Essential Organic Chemistry, Global Edition
3rd Edition
ISBN: 9781292089034
Author: Paula Yurkanis Bruice
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Concept explainers
Textbook Question
Chapter 1, Problem 50P
Predict the approximate bond angles for the following:
- a. the H 8 C 8 H bond angle in H2C 8 O
- b. the C 8 C 8 N bond angle in CH3C : N
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
Atom A has 4 valence electrons. Atom Z has 6 valence electrons.
For the AZ3-2 ion
How many valence electrons are in the structure?
b. How many single bonds are in the structure?
c. How many double bonds are in the structure?
d. How many triple bonds are in the structure?
e. How many lone pairs are on the central atom in the structure?
f. What is the shape of the structure?
g. What are the bond angles of this ion?
S5) Since the F-C-F bond angle in CH2F2 molecule is 108.3 °; a) What is the% s character of the hybrid orbital used in the formation of the C-H bond of the carbon? b) What is the angle between H-C-H?
12. The presence of a lone pair in the structure of ammonia (NH ) causes the H-N-H bond angle to deviate from the ideal value of 109.5° for tetrahedral geometry. What is the expected deviation for the value of the H-N-H bond angle?
a. H-N-H bond angle > 109.5°b. it will not deviate from the ideal valuec. H-N-H bond angle < 109.5°d. cannot be determined
13. Which of the following statements are TRUE regarding the valence shell electron pair repulsion (VSEPR) theory? (Choose all that applies.
a. 3D arrangement of the nuclei joined by electron groups result to the molecular shapeb. each electron group repels other groups to minimize the angle between themc. electron group arrangements are defined by both the bonding and nonbonding valence electron groups around the central atom
14. TRUE/FALSE: Secondary bonds are stronger than primary bonds due to the longer distance between the molecules involved in the interactions.
Chapter 1 Solutions
Essential Organic Chemistry, Global Edition
Ch. 1.1 - Oxygen has three isotopes, 16O, 17O, and 18O. The...Ch. 1.2 - Prob. 2PCh. 1.2 - How many valence electrons do chlorine, bromine,...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?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 - After examining the potential maps for LiH, HF,...Ch. 1.4 - An atom with a formal charge does not necessarily...
Ch. 1.4 - Prob. 12PCh. 1.4 - a. Draw two Lewis structures for C2H6O. b. Draw...Ch. 1.4 - Draw the lone-pair electrons that are not shown in...Ch. 1.4 - Prob. 16PCh. 1.4 - Which of the atoms in the molecular models in...Ch. 1.4 - Prob. 18PCh. 1.7 - What orbitals are used to form the 10 sigma bonds...Ch. 1.9 - Put a number in each of the blanks: a. ___ s...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. 25PCh. 1.13 - a. Predict the relative lengths and strengths of...Ch. 1.13 - Prob. 28PCh. 1.14 - Which of the bonds in a carbonoxygen double bond...Ch. 1.14 - Caffeine is a natural insecticide, found in the...Ch. 1.14 - a. What is the hybridization of each of the carbon...Ch. 1.14 - Prob. 33PCh. 1.14 - Describe the orbitals used in bonding and the bond...Ch. 1.15 - Account for the difference in the shape and color...Ch. 1.15 - Which of the following molecules would you expect...Ch. 1 - Draw a Lewis structure for each of the following...Ch. 1 - Prob. 38PCh. 1 - What is the hybridization of all the atoms (other...Ch. 1 - Prob. 40PCh. 1 - Draw the condensed structure of a compound that...Ch. 1 - Prob. 42PCh. 1 - Prob. 43PCh. 1 - Draw a Lewis structure for each of the following...Ch. 1 - Prob. 45PCh. 1 - List the bonds in order from most polar to least...Ch. 1 - What is the hybridization of the indicated atom in...Ch. 1 - Write the Kekul structure for each of the...Ch. 1 - Assign the missing formal charges.Ch. 1 - Predict the approximate bond angles for the...Ch. 1 - Prob. 51PCh. 1 - a. Which of the indicated bonds in each compound...Ch. 1 - In which orbitals are the lone pairs in nicotine?...Ch. 1 - Draw the missing lone-pair electrons and assign...Ch. 1 - Rank the following compounds from highest dipole...Ch. 1 - Prob. 56PCh. 1 - a. Which of the species have bond angles of 109.5?...Ch. 1 - Prob. 58PCh. 1 - Sodium methoxide (CH3ONa) has both ionic and...Ch. 1 - a. Why is a H 8 H bond (0.74 ) shorter than a C 8...Ch. 1 - Which compound has a larger dipole moment, CHCl3...Ch. 1 - Which compound has a longer C 8 Cl bond?Ch. 1 - Prob. 63PCh. 1 - The following compound has two isomers. One isomer...
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Identify the molecules with a dipole moment: (a) SF4 (b) CF4 (c) Cl2CCBr2 (d) CH3Cl (e) H2COarrow_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 VSEPR model. Would you expect the actual bond angles to be greater or less than this? a OF2 b NCl3 c CF2CF2 d GeF4arrow_forwardMenthol is used in soaps, perfumes, and foods. It is present in the common herb mint, and it can be prepared from turpentine. (a) What are the hybridizations used by the C atoms in the molecule? (b) What is the approximate COH bond angle? (c) Is the molecule polar or nonpolar? (d) Is the six-member carbon ring planar or non-planar? Explain why or why not.arrow_forward
- Lactic acid is a natural compound found in sour milk. (a) How many bond occur in lactic acid? How many u bonds? (b) What is the hybridization of atoms 1, 2, and 3? (c) Which CO bond is the shortest in the molecule? Which CO bond is the strongest? (d) What are the approximate value of the bond angles A, B, and C?arrow_forwardExplain in terms of bonding theory why all atoms of H2CCCCH2 must lie in the same plane.arrow_forwardGive approximate values for the indicated bond angles. (a) OSO angle in SO2 (b) FBF angle in BF3 (c) ClCCl angle in Cl2CO (d) HCH (angle 1) and CCN (angle 2) acetonitrilearrow_forward
- True or false The F – N – F bond angle in NF3 is smaller than the H – N – H bond angle in NH3.arrow_forwardHow do I draw the simplified formulas, with the angles? I know the C N is sp so it's supposed to be a straight line. But I'm not sure I understand how I should draw itarrow_forward4. Draw Lewis structures for the following molecules. Describe how the bond angles would bealtered based on the Lewis structure.a. CH2Sb. SCl2arrow_forward
- Select the correct bond angles from the following list: a) 120°b) slightly less than 109.5°c) 180°d) slightly greater than 109.5°e) 60°f) slightly less than 120°g) 30°h) 90°i) 109.5°j) none of the above for the following the F-B-F bond angle in BF2- the Cl-Si-Cl bond in SiCl4 the O-S-O bond in SO2 the O-C-O bond in CO32- the F-N-F bond in NF3 the Cl-C-Cl in CCl2O the F-Xe-F in XeF4arrow_forwardPredict the approximate bond angles: a. the C¬N¬H bond angle in (CH3)2+ NH2 b. the C¬O¬H bond angle in CH3OH c. the C¬N¬H bond angle in (CH3)2NH d. the C¬N¬C bond angle in (CH3)2NHarrow_forwardHow many of the atoms in the structure shown in Figure 7 has sp² hybridisation? [The answer is a whole number.] * Your answerarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Types of bonds; Author: Edspira;https://www.youtube.com/watch?v=Jj0V01Arebk;License: Standard YouTube License, CC-BY