Organic Chemistry: A Guided Inquiry
2nd Edition
ISBN: 9780618974122
Author: Andrei Straumanis
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
Chapter 2, Problem 8CTQ
Interpretation Introduction
Interpretation : Whether both structures of carbon dioxide in Model 2 are legitimate structures or not should be discussed.
Concept Introduction : A legitimate Lewis structure is an electron dot and line bond representation in which the total number of valence electrons is indicated. The number of valence electrons around hydrogen is two. The number of valence electrons around carbon, nitrogen, oxygen, fluorine atom is eight. This is called the octet rule.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
How many valence electrons are there in a correctly drawn Lewis structure for formamide, HCONH2
( You should also be able to draw the lewis structure for this. Hint, the C is in the center with an O ,N and 1 H attached. The other H atoms are attached to the N)
II. Please expand each of the following bond-line formulas to the corresponding
standard Lewis structure, be sure to show all the bonds and unshared electron pairs
as well as formal charges, if it applies.
0:
(a)
(c)
O
Br
|
Br-B-Br
-N-
(b)
HO:
NO₂
0:
blos ohsup?
The resonance structures shown below have all lone pairs drawn in, but are missing formal
charges. What is the formal charge on (A) the carbon on the left
, (B) the
nitrogen on the left
(C) the carbon on the right
, and
(D) the nitrogen on the right
A
B
HC
DH
C-N
C=N
H.
H.
H
Chapter 2 Solutions
Organic Chemistry: A Guided Inquiry
Ch. 2 - Prob. 1CTQCh. 2 - The valence shell of an atom in a legitimate Lewis...Ch. 2 - Prob. 3CTQCh. 2 - Prob. 4CTQCh. 2 - Prob. 5CTQCh. 2 - It is impossible to draw a legitimate Lewis...Ch. 2 - Describe how to calculate the total number of...Ch. 2 - Prob. 8CTQCh. 2 - Prob. 9CTQCh. 2 - Prob. 10CTQ
Ch. 2 - Prob. 11CTQCh. 2 - Prob. 12CTQCh. 2 - A complete Lewis structure must show all nonzero...Ch. 2 - Prob. 14CTQCh. 2 - Prob. 15CTQCh. 2 - Prob. 16CTQCh. 2 - Prob. 17CTQCh. 2 - Prob. 18CTQCh. 2 - Complete the rest of the table for N, O or X by...Ch. 2 - Prob. 20CTQCh. 2 - Prob. 21CTQCh. 2 - Make a checklist that can be used to determine if...Ch. 2 - Prob. 2ECh. 2 - Prob. 3ECh. 2 - Draw the Lewis structure of a neutral molecule...Ch. 2 - Prob. 5ECh. 2 - For each element, predict (and draw a Lewis...Ch. 2 - Predict which of the following species is least...Ch. 2 - The molecules BH3 and SF6 and the ion SO42 exist...Ch. 2 - These are NOTlegitimate Lewisstructures (and...Ch. 2 - Fill in missing formal charges where needed (all...Ch. 2 - Below each structure in the previous question is a...Ch. 2 - Prob. 12ECh. 2 - Carbon monoxide (CO) is an example of an overall...Ch. 2 - Explain why this Lewis structure for CO is not as...Ch. 2 - Prob. 15ECh. 2 - Prob. 16ECh. 2 - Prob. 17ECh. 2 - Prob. 18ECh. 2 - Prob. 19E
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- ClO2F2+(a) Draw all of the possible Lewis structures (including reasonance structures) of the following compounds.(b) Label the formal charge for each atom.(c) Determine which resonance structure(s) is(are) the better/best and briefly explain. Question 5. Finish the questions regarding the molecule/ion in Question 4 above. (a) Draw the best Lewis structure with a three-dimensional fashion by using dash and solid wedges.(b) Name the electron geometry and molecular geometry of the molecules. Identify the bond angles. Note: For the non-standard bond angels, use “<” or “>” to suggest the deviation of the bond angles from the standard bond angel. (c) Determine wether the molecule is molecule is polar or non-polar. Briefly explain.arrow_forward5a. Draw the best Lewis structure for the following acids (hint!: the acidic H is bonded to O in an acid). Evaluate each atom using formal charge, showing your math work as well as your formal charge answers. H3PO4 H2SO4 5b. The N3- ion can be drawn with two double bonds, or with a single bond and a triple bond. Both structures satisfy the octet rule. Use formal charge to evaluate the structures. Which do you think is the better choice? Give reasons to support your choice. Please answer both parts.arrow_forwardFor each of the following covalent bonds: (a) use the symbols δ+ and δ- to indicate the direction of polarity (if any).(a) C-F; (b) N-Br; (c) B-C; (d) Si-H(b) Rank the following covalent bonds in order of increasing polarity. (i) C-H, O-H, N-H; (ii) C-N, C-O, B-O; (iii) C-P, C-S, C-Narrow_forward
- Draw Lewis structures for each of the following ions. One atom in each ion has a formal charge that is not zero.Determine which atom it is, and what the formal charge is. (a) the C2H5 anion; (b) the CH3O cation; (c) the CH6N cation;(d) the CH5O cation; (e) the C3H3 anion (all three H atoms are on the same carbon)arrow_forward3a.Draw the best Lewis structure for the HClO3 acid molecule. (Hint: the acidic H is bonded to O in an oxy-acid molecule).Evaluate each atom using formal charge to prove you have the best structure. Show your math work as well as your formal charge answers. 3b. Draw all the resonance structures for the ClO3– polyatomic anion. (Hint: make sure you have the best initial structure first!)arrow_forward7) 2 OH- H.arrow_forward
- In the following Lewis structure of [SiF6]², every atom, bond and lone pair is positioned. To complete the structure, drag the formal charge tags to the appropriate atom(s). Each marker may be used more than once, or not at all. If an atom has a formal charge of zero, do not drag a tag to it. When you drag the marker in, place the little crosshairs in the upper left corner of the marker directly over the atom(s) in question (not above them). :F: :F : :ד: Si 1 :F: 0 0 0 2+ :H: Ë: 0 2-arrow_forward1₁ 9) CNN B G O Bond H-O C=C H-C C-C C-O This question has multiple parts. Work all the parts to get the Enthalpy change COWLV2... 2-Propanol can be made by the reaction of propene and water: CH3-HC=CH₂(g) + H₂O(g) → CH3 CH(OH)CH3(g) a Use bond dissociation enthalpies to estimate the enthalpy change in this reaction. ΔΗ (kJ/mol) Substance 463 610 413 346 358 CH3 CH(OH)CH3(g) Enthalpy change = b Calculate the enthalpy change for this reaction from enthalpies of formation. Af H (kJ/mol) H₂O(g) CH3-H₂C=CH₂(g) KJ * prod03-cnow-owl.cengagenow.c -272.8 -241.83 20.42 kJ Referensarrow_forward4. The following are valid Lewis structures for CH3SOCH3. Label the formal charges and circle the best Lewis structure. H :ö: H H :0 H a) H-C=S-C-H b) Н—С—S— С-н H. H. H. H. Н :0: Н H :ö: H d) H-C=$-C-H c) Н—С—$—С-н H. H. H Harrow_forward
- Draw the correc (best) Lewis structure (LS) for the ionic compound K2SeO3 (on looose leaf paper--NOT TO BE SUBMITTED) and then answer the following questions.(NOTE: Use the cardinal numbers 0, 1, 2, 3, and so on for any quantity required)a) What charge does the K ion have in this compound? (give size & sign of charge: e.g., 1+, 2-, etc.) b) What charge does the SeO3 ion have in this compound? (give size & sign of charge: e.g., 1+, 2-, etc.) c) How many lines, if any, attach each K ion to the SeO3 ion? d) How many valence electrons does the SeO3 ion (alone) have? e) How many single bonds does the LS of the SeO3 ion have? f) What is the number of lone electron pairs in the LS of the SeO3 ion?arrow_forwardDraw a Lewis structure of sodium isopropoxide (NaOCH (CH3)2). Be sure to show all relevant formal charges and lone pairs! (Na OCH(CH3)₂) Ⓒ Naarrow_forwardChoose the best Lewis structure for C2H30¯. (It will help to work out the missing formal charges for the atoms in these different structures) [Image description: Lewis structure A two C atoms doubly bound to each other. One C has two other single bonds to H atoms. The other C has one more single bond to a H atom and one more single bond to a O atom. There are three electron pairs on O. Lewis structure B has a C atom and a O atom doubly bound to each other. The C has two other single bonds to H atoms. The O has one more single bond to a H atom and one more single bond to a C atom. There are three electron pairs on this C. Lewis structure C has a O atom and a C atom doubly bound to each other. The O has two other single bonds to H atoms. The C has one more single bond to a H atom and one more single bond to another C atom. There are three electron pairs on this C. Lewis structure D has two C atoms singly bound to each other. One C has an electron pair plus two more single bonds to H…arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY