Pearson eText Organic Chemistry -- Instant Access (Pearson+)
8th Edition
ISBN: 9780135213711
Author: Paula Bruice
Publisher: PEARSON+
expand_more
expand_more
format_list_bulleted
Concept explainers
Textbook Question
Chapter 1, Problem 72P
a. Which of the species have bond angles of 109.5°?
b. Which of the species have bond angles of 120°?
H2O
H3O+
+CH3
BF3
NH3
+NH4
–CH3
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
10. Which of the following compounds does not exhibit delocalization of pi
electrons?
H₂N
A
CH 2
A
A. 1
B
11. Which of the following resonance structures is most stable?
+
CH3
H₂C
H₂C
CH3
CH3
H₂C
B.2
H₂N
B
12. Which nitrogen has the highest electron density?
1
HN
C
H2
C. 3
H₂N
+
C
F
D
H₂C
D. 4
H₂N
D
CH3
a. Which of the species have bond angles of 109.5°?b. Which of the species have bond angles of 120°?H2O H3O++CH3 BF3 NH3 +NH4 −CH3
Of the following species,
will have bond angles of 120°.
A
BC13
NC13
All of these will have bond angles of 120°.
D
PH3
E) CIF3
Chapter 1 Solutions
Pearson eText Organic Chemistry -- Instant Access (Pearson+)
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...
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
- 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_forwardWhat is the steric number and the bond angles associated with each of the following molecules if A is the central atom, X refers to the atoms bonded to it and there are no lone pairs on the central atom. 1. АХз 2. AX4 3. АХ6arrow_forwardArrange the following AX, species in order of decreasing X-A-X bond angles: HCN, SF6, H20, PbCl2, PF3. НCN HCN HCN HCN HCN SF6 SF6 SF6 SF6 SF6 H20 H20 H20 > H20 H20 > > > PbCl2 PbCl2 PbCl2 PbCl2 PbCl2 PF3 PF3 PF3 O PF3 PF3arrow_forward
- What kind of orbitals are overlapping in bond A indicated below? A NH₂ H * CH3 o bond: overlap of sp³ orbital on C and sp² orbital on N bond: overlap of sp³ orbital on C and sp² orbital on N o bond: overlap of sp² orbital on C and sp² orbital on N bond: overlap of p orbital on C and p orbital on N o bond: overlap of sp² orbital on C and sp² orbital on N bond: overlap of sp² orbital on C and sp² orbital on Narrow_forwardWhich of the molecules below has a trigonal planar molecular geometry? COCI2 H2CO H2O BF3 NH3 OCH4arrow_forwardPredict all bond angles in each compound. a. CH3Cl b. NH2OH c. CH2=NCH3 d. HC≡CCH2OHarrow_forward
- Explain the trends in the bond angles and bond lengths of the following ions. Bond length (X-O) Bond Angle (O-X-0) CIO3 149 pm 107° 165 pm 104° BrO3 181 pm 100° 103arrow_forwardEffect of Differences in Electronegativity on Molecular Polarity For each molecule: Sketch each molecule as shown in the simulation. Include arrows to show the bond dipoles as well as a molecular dipole (if present). Circle polar or nonpolar to indicate the polarity of the molecule. Fill in the electronegativity values for each atom C. Oz vs HF O2 HF polar Electronegativity nonpolar polar nonpolar H=D F = Question 2a: Both of these molecules have the same molecular geometry; they are linear. How do differences in electronegativity affect the molecular polarity in linear molecules? Page 8 of 9 CHM CZ1 ONL Genmetru chrt p-ts voih 1032 Corvrinht e 2020-2021 B CSI Aarrow_forwardFor which two molecules would you expect deviation from ideal bond angles? Ideal bond angles are angles you would expect from electron's geometry (i.e: Tetrahedral ideal bond angle is 109.5°) O H20 PCI5 SF6 O SO2arrow_forward
- Sort the following molecules by electron group geometry by dragging and dropping each symbolic representation into the appropriate box. Trigonal bipyramidal CIF3 SF6 PH3 H20 Octahedral Neither trigonal bipyramidal or octahedralarrow_forwardA. Identify which atomic orbitals are used to construct the specified sigma bonds: Bond a is bond b is: bond c 1s1 Identify which orbital is used to construct the a-bond at the marked atom: B. Identify which atomic orbitals are used to construct the specified sigma bonds: a, CH2 HC=C b. H. Bond a is bond b is: bond c is: Identify which orbital is used to construct the T-bond at the marked atom Submit Answer Try Another Version 10 item attempts remainingarrow_forwardConsider the following molecules: A - BrCl B - SF4 C - BF3 D - F2 E - CF4 Which one of these molecules has bonds that are most polar? Which have a molecular dipole moment? BrCl SF4 BF3 F2 CF4arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher: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 Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher: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
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
Stoichiometry - Chemistry for Massive Creatures: Crash Course Chemistry #6; Author: Crash Course;https://www.youtube.com/watch?v=UL1jmJaUkaQ;License: Standard YouTube License, CC-BY
Bonding (Ionic, Covalent & Metallic) - GCSE Chemistry; Author: Science Shorts;https://www.youtube.com/watch?v=p9MA6Od-zBA;License: Standard YouTube License, CC-BY
General Chemistry 1A. Lecture 12. Two Theories of Bonding.; Author: UCI Open;https://www.youtube.com/watch?v=dLTlL9Z1bh0;License: CC-BY