Organic Chemistry
6th Edition
ISBN: 9781936221349
Author: Marc Loudon, Jim Parise
Publisher: W. H. Freeman
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Chapter 1, Problem 1.10P
Interpretation Introduction
Interpretation:
In the given molecule, all the bond angles and the increasing order of the bond lengths are to be estimated.
Concept introduction:
The three dimensional arrangement of atoms possesses by the molecule in space is known as the molecular geometry. The molecular geometry of any molecule is identified by using the central metal atom, pair of electrons and atoms surrounding the central atom with the help of VSEPR theory. The shape in VSEPR model gives specific angles between the bonds for the corresponding shape and these angles are known as bond angles.
The bond angle for tetrahedral geometry is
The bond angle for trigonal planar geometry is
The bond angle for linear geometry is
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Look at the Lewis structure below and determine the bond angle (See Table at end of problem). What are the bond angles at position 1
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Look at the Lewis structure below. What is the bond angle at position 1
hybridization for the central atom at positions 1
and 2
? What is the
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2
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Look at the Lewis structure below. What is the bond angle at position 1
hybridization for the central atom at positions 1
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H.
1
... ...
H.
..
2
The possibilities for bond angle and hybridization are given in this table.
Bond Angles
< 90 90 <109.5 109.5 <120 120 180
Hybridization
sp sp² sp³ sp³d sp³d²
For each molecule shown here, indicate the hybridization of the central atom.
How do sigma and pi bonds differ? How are they similar? What are all of the types of hybrid orbitals that are generated by combining the valence s orbital and all three valence p orbitals of an atom? How many hybrid orbitals result? Use table to organize your response.
Chapter 1 Solutions
Organic Chemistry
Ch. 1 - Prob. 1.1PCh. 1 - Prob. 1.2PCh. 1 - Prob. 1.3PCh. 1 - Prob. 1.4PCh. 1 - Prob. 1.5PCh. 1 - Prob. 1.6PCh. 1 - Prob. 1.7PCh. 1 - Prob. 1.8PCh. 1 - Prob. 1.9PCh. 1 - Prob. 1.10P
Ch. 1 - Prob. 1.11PCh. 1 - Prob. 1.12PCh. 1 - Prob. 1.13PCh. 1 - Prob. 1.14PCh. 1 - Prob. 1.15PCh. 1 - Prob. 1.16PCh. 1 - Prob. 1.17PCh. 1 - Prob. 1.18PCh. 1 - Prob. 1.19PCh. 1 - Prob. 1.20PCh. 1 - Prob. 1.21APCh. 1 - Prob. 1.22APCh. 1 - Prob. 1.23APCh. 1 - Prob. 1.24APCh. 1 - Prob. 1.25APCh. 1 - Prob. 1.26APCh. 1 - Prob. 1.27APCh. 1 - Prob. 1.28APCh. 1 - Prob. 1.29APCh. 1 - Prob. 1.30APCh. 1 - Prob. 1.31APCh. 1 - Prob. 1.32APCh. 1 - Prob. 1.33APCh. 1 - Prob. 1.34APCh. 1 - Prob. 1.35APCh. 1 - Prob. 1.36APCh. 1 - Prob. 1.37APCh. 1 - Prob. 1.38APCh. 1 - Prob. 1.39APCh. 1 - Prob. 1.40APCh. 1 - Prob. 1.41APCh. 1 - Prob. 1.42APCh. 1 - Prob. 1.43APCh. 1 - Prob. 1.44APCh. 1 - Prob. 1.45APCh. 1 - Prob. 1.46APCh. 1 - Prob. 1.47APCh. 1 - Prob. 1.48APCh. 1 - Prob. 1.49AP
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- 2) a) Consider the following molecule . Given what you have learned about hybridization theory, draw an image or images explaining the bonding situation in this molecule. I want you to draw out all of the orbitals, hybrid orbitals and how they overlap to form the bonds in the molecule. Indicate the % s or p character in the given atomic and hybrid orbitals. Which C-C bond or bonds are the longest? In a paragraph or so explain the image or images you just drew. b) Lastly, consider the molecule below. Indicate the Molecular formula, the molar mass, label the hybridization of each atom except for hydrogen, indicate any chiral centers with a *, which bond or bonds are the shortest, identify by name of each functional group with an arrow pointing to the group.arrow_forwardWhat is the role of wave interference in determining whether a molecular orbital is bonding or antibonding? Match the words in the left column to the appropriate blanks in the sentences on the right. constructive an increased a diminished higher opposite phases the same phase particles waves destructive lower Reset Help The electrons in orbitals behave like waves therefore the bonding molecular orbital arises from the constructive interference between the atomic orbitals, because orbitals have the same phase; the antibonding molecular orbital arises from the destructive interference between the atomic orbitals, because the interacting orbitals have opposite phases The bonding orbital has higher electron density in the internuclear region and, therefore, lower energy. The antibonding orbital has a node in the internuclear region and, therefore, higher in energy than atomic orbitals. "arrow_forwardGiven the molecule CH2CHCN Please draw a Lewis structure for this compound with CORRECT GEOMETRY and label all sigma and pi bonds with the orbitals it is made from (what orbitals are overlapping to form the bond). You may draw the hybridized sigma orbitals as sticks and the unhybridized p-orbitals as lobes for clarity. For this question, you DO need to draw out the orbitals.arrow_forward
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