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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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).
Consider 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.
?????
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_forwardConsider three molecules: A, B, and C. Molecule A has a hybridization of sp3 Molecule B has two more effective pairs (electron pairs around the central atom) than molecule A. Molecule C consists of two bonds and two bonds. Give the molecular structure, hybridization, bond angles, and an example for each molecule.arrow_forward
- For 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_forwardIn 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_forwardPut the following three molecules in order of increasing H-X-H bond angle, where X is the central atom. CH4 H2S PH3 A. CH4 < H2S < PH3 B. H2S < PH3 < CH4 C. CH4 < PH3 < H2S D. H2S < CH4 < PH3 E. PH3 < CH4 < H2S く くarrow_forward
- What are the angles a and b in the actual molecule of which this is a Lewis structure? H- H a-0° b = 1⁰ C H a b H Note for advanced students: give the ideal angles, and don't worry about small differences from the ideal that might be caused by the fact that different electron groups may have slightly different sizes. X Sarrow_forward● X E X X View 1 View 2 Which one of your two Views is easier to understand? Explain why? How many different bond angles are there in this geometry. Hint, label each X with a number....e.g. X₁ through X5. A bond angle is then represented by any combination of XAX atoms.arrow_forwardTo answer this question, you may need access to the periodic table of elements, a calculator, and the equations and charts in the tutorial associated with this question. Which of the following is polar and has a linear molecular geometry? a.) HCN b.) I₂ c.) CCl₄ d.) H₂Oarrow_forward
- Question 5arrow_forwardPredict all bond angles in each compound. a. CH3Cl b. NH2OH c. CH2=NCH3 d. HC≡CCH2OHarrow_forwardWhich of the following molecules have net dipole moments? For the molecules that are pola1, indicate the polarity of each bond and the direction of the net dipole moment of the molecule. a. CH2Cl2, CHCl3,CCl4 b. CO2, N20 c. PH3, NH3arrow_forward
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