Custom eBook for Organic Chemistry
2nd Edition
ISBN: 9798214171104
Author: Straumanis
Publisher: Cengage Custom
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Chapter 3, Problem 8CTQ
Interpretation Introduction
Interpretation: The blank that is related to overlap of orbitals in
Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy although they may differ in shape and orientation. This phenomenon is referred as hybridization.
The energy and orientation of the new hybrid orbital depends upon by the kind and number of orbitals used in the hybridization. The new hybrid orbitals are always equal in number to number of atomic orbitals that combine.
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Students have asked these similar questions
B. Answer the next two questions about the Lewis structure
of XYZ shown below.
メー三
-YEz:
I. What is the hybridization of the central atom?
II. For all covalent bonds, specify the type of bond (o vs. T)
and the atomic orbitals that overlap to form the bond.
For example, in a molecule of H2, the only bond is o:
H(s)-H(s).
4. Valence Bond Theory. Consider formaldehyde, H₂CO. (
a) Draw a Lewis structure of formaldehyde.
b) Draw a picture using valence bond theory showing the bonding of
formaldehyde using appropriate hybrid orbitals. (Include electrons)
c) Describe the bonding of the C-O bond and C-H bond by listing the bond
type (σ, π) and the orbitals contributing to the bonding.
C-O:
C-H:
Consider the following Lewis structure. Note: the lone pairs are not indicated.
но н н
||
Н-С—С—С-С-Н
3 2 1
H
Which statement below about the molecule is false?
There are 10 o and 2 r bonds.
C-2 is sp2 hybridized with bond angles of 120°
Oxygen is sp3 hybridized.
This m
cule contains 28 va
nce electrons.
There are some H-C-H bond angles of about 109° in the molecule.
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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- 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_forwardIn Chapter 6, we study a group of organic cations called carbocations. Following is the structure of one such carbocation, the tert-butyl cation. (a) How many electrons are in the valence shell of the carbon bearing the positive charge? (b) Using VSEPR, predict the bond angles about this carbon. (c) Given the bond angle you predicted in (b), what hybridization do you predict for this carbon?arrow_forwardConsider acetyl salicylic acid, better known as aspirin. Its structure is (a) How many sigma and pi bonds are there in aspirin? (b) What are the approximate values of the angles marked (in blue) A, B, and C? (c) What is the hybridization of each atom marked (in red) 1, 2, and 3?arrow_forward
- 9. Ethyl amine (H;CCH2NH2) and acetonitrile (H3CCN) both have lone pairs on N. Draw structures for both of these molecules in the space below. Show each with its 3-dimensional geometry using lines, wedges, and dashes to show all sigma bonds (note that the framework is provided for acetonitrile, but not ethyl amine). Do not change any of the lines already drawn. Draw orbitals for any pi bonds and orbitals containing lone pairs. H C- C N H H ethyl amine acetonitrile What is the hybridization of the orbital that contains the lone pair in each? Ethyl amine: Acetonitrile:arrow_forwardConsider the following structure, which focuses on three atoms labelled 1, 2, and 3. a) What is the hybridization (sp, sp2, sp3, sp3d, sp3d2) of the atom labeled 2? ___________b) How many σ-bonds (sigma bonds) are there? ________c) How many π-bonds (pi bonds) are there? _______arrow_forwardDraw the Lewis structure of SF2, showing all lone pairs. Select Draw Templates More G S sp sp² sp³ d sp³ sn³d² F What is the hybridization of the central atom? Erase Q2 Q Identify the molecular geometry of SF2. bent linear T-shaped octahedral O trigonal planar trigonal bipyramidal square planar O trigonal pyramidal tetrahedral see-saw square pyramidal What is the approximate bond angle in SF₂? O 90° 120° 109.5° 180°arrow_forward
- сс с C-C= C C-C C- C C a. Complete the formula, number the carbon atoms and name the molecule b. Draw and label in terms of the overlapping hybrid orbitals forming each bond c. Identify the hybrid orbitals forming each bond For your answers for letters d,e,f, give the number of the C atom (from a) only (ex. C10 - C11) d. Which C to C bond is the strongest e. Which C to H bond is the most polar f. Which C to C bond is the least free to rotate g. What is the mobile bond orderarrow_forward$ A: What is the hybridization of the central atom in CIF3? Hybridization = What are the approximate bond angles in this substance? Bond angles = B. What is the hybridization of the central atom in IFs Hybridization = R What are the approximate bond angles in this substance? Bond angles = Submit Answer F4 NOTE: If more than one bond angle is possible, separate each with a space. For example, trigonal bipyramid geometry can lead to 3 different bond angles. Octahedral geometry can lead to 2. % [Review Topics] [References] Use the References to access important values if needed for this question. F5 T Retry Entire Group 7 more group attempts remaining Cengage Learning Cengage Technical Support MacBook Air F6 Y & 7 F7 * 00 8 J F8 ( 9 A F9 ) 0 A F10 11 F11 Previous + 11 = Next Save and Exit 4) F12arrow_forwardA σ bond arises from the straight-on overlap of two atomic orbitals. The electron density lies along the axis of the two bonded nuclei. Example:Sigma Bonding in methane, CH4 What atomic or hybrid orbitals make up the sigma bond between C2 and O1 in acetic acid, CH3COOH?(C2 is the second carbon in the structure as written.) orbital on C2 + orbital on O1 What is the approximate C1-C2-O1 bond angle? ... °arrow_forward
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