Chemistry: Structure and Properties (2nd Edition)
2nd Edition
ISBN: 9780134293936
Author: Nivaldo J. Tro
Publisher: PEARSON
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Textbook Question
Chapter 6, Problem 34E
Write a hybridization and bonding scheme for each molecule. Sketch the molecule, including overlapping orbitals, and label all bonds using the notation shown in Examples 6.1 and 6.2.
- CH2Br2
- SO2
- NF3
- BF3
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VSEPR Theory: The 3-dimensional arrangement of atoms around any central atom is determined
primarily by the repulsions between electrons in the valence shell of the atom.
General
Formula
Lewis
Atoms Bonded
Unbonded Electron
Pairs
(Lone Pairs, E)
Hybridization and
Electron
Example Molecular Shape
Structure
to Central Atom
(X)
Arrangement
Name
Diagram
sp
Linear
H-Be
-H
AX2
X-A-X
BeHz
Linear
AX3
sp?
BH3
AX2E
sp?
SO2
sp3
CH4
AX4
sp3
NH3
AX3E
2.
For each of the following molecules (in which the central atom is underlined),
classify it according to the AXnEm nomenclature of the VSEPR theory,
draw the 3-dimensional structure, showing all valence shell electrons of all atoms,
draw the net dipole moment vector (if one exists) on the structure diagram,
name the hybrid atomic orbitals used by the central atom for σ bonding and
name the orbitals used by the central atom for π bonding (if applicable).
Molecule or Ion
SbOCl3
ArOF4
a. AXE formula
b. 3-dimensional
structure
c. Indicate the net dipole moment vector (if any) on this diagram.
d. σ- bonding orbitals used by the central atom
e. π-bonding orbitals used by the central atom
The concept of valence-shell electron-pair repulsion
(VSEPR) is presented in introductory organic chemistry
as a way to predict molecular geometries. The idea be-
hind VSEPR is that areas of electron density repel each
other so that the geometry of bonds and/or lone pairs
of electrons around any one atom places these areas as
far apart as possible. For four areas of electron density,
a tetrahedral geometry is predicted. For three areas of
electron density, a trigonal planar geometry is predicted.
Two areas of electron density lead to a linear geometry.
VSEPR is simply a predictive tool, but in some
cases, it gives an incorrect prediction. In these
instances, additional insights into bonding are
necessary, such as resonance. Interestingly, several
important situations are critical to biochemistry where
VSEPR breaks down. Two examples are shown here.
:O:
CH3
H,N
H3N
CH3 H
:0:
:0:
Histidine
The circled nitrogen atoms are predicted by VSEPR
to be tetrahedral in geometry because each…
Chapter 6 Solutions
Chemistry: Structure and Properties (2nd Edition)
Ch. 6 - Prob. 1ECh. 6 - What is a chemical bond according to valence bond...Ch. 6 - In valence bond theory, what determines the...Ch. 6 - In valence bond theory, the interaction energy...Ch. 6 - What is hybridization? Why is hybridization...Ch. 6 - How does hybridization of the atomic orbitals in...Ch. 6 - How is the number of hybrid orbitals related to...Ch. 6 - Sketch each hybrid orbital sp sp2 sp3 sp3d sp3d2Ch. 6 - Prob. 9ECh. 6 - Name the hybridization scheme that corresponds to...
Ch. 6 - What is a chemical bond according to molecular...Ch. 6 - Explain the difference between hybrid atomic...Ch. 6 - What is a bonding molecular orbital?Ch. 6 - Prob. 14ECh. 6 - What is the role of wave interference in...Ch. 6 - Prob. 16ECh. 6 - Prob. 17ECh. 6 - Prob. 18ECh. 6 - Prob. 19ECh. 6 - Prob. 20ECh. 6 - Prob. 21ECh. 6 - When applying molecular orbital theory to...Ch. 6 - In molecular orbital theory, what is a nonbonding...Ch. 6 - Write a short paragraph describing chemical...Ch. 6 - The valence electron configurations of several...Ch. 6 - The valence electron configurations of several...Ch. 6 - Draw orbital diagrams (boxes with arrows in them)...Ch. 6 - Draw orbital diagrams (boxes with arrows in them)...Ch. 6 - Prob. 29ECh. 6 - Draw orbital diagrams (boxes with arrows in them)...Ch. 6 - Which hybridization scheme allows the formation of...Ch. 6 - Which hybridization scheme allows the central atom...Ch. 6 - Write a hybridization and bonding scheme for each...Ch. 6 - Write a hybridization and bonding scheme for each...Ch. 6 - Write a hybridization and bonding scheme for each...Ch. 6 - Write a hybridization and bonding scheme for each...Ch. 6 - Write a hybridization and bonding scheme for each...Ch. 6 - Write a hybridization and bonding scheme for each...Ch. 6 - Consider the structure of the amino acid alanine...Ch. 6 - Consider the structure of the amino acid aspartic...Ch. 6 - Sketch the bonding molecular orbital that results...Ch. 6 - Sketch the antibonding molecular orbital that...Ch. 6 - Draw an MO energy diagram and predict the bond...Ch. 6 - Draw an MO energy diagram and predict the bond...Ch. 6 - Sketch the bonding and antibonding molecular...Ch. 6 - Sketch the bonding and antibonding molecular...Ch. 6 - Using the molecular orbital energy ordenng for...Ch. 6 - Using the molecular orbital energy ordering for...Ch. 6 - Apply molecular orbital theory to predict if each...Ch. 6 - Apply molecular orbital theory to predict if each...Ch. 6 - According to MO theory, which molecule or ion has...Ch. 6 - According to MO theory, which molecule or ion has...Ch. 6 - Draw an MO energy diagram for CO. (Use the energy...Ch. 6 - Draw an MO energy diagram for HCI. Predict the...Ch. 6 - For each compound, draw the Lewis structure,...Ch. 6 - For each compound, draw the Lewis structure,...Ch. 6 - Amino acids are biological compounds that link...Ch. 6 - The genetic code is based on four different bases...Ch. 6 - The structure of caffeine, present in coffee and...Ch. 6 - The structure of acetylsalicylic acid (aspirin) is...Ch. 6 - Draw a molecular orbital energy diagram for CIF....Ch. 6 - Draw Lewis structures and MO diagrams for CN+, CN,...Ch. 6 - Bromine can form compounds or ions with any number...Ch. 6 - The compound C3H4 has two double bonds. Describe...Ch. 6 - How many hybrid orbitals do we use to describe...Ch. 6 - Prob. 66ECh. 6 - In VSEPR theory, which uses the Lewis model to...Ch. 6 - The resuts of a molecular orbital calculation for...Ch. 6 - Prob. 69ECh. 6 - cis-2-Butene isomerizes (changes its structure) to...Ch. 6 - The ion CH5 + can form under very special...Ch. 6 - Neither the VSEPR model nor the hybridization...Ch. 6 - Prob. 73ECh. 6 - The most stable forms of the nonmetals in groups...Ch. 6 - Consider the bond energies of three iodine...Ch. 6 - How many atomic orbitals form a set of sp3hybrid...Ch. 6 - Have each group member pick one of these...Ch. 6 - Divide your group into two subgroups. Have one...Ch. 6 - A molecular orbital calculation for Hi results in...Ch. 6 - Determine the hybridization about 0 in CH3OH.Ch. 6 - Determine the hybridization about C in H2CO.Ch. 6 - According to the valance bond theory, which kind...Ch. 6 - Use molecular orbital theory to determine the bond...Ch. 6 - Use molecular orbital theory to predict which...Ch. 6 - Use molecular orbital theory to determine which...Ch. 6 - Which hybridization scheme occurs about nitrogen...Ch. 6 - Prob. 8SAQCh. 6 - Prob. 9SAQCh. 6 - Prob. 10SAQCh. 6 - Which type of orbitals overlap to form the sigma...
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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
- In each of the following molecules, a central atom is surrounded by a total of three atoms or unshared electron pairs: SnCl2, BCl3, SO2. In which of these molecules would you expect the bond angle to be less than 120? Explain your reasoning.arrow_forward7.59 What type of hybrid orbital is generated by combining the valence s orbital and all three valence p orbitals of an atom? How many hybrid orbitals result?arrow_forwardLets look more closely at the process of hybridization. (a) What is the relationship between the number of hybrid orbitals produced and the number of atomic orbitals used to create them? (b) Do hybrid atomic orbitals form between different p orbitals without involving 5 orbitals? (c) What is the relationship between the energy of hybrid atomic orbitals and the atomic orbitals from which they are formed?arrow_forward
- Specify the electron-pair and molecular geometry for each underlined atom in the following list. Describe the hybrid orbital set used by this atom in each molecule or ion. (a) BBr3 (b) CO2 (c) CH2Cl2 (d) CO32arrow_forwardA student who missed this class needs to know how to predict the bond angles and shape of amolecule from looking at its bond-line representation. Write a concise but complete explanationfor this student.arrow_forwardSpecify the electron-pair and molecular geometry for each underlined atom in the following list. Describe the hybrid orbital set used by this atom in each molecule or ion. (a) CSe2 (b) SO2 (c) CH2O (d) NH4ssarrow_forward
- Why is the concept of hybridization required in valence bond theory?arrow_forwardSuppose that a molecule has four bonding groups and one lone pair on the central atom. Suppose further that the molecule is confined to two dimensions (this is a purely hypothetical assumption for the sake of understanding the principles behind VSEPR theory). Make a sketch of the molecule and estimate the bond angles.arrow_forward7. Trichloromethane (CHCI3, also called chloroform) has a larger dipole moment than CFCI3. Use three- dimensional structures and bond moments to explain this fact.arrow_forward
- 3 2 4 5 Consider the following second-period heteronuclear diatomic molecule. Combining the valence orbitals (2px, 2py, 2pz, and 2s) of each of the two atoms creates eight new orbitals (one 02s*, one 02s, one 02p, one 02p, two л₂p, and two л₂p) that span the entire molecule and explain it's electronic properties. Those eight new orbitals exist at six energy levels. Rank the molecular orbitals of a F2 molecule from lowest (1) to highest (6) energy. Fatom 6- highest 1- lowest F2 molecule [Choose ] [Choose ] [Choose ] [Choose ] [Choose ] [Choose ] F atomarrow_forwardIn VSEPR theory, which uses the Lewis model to determine molecular geometry, the trend of decreasing bond angles in CH4, NH3, and H2O is accounted for by the greater repulsion of lone pair electrons compared to bonding pair electrons. How would this trend be accounted for in valence bond theory?arrow_forwardDraw two resonance structures that describe the bonding in SO2. Then describe the bonding in this compound using MO theory. How does MO theory rationalize the bond order of 1.5 for the two S-O bonds in this compound?arrow_forward
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