Custom eBook for Organic Chemistry
2nd Edition
ISBN: 9798214171104
Author: Straumanis
Publisher: Cengage Custom
expand_more
expand_more
format_list_bulleted
Concept explainers
Textbook Question
Chapter 1, Problem 20CTQ
A student who missed this class needs to know how to predict the bond angles and shape of amolecule from looking at its bond-line representation. Write a concise but complete explanationfor this student.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
ELECTRONIC STRUCTURE AND CHEMICAL BONDING
Predicting the arrangement of electron groups around the centr...
Answer the questions in the table below about the shape of the hydrogen cyanide (HCN) molecule.
How many electron groups are around the central carbon atom?
Note: one "electron group" means one lone pair, one single bond,
one double bond, or one triple bond.
What phrase best describes the arrangement of these electron
groups around the central carbon atom?
(You may need to use the scrollbar to see all the choices.)
(choose one)
X
Ś
The molecular structure of hinokitiol is represented below (See attached image)
Draw a complete Lewis structure of the molecule and answer the following questions.
Complete the structure by adding ONLY hydrogen atoms to carbon atoms where needed. You must not create any other bonds. Atoms such as oxygen or nitrogen may have lone pairs to complete their octets.
Each of the non-hydrogen atoms of this skeletal structure has been randomly numbered.
Match the atom number with the orbital hybridization invoked for sigma bonding.
Match these to the below (A)) (Options: sp3, sp2, sp, s, p, d2sp3, dsp3)
A) 12, 9, 7, 2, 4
B) How many pairs of non-bonding electrons are there in the molecule?
C) How many CH3 (methyl) groups are there in the molecule?
D) How many CH2 (methylene) groups are there in the molecule? (i.e. # of C-atoms having exactly two bonded H-atoms)
E) How many CH (methyne) groups are there in the molecule? (i.e. # of C-atoms having exactly one bonded H-atom)
F) How many…
I already answered the first part which was satisfying the balances filling in the double and triple bonds as well as the unshared electron pairs, as you can see in the second picture I have written those answers and pin. I’m having trouble with converting the Lewis structure into bondline structures if you could please help me out I would appreciate it.
Chapter 1 Solutions
Custom eBook for Organic Chemistry
Ch. 1 - (E) What does the number (+Z) at the center of...Ch. 1 - Prob. 2CTQCh. 1 - Prob. 3CTQCh. 1 - Prob. 4CTQCh. 1 - Prob. 5CTQCh. 1 - Prob. 6CTQCh. 1 - Prob. 7CTQCh. 1 - You hear a student from a nearby group say that...Ch. 1 - Use VSEPR to explain why the HBH bond angle of BH3...Ch. 1 - Both the HCH and HCO bond angles of H2CO...
Ch. 1 - Prob. 11CTQCh. 1 - Consider the following flat drawing of methane...Ch. 1 - Use VSEPR to assign a value of (close to) 109.5,...Ch. 1 - A student draws the picture of ammonia (NH3) in...Ch. 1 - Prob. 15CTQCh. 1 - How many central atoms does the molecule H2NCH3...Ch. 1 - Indicate the bond angle and shape about each...Ch. 1 - Explain how there can be two kinds of bent:...Ch. 1 - A student makes the following statement: “The...Ch. 1 - A student who missed this class needs to know how...Ch. 1 - Prob. 1ECh. 1 - Prob. 2ECh. 1 - Consider the incomplete valence shell...Ch. 1 - How many valence electrons does a neutral a. K...Ch. 1 - Consider the molecules AlCl3 (aluminum chloride)...Ch. 1 - Draw an example of a bent molecule with a bond...Ch. 1 - Label each atom marked with an arrow with the...Ch. 1 - a model of each of the following molecules: a....
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
- A student draws the picture of ammonia (NH3) in the box below, left, and predicts it will be a flatmolecule with HNH bond angles of exactly 120°. Unfortunately, the student left something out. a. What did the student omit from his drawing? b. What is the actual HNH bond angle of ammonia (based on the draw g above, right)? c. Explain why water, ammonia, and methane (shown below) all have about the same bondangles (close to 109.5°) even though they have different numbers of bonds.arrow_forwardWould you mind to check all the answer on this table because I try to understand the line bond structure and re-draw structure my homework? Could you help me with this question CS2?arrow_forwardNF3?arrow_forward
- For each of the Lewis structures shown below, predict the Electron Geometry, Molecular Geometry and Bond Angle. Lastly, using the same format as shown in the last column of Table 1, draw a sketch (using wedges and dashes to show 3D if needed) of the Molecular Geometry.arrow_forwardCould you try to explain in 3-4 sentences or less if possible?arrow_forwardA model for SiH4 is shown in the chem3D window. SiH4 has tetrahedral geometry. ball & stick |+ labels Rotate the molecule until you have a feeling for its three-dimensional shape. How many atoms are bonded to the central atom? If you take any three of the outer atoms, what shape do they define? | Consider the bond angles at the central atom. Do they all have the approximately the same numerical value? What is the approximate numerical value of this angle? | degrees. Are all four positions about the central atom equivalent, or is one of them different from the other three. For practice, type in the name of the geometry of the molecule: Previous Nextarrow_forward
- Please in paragraph form explain how we can know how many hydrogen atoms are bonded to a carbon atom in a line angle formula given that our equation is C5H12. I need detail and you to elaborate on how to identify the amount of hydrogen atoms can bondarrow_forwardI would like to you help me with my homework because I struggled with step 6. Can you help me with step 6, please?arrow_forwardGive me detailed Solution with explanation needed..don't give Handwritten answer.....draw the Lewis structure alsoarrow_forward
- I would like to you help me with my homework because I struggled with step 6. Can you help me with step 6, please?arrow_forwardIII. Determine the molecular geometry of the encircled atom in the following organic molecules by giving the required information in the table below: (Type your answers except for the Lewis structure. Draw the Lewis structure in a sheet of paper, scan copy or shot a picture of it and paste it next page.) LEWIS ELECTRON PAIR MOLECULAR MOLECULE STRUCTURE GEOMETRY SHAPE (4) CHs-CH-CH2-CNH-CH3 CH2CH3 (5) ATOM' 'ALENCE ELECTRON NO. OF BONDING PAIRS NO. OF NON- BONDING PAIRS TOTAL ELECTRON GENERAL FORMULA BOND ANGLE HYBRID ORBITALarrow_forwardA resonance hybrid is a structure that can be depicted by more than one valid Lewis structure. part1: Draw the major resonance form of fulminic acid, HCNO, with the atoms connected as indicated in the formula. Your structure should have nonzero formal charges minimized, and it should include all nonzero formal charges and all nonbonding electrons. part2: Draw the second most important resonance form of fulminic acid, HCNO, with the atoms connected as indicated in the formula. Your structure should have nonzero formal charges minimized, and it should include all nonzero formal charges and all nonbonding electrons. part3: Draw the least important resonance contributor for fulminic acid, HCNO, with the atoms connected as indicated in the formula. Your structure should have nonzero formal charges minimized and should include all nonzero formal charges and all nonbonding electrons.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningPrinciples of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub CoChemistry for Today: General, Organic, and Bioche...ChemistryISBN:9781305960060Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. HansenPublisher:Cengage Learning
Organic Chemistry: A Guided Inquiry
Chemistry
ISBN:9780618974122
Author:Andrei Straumanis
Publisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Chemistry: Matter and Change
Chemistry
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Glencoe/McGraw-Hill School Pub Co
Chemistry for Today: General, Organic, and Bioche...
Chemistry
ISBN:9781305960060
Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen
Publisher:Cengage Learning
Stoichiometry - Chemistry for Massive Creatures: Crash Course Chemistry #6; Author: Crash Course;https://www.youtube.com/watch?v=UL1jmJaUkaQ;License: Standard YouTube License, CC-BY
Bonding (Ionic, Covalent & Metallic) - GCSE Chemistry; Author: Science Shorts;https://www.youtube.com/watch?v=p9MA6Od-zBA;License: Standard YouTube License, CC-BY
General Chemistry 1A. Lecture 12. Two Theories of Bonding.; Author: UCI Open;https://www.youtube.com/watch?v=dLTlL9Z1bh0;License: CC-BY