
General Chemistry
7th Edition
ISBN: 9780073402758
Author: Chang, Raymond/ Goldsby
Publisher: McGraw-Hill College
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Chapter 10, Problem 10.55QP
Interpretation Introduction
Interpretation:
By using molecular orbital theory, the bond order in given species has to be compared.
Concept introduction:
Molecular orbital theory
The atomic orbitals involved in bonding actually combine to form new orbitals that are the “property” of the entire molecule, rather than of the individual atoms forming the bonds. These new orbitals are called molecular orbitals.
- In molecular orbital theory, electrons shared by atoms in a molecule reside in the molecular orbitals.
- If longer the bond the weaker the bond and this rule will help you while analysing this concept.
- Higher the bond order, the more stable the bond.
Bond order
The number of
- We can justify the order of increasing stability by using bond order and molecular orbital diagram.
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Rank each of the following substituted benzene molecules in order of which will react fastest (1) to slowest (4) by electrophilic
aromatic substitution.
Explanation
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CF3
(Choose one)
OH
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H
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Identifying electron-donating and electron-withdrawing effects
For each of the substituted benzene molecules below, determine the inductive and resonance effects the substituent will have on the
benzene ring, as well as the overall electron-density of the ring compared to unsubstituted benzene.
Molecule
Inductive Effects
Resonance Effects
Overall Electron-Density
CF3
O donating
O donating
O electron-rich
O withdrawing
withdrawing
O no inductive effects
O no resonance effects
O electron-deficient
O similar to benzene
OCH3
Explanation
Check
O donating
O donating
○ withdrawing
withdrawing
O no inductive effects
no resonance effects
electron-rich
electron-deficient
O similar to benzene
Х
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The acid-base chemistry of both EDTA and EBT are important to ensuring that the reactions proceed as desired, thus the pH is controlled using a buffer. What percent of the EBT indicator will be in the desired HIn2- state at pH = 10.5. pKa1 = 6.2 and pKa2 = 11.6 of EBT
Chapter 10 Solutions
General Chemistry
Ch. 10.1 - Practice Exercise Use the VSEPR model to predict...Ch. 10.1 - Review of Concepts
Which of the following...Ch. 10.2 - Prob. 1PECh. 10.2 - Prob. 1RCCh. 10.3 - Prob. 1RCCh. 10.4 - Prob. 1PECh. 10.4 - Prob. 2PECh. 10.4 - Prob. 1RCCh. 10.5 - Prob. 1PECh. 10.5 - Prob. 1RC
Ch. 10.6 - Prob. 1RCCh. 10.6 - Prob. 2RCCh. 10.6 - Prob. 1PECh. 10 - Prob. 10.1QPCh. 10 - Prob. 10.2QPCh. 10 - 10.3 How many atoms arc directly bonded to the...Ch. 10 - 10.4 Discuss the basic features of the VSEPR...Ch. 10 - 10.5 In the trigonal bipyramidal arrangement, why...Ch. 10 - 10.6 The geometry of CH4 could be square planar,...Ch. 10 - Prob. 10.7QPCh. 10 - Prob. 10.8QPCh. 10 - Prob. 10.9QPCh. 10 - Prob. 10.10QPCh. 10 - 10.11 Describe the geometry around each of the...Ch. 10 - 10.12 Which of these species are tetrahedral?...Ch. 10 - 10.13 Define dipole moment. What are the units and...Ch. 10 - 10.14 What is the relationship between the dipole...Ch. 10 - 10.15 Explain why an atom cannot have a permanent...Ch. 10 - 10.16 The bonds in beryllium hydride (BeH2)...Ch. 10 - 10.17 Referring to Table 10.3. arrange the...Ch. 10 - 10.18 The dipole moments of the hydrogen halides...Ch. 10 - 10.19 List these molecules in order of increasing...Ch. 10 - 10.20 Docs the molecule OCS have a higher or lower...Ch. 10 - 10.21 Which of these molecules has a higher dipole...Ch. 10 - 10.22 Arrange these compounds in order of...Ch. 10 - 10.23 What is valence bond theory? How does it...Ch. 10 - 10.24 Use valence bond theory to explain the...Ch. 10 - 10.25Draw a potential energy curve for the bond...Ch. 10 - 10.26 What is the hybridization of atomic...Ch. 10 - 10.27 How does a hybrid orbital differ from a pure...Ch. 10 - 10.28 What is the angle between these two hybrid...Ch. 10 - 10.29 How would you distinguish between a sigma...Ch. 10 - 10.30 Which of these pairs of atomic orbitals of...Ch. 10 - 10.31 The following potential energy curve...Ch. 10 - 10.32 What is the hybridization state of Si in...Ch. 10 - 10.33 Describe the change in hybridization (if...Ch. 10 - 10.34 Consider the reaction
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