Organic Chemistry (9th Edition)
9th Edition
ISBN: 9780321971371
Author: Leroy G. Wade, Jan W. Simek
Publisher: PEARSON
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Chapter 1.9B, Problem 1.7P
Draw the important resonance forms for the following molecules and ions
- a.
- b.
- c.
- d.
- e.
- f.
- g. [CH3C(OCH3)2]+
- h. B(OH)3
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3. Use electronegative trends to predict which bond in each of the following groups will
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с. С-Оor Si - O
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4. Ch 8, Problem 54 For each of group, order the atoms and/or ions by decreasing size.
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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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- 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.arrow_forwardwhich of these species have resonance or isomers? CH4, CH2Cl2,CH4O,H2O,H3O+,HF,NH3,H2O2,N2,P4arrow_forwardWhich has the higher electronegativity? C or O? Br or Cl? Pb or H? O or H? C or H?arrow_forward
- If A represents the central atom, in which choice are the species listed in order of increasing H-A-H bond angle? O a. NH4* < H2F* < H3O* O b. NH, < H30* < H2F* O c. H2F* < H3o* < NH, O d. H;O < NH4 < H2F*arrow_forwardH H a) H-C-N-H b) H-N-C-N-H H H H. H. 0-C-C-N-H c) d) Н-с—с—с-н H-C-H For each structure in question 4, draw a resonance hybrid (if it has one) and assign non-zero formal and/or partial charges as needed. SIC HICIH エ-Z-エ HICICIHarrow_forwardDraw the attraction between a water molecule and a molecule of BrCl4F. Br is the central atom in an expanded octet - count your electrons carefully. First, draw one molecule and add the partial charges where needed - use the ΔEN to determine the types of bonds. Then, draw the second molecule so that the δ+ on one molecule lines up across from the δ- on the other. Since we can't draw the molecules here you will answer questions about the drawings that you made on the homework worksheet. BrCl4F has one __________ bond between the Br and F with ΔEN = ____________ , and four ________ bonds between the Br and Cl with a ΔEN = _________ . The central Br has 6 REDs and the molecule is symmetrical/asymmetrical (answer is ___________ ) making it a polar/nonpolar (answer is __________ ) molecule. The central Br has a ___________ charge and the F has a ________ charge. H2O has 2 ____________ bonds with a ΔEN = ___________ . H2O has 4 REDs and is symmetrical/asymmetrical (answer…arrow_forward
- a. Use bond energy values to estimate AH for the following reaction. CEN ΔΗ = C - N H - H C-H N - H ΔΗ = b. Use bond energy values to estimate AH for the following reaction. H-F N - H H-C=N (g) + 2 H₂(g): NEN (891 kJ/mol) (305 kJ/mol) (432 kJ/mol) (413 kJ/mol) (391 kJ/mol) N - N (160. kJ/mol) (565 kJ/mol) (391 kJ/mol) (941 kJ/mol) (154 kJ/mol) F-F kJ H- kJ H C- H H -N(g) H H (g) +2F2(g) → N=N(g) + 4HF(g) Harrow_forward14. Arrange the following in order of decreasing N-O bond strength. a. H2NOH > NO3- > NO2 b. H2NOH > NO2 > NO3 c. NO2- > H2NOH > NO3 d. NO2-> N03> H2NOH e. NO3> NO2> H2NOHarrow_forwardJ J 9. Which of the following correctly show the curved arrows for resonance in the structure. 8+ 8+ A * t X 10. One resonance structure of a molecule is show below. Consider its other resonance structures and select the overall resonance hybrid for this molecule. 8+ d+ 8+ (CH₂)₂ CH₂ N B 8+ Co C 8+ 8+ 8+ D. 8+ E d+ d+ you :O: Darrow_forward
- Given below is a Lewis structure skeleton of a molecule. Rank the C-N bonds, A, B, C, in terms of decreasing bond strength. H H3C А. H N-C-N H;C С—с—с-N H H H Blank 1> Blank 2 > Blank 3 Blank 1 Add your answer Blank 2 Add your answer Blank 3 Add your answer 8.arrow_forwardWhich of the following is the Lewis structure for CH3CO2H? D CH;CO,H H H H-c-c-ö-ö- H. C-H-c-ö-H H H 1 3 H o: H H-c-c-ö-H H-c-ö=c-ö-H H 4 01 O 2 O 3 O 4 2.arrow_forward23. Which of the following does have the resonance structures? Z of C = 6, N = 7, H = 1, O = 8, P = 15, F = 9, Cl = 17 a.PF3b.CCl4c.NH4+d.NO3-arrow_forward
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