3. Use Kapustinskii's equation and data from Table 4.10 in your textbook to calculate latticeenergies of Cu(OH)2 and CuCO3(4 points)

Step 1:Introduction and Overview of the QuestionThe goal is to use Kapustinskii's equation to…

Answered: 3. Use Kapustinskii's equation and data…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter20: Chemistry Of Selected Transition Elements And Coordination Compounds

Section: Chapter Questions

Problem 84QRT

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4. The common oxidation number for an alkaline earth metal is +2. (a) Using the Born-Mayer equation (for determining the lattice enthalpy) and a Born-Haber cycle (draw it), show that CaCl is an exothermic compound (negative AHf). Make a reasonable prediction to estimate the ionic radius of Ca (explain your reasoning). The sublimation (atomization) enthalpy for Ca(s) is 178 kJ/mol. (b) Show that an explanation for the non-existence of CaCl can be found in the enthalpy change for the reaction below. The AHf for CaCl2(s) is -190.2 kcal/mol. 2 CaCl(s) → Ca(s) + CaCl2(s)
3. On the basis of ionic charge and ionic radii given in Table 1, predict crystal structures for the following materials: ( a. CaO (b) MnS (c) KBr (d) CsBr b. Justify your selections. Table 1: Ionic Radii for Several Cations and Anions Ionic Radius (am) Ionic Cation Radius (nm) Anion 0.053 Br 0.196 Ba?+ Ca?+ 0.136 0.181 0.100 F 0.133 Cs* 0.170 0.220 Fe2+ 0.077 0.140 Fe 0.069 0.184 K* 0.138 Mg Mn2* 0.072 0.067 Na* 0.102 Ni+ 0.069 Sit+ 0.040 0.061
Calcutlate the heat of reaction for: 2NaHCO3(s)->NaCO3+CO2(g)+2H2O(1)
Calculate the lattice energy of AgBr(s) using the following thermodynamic data (all data is in kJ/mol). Ag(s) ΔHsublimation = 265 kJ/mol Ag(g) Ionization energy = 711 kJ/mol Br-Br(g) Bond energy = 173 kJ/mol Br(g) Electron affinity = -345 kJ/mol AgBr(s) ΔH°f = -120 kJ/mol ______________ kJ/mol
Explain in detail and with the aid of diagrams the absence of the C and F type lattices in the Tetragonal system.
Why is SnCl4 not classified as a salt?
Calculate the lattice energy of TICI(s), in kJ/mol, using the following thermodynamic data: Heat of sublimation 161 kJ/mol for TI lonization energy for TI 569 kJ/mol Cl-CI bond energy 223 kJ/mol Electron affinity -369 kJ/mol for CI Heat of formation for -224 kJ/mol TICI
Using the following thermodynamic data, calculate the lattice enthalpy of lithium oxide: Li(g) → Li*(g) + e* AH₁= 540 kJ /mol Li(s) → Li(g) AHS= +146 kJ/mol O₂(s) → 20(g) AH₂= +488 kJ /mol O(g) + 1e →→ O(g) AHA1= -142 kJ /mol O` (g) + 1e¯ → 0²-(g) AHÃ₂= +844 kJ /mol 2Li(s) + 1/2O₂(g) → Li₂O(s) AH₁= -586 kJ /mol NOTE: Give your answer in kJ mol-¹
Why is a potassium salt such as KCI frequently added when one wants to measure elemental sodium by flame photometer? Remember that the potential for the first ionization of potassium is 419 KJ/KJ/ mol while that for sodium is 496 mol
Mercury ions, Hg(1) and Hg(II), are poisonous due to their ability to displace other metal ions in enzymes and disrupt the biological function. a) Are these ions hard or soft? b) Common ligands for metal ions in biological environments are amino acids (building blocks of proteins). Of the amino acids depicted below (focus on the highlighted atoms), which would be the best ligand for Hg(1) and Hg(II), and why? H H H O H3Nt CH2 H H H3N* -c CH2 H3Nt C-c CH2 H3Nt CH2 H3N+-C-c CH CH2 HO CH3 OH SH он H2N H2N Serine (S) Ser Threonine (T) Thr Cysteine Сys Tyrosine (Y) Asparagine (N) Glutamine (Q) Asn Тyr Gln c) Other metal ions that are toxic at certain concentrations include cadmium, chromium, iron, arsenic, and lead. For each of these metals, predict whether they would have similar chemistry to mercury using HSAB concepts. (Note that toxicity is dose-dependent; even water can be poisonous at too high a concentration in the body)
Write expressions for Ksp for each of the ionic compounds: • • BaSO4 Mn(OH)2
8a) Sketch a diagram showing the formation of energy levels from the valence orbitals for Rb, Rb2, Rb3, and Rbn. On the diagram, place arrows indicating how the electrons fill these energy levels. b) How many energy levels are present in the valence band of a single crystal of rubidium with a mass of 48.3 g?

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3. Use Kapustinskii's equation and data from Table 4.10 in your textbook to calculate lattice energies of Cu(OH)2 and CuCO3 (4 points)