Custom eBook for Organic Chemistry
2nd Edition
ISBN: 9798214171104
Author: Straumanis
Publisher: Cengage Custom
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Textbook Question
Chapter 3, Problem 16CTQ
Now consider the fully formed molecule on the right side of Figure 3.7.
a. Draw a Lewis structure of this molecule.
b. Identify orbital representations of the two
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1) For each condensed or skeletal structure below:
A. Draw a complete Lewis structure. Note: show all non-bonding electron pairs.
B. Indicate the hybridization of all C, O, and N atoms in each of the molecules.
C.
Label each of the indicated bonds (marked by an arrow) as either a sigma or pi bond. (Note: Remember,
e.g. that a double bond is made up of both a o and a π bond). Also indicate which orbitals overlap to form
the bond (e.g., Ols-2sp3).
D.
For atoms having lone pairs in the molecules below, indicate in which orbitals the lone pairs are located.
E. Which of the bonds indicated by arrows is shorter?
a)
c) H
CH3
C=CHC=C-CH
g) (CH3)3CCN
CH3
CH₂CH=CHCECH
b)
d)
CH3
Lo
LOH
f) CH₂CH(CH3)SH
h) (CH3)2CH(CH₂)3Br
Q/ For the Lewis structure below…• Draw all of its important resonance structures. Show all charges and lone pair electrons. Use curved arrows to show the flow of electrons leading to each successive structure.• Draw the resonance hybrid. Label the average bond order and average charges
a) Draw the Lewis structure for the molecule on the left (labeled as Molecule A above). Draw the Lewis structure which has minimum formal charges.
b) Draw the correct Lewis structure for the molecule on the right (labeled as Molecule B above). Draw the Lewis structure which has minimum formal charges.
c) Select the three TRUE statements from those provided below.
The molecule on the right (Molecule B) is planar (all atoms lie within the same plane).
The molecule on the left (Molecule A) is planar (all atoms lie within the same plane).
The molecule on the right (Molecule B) has polar bonds.
The molecule on the left (Molecule A) has polar bonds.
We can distinguish between the two molecules (Molecule A and Molecule B) based upon their dipole moment.
Chapter 3 Solutions
Custom eBook for Organic Chemistry
Ch. 3 - Prob. 1CTQCh. 3 - What neutral atom is represented by the electron...Ch. 3 - Prob. 3CTQCh. 3 - Consider any one of the four identical hybrid...Ch. 3 - Prob. 5CTQCh. 3 - Prob. 6CTQCh. 3 - Prob. 7CTQCh. 3 - Prob. 8CTQCh. 3 - Prob. 9CTQCh. 3 - Prob. 10CTQ
Ch. 3 - On the left side of Figure 3.6, label the areas...Ch. 3 - Prob. 12CTQCh. 3 - Prob. 13CTQCh. 3 - Prob. 14CTQCh. 3 - Prob. 15CTQCh. 3 - Now consider the fully formed molecule on the...Ch. 3 - Prob. 1ECh. 3 - Explain why the two molecules below cannot...Ch. 3 - Prob. 3ECh. 3 - Consider the incomplete orbital representation of...Ch. 3 - Consider the following orbital representation of...Ch. 3 - Summarize how one determines the hybridization...Ch. 3 - Explain what is wrong with each of the following...Ch. 3 - Prob. 8ECh. 3 - Prob. 9ECh. 3 - Complete the following tables, and memorize their...Ch. 3 - Draw orbital representations of bonding in water...Ch. 3 - Draw electron configuration diagrams for carbon in...Ch. 3 - Prob. 13E
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- 1. Do all of the following for each molecule or ion. a. Draw the Lewis Dot structure that minimizes formal charges. b. Draw the 3-D structure. c. Determine the Hybridization designation of the central atom. d. Determine the VSEPR designation. e. State what is its Molecular shape. f. Determine whether it is Polar (P) or Nonpolar (N). g. Determine the number of sigma (0) and pi (0) bonds in each structure А. РОд 3- B. SeF4 C. CH,O D. BrF5 Е. СН2arrow_forwardHelp me pleasearrow_forward7. Predict the polarity of 6 real molecules. First, draw the molecules and any bond dipoles. Then draw any molecular dipoles. Explain your reasoning before you check your predictions with the simulation.arrow_forward
- 3. a. E,R is? b. E,S c. S,Z 4. What is the π-energy diagram of the compound in question 3? a. b. d. R,Z e. not a.-d. d. e. not a.-d.arrow_forwardNumber of Molecule valence electrons Formal Charge Electron-Group Geometry Molecular Geometry Resonance AIH2ATCI- Al: Al: Select one.. Al: Select one .. Select one ... AIHAT,Br Al: Al: Select one ... Al: Select one ... Select one ... FSIAS Si: Si: Select one .. Si: Select one ... Select one .. PHATCI P: P: Select one ... P: Select one.. Select one .. PCIFI P: P: Select one ... P: Select one ... Select one ... varrow_forward3. 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 Garrow_forward
- Number of Molecule valence electrons Formal Charge Electron-Group Geometry Molecular Geometry Resonance SiSeH2 Si: Si: Select one ... Si: Select one ... Select one ... AIHCI2l" Al: Al: Select one ... Al: Select one ... Select one.. AsSel3 As: As: Select one ... As: Select one ... Select one ... AIH2CI- Al: Al: Select one ... Al: Select one .. Select one.. PTEF3 P: P: Select one ... P: Select one ... Select one ...arrow_forwardWhat is delocalization energy? How is it related to resonance energy? Answer by selecting all true statements. 00 Resonance energy is a term used in VB theory. Resonance energy and delocalization energy are term that describe different conditions. Resonance energy is a term used in MO theory. Resonance energy and delocalization energy are essentially the same thing. Resonance energy and delocalization energy represent the additional stability associated with a spreading out of electron density. Delocalization energy is a term used in VB theory. Delocalization energy is a term used in MO theory. Resonance energy and delocalization energy represent the additional stability associated with concentrating electron density.arrow_forwardFor each of the Lewis structures shown below, predict the Electron Geometry, Molecular Geometry and Bond Angle. Lastly, using the same format as shown in the last column of Table 1, draw a sketch (using wedges and dashes to show 3D if needed) of the Molecular Geometry.arrow_forward
- On the left side of Figure 3.6, label the areas shown with a dotted line where... one bond can form. one bond can form.arrow_forwardA student draws the picture of ammonia (NH3) in the box below, left, and predicts it will be a flatmolecule with HNH bond angles of exactly 120°. Unfortunately, the student left something out. a. What did the student omit from his drawing? b. What is the actual HNH bond angle of ammonia (based on the draw g above, right)? c. Explain why water, ammonia, and methane (shown below) all have about the same bondangles (close to 109.5°) even though they have different numbers of bonds.arrow_forwardHow many valence electrons does a neutral a. K atom have? b. C atom? N atom? O atom?arrow_forward
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