EBK STUDY GUIDE TO ACCOMPANY CHEMISTRY:
7th Edition
ISBN: 9781119360889
Author: HYSLOP
Publisher: VST
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Textbook Question
Chapter 9, Problem 37RQ
Will the combination of 3d. orbitals in Question 9.36 yield a
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Use MO theory to explain the following:
O2P
*
2p, 2pх 2ру
TT 2p
2р, 2рx 2ру
2р, 2рх 2ру
2р, 2рх 2ру
O 2P
O 2P
TT 2p
O2s
02s
2s
2s
2s
2s
O2s
O2s
i. The ionization energy of fluorine (F) is ~1700 kJ/mol, while the ionization
energy of difluorine (F2) is ~1500 kJ/mol.
+
iii. The longest wavelength of light that can be absorbed by N2 is ~80 nm, while
the longest wavelength of light that can be absorbed by F2 is ~100 nm. (No
calculations are required for this).
ii. Bez cannot exist, while both Be,* and Be,¯ can exist.
Consider a ring system made up of 8 atoms (each one contributing a p atomic orbital to make 8 pi molecular orbitals). If the system is filled with 6
orbitals containing single,
electrons, there will 6
orbitals containing pairs of electrons and 1
unpaired electrons. Hint: Use a Frost Circle.
Use numbers rather than text for your answers.
is a carbon atom diamagnetic or paramagnetic?
Chapter 9 Solutions
EBK STUDY GUIDE TO ACCOMPANY CHEMISTRY:
Ch. 9 - Practice Exercise 9.1 Label the shapes of the...Ch. 9 - Practice Exercise 9.2 What is the shape of the...Ch. 9 - Practice Exercise 9.3
What shape is expected for...Ch. 9 - Practice Exercise 9.4 The first known compound of...Ch. 9 - Practice Exercise 9.5
What shape is expected for...Ch. 9 - Practice Exercise 9.6 What shape is expected for...Ch. 9 - Practice Exercise 9.7 Is the sulfur tetrafluoride...Ch. 9 - Practice Exercise 9.8 Explain how you decided...Ch. 9 - Practice Exercise 9.9 Use the principles of VB...Ch. 9 - Practice Exercise 9.10 The phosphine molecule,...
Ch. 9 - Practice Exercise 9.11
The molecule has a planar...Ch. 9 - Practice Exercise 9.12 In the gas phase, beryllium...Ch. 9 - Practice Exercise 9.13
What kind of hybrid...Ch. 9 - What kind of hybrid orbitals are expected to be...Ch. 9 - Use the VSEPR model to predict the shape of the...Ch. 9 - What kind of orbitals arc used by Xe in the XeF4...Ch. 9 - Explain how to decide what kind of hybrid orbitals...Ch. 9 - If we assume that nitrogen uses sp3 hybrid...Ch. 9 - Practice Exercise 9.19
What is the shape of the ...Ch. 9 - Practice Exercise 9.20
Consider the molecule...Ch. 9 - Practice Exercise 9.21
Consider the molecule...Ch. 9 - The molecular orbital energy level diagram for the...Ch. 9 - The MO energy level diagram for the nitrogen...Ch. 9 - Practice Exercise 9.24
The nitrate ion, , has...Ch. 9 - Prob. 25PECh. 9 - Arrange the following elements in order of...Ch. 9 - Practice Exercise 9.27
What is the hybridization...Ch. 9 - Sketch the following molecular shapes and give the...Ch. 9 - Sketch the following molecular shapes and give the...Ch. 9 - 9.3 What is the underlying principle on which the...Ch. 9 - What is an electron domain? How are nonbonding and...Ch. 9 - 9.5 How many bonding domains and how many...Ch. 9 - Sketch the following molecular shapes and give the...Ch. 9 - What arrangements of domains around an atom are...Ch. 9 - Why is it useful to know the polarities of...Ch. 9 - Prob. 9RQCh. 9 - 9.10 Under what conditions will a molecule be...Ch. 9 - What condition must be met if a molecule having...Ch. 9 - Use a drawing to show why the SO2 molecule is...Ch. 9 - What is meant by orbital overlap?Ch. 9 - How is orbital overlap related to bond energy?Ch. 9 - Use sketches of orbitals to describe how VB theory...Ch. 9 - 9.16 Why do atoms usually use hybrid orbitals for...Ch. 9 - 9.17 Sketch figures that illustrate the...Ch. 9 - 9.18 Sketch figures that illustrate the...Ch. 9 - 9.19 Why do Period 2 elements never use hybrid...Ch. 9 - What relationship is there, if any, between Lewis...Ch. 9 - How can the VSEPR model be used to predict the...Ch. 9 - If the central oxygen in the water molecule did...Ch. 9 - Using orbital diagrams, describe how sp3...Ch. 9 - Sketch the way the orbitals overlap to form the...Ch. 9 - We explained the bond angles of 107inNH3 by using...Ch. 9 - Using sketches of orbitals and orbital diagrams,...Ch. 9 - What two basic shapes have hybridizations that...Ch. 9 - 9.28 The ammonia molecule, , can combine with a...Ch. 9 - 9.29 How does the geometry around B and O change...Ch. 9 - How do and bonds differ?Ch. 9 - Why can free rotation occur easily around a -bond...Ch. 9 - 9.32 Using sketches, describe the bonds and bond...Ch. 9 - Sketch the way the bonds form in acetylene, C2H2.Ch. 9 - How does VB theory treat the benzene molecule?...Ch. 9 - Why is the higher-energy MO in H2 called an...Ch. 9 - Below is an illustration showing two 3d. orbitals...Ch. 9 - 9.37 Will the combination of 3d. orbitals in...Ch. 9 - Explain why He2 does nor exist but H2 does.Ch. 9 - 9.39 How does MO theory account for the...Ch. 9 - 9.40 On the basis of MO theory, explain why ...Ch. 9 - 9.41 What relationship is there between bond order...Ch. 9 - Sketch the shapes of the 2p,and*2p,MOs.Ch. 9 - 9.43 What is the theoretical basis of both valence...Ch. 9 - What shortcomings of Lewis structures and VSEPR...Ch. 9 - What is the main difference in the way VB and MO...Ch. 9 - What is a delocalized MO? Explain, in terms of...Ch. 9 - 9.47 What effect does delocalization have on the...Ch. 9 - Prob. 48RQCh. 9 - Prob. 49RQCh. 9 - 9.50 What is required to form a conduction band?
Ch. 9 - Prob. 51RQCh. 9 - Prob. 52RQCh. 9 - In calcium, why cant electrical conduction take...Ch. 9 - 9.54 What are allotropes? How do they differ from...Ch. 9 - Why are the Period 2 elements able to form much...Ch. 9 - Even though the nonmetals of Periods 3, 4, and 5...Ch. 9 - Which of the nonmetals occur in nature in the form...Ch. 9 - 9.58 Describe the structure of diamond. What kind...Ch. 9 - Describe the structure of graphene. What kind of...Ch. 9 - How is the structure of graphite related to the...Ch. 9 - Prob. 61RQCh. 9 - 9.62 How is the structure of a carbon nanotube...Ch. 9 - 9.63 What is the molecular structure of silicon?...Ch. 9 - Make a sketch that describes the molecular...Ch. 9 - 9.65 What are the different allotropes of...Ch. 9 - 9.66 What are the P—P—P bond angles in the ...Ch. 9 - Prob. 67RQCh. 9 - 9.68 What is the molecular structure of black...Ch. 9 - What are the two allotropes of oxygen?Ch. 9 - Draw the Lewis structure for O3. Is the molecule...Ch. 9 - 9.71 What beneficial function does ozone serve in...Ch. 9 - What is the molecular structure of sulfur in its...Ch. 9 - 9.73 Predict the shapes of (a) , (b) , (c) , (d) ,...Ch. 9 - Predict the shapes of (a) SF3+, (b) GeF4, (c) ,...Ch. 9 - Predict the shapes of...Ch. 9 - Predict the shapes of (a) TeF4, (b) SbCl6, (c)...Ch. 9 - Predict the shapes of...Ch. 9 - 9.78 Predict the shapes of .
Ch. 9 - Which of the following has a shape described by...Ch. 9 - Which of the following has a shape described by...Ch. 9 - Ethene, also called ethylene, is a gas used to...Ch. 9 - Ethyne, more commonly called acetylene, is a gas...Ch. 9 - 9.83 Predict the bond angle for each of the...Ch. 9 - 9.84 Predict the bond angle for each of the...Ch. 9 - 9.85 Which of the following molecules would be...Ch. 9 - Which of the following molecules would he expected...Ch. 9 - Which of the following molecules or ions would be...Ch. 9 - Which of the following molecules or ions would be...Ch. 9 - 9.89 Explain why is nonpolar, but is polar.
Ch. 9 - 9.90 Explain why is polar, but is not.
Ch. 9 - Use sketches of orbitals to show how VB theory...Ch. 9 - Hydrogen selenide is one of nature's most...Ch. 9 - Use orbital diagrams to explain how the beryllium...Ch. 9 - Use orbital diagrams to describe the bonding in...Ch. 9 - 9.95 Use orbital diagrams to describe the bonding...Ch. 9 - Describe the bonding in tellurium hexafluoride, a...Ch. 9 - Draw Lewis structures for the following and use...Ch. 9 - Draw Lewis structures for the following and use...Ch. 9 - Use the VSEPR model to help you describe the...Ch. 9 - Use the VSEPR model to help you describe the...Ch. 9 - 9.101 Use orbital diagrams to show that the...Ch. 9 - What kind of hybrid orbitals are used by tin in...Ch. 9 - A nitrogen atom can undergo sp2 hybridization when...Ch. 9 - A nitrogen atom can undergo sp hybridization and...Ch. 9 - Tetrachloroethylene, a common dry-cleaning...Ch. 9 - 9.106 Phosgene, , was used as a war gas during...Ch. 9 - 9.107 What kind of hybrid orbitals do the numbered...Ch. 9 - What kind of hybrid orbitals do the numbered atoms...Ch. 9 - 9.109 What kinds of bonds are found in the...Ch. 9 - 9.110 What kinds of bondsare found in the numbered...Ch. 9 - Construct the molecular orbital diagram for O2....Ch. 9 - Construct the molecular orbital diagram for N2....Ch. 9 - Use the MO energy diagram to predict (a) the bond...Ch. 9 - Use the MO energy diagram to predict (a) the bond...Ch. 9 - Assume that in the NO molecule the molecular...Ch. 9 - 9.116 Assume that in the NO molecule the molecular...Ch. 9 - Which of the following molecules or ions are...Ch. 9 - 9.118 Which of the following molecules or ions are...Ch. 9 - *9.119 Construct the MO energy level diagram for...Ch. 9 - If boron and nitrogen were to form a molecule with...Ch. 9 - 9.121 Formaldehyde has the Lewis structure
What...Ch. 9 - Prob. 122RQCh. 9 - Antimony forms a compound with hydrogen that is...Ch. 9 - Describe the changes in molecular geometry and...Ch. 9 - Prob. 125RQCh. 9 - Prob. 126RQCh. 9 - Phosphorus trifluoride, PF3, has FPF bond angles...Ch. 9 - A six-membered ring of carbons can hold a double...Ch. 9 - The more electronegative are the atoms bonded to...Ch. 9 - Alone pair of electrons in the valence shell of an...Ch. 9 - *9.131 The two electron pairs in a double bond...Ch. 9 - In a certain molecule, ap orbital overlaps with a...Ch. 9 - *9.133 If we assign the internuclear axis in a...Ch. 9 - The peroxynitrite ion, OONO-, is a potent toxin...Ch. 9 - *9.135 An ammonia molecule, , is very polar,...Ch. 9 - There exists a hydrocarbon called butadiene, which...Ch. 9 - Prob. 137RQCh. 9 - 9.138 Five basic molecular shapes were described...Ch. 9 - 9.139 Compare and contrast the concepts of...Ch. 9 - Why doesnt a carbon-carbon quadruple bond exist?Ch. 9 - What might the structure of the iodine...Ch. 9 - The FF bond in F2 is weaker than the ClCl bond in...Ch. 9 - Molecular orbital theory predicts the existence of...Ch. 9 - The structure of the diborane molecule, B2H6, is...
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- Consider a heteronuclear diatomic molecule, AB, where A and B are period 2 elements. Using the following pieces of information, provide details on the molecular orbital diagram of AB: Clue 1: The MO diagram of AB does not contain non- bonding electrons. Clue 2: The s and p orbital energies of both atoms are quite close to one another that interactions between different orbital types occur. Clue 3: AB" is more stable than AB, but AB2 is less stable than AB". Clue 4: The potential energies of the atomic orbitals of A are higher than the potential energies of the atomic orbitals of B. Table 1. Atomic orbital energies of period 2 elements. Atom Orbital energy Orbital energy (2s) (2p) Li -5.45 Ве -9.30 B -14.0 -8.30 C -19.5 -10.7 -25.5 -13.1 -32.3 -15.9 F -46.4 -18.7 Ne -48.5 -21.5arrow_forwardHuckel theory: All atomic orbital coefficients in the lowest energy MO (Ψ1) should have the same value – explain why?arrow_forwardOrder the following atomic orbitals according to their relative energy levels in homodiatomic molecules and explain your choice: F 2s, F 2px, F 2pz, O 2px, O 2pz; O 2s; N 2px, N 2p:; N 2sarrow_forward
- 4. Molecular Orbital Theory Let's construct an MO diagram for KrBr*, the krypton bromide cation. Let's focus only on the n=4 valence shell in for both species. a) Which of the two atoms, Kr or Br, has a 4p electrons that are lower in energy? Justify your answer in terms of periodic trends. Also provide experimental evidence for your answer in terms of ionization energies (available online). b) Based on part (a), draw an MO diagram for KrBr*, reflecting the appropriate relative energies of the Kr/Br valence electrons. Connect the orbitals that mix/split with dashed lines. c) Populate the MO diagram with the appropriate number of valence electrons. What is the expected bond order?arrow_forwardDraw the molecular orbital diagram for the oxygen molecule, O2. From this diagram, calculate the bond order for O2. How does this diagram account for the paramagnetism of O2?arrow_forwardQ2) Consider the following atoms: a- CI, Ga, Br, P, S and Si What is the effective nuclear charge for each atom? b- What are the possible quantum numbers for n=1, n=2 and n=3? Q3) What are the orbital hybridization for each of the following: Explain 1- BCI, 2- C,H. 3- Cr(CO), 4- Fe(CO), 5- CH, 6- PtBr,arrow_forward
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