1 Chemical Foundations 2 Atomic Structure And Periodicity 3 Bonding: General Concepts 4 Molecular Structure And Orbitals 5 Stoichiometry 6 Types Of Chemical Reactions And Solution Stoichiometry 7 Chemical Energy 8 Gases 9 Liquids And Solids 10 Properties Of Solutions 11 Chemical Kinetics 12 Chemical Equilibrium 13 Acids And Bases 14 Acid- Base Equilibria 15 Solubility And Complex Lon Equilibria 16 Spontaneity, Entropy, And Free Energy 17 Electrochemistry 18 The Nucleus: A Chemist's View 19 The Representative Elements 20 Transition Metals And Coordination Chemistry 21 Organic And Biological Molecules Chapter4: Molecular Structure And Orbitals
Chapter Questions Section: Chapter Questions
Problem 1RQ: Explain the main postulate of the VSEPR model. List the five base geometries (along with bond... Problem 2RQ: Explain why CF4 and Xef4 are nonpolar compounds (have no net dipole moments) while SF4 is polar (has... Problem 3RQ: Consider the following compounds: CO2, SO2, KrF2, SO3, NF3, IF3, CF4, SF4, XeF4, PF5, TF5, and SCl6.... Problem 4RQ Problem 5RQ: What hybridization is required for central atoms that have a tetrahedral arrangement of electron... Problem 6RQ Problem 7RQ Problem 1ALQ: What are molecular orbitals? How do they compare with atomic orbitals? Can you tell by the shape of... Problem 2ALQ: Explain the difference between the and MOs for homonuclear diatomic molecules. How are bonding and... Problem 3ALQ Problem 4ALQ: Which of the following would you expect to be more favorable energetically? Explain. a. an H2... Problem 5ALQ: Arrange the following molecules from most to least polar and explain your order: CH4, CF2Cl2, CF2H2,... Problem 6ALQ: Which is the more correct statement: The methane molecule (CH4) is a tetrahedral molecule because it... Problem 7ALQ Problem 8ALQ Problem 9Q: Which of the following statements is/are true? Correct the false statements. a. The molecules SeS3.... Problem 10Q: Give one example of a compound having a linear molecular structure that has an overall dipole moment... Problem 11Q: In the hybrid orbital model, compare and contrast bonds with bonds. What orbitals form the bonds... Problem 13Q Problem 14Q Problem 15Q Problem 16Q Problem 17Q: Compare and contrast bonding molecular orbitals with antibonding molecular orbitals. Problem 18Q Problem 19Q: Why does the molecular orbital model do a better job in explaining the bonding in NO and NO than the... Problem 20Q: The three NO bonds in NO3 are all equivalent in length and strength. How is this explained even... Problem 21E: Predict the molecular structure (including bond angles) for each of the following. a. SeO3 b. SeO2 Problem 22E: Predict the molecular structure (including bond angles) for each of the following. a. PCl3 b. SCl2... Problem 23E: Predict the molecular structure and bond angles for each molecule or ion in Exercises 81 and 87 from... Problem 24E Problem 25E Problem 26E: Two variations of the octahedral geometry (see Table 4-1) are illustrated below. Which of the... Problem 27E: Predict the molecular structure (including bond angles) for each of the following. (See Exercises 25... Problem 28E: Predict the molecular structure (including bond angles) for each of the following. (See Exercises 25... Problem 29E: State whether or not each of the following has a permanent dipole moment. a. b. c. d. e. f. Problem 30E: The following electrostatic potential diagrams represent CH4, NH3, or H2O. Label each and explain... Problem 31E: Which of the molecules in Exercises 21 and 22 have net dipole moments (are polar)? Problem 32E: Which of the molecules in Exercises 27 and 28 have net dipole moments (are polar)? Problem 33E: Write Lewis structures and predict the molecular structures of the following. (See Exercises 25 and... Problem 34E: Write Lewis structures and predict whether each of the following is polar or nonpolar. a. HOCN... Problem 35E: Consider the following Lewis structure where E is an unknown element: What are some possible... Problem 36E: Consider the following Lewis structure where E is an unknown element: What are some possible... Problem 37E: The molecules BF3, CF4, CO2, PF5, and SF6 are all nonpolar, even though they all contain polar... Problem 38E: Two different compounds have the formula XeF2Cl2. Write Lewis structures for these two compounds,... Problem 39E: Use the localized electron model to describe the bonding in H2O. Problem 40E: Use the localized electron model to describe the bonding in CCl4. Problem 41E: Use the localized electron model to describe the bonding in H2CO (carbon is the central atom). Problem 42E: Use the localized electron model to describe the bonding in C2H2 (exists as HCCH). Problem 43E: The space-filling models of ethane and ethanol are shown below. Use the localized electron model to... Problem 44E: The space-filling models of hydrogen cyanide and phosgene are shown below. Use the localized... Problem 45E Problem 46E Problem 47E Problem 48E: Give the expected hybridization of the central atom for the molecules in Exercises 27 and 28. Problem 49E: For each of the following molecules, write the Lewis structure(s), predict the molecular structure... Problem 50E: For each of the following molecules or ions that contain sulfur, write the Lewis structure(s),... Problem 51E Problem 52E: The allene molecule has the following Lewis structure: Must all hydrogen atoms lie the same plane?... Problem 53E: Indigo is the dye used in coloring blue jeans. The term navy blue is derived from the use of indigo... Problem 54E Problem 55E Problem 56E: Many important compounds in the chemical industry are derivatives of ethylene (C2H4). two of them... Problem 57E: Two molecules used in the polymer industry are azodicarbonamide and methyl cyanoacrylate. Their... Problem 58E: Hot and spicy foods contain molecules that stimulate paindetecting nerve endings. Two such molecules... Problem 59E: One of the first drugs to be approved for use in treatment of acquired immune deficiency syndrome... Problem 60E: The antibiotic thiarubin-A was discovered by studying the feeding habits of wild chimpanzees in... Problem 61E Problem 62E: Sketch the molecular orbital and label its type ( or , bonding or antibonding) that would be formed... Problem 63E Problem 64E: Which of the following are predicted by the molecular orbital model to be stable diatomic species?... Problem 65E Problem 66E Problem 67E Problem 68E: Using the molecular orbital model to describe the bonding in F2+, F2, and F2, predict the bond... Problem 69E Problem 70E: A Lewis structure obeying the octet rule can be drawn for O2 as follows: Use the molecular orbital... Problem 71E: Using the molecular orbital model, write electron configurations for the following diatomic species... Problem 72E: Using the molecular orbital model, write electron configurations for the following diatomic species... Problem 73E: In which of the following diatomic molecules would the bond strength be expected to weaken as an... Problem 74E: In terms of the molecular orbital model, which species in each of the following two pairs will roost... Problem 75E Problem 76E: Show how a hydrogen 1s atomic orbital and a fluorine 2p atomic orbital overlap to form bonding and... Problem 77E: Use Figs. 4-54 and 4-55 to answer the following questions. a. Would the bonding molecular orbital in... Problem 78E: The diatomic molecule OH exists in the gas phase. The bond length and bond energy have been measured... Problem 79E Problem 80E: Describe the bonding in NO+, NO, and NO, using both the localized electron and molecular orbital... Problem 81E: Describe the bonding in the O3 molecule and the NO2 ion, using the localized electron model. How... Problem 82E Problem 83AE Problem 84AE: Vitamin B6 is an organic compound whose deficiency in the human body can cause apathy, irritability,... Problem 85AE: Two structures can be drawn for cyanuric acid: a. Are these two structures the same molecule?... Problem 86AE Problem 87AE: What do each of the following sets of compounds/ions have in common with each other? a. XeCl4, XeCl2... Problem 88AE: Aspartame is an artificial sweetener marketed under the name Nutra-Sweet. A partial Lewis structure... Problem 89AE Problem 90AE: The three most stable oxides of carbon are carbon monoxide (CO), carbon dioxide (CO2), and carbon... Problem 91AE Problem 92AE: Which of the following molecules have net dipole moments? For the molecules that are polar, indicate... Problem 93AE: The strucrure of TeF5 is Draw a complete Lewis structure for TeF5, and explain the distortion from... Problem 94AE: Complete the following resonance structures for POCl3. a. Would you predict the same molecular... Problem 95AE Problem 96AE: Describe the bonding in the first excited state of N2 (the one closest in energy to the ground... Problem 97AE: Using an MO energy-level diagram, would you expect F2 to have a lower or higher first ionization... Problem 98AE: Show how a dxz. atomic orbital and a pz, atomic orbital combine to form a bonding molecular orbital.... Problem 99AE: What type of molecular orbital would result from the in-phase combination of the two dxz atomic... Problem 100AE: Consider three molecules: A, B, and C. Molecule A has a hybridization of sp3 Molecule B has two more... Problem 101CWP Problem 102CWP: Predict the molecular structure, bond angles, and polarity (has a net dipole moment or has no net... Problem 103CWP: Draw the Lewis structures for SO2, PCl3, NNO, COS, and PF3 Which of the compounds are polar? Which... Problem 104CWP: Draw the Lewis structures for TeCl4, ICl5, PCl5, KrCl4, and XeCl2. Which of the compounds exhibit at... Problem 105CWP: A variety of chlorine oxide fluorides and related cations and anions are known. They tend to be... Problem 106CWP: Pelargondin is the molecule responsible for the red color of the geranium flower. It also... Problem 107CWP: Complete a Lewis structure for the compound shown below, then answer the following questions. What... Problem 108CWP Problem 109CWP: Consider the molecular orbital electron configurations for N2, N2+, and N2. For each compound or... Problem 110CWP: Place the species B2+ , B2, and B2 in order of increasing bond length and increasing bond energy. Problem 111CP: The compound NF3 is quite stable, but NCl3 is very unstable (NCl3 was first synthesized in 1811 by... Problem 112CP: Predict the molecular structure for each of the following. (See Exercises 25 and 26.) a. BrFI2 b.... Problem 113CP Problem 114CP: Cholesterol (C27liu;O) has the following structure: In such shorthand structures, each point where... Problem 115CP: Cyanamide (H2NCN), an important industrial chemical, is produced by the following steps: Calcium... Problem 116CP: As compared with CO and O2, CS and S2 are very unstable molecules. Give an explanation based on the... Problem 117CP Problem 118CP: Use the MO model to explain the bonding in BeH2. When constructing the MO energy-level diagram,... Problem 119CP Problem 120CP: Arrange the following from lowest to highest ionization energy: O, O2, O2 , O2+. Explain your... Problem 121CP Problem 122CP Problem 123CP: Carbon monoxide (CO) forms bonds to a variety of metals and metal ions. liS ability to bond to iron... Problem 124CP: The space-filling model for benzoic acid, a food preservative, is shown below. Describe the bonding... Problem 125IP: As the bead engineer of your starship in charge of the warp drive, you notice that the supply of... Problem 126IP: A flask containing gaseous N2 is irradiated with 25-nm light. a. Using the following information,... Problem 127IP: Determine the molecular structure and hybridization of the central atom X in the polyatomic ion XY3+... Problem 3RQ: Consider the following compounds: CO2, SO2, KrF2, SO3, NF3, IF3, CF4, SF4, XeF4, PF5, TF5, and SCl6....
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Concept explainers
The most stable forms of the nonmetals in groups 4A, 5A, and 6A of the first period are molecules with multiple bonds. Beginning with the second period, the most stable forms of the nonmetals of these groups are molecules without multiple bonds. Propose an explanation for this observation based on valence bond theory .
Definition Definition Theory that explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. VBT gives a quantum mechanical approach to the formation of covalent bonds with the help of wave functions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.
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