Organic Chemistry (9th Edition)
9th Edition
ISBN: 9780321971371
Author: Leroy G. Wade, Jan W. Simek
Publisher: PEARSON
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Textbook Question
Chapter 1.16, Problem 1.15P
- a. Use your molecular models to make ethane, and compare the model with the preceding structures.
- b. Make a model of propane (C3H3), and draw this model using dashed lines and wedges to represent bonds going back and coming forward.
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3. The following shows all resonance structures for the following molecule.
a. Draw in all implied lone pairs.
b. Draw in curved arrows that show the flow of electrons, making sure the arrows show the precise
starting point and destination of the electrons.
Label each arrow as: lp →→→л (p=lone pair)
c.
d.
Rank the resonance structures from most stable to least based on the number of formal charges and
atoms that lack an octet of electrons.
ol-of-o.
B
A
D
d-d-d-o
E
C
F
G
10. Build a model of CHBRCIF. Next, build a
model of the mirror image of your first
molecule. How are these molecules related?
B. Cycloalkanes
1) Construct a model of the cyclic alkane: cyclopentane (C5H₁0). Because the five carbon atoms are locked in a ring,
rotation about the single bonds is restricted; the plane of the ring a fixed geometry within the molecule. Toggle between
full Lewis structures and skeletal structures by clicking the C-H tool.
Model 1: Use the solid wedge tool to attach a methyl group to each of two different carbon atoms in the cyclopentane.
Note the five carbons of the ring are in the plane of the paper, and the solid wedge indicates both methyls project forward,
in front of the plane of the paper.
Model 2: Use the solid wedge tool to attach first methyl group to one of two different carbon atoms in the cyclopentane,
and use the dashed wedge tool to attach the second. Note the solid wedge indicates that one methyl projects forward, in
front of the plane of the paper. The dashed wedge indicates the other methyl extends back, behind the plane of the paper.
Click the broom to tidy up the…
Chapter 1 Solutions
Organic Chemistry (9th Edition)
Ch. 1.2C - a. Nitrogen has relatively stable isotopes...Ch. 1.4 - Draw Lewis structures for the following compounds....Ch. 1.5 - Write Lewis structures for the following molecular...Ch. 1.5 - Circle any lone pairs (pairs of nonbonding...Ch. 1.6 - Use electronegativities to predict the direction...Ch. 1.8 - Prob. 1.6PCh. 1.9B - Draw the important resonance forms for the...Ch. 1.9B - Prob. 1.8PCh. 1.9B - Prob. 1.9PCh. 1.9B - Use resonance structures to identify the areas of...
Ch. 1.10A - Draw complete Lewis structures for the following...Ch. 1.10B - Give Lewis structures corresponding to the...Ch. 1.10B - Prob. 1.13PCh. 1.11 - Compute the empirical and molecular formulas for...Ch. 1.16 - a. Use your molecular models to make ethane, and...Ch. 1.17 - a. Predict the hybridization of the oxygen atom in...Ch. 1.17 - Predict the hybridization geometry and bond angles...Ch. 1.17 - Predict the hybridization, geometry, and bond...Ch. 1.17 - Prob. 1.19PCh. 1.17 - Allene, CH2=C=CH2, has the structure shown below...Ch. 1.17 - 1. Draw the important resonance forms for each...Ch. 1.18B - Prob. 1.22PCh. 1.18B - Two compounds with the formula CH3CH=NCH3 are...Ch. 1.19B - Prob. 1.24PCh. 1.19B - Give the relationship between the following pairs...Ch. 1 - a. Draw the resonance forms for SO2 (bonded OSO)....Ch. 1 - Name the element that corresponds to each...Ch. 1 - Prob. 1.28SPCh. 1 - For each compound, state whether its bonding is...Ch. 1 - a. Both PCl3 and PCl5 are stable compounds Draw...Ch. 1 - Draw a Lewis structure for each species a. N2H4 b....Ch. 1 - Prob. 1.32SPCh. 1 - Prob. 1.33SPCh. 1 - Draw Lewis structures for a. two compounds of...Ch. 1 - Prob. 1.35SPCh. 1 - Some of the following molecular formulas...Ch. 1 - Prob. 1.37SPCh. 1 - Give the molecular formula of each compound shown...Ch. 1 - 1. From what you remember of electronegativities,...Ch. 1 - For each of the following structures, 1. Draw a...Ch. 1 - Prob. 1.41SPCh. 1 - Prob. 1.42SPCh. 1 - Prob. 1.43SPCh. 1 - Prob. 1.44SPCh. 1 - For each pair of ions, determine which on is more...Ch. 1 - Use resonance structures to identify the areas of...Ch. 1 - Prob. 1.47SPCh. 1 - In 1934, Edward A. Doisy of Washington University...Ch. 1 - If the carbon atom in CH2Cl2 were fat. there would...Ch. 1 - Cyclopropane (C3H6, a three-membered ring) is more...Ch. 1 - Prob. 1.51SPCh. 1 - Prob. 1.52SPCh. 1 - In most amines, the nitrogen atom is sp3...Ch. 1 - Predict the hybridization and geometry of the...Ch. 1 - Draw orbital pictures of the pi bonding in the...Ch. 1 - Prob. 1.56SPCh. 1 - Prob. 1.57SPCh. 1 - Which of the following compounds show cis-trans...Ch. 1 - Give the relationships between the following pairs...Ch. 1 - Dimethyl sulfoxide (DMSO) has been used as an...
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- 3. Draw the Lewis-dot structure for C4H10 below. Remember the Lewis-dot structure is the same as the Expanded structure. A. What is the main intermolecular force acting on this molecule? B. Is this molecule polar or nonpolar? Provide a brief explanation (2-3 sentences) for your answer.arrow_forward1. For each molecule and ion below, indicate the total number of valence electrons. Based on that number of electrons, draw a valid Lewis structure.2. Use VSEPR theory to determine the electron arrangement and the geometry of the molecule around the central atom(s). A table of geometries is attached.3. Build the molecule using the molecular models provided in the lab. Sketch your model well enough to show the geometry. Include bond angles.4. Using your understanding of electronegativity and its trends in the Periodic Table, determine if polar bonds exist in the molecule.5. Using bond polarity and molecular shape, determine if the molecule has an overall dipole. If all the bonds are nonpolar, the molecule is nonpolar. If polar bonds are present, then consider the shape to determine if the molecule has an overall dipole.arrow_forward3. Write the Lewis dot (electron dot) symbol for each covalent molecule. Remember the number of unpaired electrons in the Lewis dot symbol of the atom determines the number of bonds each atom makes. If your molecule has unpaired electrons you are not done. If your molecule has the wrong number of bonds for some atoms it is wrong. Try a different arrangement of atoms. Working left to right will help you. Show loan pairs. a. CH3CH₂OH b. CHCl, Br C. CH3NH₂ d. CHỊCH,CH,CH,CH3 e. CH3SCH 3 4. Write the Lewis dot (electron dot) symbol for each covalent molecule. Remember the number of unpaired electrons in the Lewis dot symbol of the atom determines the number of bonds each atom makes. If your molecule has unpaired electrons you are not done. If your molecule has the wrong number of bonds for some atoms it is wrong. Try a different arrangement of atoms. Working left to right will help you. Show loan pairs. a. HCN b. CH3COOH c. H₂CCONHCH3 d. HCCH e. C6H12arrow_forward
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