need to give actual molecules to represent them. 田 Polar or Non-polar Explanation 1. QR (Q=1, R=7)arrow_forward
- (a) In one of the two boxes below, draw a wedge and dashed wedge structure (picture) of CH3Cl that best illustrates the geometry about the central atom. In the other box, draw another picture of the model from a different angle (viewpoint). (b) In CH3Cl, are the three hydrogen atoms equivalent (i.e., do they have identical environments with respect to the other atoms adjacent to themselves)? Briefly explain the evidence for your answerarrow_forward2. Use the curved arrow formation to show how the electrons flow in the distance from on the left to give the one on the rightarrow_forwardA. Classify the following molecules as polar or non-polar (write below the chemical formula in the first column. Explain your answer in terms of the (a) Lewis structure (b) molecular geometry and (c) bond polarity. (You can add rows if you need more spaces for your explanation.) Hint: Although I am not asking you to give the no. of bonding and non-bonding pairs, you have to do it to be able to identify the electron pair geometry and molecular geometry. Note: Items #1 to #4 are hypothetical molecules. The number of valence electron/s of the hypothetical atoms are given in parenthesis.) There is no need to give actual molecules to represent them. Polar or Non-polar Explanation 1. Z2 (Z =7)arrow_forward
- he structure of 1,2-propadiene (allene) is shown to the right. Q.) Predict all approximate bond angles in this molecule.arrow_forward3. Which of the following molecules are conjugated? For those which are conjugated, write a resonance structure.arrow_forwardA reaction can take place and a new bond is formed when an electron rich species attacks an electron poor species. With this in mind, explain the following molecular orbital energy diagram. The "n" orbital refers to the nonbonding electrons on oxygen (electron rich), which is slightly higher in energy than the bonding electrons in the C=0 bond. Apply what you know, and think a little outside of the box.arrow_forward
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