Organic Chemistry (8th Edition)
8th Edition
ISBN: 9780134042282
Author: Paula Yurkanis Bruice
Publisher: PEARSON
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Textbook Question
Chapter 1, Problem 74P
Which compound has a larger dipole moment: CH3Cl or CH2Cl2?
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why does CH2F2 have a higher dipole moment than CH3F?
Draw a Lewis structure for a compound with molecular formula C4H11N in which three of the carbon atoms are bonded to the nitrogen atom. What is the geometry of the nitrogen atom in this compound? Does this compound exhibit a molecular dipole moment? If so, indicate the direction of the dipole moment.
Acrylamide, H2 C=CHC(=0)NH2 , is a known neurotoxin and possible carcinogen. It was a shock to all consumers of potato chips and french fries a few years ago
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H
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a Identify all bond angles.
O The bond angles around N are approximately 120°. All other angles are 109°.
O The bond angles around N are approximately 90°. All other angles are 120°.
O The bond angles around N are approximately 109°. All other angles are also 109°.
O The bond angles around N are approximately 120°. All other angles are also 120°.
Chapter 1 Solutions
Organic Chemistry (8th Edition)
Ch. 1.1 - Oxygen has three isotopes, 16O, 17O, and 18O. The...Ch. 1.1 - a. How many protons do the following species...Ch. 1.1 - Chlorine has two isotopes, 35Cl and 37Cl; 75.77%...Ch. 1.2 - Prob. 4PCh. 1.2 - a. Write the ground-state electronic configuration...Ch. 1.2 - Look at the relative positions of each pair of...Ch. 1.3 - a. Find potassium (K) in the periodic table and...Ch. 1.3 - Which bond is more polar? a. b. c. d.Ch. 1.3 - Which of the following has a. the most polar bond?...Ch. 1.3 - Use the symbols + and to show the direction of...
Ch. 1.3 - Explain why HCL has a smaller dipole moment than...Ch. 1.3 - After examining the potential maps for LiH, HF,...Ch. 1.4 - An atom with a formal charge does not necessarily...Ch. 1.4 - Prob. 16PCh. 1.4 - a. Draw two Lewis structure for C2H6O. b. Draw...Ch. 1.4 - Draw the lone-pair electrons that are not shown in...Ch. 1.4 - Prob. 20PCh. 1.4 - Which of the atoms in the molecular models in...Ch. 1.4 - Prob. 22PCh. 1.4 - Prob. 23PCh. 1.5 - Draw the following orbitals: a. 3s orbital b. 4s...Ch. 1.6 - Prob. 25PCh. 1.6 - Indicate the kind of molecular orbital (, , , or )...Ch. 1.7 - What orbitals are used to form the 10 sigma bonds...Ch. 1.7 - Explain why a bond formed by overlap of s orbital...Ch. 1.9 - Put n number in each of the blanks: a. __ s...Ch. 1.9 - For each of the given species: a. Draw its Lewis...Ch. 1.11 - Predict the approximate bond angles in a. the...Ch. 1.11 - According to the potential map for the ammonium...Ch. 1.12 - Prob. 35PCh. 1.13 - a. What are the relative lengths and strengths of...Ch. 1.13 - Prob. 38PCh. 1.14 - Describe the orbitals used in bonding and the bond...Ch. 1.15 - Which of the bond in a carbon-oxygen double bond...Ch. 1.15 - Would you expect a CC bond formed by sp2sp2...Ch. 1.15 - Caffeine is a natural insecticide found in the...Ch. 1.15 - a. What is the hybridization of each of the carbon...Ch. 1.15 - Predict the approximate bond angles for a. the CNC...Ch. 1.16 - What of the following molecules would you expect...Ch. 1.16 - Account for the difference in the shape and color...Ch. 1.16 - If the dipole moment of CH3F is 1.847 D and the...Ch. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - Prob. 50PCh. 1 - What is the hybridization of all the atoms (other...Ch. 1 - Draw the condensed structure of a compound that...Ch. 1 - Predict the approximate bond angles: a. the CNH...Ch. 1 - Prob. 54PCh. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - What is the hybridization of each of the carbon...Ch. 1 - Rank the bonds from most polar. a. CO, CF, CN b....Ch. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - Prob. 59PCh. 1 - What is the hybridization of the indicated atom in...Ch. 1 - Predict the approximate bond angles for the...Ch. 1 - Prob. 62PCh. 1 - Draw the missing lone-pair electrons and assigns...Ch. 1 - a. Which of the indicated bonds in each molecule...Ch. 1 - For each of the following molecules, indicate the...Ch. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - Prob. 67PCh. 1 - Rank the following compounds from highest dipole...Ch. 1 - In which orbitals are the lone pairs in nicotine?Ch. 1 - Prob. 70PCh. 1 - Prob. 71PCh. 1 - a. Which of the species have bond angles of 109.5?...Ch. 1 - Prob. 73PCh. 1 - Which compound has a larger dipole moment: CH3Cl...Ch. 1 - Prob. 75PCh. 1 - Explain why CH3Cl has a greater dipole moment than...Ch. 1 - a. Draw a Lewis structure for each of the...Ch. 1 - There are three isomers with molecular formula...
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- Sort the following molecules by electron group geometry by dragging and dropping each symbolic representation into the appropriate category Tetrahedral, octahedral, or neither octahedral or tetrahedral. SF4 PBr5 PH3 NH3arrow_forwardDraw the Lewis structures for each compound and then identify which one is polar. CH₂O CO₂ C₂H4 C2H2arrow_forward2. In measurements of the structure of molecules, some interesting trends are observed. The bond angle (H-C-H) in CH4 is 109°, as we would expect for a molecule in the tetrahedral VSEPR class. However, other molecules in the same VSEPR class, such as ammonia (NH3, H-N-H= 107°) and water (H2O, H-O-H = 105°), have smaller bond angles than expected. Explain the basis for the bond angle trend: CH4 > NH3 > H2O. %3Darrow_forward
- Predict the bond angles around each indicated atom in the following compound. Assume all atoms have formal charges of 0. H₂C=N=CH₂ Part 1 of 2 Atom a: (Choose one) ▼ Part 2 of 2 Atom b: (Choose one) X X Ś Sarrow_forwardPredict the molecular structure, bond angles, and polarity (dipole moment) for each of the following. SF4 NH4+ ХeF2 ХeF4 SO2 H2Sarrow_forwardThe geometry of this compound. Br Br cis trans- E- Z- The molecular formula of this compound. C6H6 C6H8 C6H10 OC6H12arrow_forward
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