Organic Chemistry-Package(Custom)
4th Edition
ISBN: 9781259141089
Author: SMITH
Publisher: MCG
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Textbook Question
Chapter 1, Problem 1.80P
The principles of this chapter can be applied to organic molecules of any size. Answer the following questions about amoxicillin, an antibiotic from the penicillin family.
a. Predict the hybridization and geometry d. How many
around each indicated atom. Label them.
b. Label five polar bonds using the e. Find a
symbols
c. Draw the skeletal structure.
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Answer the following questions about amoxicillin, an antibiotic from the penicillin family.
a. Predict the hybridization and geometry around each highlighted atom.
b. Label five polar bonds using the symbols δ+ and δ–.
c. How many π bonds does amoxicillin have? Label them.
d. Find a C – H bond containing a carbon atom having a hybrid orbital with 33% s-character
B. Answer the next two questions about the Lewis structure
of XYZ shown below.
メー三
-YEz:
I. What is the hybridization of the central atom?
II. For all covalent bonds, specify the type of bond (o vs. T)
and the atomic orbitals that overlap to form the bond.
For example, in a molecule of H2, the only bond is o:
H(s)-H(s).
Find the hybrid orbital type for each atom, the carbon-carbon-oxygen bond angle, the molecular geometry of oxygen, and the number of sigma and pi bonds in the molecule.
Chapter 1 Solutions
Organic Chemistry-Package(Custom)
Ch. 1 - While the most common isotope of nitrogen has a...Ch. 1 - Label each bond in the following compounds as...Ch. 1 - How many covalent bonds are predicted for each...Ch. 1 - Draw a valid Lewis structure for each species. a....Ch. 1 - Draw an acceptable Lewis structure for each...Ch. 1 - Prob. 1.6PCh. 1 - Draw a Lewis structure for each ion. a. CH3Ob....Ch. 1 - Draw Lewis structures for each molecular formula....Ch. 1 - Prob. 1.9PCh. 1 - Prob. 1.10P
Ch. 1 - Prob. 1.11PCh. 1 - Prob. 1.12PCh. 1 - Draw a second resonance structure for each...Ch. 1 - Prob. 1.14PCh. 1 - Draw a second resonance structure for nitrous...Ch. 1 - Prob. 1.16PCh. 1 - Prob. 1.17PCh. 1 - Prob. 1.18PCh. 1 - Prob. 1.19PCh. 1 - Prob. 1.20PCh. 1 - Simplify each condensed structure by using...Ch. 1 - Prob. 1.22PCh. 1 - Prob. 1.23PCh. 1 - Convert each skeletal structure to a complete...Ch. 1 - Draw in all hydrogens and lone pairs on the...Ch. 1 - Prob. 1.26PCh. 1 - What orbitals are used to form each of the CC, and...Ch. 1 - What orbitals are used to form each bond in the...Ch. 1 - Determine the hybridization around the highlighted...Ch. 1 - Classify each bond in the following molecules as ...Ch. 1 - Prob. 1.31PCh. 1 - Rank the following atoms in order of increasing...Ch. 1 - Prob. 1.33PCh. 1 - Prob. 1.34PCh. 1 - Provide the following information about...Ch. 1 - Use the ball-and-stick model to answer each...Ch. 1 - Citric acid is responsible for the tartness of...Ch. 1 - Zingerone gives ginger its pungent taste. a.What...Ch. 1 - Two radioactive isotopes of iodine used for the...Ch. 1 - Prob. 1.40PCh. 1 - Assign formal charges to each carbon atom in the...Ch. 1 - Assign formal charges to each N and O atom in the...Ch. 1 - Draw one valid Lewis structure for each compound....Ch. 1 - Prob. 1.44PCh. 1 - Prob. 1.45PCh. 1 - Prob. 1.46PCh. 1 - Draw all possible isomers for each molecular...Ch. 1 - 1.45 Draw Lewis structures for the nine isomers...Ch. 1 - Prob. 1.49PCh. 1 - Prob. 1.50PCh. 1 - Prob. 1.51PCh. 1 - Prob. 1.52PCh. 1 - Prob. 1.53PCh. 1 - Prob. 1.54PCh. 1 - Draw all reasonable resonance structures for each...Ch. 1 - Prob. 1.56PCh. 1 - Rank the resonance structures in each group in...Ch. 1 - 1.56 Consider the compounds and ions with curved...Ch. 1 - 1.57 Predict all bond angles in each...Ch. 1 - Predict the geometry around each indicated atom....Ch. 1 - Prob. 1.61PCh. 1 - Prob. 1.62PCh. 1 - Draw in all the carbon and hydrogen atoms in each...Ch. 1 - Prob. 1.64PCh. 1 - Prob. 1.65PCh. 1 - Prob. 1.66PCh. 1 - Prob. 1.67PCh. 1 - Each of the following condensed or skeletal...Ch. 1 - Prob. 1.69PCh. 1 - Prob. 1.70PCh. 1 - Prob. 1.71PCh. 1 - Prob. 1.72PCh. 1 - Prob. 1.73PCh. 1 - Prob. 1.74PCh. 1 - Two useful organic compounds that contain Cl atoms...Ch. 1 - Use the symbols + and to indicate the polarity of...Ch. 1 - Label the polar bonds in each molecule. Indicate...Ch. 1 - Answer the following questions about acetonitrile...Ch. 1 - Prob. 1.79PCh. 1 - The principles of this chapter can be applied to...Ch. 1 -
a. What is the hybridization of each N atom in...Ch. 1 - 1.77 Stalevo is the trade name for a medication...Ch. 1 - 1.78 and are two highly reactive carbon...Ch. 1 - 1.79 The N atom in (acetamide) is hybridized,...Ch. 1 - Prob. 1.85PCh. 1 - Prob. 1.86PCh. 1 - Prob. 1.87PCh. 1 - Prob. 1.88PCh. 1 - Prob. 1.89PCh. 1 - Prob. 1.90P
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- A molecular compound is composed of 58.8% Xe, 7.2%. O, and 34.0%. F, by mass. If the molecular weight is 223 amu, what is the molecular formula? What is the Lewis formula? Predict the molecular geometry using the VSEPR model.arrow_forwardPredict the valence electron molecular orbital configurations for the following, and state whether they will be stable or unstable ions. (a) Na,2+ (b) Mg,2 (c) AI,2 (d) Si,2 (e) p2+ (f) s,2 (g) F,2 (h) Ar,2 40. Predict the valence electron molecular orbital configurations for the following, and state whether they will be stable or unstable ions. (a) Na22+ (b) Mg22+ (c) Al22+ (d) Si22+ (e) P22+ (f) S22+ (g) F22+ (h) Ar22+arrow_forwardFor each of the following molecules, state the bond angle (or bond angles, as appropriate) that you would expect to see on the central atom based on the simple VSEPR model. Would you expect the actual bond angles to be greater or less than this? a CCl4 b SCl2 c COCl2 d AsH3arrow_forward
- In Chapter 6, we study a group of organic cations called carbocations. Following is the structure of one such carbocation, the tert-butyl cation. (a) How many electrons are in the valence shell of the carbon bearing the positive charge? (b) Using VSEPR, predict the bond angles about this carbon. (c) Given the bond angle you predicted in (b), what hybridization do you predict for this carbon?arrow_forwardConsider NH3 and PH3. Electronegativities: P = 2.1, H = 2.1, N=3.0. Which statement is false? O A. The P-H bonds are more polar than the N-H bonds. OB. The bond dipoles in NH3 are directed toward the nitrogen atom. For PH3 there is no bond dipole moment. OC. Both are sp hybridized at the central atom. に O D. There are no false statements. All of these statements are corect. OE. Both molecules are polar.arrow_forwardAnswer the following questions about amoxicillin, an antibiotic from the penicillin family. NH2 H N. N. НО Но amoxicillin a. Predict the hybridization and geometry around each highlighted atom. b. Label five polar bonds using the symbols &+ and 8–. C. How many n bonds does amoxicillin have? Label them. d. Find a C- H bond containing a carbon atom having a hybrid orbital with 33% s-character.arrow_forward
- 8. Consider the following organic molecules. What are the hybridizations around each carbon atom? What are the shapes around each carbon atom? You may want to number your carbon atoms for clarity. H H H H. C-H .C H. H-C=C-H C H C= H.arrow_forwardHelp filling in the Lewis structures grapharrow_forward1. Ethanol, C,H,0 (CH,CH,OH) Lewis structure using dots to represent bonding electrons: Lewis structure using lines to represent pairs of bonding electrons: Label the carbon bonded to only hydrogen and other carbon atom as carbon A, and the other carbon atom as carbon B. Carbon atom A: Total number of electron groups: Number of lone pairs: Number of bonding groups/pairs: Bond angles: Electron geometry: Molecular geometry: Hybridization: Number of hybrid orbitals: Carbon atom B: Total number of electron groups: Number of lone pairs: Number of bonding groups/pairs: Bond angles: Electron geometry: Molecular geometry: Hybridization: Number of hybrid orbitals: Oxygen atom Total number of electron groups: Number of lone pairs: Number of bonding groups/pairs: Bond angles: Electron geometry: Molecular geometry: Hybridization: Number of hybrid orbitals: Is this molecule polar? (Y/N) Can this molecule hydrogen bond with itself? Number of sigma bonds: Number of pi bonds: MacBook Proarrow_forward
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