Chemistry 10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
1 Chemical Foundations 2 Atoms, Molecules, And Ions 3 Stoichiometry 4 Types Of Chemical Reactions And Solution Stoichiometry 5 Gases 6 Thermochemistry 7 Atomic Structure And Periodicity 8 Bonding: General Concepts 9 Covalent Bonding: Orbitals 10 Liquids And Solids 11 Properties Of Solutions 12 Chemical Kinetics 13 Chemical Equilibrium 14 Acids And Bases 15 Acid-base Equilibria 16 Solubility And Complex Ion Equilibria 17 Spontaneity, Entropy, And Free Energy 18 Electrochemistry 19 The Nucleus: A Chemist's View 20 The Representative Elements 21 Transition Metals And Coordination Chemistry 22 Organic And Biological Molecules Chapter9: Covalent Bonding: Orbitals
Chapter Questions Section: Chapter Questions
Problem 1RQ: Why do we hybtidize atomic orbitals to explain the bonding in covalent compounds? What type of bonds... Problem 2RQ: What hybridization is required for central atoms that have a tetrahedral arrangement of electron... Problem 3RQ: Describe the bonding in H2S, CH4, H2CO and HCN using the localized electron model. Problem 4RQ: What hybridization is required for central atoms exhibiting trigonal bipyramidal geometry?... Problem 5RQ: Electrons in bonding molecular orbitals are most likely to be found in the region between the two... 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: Compare Figs. 4-47 and 4-49. Why are they different? Because B2 is known to be paramagnetic, the 2p... Problem 4ALQ: Which of the following would you expect to be more favorable energetically? Explain. a. an H2... Problem 5ALQ: Draw the Lewis structure for HCN. Indicate the hybrid orbitals, and draw a picture showing all the... Problem 6ALQ: Which is the more correct statement: The methane molecule (CH4) is a tetrahedral molecule because it... Problem 7ALQ: Compare and contrast the MO model with the local electron model. When is each useful? Problem 8ALQ: What are the relationships among bond order, bond energy, and bond length? Which of these quantities... Problem 9ALQ: The molecules N2 and CO are isoelectronic but their properties are quite different. Although as a... Problem 10ALQ: Do lone pairs about a central atom affect the hybridization of the central atom? If so, how? Problem 11Q: In the hybrid orbital model, compare and contrast bonds with bonds. What orbitals form the bonds... Problem 12Q: In the molecular orbital mode l, compare and contrast bonds with bonds. What orbitals form the ... Problem 13Q: Why are d orbitals sometimes used to form hybrid orbitals? Which period of elements does not used... Problem 14Q: The atoms in a single bond can rotate about the internuclear axis without breaking the bond. The... Problem 16Q: As compared with CO and O2, CS and S2 are very unstable molecules. Give an explanation based on the... Problem 17Q: Compare and contrast bonding molecular orbitals with antibonding molecular orbitals. Problem 18Q: What modification to the molecular orbital model was made from the experimental evidence that B2 is... 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: Use the localized electron model to describe the bonding in H2O. Problem 22E: Use the localized electron model to describe the bonding in CCl4. Problem 23E: Use the localized electron model to describe the bonding in H2CO (carbon is the central atom). Problem 24E: Use the localized electron model to describe the bonding in C2H2 (exists as HCCH). Problem 25E: The space-filling models of ethane and ethanol are shown below. Use the localized electron model to... Problem 26E: The space-filling models of hydrogen cyanide and phosgene are shown below. Use the localized... Problem 27E: Give the expected hybridization of the central atom for the molecules or ions in Exercises 81 and 87... Problem 28E: Give the expected hybridization of the central atom for the molecules or ions in Exercises 82 and 88... Problem 29E: Give the expected hybridization of the central atom for the molecules in Exercises 21 and 22. Problem 30E: Give the expected hybridization of the central atom for the molecules in Exercises 27 and 28. Problem 33E: For each of the following molecules, write the Lewis structure(s), predict the molecular structure... Problem 34E: For each of the following molecules or ions that contain sulfur, write the Lewis structure(s),... Problem 35E Problem 36E: The allene molecule has the following Lewis structure: Must all hydrogen atoms lie the same plane?... Problem 37E: Indigo is the dye used in coloring blue jeans. The term navy blue is derived from the use of indigo... Problem 38E: Urea, a compound formed in the liver, is one of the ways humans excrete nitrogen. The Lewis... Problem 39E: Biacetyl and acetoin are added to margarine to make it taste more like butter. Biacetyl Acetion... Problem 40E: Many important compounds in the chemical industry are derivatives of ethylene (C2H4). two of them... Problem 41E: Two molecules used in the polymer industry are azodicarbonamide and methyl cyanoacrylate. Their... Problem 42E: Hot and spicy foods contain molecules that stimulate paindetecting nerve endings. Two such molecules... Problem 43E: One of the first drugs to be approved for use in treatment of acquired immune deficiency syndrome... Problem 44E: Minoxidil (C9H15N15O) is a compound produced by the Pharmacia Upjohn Company that has been approved... Problem 45E: Consider the following molecular orbitals formed from the combination of two hydrogen 1s orbitals:... Problem 46E: Sketch the molecular orbital and label its type ( or , bonding or antibonding) that would be formed... Problem 47E: Which of the following are predicted by the molecular orbital model to be stable diatomic species?... Problem 48E: Which of the following are predicted by the molecular orbital model to be stable diatomic species?... Problem 49E: Using the molecular orbital model, write electron configurations for the following diatomic species... Problem 50E: Consider the following electron configuration: (3s)2(3s)2(3p)2(3p)4(3p)4 Give four species that, in... Problem 52E: Using the molecular orbital model to describe the bonding in F2+, F2, and F2, predict the bond... Problem 54E: A Lewis structure obeying the octet rule can be drawn for O2 as follows: Use the molecular orbital... Problem 55E: Using the molecular orbital model, write electron configurations for the following diatomic species... Problem 56E: Using the molecular orbital model, write electron configurations for the following diatomic species... Problem 57E: In which of the following diatomic molecules would the bond strength be expected to weaken as an... Problem 58E: In terms of the molecular orbital model, which species in each of the following two pairs will roost... Problem 59E: Show how two 2p atomic orbitals can combine to form a or a molecular orbital. Problem 60E: Show how a hydrogen 1s atomic orbital and a fluorine 2p atomic orbital overlap to form bonding and... Problem 61E: Use Figs. 4-54 and 4-55 to answer the following questions. a. Would the bonding molecular orbital in... Problem 63E: Acetylene (C2H2) can be produced from the reaction of calcium carbide (CaC2) with water. Use both... Problem 64E: Describe the bonding in NO+, NO, and NO, using both the localized electron and molecular orbital... Problem 65E: Describe the bonding in the O3 molecule and the NO2 ion, using the localized electron model. How... Problem 66E: Describe the bonding in the CO32 ion using the localized electron model. How would the molecular... Problem 67AE: Draw the Lewis structures, predict the molecular structures, and describe the bonding (in terms of... Problem 68AE: The antibiotic thiarubin-A was discovered by studying the feeding habits of wild chimpanzees in... Problem 69AE: Two structures can be drawn for cyanuric acid: a. Are these two structures the same molecule?... Problem 70AE: Give the expected hybridization for the molecular structures illustrated in the previous question. Problem 71AE: Vitamin B6 is an organic compound whose deficiency in the human body can cause apathy, irritability,... Problem 72AE: Aspartame is an artificial sweetener marketed under the name Nutra-Sweet. A partial Lewis structure... Problem 73AE Problem 74AE: The three most stable oxides of carbon are carbon monoxide (CO), carbon dioxide (CO2), and carbon... Problem 76AE: Complete the following resonance structures for POCl3. a. Would you predict the same molecular... Problem 77AE Problem 78AE: The transport of O2 in the blood is carried out by hemoglobin. Carbon monoxide (CO) can interfere... Problem 79AE: Using molecular orbital theory, explain why the removal of one electron in O2 strengthens bonding,... Problem 80AE: Describe the bonding in the first excited state of N2 (the one closest in energy to the ground... Problem 81AE: Using an MO energy-level diagram, would you expect F2 to have a lower or higher first ionization... Problem 82AE: Show how a dxz. atomic orbital and a pz, atomic orbital combine to form a bonding molecular orbital.... Problem 83AE: What type of molecular orbital would result from the in-phase combination of the two dxz atomic... Problem 84AE: Consider three molecules: A, B, and C. Molecule A has a hybridization of sp3 Molecule B has two more... Problem 86CWP: Draw the Lewis structures for TeCl4, ICl5, PCl5, KrCl4, and XeCl2. Which of the compounds exhibit at... Problem 87CWP: A variety of chlorine oxide fluorides and related cations and anions are known. They tend to be... Problem 88CWP: Pelargondin is the molecule responsible for the red color of the geranium flower. It also... Problem 89CWP: Complete a Lewis structure for the compound shown below, then answer the following questions. What... Problem 90CWP: Which of the following statements concerning SO2 is(are) true? a. The central sulfur atom is sp2... Problem 91CWP: Consider the molecular orbital electron configurations for N2, N2+, and N2. For each compound or... Problem 92CWP: Place the species B2+ , B2, and B2 in order of increasing bond length and increasing bond energy. Problem 93CP: Consider the following computer-generated model of caffeine: Complete a Lewis structure for caffeine... Problem 94CP: Cholesterol (C27liu;O) has the following structure: In such shorthand structures, each point where... Problem 95CP: Cyanamide (H2NCN), an important industrial chemical, is produced by the following steps: Calcium... Problem 97CP: A flask containing gaseous N2 is irradiated with 25-nm light. a. Using the following information,... Problem 99CP: Values of measured bond energies may vary greatly depending on the molecule studied. Consider the... Problem 100CP: Use the MO model to explain the bonding in BeH2. When constructing the MO energy-level diagram,... Problem 101CP Problem 102CP: Arrange the following from lowest to highest ionization energy: O, O2, O2 , O2+. Explain your... Problem 103CP: Use the MO model to determine which of the following has the smallest ionization energy: N2, O2,... Problem 104CP: Given that the ionization energy of F2 is 290 kJ/mol, do the following: a. Calculate the bond energy... Problem 105CP: Carbon monoxide (CO) forms bonds to a variety of metals and metal ions. liS ability to bond to iron... Problem 106CP Problem 107IP: As the bead engineer of your starship in charge of the warp drive, you notice that the supply of... Problem 109IP: Determine the molecular structure and hybridization of the central atom X in the polyatomic ion XY3+... Problem 110IP: Although nitrogen trifluoride (NF3) is a thermally stable compound, nitrogen triiodide (NI3) is... Problem 68AE: The antibiotic thiarubin-A was discovered by studying the feeding habits of wild chimpanzees in...
Related questions
2. X is isoelectronic with Xe. It is reactive with anions. a. Give the electronic configuration and orbital diagram of X. b. Show its reaction with chloride anion and identify the chemical bond formed.
Definition Definition Connection between particles in a compound. Chemical bonds are the forces that hold the particles of a compound together. The stability of a chemical compound greatly depends on the nature and strength of the chemical bonding present in it. As the strength of the chemical bonding increases the stability of the compound also increases.
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