Arrange the following compounds in order of increasing expected lattice energy.Hint-use coulomb's law to estimate:KQ1Q2E =αQ+QIR++IR_Where the numerator is the product of the ion charges and the denominator is the sum of the ionic radii. More negative E means greater LE.Lowest LE1MgCl22⠀⠀Sro3SrCl2Highest LEMgO

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Answered: Arrange the following compounds in…

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Write the empirical formula of at least four binary ionic compounds that could be formed from the following ions: Ca+2, V+5, F−,O−2
1) Calculate the lattice energy for NaCl(s) using a Born-Haber cycle and the following information: NaCl(s) → Nat(g) + Cl-(g) Na(s) + 1/2 C12(g) → NaCl(s) Na(s) → Na(g) Na(g) → Na+(g) + e- 1/2 C12(g) → Cl(g) Cl(g) + e- → Cl-(g) ? -411.0 kJ/mol +107.3 kJ/mol +495.8 kJ/mol +121.7 kJ/mol -348.6 kJ/mol
Write the empirical formula for at least four ionic compounds that could be formed from the following ions: 2+ 3+ Fe²+, MnO, CO, Fe³+ 11 0,0,... X
Consider an ionic compound, MX, , composed of generic metal M and generic gaseous halogen X. • The enthalpy of formation of MX, is AH; = -813 kJ/mol. t. • The enthalpy of sublimation of M is AHsub = 181 kJ/mol. • The first, second, and third ionization energies of M are IE¡ = 589 kJ/mol, IE2 = 1609 kJ/mol, and IE3 = 2571 kJ/mol. • The electron affinity of X is AHEA = -321 kJ/mol. (Refer to the hint). • The bond energy of X, is BE = 179 kJ/mol. Determine the lattice energy of MX,. AHjattice = kJ/mol
Write the empirical formula of at least four binary ionic compounds that could be formed from the following ions: Mg²+, Al³+, I, 0²- 0,0,... X
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Place the following elements in... increasing electronegativity: Se Cl S increasing ionization energy: Al P Sr increasing affinity for electrons: K Ge Cl increasing lattice energy: Na2S KCl MgS
Given the following information, use the Kapustinskii equation (shown below and included in the additional information sheet I encouraged you to download and have available) to calculate the lattice energy for Cr2S3 in kJ/mol. Ionic radii: Cr3+ (62 pm), S2− (184 pm) d* = 34.5 pm Κ = 1.21 × 105 kJ pm/mol
Write the empirical formula of at least four binary ionic compounds that could be formed from the following ions: 2+ 3+ Mgʻ", Al*, Br,s²-
Using the following data, estimate the overall enthalpy of formation (in kJ/mol) for potassium chloride: K(s) + ½ Cl₂(g) → KCI(s). Process Lattice energy of KCI lonization energy of K Electron affinity of Cl Bond dissociation energy of Cl, Enthalpy of sublimation for K Question 21 of 28 Change in Energy (AHO) -690 kJ/mol 419 kJ/mol -349 kJ/mol 239 kJ/mol 90 kJ/mol
Write the empirical formula of at least four binary ionic compounds that could be formed from the following ions: 2+ Zn*, v°*, F¯, O²- 0,..

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