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 Chapter8: Bonding: General Concepts
Chapter Questions Section: Chapter Questions
Problem 1RQ: Distinguish between the terms electronegativity versus electron affinity, covalent bond versus ionic... Problem 2RQ: When an element forms an anion, what happens to the radius? When an element forms a cation, what... Problem 3RQ: Define the term lattice energy. Why, energetically, do ionic compounds form? Fig. 3-8 illustrates... Problem 4RQ: Explain how bond energies can be used to estimate E for a reaction. Why is this an estimate of E?... Problem 5RQ Problem 6RQ: Explain the terms resonance and delocalized electrons. When a substance exhibits resonance, we say... Problem 7RQ: Define formal charge and explain how to calculate it. What is the purpose of the formal charge?... Problem 9RQ: Give two requirements that should be satisfied for a molecule to be polar. Explain why CF4 and XeF4... Problem 10RQ: Consider the following compounds: CO2, SO2, KrF2, SO3, NF3, IF3, CF4, SF4, XeF4, PF5, IF5, and SCl6.... Problem 1ALQ: Explain the electronegativity trends across a row and down a column of the periodic table. Compare... Problem 2ALQ: The ionic compound AB is formed. The charges on the ions may be +1, 1; +2, 2; +3, 3; or even larger.... Problem 3ALQ Problem 4ALQ: The bond energy for a CH bond is about 413 kJ/mol in CH4 but 380 kJ/mol in CHBr3. Although these... Problem 5ALQ Problem 6ALQ: Which has the greater bond lengths: NO2 or NO3? Explain. Problem 7ALQ: The following ions are best described with resonance structures. Draw the resonance structures, and... Problem 9ALQ: The second electron affinity values for both oxygen and sulfur are unfavorable (positive). Explain. Problem 10ALQ: What is meant by a chemical bond? Why do atoms form bonds with each other? Why do some elements... Problem 11ALQ: Why are some bonds ionic and some covalent? Problem 12ALQ: How does a bond between Na and Cl differ from a bond between C and O? What about a bond between N... Problem 13ALQ: Arrange the following molecules from most to least polar and explain your order: CH4, CF2C12, CF2H2,... Problem 14ALQ: Does a Lewis structure tell which electron come from which atoms? Explain. Problem 15ALQ: True or false? In general, a large atom has a smaller electro-negativity. Explain. Problem 16ALQ: What is the central idea of the VSEPR model? Problem 17ALQ: In Section 8.13 of the text, the term effective pair is used. What does this term mean? Problem 20Q: Describe the type of bonding that exists in die F2(g) molecule. How does this type of bonding differ... Problem 21Q: Some plant fertilizer compounds are (NH4)2SO4, Ca3(PO4)2, K2O, P2O5, and KC1. Which of these... Problem 22Q: Some of the important properties of ionic compounds are as follows: i. low electrical conductivity... Problem 23Q: What is the electronegativity trend? Where does hydrogen fit into the electronegativity trend for... Problem 24Q: Give one example of a compound having a linear molecular structure that has an overall dipole moment... Problem 25Q: When comparing the size of different ions, the general radii trend discussed in Chapter 2 is usually... Problem 26Q: In general the higher the charge on the ions in an ionic compound, the more favorable the lattice... Problem 27Q: Combustion reactions of fossil fuels provide most of the energy needs of the world. Why do the... Problem 28Q: Which of the following statements is/are true? Correct the false statements. a. It is impossible to... Problem 29Q Problem 30Q: The molecules BF3, CF4, CO2, PF5, and SF6 are all nonpolar, even though they contain polar bonds.... Problem 31E: Without using Fig. 3-4, predict the order of increasing electronegativity in each of the following... Problem 32E: Without using Fig. 3-4, predict the order of increasing electronegativity in each of the following... Problem 33E: Without using Fig. 3-4, predict which bond in each of the following groups will be the most polar.... Problem 34E: Without using Fig. 3-4, predict which bond in each of the following groups will be the most polar.... Problem 35E Problem 36E Problem 37E: Which of the following incorrectly shows the bond polarity? Show the correct bond polarity for those... Problem 38E: Indicate the bond polarity (show the partial positive and partial negative ends) in the following... Problem 39E: Predict the type of bond (ionic, covalent, or polar covalent) one would expect to form between the... Problem 40E: List all the possible bonds that can occur between the elements P, Cs, O, and H. Predict the type of... Problem 41E: Hydrogen has an electronegativity value between boron and carbon and identical to phosphorus. With... Problem 42E: Rank the following bonds in order of increasing ionic character: NO, CaO, CF, BrBr, KF. Problem 43E: State whether or not each of the following has a permanent dipole moment. a. b. c. d. e. f. Problem 44E: The following electrostatic potential diagrams represent CH4, NH3, or H2O. Label each and explain... Problem 45E Problem 46E Problem 47E: Predict the empirical formulas of the ionic compounds formed from the following pairs of elements.... Problem 48E: Predict the empirical formulas of the ionic compounds formed from the following pairs of elements.... Problem 49E: Write electron configurations for a. the cations Mg2+, K+, and Al3+. b. the anions N3, O2, F, and... Problem 50E: Write electron configurations for a. the cations Sr2+, Cs+, In+, and Pb2+. b. the anions P3, S2, and... Problem 51E: Which of the following ions have noble gas electron configurations? a. Fe2+, Fe3+, Sc3+, Co3+ b.... Problem 52E: What noble gas has the same electron configuration as each of the ions in the following compounds?... Problem 53E: Give the formula of a negative ion that would have the same number of electrons as each of the... Problem 54E Problem 55E: Give three ions that are isoelectronic with neon. Place these ions in order of increasing size. Problem 56E: Consider the ions Sc3+, Cl, K+, Ca2+, and S2. Match these ions to the following pictures that... Problem 57E Problem 58E: For each of the following groups, place the atoms and/or ions in order of decreasing size. a. V,... Problem 59E: Which compound in each of the following pairs of ionic substances has the most negative lattice... Problem 60E: Which compound in each of the following pairs of ionic substances has the most negative lattice... Problem 61E: Use the following data for potassium chloride to estimate E for the reaction: K(s)+12Cl2(g)KCL(s)E=?... Problem 62E: Use the following data for magnesium fluoride to estimate E for the reaction: Mg(s)+F2(g)MgF2(s)E=?... Problem 63E: Consider the following energy changes: E(kJ/mol) Mg(g) Mg+(g) + e 735 Mg+ (g) Mg2+(g) + e 1445... Problem 64E: Compare the electron affinity of fluorine to the ionization energy of sodium. Does the process of an... Problem 65E Problem 66E: Use the following data (in kJ/mol) to estimate E for the reaction S(g)+e S2(g). Include an estimate... Problem 67E: Rationalize the following lattice energy values: Compound Lattice Energy (kJ/mol) CaSe 2862 Na2Se... Problem 68E: The lattice energies of FeCl3, FeCl2, and Fe2O3 are (in no particular order) 2631, 5359, and 14,774... Problem 69E: Use bond energy values (Table 3-3) to estimate E for each of the following reactions in the gas... Problem 70E: Use bond energy values (Table 3-3) to estimate E for each of the following reactions. a. b. Problem 71E Problem 72E: Acetic acid is responsible for the sour taste of vinegar. It can be manufactured using the following... Problem 73E: Use bond energies to predict E for the following reaction: H2S(g)+3F2(g)SF4(g)+2HF(g) Problem 74E: The major industrial source of hydrogen gas is by the following reaction: CH4(g)+H2O(g)CO(g)+3H2(g)... Problem 75E: Use bond energies to estimate E for the combustion of one mole of acetylene:... Problem 76E Problem 77E Problem 78E: Consider the following reaction: A2+B22AB E = 285kJ The bond energy for A2 is one-half the amount of... Problem 79E: Compare your answers from parts a and b of Exercise 69 with H values calculated for each reaction... Problem 80E: Compare your answers from Exercise 72 to the H values calculated from standard enthalpies of... Problem 81E: The standard enthalpies of formation for S(g), F(g), SF4(g), and SF6(g) are + 278.8, + 79.0, 775,... Problem 82E: Use the following standard enthalpies of formation to estimate the NH bond energy in ammonia: N(g),... Problem 83E: The standard enthalpy of formation for N2H2(g) is 95.4 kJ/mol. Use this and the data in Exercise 82... Problem 84E: The standard enthalpy of formation for NO(g) is 90. kJ/mol. Use this and the values for the O=O and... Problem 85E: Write Lewis structures that obey the octet rule (duet rule for H) for each of the following... Problem 86E: Write Lewis structures that obey the octet rule (duet rule for H) for each of the following... Problem 87E: Write Lewis structures that obey the octet rule for each of the following molecules. a. CCl4 b. NCl3... Problem 88E: Write Lewis structures that obey the octet rule for each of the following molecules and ions. (In... Problem 89E: One type of exception to the octet rule are compounds with central atoms having fewer than eight... Problem 90E: Lewis structures can be used to understand why some molecules react in certain ways. Write the Lewis... Problem 91E: The most common exceptions to the octet rule are compounds or ions with central atoms having more... Problem 92E Problem 93E: Write Lewis structures for the following. Show all resonance structures where applicable. a. NO2,... Problem 94E Problem 95E: Benzene (C6H6) consists of a six-membered ring of carbon atoms with one hydrogen bonded to each... Problem 96E: Borazine (B3N3H6) has often been called inorganic benzene. Write Lewis structures for borazine.... Problem 97E: An important observation supporting the concept of resonance in the localized electron model was... Problem 98E: Consider the following bond lengths: CO143pmC9O123 pmC:O109 pm In the Co32 ion, all three C8O bonds... Problem 99E: A toxic cloud covered Bhopal, India, in December 1984 when water leaked into a tank of methyl... Problem 103E Problem 104E Problem 105E: Write Lewis structures that obey the octet rule for the following species. Assign the formal charge... Problem 106E: Write Lewis structures for the species in Exercise 99 that involve minimum formal charges. Problem 108E: Oxidation of the cyanide ion produces the stable cyanate ion, OCN. The fulminate ion, CNO, on the... Problem 109E: When molten sulfur reacts with chlorine gas, a vile-smelling orange liquid forms that has an... Problem 110E: Carbon and sulfur form compounds with each other with the formulas CS2 and C3S2. Draw a Lewis... Problem 112E Problem 113E: Predict the molecular structure and bond angles for each molecule or ion in Exercises 87 and 93. a.... Problem 114E: Predict die molecular structure and bond angles for each molecule or ion in Exercises 88 and 94. a.... Problem 115E: There are several molecular structures based on the trigonal bipyramid geometry (see Table 8.9).... Problem 116E: Two variations of the octahedral geometry (see Table 8.7) are illustrated below. Which of the... Problem 117E Problem 118E: Consider the molecular structures illustrated in the previous exercise. For each structure, give an... Problem 119E: Predict the molecular structure (including bond angles) for each of the following. a. SeO3 b. SeO2 Problem 120E: Predict the molecular structure (including bond angles) for each of the following. a. PCl3 b. SCl2... Problem 121E: Predict the molecular structure (including bond angles) for each of the following. (See Exercises... Problem 122E: Predict the molecular structure (including bond angles) for each of the following. (See Exercises... Problem 123E Problem 124E: Which of the molecules in Exercise 120 have net dipole moments (are polar)? Problem 125E: Which of the molecules in Exercise 121 have net dipole moments (are polar)? Problem 126E: Which of the molecules in Exercise 122 have net dipole moments (are polar)? Problem 127E: Write Lewis structures and predict the molecular structures of the following. (See Exercises 115 and... Problem 128E: Write Lewis structures and predict whether each of the following is polar or nonpolar. a. HOCN... Problem 129E: Consider the following Lewis structure where E is an unknown element: What are some possible... Problem 130E: Consider the following Lewis structure where E is an unknown element: What are some possible... Problem 131E: Two different compounds exist having the formula N2F2. One compound is polar whereas the other is... Problem 132E: Two different compounds have the formula XeF2Cl2. Write Lewis structures for these two compounds,... Problem 133AE: Arrange the following in order of increasing radius and increasing ionization energy. a. N+, N, N b.... Problem 134AE: For each of the following, write an equation that corresponds to the energy given. a. lattice energy... Problem 135AE: Use bond energies (table 3-3), values of electron affinities (table 2-7), and the ionization energy... Problem 136AE: Write Lewis structures for CO32, HCO3, and H2CO3. When acid is added to an aqueous solution... Problem 137AE: Which member of the following pairs would you expect to be more energetically stable? Justify each... Problem 138AE: What do each of the following sets of compounds/ions have in common? a. SO3, NO3, CO32 b. O3, SO2,... Problem 139AE Problem 140AE: Although both Br3 and I3 ions are known, the F3 ion has not been observed. Explain. Problem 142AE Problem 144AE: Which of the following molecules have not dipole moments? For the molecules that are polar, indicate... Problem 145AE Problem 146AE: Look up the energies for the bonds in CO and N2. Although the bond in CO is stronger, CO is... Problem 147CWP: Classify the bonding in each of the following molecules as ionic, polar covalent, or nonpolar... Problem 148CWP: List the bonds PCl, PF, OF, and SiF from least polar to most polar. Problem 149CWP: Arrange the atoms and/or ions in the following groups in order of decreasing size. a. O, O, O2 b.... Problem 150CWP: Use the following data to estimate E for the reaction: Ba(s)+Br2(g)BaBr2(s)E=? Lattice energy 1985... Problem 151CWP: Use bond energy values to estimate E for the following gas phase reaction: C2H4+H2O2CH2OHCH2OH Problem 152CWP: Which of the following compounds or ions exhibit resonance? a. O3 b. CNO c. Asl3 d. CO32 e. AsF3 Problem 153CWP: The formulas of several chemical substances are given in the table below. For each substance in the... Problem 154CWP: Predict the molecular structure, bond angles, and polarity (has a net dipole moment or has no net... Problem 155CP: Use Coulombs Jaw, V=Q1Q240r=2.311019Jnm(Q1Q2r) to calculate the energy of interaction, V. for the... Problem 156CP Problem 157CP: Calculate the standard heat of formation of the compound ICl(g) at 25C. (Hint: Use Table 8.5 and... Problem 158CP: Given the following information: Energy of sublimation of Li(s) = 166 kJ/mol Bond energy of HCl =... Problem 159CP Problem 160CP: Think of forming an ionic compound as three steps (this is a simplification, as with all models):... Problem 161CP: The compound NF3 is quite stable, but NCl3, is very unstable (NCl3, was first synthesized in 1811 by... Problem 162CP: Three processes that have been used for the industrial manufacture of acrylonitrile (CH2CHCN), an... Problem 163CP: The compound hexaazaisowurtzitane is one of the highest-energy explosives known (C E News, Jan. 17,... Problem 164CP: Many times extra stability is characteristic of a molecule or ion in which resonance is possible.... Problem 165CP: The study of carbon-containing compounds and their properties is called organic chemistry. Besides... Problem 166CP: Draw a Lewis structure for the N, N-dimethylformamide molecule. The skeletal structure is Various... Problem 167CP Problem 168CP: Consider the following computer-generated model of caffeine. Draw a Lewis structure for caffeine in... Problem 169CP: Cholesterol (C27H46O) has the following structure: In such shorthand structures, each point where... Problem 171IP: A compound, XF5, is 42.81% fluorine by mass. Identify the element X. What is the molecular structure... Problem 173IP: Identify the following elements based on their electron configurations and rank them in order of... Problem 130E: Consider the following Lewis structure where E is an unknown element: What are some possible...
Related questions
Concept explainers
Which one of the following elements will gain 2 electrons to have the electron configuration of a noble gas when they form a chemical bonding with other elements?
A. N
B. S
C. F
D. Ba
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.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 2 steps with 1 images
