Chemistry & Chemical Reactivity
9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Chapter 12, Problem 50GQ
Using the thermochemical data below and an estimated value of −2481 kJ/mol for the lattice energy for Na2O, calculate the value for the second
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Using the following data, calculate the lattice energy of calcium chloride:
Ca2+(g) + 2Cl– (g) → CaCl2(s) ΔHlattice = ?
Sublimation enthalpy of calcium ΔH = 177.8 kJ/mol
First ionization energy of calcium ΔH = 590.2 kJ/mol
Second ionization energy of calcium ΔH = 1144.2 kJ/mol
First electron affinity of chlorine ΔH = –349 kJ/mol
Heat of formation of CaCl2(s) ΔH = –795.4 kJ/mol
Bond energy of Cl2 (see Table 2)
Use Hess’s law to calculate the lattice energy of calcium chloride. set-up must show all the chemical equations and you must show how their H values add up to give your answer.
Use the Born-Haber cycle to calculate the lattice energy of KF. [The heat of sublimation of K is 91.6 kJ·mol−1 and
ΔfH(KF) = −567.3 kJ·mol−1.
Bond enthalpy for F2 is
158.8 kJ·mol−1.
Other data may be found in the Ionization Energies Table and the Electron Affinities Table.]
The standard heat of formation of BaBr2BaBr2 is −−764 kJ/molkJ/mol. The first ionization energy of BaBa is 503 kJ/molkJ/mol and its second ionization energy is 965 kJ/molkJ/mol. The heat of sublimation of Ba[Ba(s)→Ba(g)]Ba[Ba(s)→Ba(g)] is 175 kJ/molkJ/mol. The bond energy of Br2Br2 is 193 kJ/molkJ/mol, the heat of vaporization of Br2(l)Br2(l) is 31 kJ/molkJ/mol, and the electron affinity of BrBr is −−325 kJ/molkJ/mol.
Calculate the lattice energy of BaBr2BaBr2.
Chapter 12 Solutions
Chemistry & Chemical Reactivity
Ch. 12.1 - (a) Determining an Atom Radius from Lattice...Ch. 12.1 - Prob. 1RCCh. 12.1 - Prob. 2RCCh. 12.2 - If an ionic solid has an fcc lattice of anions (X)...Ch. 12.2 - Potassium chloride has the same unit cell as NaCl....Ch. 12.2 - 1. The unit cell of silicon carbide. SiC is...Ch. 12.2 - If one edge of the silicon carbide unit cell is...Ch. 12.2 - Prob. 1QCh. 12.2 - Describe the unit cell of lithium (see Figure).Ch. 12.2 - Prob. 3Q
Ch. 12.2 - Prob. 4QCh. 12.3 - Prob. 1RCCh. 12.3 - Prob. 2RCCh. 12.3 - Prob. 3RCCh. 12.4 - Prob. 1RCCh. 12.5 - Prob. 1QCh. 12.5 - Prob. 2QCh. 12.5 - Prob. 3QCh. 12.5 - 1. Which of the following allotropes of carbon is...Ch. 12.5 - Prob. 2RCCh. 12.6 - Prob. 1RCCh. 12.6 - Suppose you wanted to cool 100. g of water from 20...Ch. 12.7 - Prob. 1RCCh. 12.7 - How many tin atoms are contained in the tetragonal...Ch. 12.7 - Prob. 2QCh. 12.7 - Prob. 3QCh. 12.7 - Prob. 4QCh. 12 - Outline a two-dimensional unit cell for the...Ch. 12 - Outline a two-dimensional unit cell for the...Ch. 12 - Prob. 3PSCh. 12 - Rutile, TiO2, crystallizes in a structure...Ch. 12 - Cuprite is a semiconductor. Oxide ions are at the...Ch. 12 - The mineral fluorite, which is composed of calcium...Ch. 12 - Calcium metal crystallizes in a face-centered...Ch. 12 - The density of copper metal is 8.95 g/cm3. If the...Ch. 12 - Potassium iodide has a face-centered cubic unit...Ch. 12 - A unit cell of cesium chloride is illustrated in...Ch. 12 - Predict the trend in lattice energy, from least...Ch. 12 - Prob. 12PSCh. 12 - To melt an ionic solid, energy must be supplied to...Ch. 12 - Which compound in each of the following pairs...Ch. 12 - Prob. 15PSCh. 12 - Prob. 16PSCh. 12 - Considering only the molecular orbitals formed by...Ch. 12 - Prob. 18PSCh. 12 - Prob. 19PSCh. 12 - Prob. 20PSCh. 12 - Prob. 21PSCh. 12 - Prob. 22PSCh. 12 - Prob. 23PSCh. 12 - Prob. 24PSCh. 12 - A diamond unit cell is shown here. Unit cell of...Ch. 12 - The structure of graphite is given in Figure...Ch. 12 - We have identified six types of solids (metallic,...Ch. 12 - Prob. 28PSCh. 12 - Classify each of the following materials as...Ch. 12 - Prob. 30PSCh. 12 - Benzene, C6H6, is an organic liquid that freezes...Ch. 12 - The specific heat capacity of silver is 0.235 J/g ...Ch. 12 - Prob. 33PSCh. 12 - Prob. 34PSCh. 12 - Prob. 35PSCh. 12 - If your air conditioner is more than several years...Ch. 12 - Sketch a phase diagram for O2 from the following...Ch. 12 - Tungsten crystallizes in the unit cell shown here....Ch. 12 - Silver crystallizes in a face-centered cubic unit...Ch. 12 - The unit cell shown here is for calcium carbide....Ch. 12 - The very dense metal iridium has a face-centered...Ch. 12 - Vanadium metal has a density of 6.11 g/cm3....Ch. 12 - Prob. 43GQCh. 12 - Prob. 44GQCh. 12 - Prob. 45GQCh. 12 - Consider the three types of cubic units cells. (a)...Ch. 12 - The solid-state structure of silicon is shown...Ch. 12 - The solid-state structure of silicon carbide is...Ch. 12 - Spinels are solids with the general formula AB2O4...Ch. 12 - Using the thermochemical data below and an...Ch. 12 - Prob. 51GQCh. 12 - Prob. 52GQCh. 12 - Prob. 53GQCh. 12 - Prob. 54GQCh. 12 - Prob. 55GQCh. 12 - Prob. 56GQCh. 12 - Like ZnS, lead(II) sulfide, PbS (commonly called...Ch. 12 - CaTiO3, a perovskite, has the structure below. (a)...Ch. 12 - Potassium bromide has the same lattice structure...Ch. 12 - Calculate the lattice energy of CaCl2 using a...Ch. 12 - Why is it not possible for a salt with the formula...Ch. 12 - Prob. 63SCQCh. 12 - Prob. 64SCQCh. 12 - Prob. 65SCQCh. 12 - Phase diagrams for materials that have allotropes...
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- Arrange the following series of compounds in order of increasing lattice energies. (a) NaBr, NaCl, KBr (b) MgO, CaO, CaCl2 (c) LiF, BeF2, BeOarrow_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_forwardEstimate H for the following reactions using bond energies given in Table 8.5. 3CH2=CH2(g) + 3H2(g) 3CH2CH3(g) The enthalpies of formation for C6H6(g) and C6H12 (g) are 82.9 and 90.3 kJ/mol. respectively. Calculate H for the two reactions using standard enthalpies of formation from Appendix 4. Account for any differences between the results obtained from the two methods.arrow_forward
- Consider the reactions of silver metal, Ag(s), with each of the halogens: fluorine, F2(g), chlorine, Cl2(g), and bromine, Br2(l). What chapter data could you use to decide which reaction is most exothermic? Which reaction is that?arrow_forwardbased on the following information calculate the approximate lattice energy of XCl2.X is 3x larger than Na+. The lattice energy for NaCl is 787kj/molearrow_forwardHow can I use the Born Haber cycle to establish the lattice energy of CsCl (s)from the following data: ΔHf° [CsCl(s)] = -442.8 kJ/mol; enthalpy of sublimation of Cesium is 78.2 kJ/mol; enthalpy of dissociation of Cl2 (g) = 243 kJ/mol Cl2 ; IE1 for Cs(g) = 375.7 kJ/mol; electron affinity enthalpy-EA1 for Cl(g) = -349kJ/mol.arrow_forward
- Use 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_forwardUse the data given below to construct a Born-Haber cycle to determine the lattice energy of CaO. A H°(kJ) Ca(s) → Ca(g) 193 Ca(g) → Cat (g) + e 590 Cat (g) → Ca2+(g) + e 1010 20(g) → O2(g) -498 O(g) + e O(g) -141 O(g) + e → O2(g) 878 Ca(s) + O2(g) → CaO(s) -> -635 O-2667 kJ O-3414 kJ O +1397 kJ +3028 kJ O-2144 kJarrow_forwardUse the following data to calculate the enthalpy change for the following reaction: 2Na(s) + O2(g) -> Na2O(s) Quantity Magnitude (kJ/mol) Ionization energy of Na(g) 495 Electron affinity of O(g) for 2e 603 Vaporization energy of Na(s) 109 Bond energy of O2(g) 499 Lattice energy for Na2O(s) –2,477arrow_forward
- Estimate the ionic radius of Cs+. The lattice energy of CsCl is 633 kJ/mol. For CsCl the Madelungconstant, M, is 1.763, and the Born exponent, n, is 10.7. The ionic radius of Cl– is known to be 1.81 Åarrow_forwardUse the data given below to construct a Born-Haber cycle to determine the lattice energy of CaO. △ H°(kJ) Ca(s) → Ca(g) 193 Ca(g) → Ca+1(g) + e⁻ 590 Ca+1(g) → Ca+2(g) + e⁻ 1010 2 O(g) → O2(g) -498 O(g) + e⁻ → O-1(g) -141 O-1(g) + e⁻ → O-2(g) 878 Ca(s) + (1/2) O2(g) → CaO(s) -635arrow_forward1a)Rank the following ionic compounds in order of lattice energy, from the least exothermic (least negative lattice enthalpy) to the most exothermic (most negative lattice enthalpy): KCI, SrO, RbBr, CaO 1b)Rank the following elements in order of decreasing metallic character (from most metallic to least metallic): S, CI, K, Cs, Se 1c) by using the table of bond enthalpies, predict ?rH of the following reaction in kJ/mol H2C=CH2 + Cl2 ---> Cl-CH2-CH2-Clarrow_forward
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