- 11.1: Indicate several ways in which the valence-bond method is superior ...
- 11.2: Explain why it is necessary to hybridize atomic orbitals when apply...
- 11.3: Describe the molecular geometry of suggested by each of the followi...
- 11.4: Describe the molecular geometry of suggested by each of the followi...
- 11.5: In which of the following, would you expect to find hybridization o...
- 11.6: In the manner of Example 11-1, describe the probable structure and ...
- 11.7: For each of the following species, identify the central atom(s) and...
- 11.8: Propose a plausible Lewis structure, geometric structure, and hybri...
- 11.9: Describe a hybridization scheme for the central Cl atom in the mole...
- 11.10: Describe a hybridization scheme for the central S atom in the molec...
- 11.11: Match each of the following species with one of these hybridization...
- 11.12: Propose a hybridization scheme to account for bonds formed by the c...
- 11.13: Indicate which of the following molecules and ions are linear, whic...
- 11.14: In the manner of Figure 11-17, indicate the structures of the follo...
- 11.15: Write Lewis structures for the following molecules, and then label ...
- 11.16: Represent bonding in the carbon dioxide molecule, by (a) a Lewis st...
- 11.17: Use the method of Figure 11-18 to represent bonding in each of the ...
- 11.18: Use the method of Figure 11-18 to represent bonding in each of the ...
- 11.19: The molecular model below represents citric acid, an acidic compone...
- 11.20: Malic acid is a common organic acid found in unripe apples and othe...
- 11.21: Shown below are ball-and-stick models. Describe hybridization and o...
- 11.22: Shown below are ball-and-stick models. Describe hybridization and o...
- 11.23: Propose a bonding scheme that is consistent with the structure for ...
- 11.24: The structure of the molecule allene, is shown here. Propose hybrid...
- 11.25: Angelic acid, shown below, occurs in sumbol root, a herb used as a ...
- 11.26: Dimethylolpropionic acid, shown below, is used in the preparation o...
- 11.27: Explain the essential difference in how the valencebond method and ...
- 11.28: Describe the bond order of diatomic carbon, with Lewis theory and m...
- 11.29: has an exceptionally high N21g2 bond energy. Would C2,
- 11.30: The paramagnetism of gaseous has been established. Explain how this...
- 11.31: In our discussion of bonding, we have not encountered a bond order ...
- 11.32: Is it correct to say that when a diatomic molecule loses an electro...
- 11.33: For the following pairs of molecular orbitals, indicate the one you...
- 11.34: For each of the species and (a) Write the molecular orbital diagram...
- 11.35: Write plausible molecular orbital diagrams for the following hetero...
- 11.36: We have used the term isoelectronic to refer to atoms with identica...
- 11.37: Consider the molecules and and use molecular orbital theory to answ...
- 11.38: Consider the molecules and and use molecular orbital theory to answ...
- 11.39: Construct the molecular orbital diagram for CF. Would you expect th...
- 11.40: Construct the molecular orbital diagram for CaF. Would you expect t...
- 11.41: Explain why the concept of delocalized molecular orbitals is essent...
- 11.42: Explain how it is possible to avoid the concept of resonance by usi...
- 11.43: In which of the following molecules would you expect to find deloca...
- 11.44: In which of the following ions would you expect to find delocalized...
- 11.45: Which of the following factors are especially important in determin...
- 11.46: Based on the ground-state electron configurations of the atoms, how...
- 11.47: How many energy levels are present in the 3s conduction band of a s...
- 11.48: Magnesium is an excellent electrical conductor even though it has a...
- 11.49: From this list of terms electrical conductor, insulator, semiconduc...
- 11.50: In what type of material is the energy gap between the valence band...
- 11.51: Which of the following substances, when added in trace amounts to s...
- 11.52: Which of the following substances, when added in trace amounts to g...
- 11.53: The effect of temperature change on the electrical conductivity of ...
- 11.54: Explain why the electrical conductivity of a semiconductor is signi...
- 11.55: The energy gap, for silicon is What is the minimum wavelength of li...
- 11.56: Explain why the solar cell in Figure 11-40 operates over a broad ra...
- 11.57: The Lewis structure of indicates that the nitrogento- nitrogen bond...
- 11.58: Show that both the valence-bond method and molecular orbital theory...
- 11.59: A group of spectroscopists believe that they have detected one of t...
- 11.60: Lewis theory is satisfactory to explain bonding in the ionic compou...
- 11.61: The compound potassium sesquoxide has the empirical formula Show th...
- 11.62: Draw a Lewis structure for the urea molecule, and predict its geome...
- 11.63: Methyl nitrate, is used as a rocket propellant. The skeletal struct...
- 11.64: Fluorine nitrate, is an oxidizing agent used as a rocket propellant...
- 11.65: Draw a Lewis structure(s) for the nitrite ion, Then propose a bondi...
- 11.66: Think of the reaction shown here as involving the transfer of a flu...
- 11.67: In the gaseous state, molecules have two nitrogen-to-oxygen bond di...
- 11.68: does not exist as a stable molecule, but there is evidence that suc...
- 11.69: The molecule formamide, has the approximate bond angles The bond le...
- 11.70: Pyridine, is used in the synthesis of vitamins and drugs. The molec...
- 11.71: One of the characteristics of antibonding molecular orbitals is the...
- 11.72: The ion is linear, but the ion is bent. Describe hybridization sche...
- 11.73: Ethyl cyanoacetate, a chemical used in the synthesis of dyes and ph...
- 11.74: A certain monomer used in the production of polymers has one nitrog...
- 11.75: A solar cell that is 15% efficient in converting solar to electric ...
- 11.76: Toluene-2,4-diisocyanate is used in the manufacture of polyurethane...
- 11.77: The anion is linear, and the anion is V-shaped, with a angle betwee...
- 11.78: Pentadiene, has three isomers, depending on the position of the two...
- 11.79: A conjugated hydrocarbon has an alternation of double and single bo...
- 11.80: Resonance energy is the difference in energy between a real molecul...
- 11.81: The 60-cycle alternating electric current (AC) commonly used in hou...
- 11.82: Furan, is a substance derivable from oat hulls, corn cobs, and othe...
- 11.83: As discussed in the Are You Wondering feature on page 457, the hybr...
- 11.84: In Chapter 10, we saw that electronegativity differences determine ...
- 11.85: Borazine, is often referred to as inorganic benzene because of its ...
- 11.86: Which of the following combinations of orbitals give rise to bondin...
- 11.87: Construct a molecular orbital diagram for HF, and label the molecul...
- 11.88: In your own words, define the following terms or symbols: (a) (b) ;...
- 11.89: Briefly describe each of the following ideas: (a) hybridization of ...
- 11.90: Explain the important distinctions between the terms in each of the...
- 11.91: A molecule in which hybrid orbitals are used by the central atom in...
- 11.92: The bond angle in is best described as (a) between and (b) less tha...
- 11.93: The hybridization scheme for the central atom includes a d orbital ...
- 11.94: Of the following, the species with a bond order of 1 is (a) (b) (c)...
- 11.95: The hybridization scheme for Xe in is (a) (b) (c) (d)
- 11.96: Delocalized molecular orbitals are found in (a) (b) (c) (d)
- 11.97: The best electrical conductor of the following materials is (a) Li(...
- 11.98: A substance in which the valence and conduction bands overlap is (a...
- 11.99: Explain why the molecular structure of cannot be adequately describ...
- 11.100: Why does the hybridization not account for bonding in the molecule ...
- 11.101: What is the total number of (a) bonds and (b) bonds in the molecule
- 11.102: Which of the following species are paramagnetic? (a) (b) (c) Which ...
- 11.103: Use the valence molecular orbital configuration to determine which ...
- 11.104: Use the valence molecular orbital configuration to determine which ...
- 11.105: Which of these diatomic molecules do you think has the greater bond...
- 11.106: Construct a concept map that embodies the ideas of valence bond the...
- 11.107: Construct a concept map that connects the ideas of molecular orbita...
- 11.108: Construct a concept map that describes the interconnection between ...
Solutions for Chapter 11: Chemical Bonding II: Additional Aspects
Full solutions for General Chemistry: Principles and Modern Applications | 10th Edition
ISBN: 9780132064521
Solutions for Chapter 11
17
3
Summary of Chapter 11: Chemical Bonding II: Additional Aspects
Since 108 problems in chapter 11: Chemical Bonding II: Additional Aspects have been answered, more than 193456 students have viewed full step-by-step solutions from this chapter. This expansive textbook survival guide covers the following chapters and their solutions. This textbook survival guide was created for the textbook: General Chemistry: Principles and Modern Applications, edition: 10. Chapter 11: Chemical Bonding II: Additional Aspects includes 108 full step-by-step solutions. General Chemistry: Principles and Modern Applications was written by and is associated to the ISBN: 9780132064521.
Key Chemistry Terms and definitions covered in this textbook
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alkyl amines
A format for naming amines containing simple alkyl groups.
-
coordinate covalent bond.
A bond in which the pair of electrons is supplied by one of the two bonded atoms; also called a dative bond. (9.9)
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cumulated diene
A compound containing two adjacent p bonds.
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Cyanohydrin
A molecule containing an !OH group and a !CN group bonded to the same carbon.
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Henry’s law
A law stating that the concentration of a gas in a solution, Sg, is proportional to the pressure of gas over the solution: Sg = kPg. (Section 13.3)
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hydrate
A compound containing two hydroxyl groups (OH) connected to the same carbon atom.
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monomers
Molecules with low molecular weights, which can be joined together (polymerized) to form a polymer. (Section 12.8)
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nanomaterial
A solid whose dimensions range from 1 to 100 nm and whose properties differ from those of a bulk material with the same composition. (Section 12.1)
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oxaphosphetane
An intermediate that is believed to be formed during Wittig reactions.
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parent ion
In mass spectrometry,the ion that is generated when the compound is ionized.
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Phasing
The sign of the wave function at particular coordinates in space, either plus or minus. Phasing is often represented by colors, such as red or blue
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photoionization
The removal of an electron from an atom or molecule by absorption of light. (Section 18.2)
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polynucleotide
A polymer constructed from nucleotides linked together.
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Primary structure of nucleic acids
The sequence of bases along the pentose-phosphodiester backbone of a DNA or RNA molecule read from the 5’ end to the 3’ end
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Tesla (T)
The SI unit for magnetic fi eld strength.
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thermodynamic control
A reaction for which the ratio of products is determined solely by the distribution of energy among the products.
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Thermodynamic control
Experimental conditions that permit the establishment of equilibrium between two or more products of a reaction. The composition of the product mixture is determined by the relative stabilities of the products.
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Thermoset plastic
A polymer that can be molded when it is fi rst prepared, but once cooled, hardens irreversibly and cannot be remelted.
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Valence-shell electron-pair repulsion (VSEPR)
A method for predicting bond angles based on the idea that electron pairs repel each other and keep as far apart as possible.
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Zwitterion
An internal salt of an amino acid; the carboxylate is negatively charged, and the ammonium group is positively charged