Student Solutions Manual for Zumdahl/Zumdahl/DeCoste?s Chemistry, 10th Edition
10th Edition
ISBN: 9781305957510
Author: ZUMDAHL, Steven S.; Zumdahl, Susan A.; DeCoste, Donald J.
Publisher: Cengage Learning
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Chapter 8, Problem 26Q
In general the higher the charge on the ions in an ionic compound, the more favorable the lattice energy. Why do some stable ionic compounds have +1 charged ions even though +4, + 5, and +6 charged ions would have a more favorable lattice energy?
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Chapter 8 Solutions
Student Solutions Manual for Zumdahl/Zumdahl/DeCoste?s Chemistry, 10th Edition
Ch. 8 - Distinguish between the terms electronegativity...Ch. 8 - When an element forms an anion, what happens to...Ch. 8 - Define the term lattice energy. Why,...Ch. 8 - Explain how bond energies can be used to estimate...Ch. 8 - Prob. 5RQCh. 8 - Explain the terms resonance and delocalized...Ch. 8 - Define formal charge and explain how to calculate...Ch. 8 - Give two requirements that should be satisfied for...Ch. 8 - Consider the following compounds: CO2, SO2, KrF2,...Ch. 8 - Explain the electronegativity trends across a row...
Ch. 8 - The ionic compound AB is formed. The charges on...Ch. 8 - Prob. 3ALQCh. 8 - The bond energy for a CH bond is about 413 kJ/mol...Ch. 8 - Prob. 5ALQCh. 8 - Which has the greater bond lengths: NO2 or NO3?...Ch. 8 - The following ions are best described with...Ch. 8 - The second electron affinity values for both...Ch. 8 - What is meant by a chemical bond? Why do atoms...Ch. 8 - Why are some bonds ionic and some covalent?Ch. 8 - How does a bond between Na and Cl differ from a...Ch. 8 - Arrange the following molecules from most to least...Ch. 8 - Does a Lewis structure tell which electron come...Ch. 8 - True or false? In general, a large atom has a...Ch. 8 - What is the central idea of the VSEPR model?Ch. 8 - In Section 8.13 of the text, the term effective...Ch. 8 - Describe the type of bonding that exists in die...Ch. 8 - Some plant fertilizer compounds are (NH4)2SO4,...Ch. 8 - Some of the important properties of ionic...Ch. 8 - What is the electronegativity trend? Where does...Ch. 8 - Give one example of a compound having a linear...Ch. 8 - When comparing the size of different ions, the...Ch. 8 - In general the higher the charge on the ions in an...Ch. 8 - Combustion reactions of fossil fuels provide most...Ch. 8 - Which of the following statements is/are true?...Ch. 8 - Prob. 29QCh. 8 - The molecules BF3, CF4, CO2, PF5, and SF6 are all...Ch. 8 - Without using Fig. 3-4, predict the order of...Ch. 8 - Without using Fig. 3-4, predict the order of...Ch. 8 - Without using Fig. 3-4, predict which bond in each...Ch. 8 - Without using Fig. 3-4, predict which bond in each...Ch. 8 - Prob. 35ECh. 8 - Prob. 36ECh. 8 - Which of the following incorrectly shows the bond...Ch. 8 - Indicate the bond polarity (show the partial...Ch. 8 - Predict the type of bond (ionic, covalent, or...Ch. 8 - List all the possible bonds that can occur between...Ch. 8 - Hydrogen has an electronegativity value between...Ch. 8 - Rank the following bonds in order of increasing...Ch. 8 - State whether or not each of the following has a...Ch. 8 - The following electrostatic potential diagrams...Ch. 8 - Prob. 45ECh. 8 - Prob. 46ECh. 8 - Predict the empirical formulas of the ionic...Ch. 8 - Predict the empirical formulas of the ionic...Ch. 8 - Write electron configurations for a. the cations...Ch. 8 - Write electron configurations for a. the cations...Ch. 8 - Which of the following ions have noble gas...Ch. 8 - What noble gas has the same electron configuration...Ch. 8 - Give the formula of a negative ion that would have...Ch. 8 - Prob. 54ECh. 8 - Give three ions that are isoelectronic with neon....Ch. 8 - Consider the ions Sc3+, Cl, K+, Ca2+, and S2....Ch. 8 - Prob. 57ECh. 8 - For each of the following groups, place the atoms...Ch. 8 - Which compound in each of the following pairs of...Ch. 8 - Which compound in each of the following pairs of...Ch. 8 - Use the following data for potassium chloride to...Ch. 8 - Use the following data for magnesium fluoride to...Ch. 8 - Consider the following energy changes: E(kJ/mol)...Ch. 8 - Compare the electron affinity of fluorine to the...Ch. 8 - Prob. 65ECh. 8 - Use the following data (in kJ/mol) to estimate E...Ch. 8 - Rationalize the following lattice energy values:...Ch. 8 - The lattice energies of FeCl3, FeCl2, and Fe2O3...Ch. 8 - Use bond energy values (Table 3-3) to estimate E...Ch. 8 - Use bond energy values (Table 3-3) to estimate E...Ch. 8 - Prob. 71ECh. 8 - Acetic acid is responsible for the sour taste of...Ch. 8 - Use bond energies to predict E for the following...Ch. 8 - The major industrial source of hydrogen gas is by...Ch. 8 - Use bond energies to estimate E for the combustion...Ch. 8 - Prob. 76ECh. 8 - Prob. 77ECh. 8 - Consider the following reaction: A2+B22AB E =...Ch. 8 - Compare your answers from parts a and b of...Ch. 8 - Compare your answers from Exercise 72 to the H...Ch. 8 - The standard enthalpies of formation for S(g),...Ch. 8 - Use the following standard enthalpies of formation...Ch. 8 - The standard enthalpy of formation for N2H2(g) is...Ch. 8 - The standard enthalpy of formation for NO(g) is...Ch. 8 - Write Lewis structures that obey the octet rule...Ch. 8 - Write Lewis structures that obey the octet rule...Ch. 8 - Write Lewis structures that obey the octet rule...Ch. 8 - Write Lewis structures that obey the octet rule...Ch. 8 - One type of exception to the octet rule are...Ch. 8 - Lewis structures can be used to understand why...Ch. 8 - The most common exceptions to the octet rule are...Ch. 8 - Prob. 92ECh. 8 - Write Lewis structures for the following. Show all...Ch. 8 - Prob. 94ECh. 8 - Benzene (C6H6) consists of a six-membered ring of...Ch. 8 - Borazine (B3N3H6) has often been called inorganic...Ch. 8 - An important observation supporting the concept of...Ch. 8 - Consider the following bond lengths: CO143pmC9O123...Ch. 8 - A toxic cloud covered Bhopal, India, in December...Ch. 8 - Prob. 103ECh. 8 - Prob. 104ECh. 8 - Write Lewis structures that obey the octet rule...Ch. 8 - Write Lewis structures for the species in Exercise...Ch. 8 - Oxidation of the cyanide ion produces the stable...Ch. 8 - When molten sulfur reacts with chlorine gas, a...Ch. 8 - Carbon and sulfur form compounds with each other...Ch. 8 - Prob. 112ECh. 8 - Predict the molecular structure and bond angles...Ch. 8 - Predict die molecular structure and bond angles...Ch. 8 - There are several molecular structures based on...Ch. 8 - Two variations of the octahedral geometry (see...Ch. 8 - Prob. 117ECh. 8 - Consider the molecular structures illustrated in...Ch. 8 - Predict the molecular structure (including bond...Ch. 8 - Predict the molecular structure (including bond...Ch. 8 - Predict the molecular structure (including bond...Ch. 8 - Predict the molecular structure (including bond...Ch. 8 - Prob. 123ECh. 8 - Which of the molecules in Exercise 120 have net...Ch. 8 - Which of the molecules in Exercise 121 have net...Ch. 8 - Which of the molecules in Exercise 122 have net...Ch. 8 - Write Lewis structures and predict the molecular...Ch. 8 - Write Lewis structures and predict whether each of...Ch. 8 - Consider the following Lewis structure where E is...Ch. 8 - Consider the following Lewis structure where E is...Ch. 8 - Two different compounds exist having the formula...Ch. 8 - Two different compounds have the formula XeF2Cl2....Ch. 8 - Arrange the following in order of increasing...Ch. 8 - For each of the following, write an equation that...Ch. 8 - Use bond energies (table 3-3), values of electron...Ch. 8 - Write Lewis structures for CO32, HCO3, and H2CO3....Ch. 8 - Which member of the following pairs would you...Ch. 8 - What do each of the following sets of...Ch. 8 - Prob. 139AECh. 8 - Although both Br3 and I3 ions are known, the F3...Ch. 8 - Prob. 142AECh. 8 - Which of the following molecules have not dipole...Ch. 8 - Prob. 145AECh. 8 - Look up the energies for the bonds in CO and N2....Ch. 8 - Classify the bonding in each of the following...Ch. 8 - List the bonds PCl, PF, OF, and SiF from least...Ch. 8 - Arrange the atoms and/or ions in the following...Ch. 8 - Use the following data to estimate E for the...Ch. 8 - Use bond energy values to estimate E for the...Ch. 8 - Which of the following compounds or ions exhibit...Ch. 8 - The formulas of several chemical substances are...Ch. 8 - Predict the molecular structure, bond angles, and...Ch. 8 - Use Coulombs Jaw, V=Q1Q240r=2.311019Jnm(Q1Q2r) to...Ch. 8 - Prob. 156CPCh. 8 - Calculate the standard heat of formation of the...Ch. 8 - Given the following information: Energy of...Ch. 8 - Prob. 159CPCh. 8 - Think of forming an ionic compound as three steps...Ch. 8 - The compound NF3 is quite stable, but NCl3, is...Ch. 8 - Three processes that have been used for the...Ch. 8 - The compound hexaazaisowurtzitane is one of the...Ch. 8 - Many times extra stability is characteristic of a...Ch. 8 - The study of carbon-containing compounds and their...Ch. 8 - Draw a Lewis structure for the N,...Ch. 8 - Prob. 167CPCh. 8 - Consider the following computer-generated model of...Ch. 8 - Cholesterol (C27H46O) has the following structure:...Ch. 8 - A compound, XF5, is 42.81% fluorine by mass....Ch. 8 - Identify the following elements based on their...
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- Write all resonance structures of chlorobenzene, C6H5Cl, a molecule with the same cyclic structure as benzene. In all structures, keep the CCl bond as a single bond. Which resonance structures are the most important?arrow_forwardWhat main factors control the magnitude of lattice energies? Give a specific example of a compound that should have a high lattice energy, and explain why its lattice energy is high.arrow_forwardBond Enthalpy When atoms of the hypothetical element X are placed together, they rapidly undergo reaction to form the X2 molecule: X(g)+X(g)X2(g) a Would you predict that this reaction is exothermic or endothermic? Explain. b Is the bond enthalpy of X2 a positive or a negative quantity? Why? c Suppose H for the reaction is 500 kJ/mol. Estimate the bond enthalpy of the X2 molecule. d Another hypothetical molecular compound, Y2(g), has a bond enthalpy of 750 kJ/mol, and the molecular compound XY(g) has a bond enthalpy of 1500 kJ/mol. Using bond enthalpy information, calculate H for the following reaction. X2(g)+Y2(g)2XY(g) e Given the following information, as well as the information previously presented, predict whether or not the hypothetical ionic compound AX is likely to form. In this compound, A forms the A+ cation, and X forms the X anion. Be sure to justify your answer. Reaction: A(g)+12X2(g)AX(s)The first ionization energy of A(g) is 400 kJ/mol. The electron affinity of X(g) is 525 kJ/mol. The lattice energy of AX(s) is 100 kJ/mol. f If you predicted that no ionic compound would form from the reaction in Part e, what minimum amount of AX(s) lattice energy might lead to compound formation?arrow_forward
- Arrange the following series of compounds in order of increasing lattice energies. (a) NaBr, NaCl, KBr (b) MgO, CaO, CaCl2 (c) LiF, BeF2, BeOarrow_forwardCompare your answers from parts a and b of Exercise 69 of Chapter 3 with H values calculated for each reaction using standard enthalpies of formation in Appendix 4. Do enthalpy changes calculated from bond energies give a reasonable estimate of the actual values?arrow_forwardUsing the bond energies in Table 7.2, determine the approximate enthalpy change for each of the following reactions: (a) Cl2(g)+3F2(g)2ClF3(g) (b) H2C=CH2(g)+H2(g)H3CCH3(g) (c) 2C2H6(g)+7O2(g)4CO2(g)+6H2O(g) .arrow_forward
- we would predict that the imaginary ionic compound XF would have a (higher /lower) lattice energy than YyF2 becausearrow_forward5. Consider the following information: 1st ionization energy of Na(g) = 495.8 kJ/mol Bond dissociation energy of O2(g) = 498.4 kJ/mol 1st electron affinity of O(g)=-142.5 kJ/mol 2nd electron affinity of O¹(g) = 844 kJ/mol Lattice energy of Na2O(s) = -2608 kJ/mol Enthalpy of formation of Na2O(s) = -416 kJ/mol a Draw the Born-Haber cycle for Na₂O(s). b Calculate the unknown. 120 C Draw the Lewis symbol for Na₂O.arrow_forwardWhich of the following ionic compounds has the largest lattice energy; that is, which has the lattice energy most favorable to a stable lattice? LiF Lil CsF MgO Cslarrow_forward
- The lattice energy of LiF is 1023 kJ/mol, and the Li–F distance is 201 pm. MgO crystallizes in the same structure as LiF but with a Mg–O distance of 205 pm. Which of the following values most closely approximates the lattice energy of MgO: 256 kJ/mol, 512 kJ/mol, 1023 kJ/mol, 2046 kJ/mol, or 4008 kJ/mol? Explain your choice.arrow_forwardThe lattice energy of NaCl is 769 kJ/mole. Which of the following is a correct statement about NaCl? When one mole each of gaseous Nat and CI- ions form solid NaCl, 769 kJ of heat is consumed. It requires 769 kJ to separate one mole of solid NaCl into one mole of each gaseous Na* and CI- ions. It requires 769 kJ to separate one mole of solid NaCl into gaseous one mole of Na* and two moles of CI- ions.arrow_forwardUse the following data to estimate Δ Hf° for barium chloride. Ba (s) + Cl2 (g) ⟶ BaCl2 (s) Lattice energy = -2056 kJ/mol First ionization energy of Ba = 503 kJ/mol Second ionization energy of Ba = 965 kJ/mol Electron affinity of Cl = -349 kJ/mol Bond energy of Cl2 = 239 kJ/mol Enthalpy of sublimation of Ba = 178 kJ/molarrow_forward
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