Which ionic solid do you expect to have the most negative lattice energy?MgOO CaCl2O CaSO NaCl

The energy needed for one mole of ionic compounds is formed from its constituents ions is known as…

Answered: Which ionic solid do you expect to have…

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter12: The Solid State

Section12.3: Bonding In Ionic Compounds: Lattice Energy

Problem 1RC

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Element First Ionization Energy (kJImol) Second Ionization Energy (kiImol) I K 419 3050 Ca 590 1140 75. Use principles of atomic structure to answer each of the following: (a) The radius of the Ca atom is 197 pm; the radius of the Ca2+ ion is 99 pm. Account for the difference. (b) The lattice energy of CaO(s) is 3460 kJ/mol; the lattice energy of K2O is 2240 kJ/mol. Account for the difference. (c) Given these ionization values, explain the difference between Ca and K with regard to their first and second ionization energies. Element First Ionization Energy (kJ/mol) Second Ionization Energy (kJ/mol) K 419 3050 Ca 590 1140 (d) The first ionization energy of Mg is 738 kJ/mol and that of Al is 578 kJ/mol. Account for this difference.
7.74 In a lattice, a positive ion is often surrounded by eight negative ions. We might reason, therefore, that the lattice energy should be related to eight times the potential of interaction between these oppositely charged particles. Why is this reasoning too simpler?
The lattice energy of LiF is 1023 kJ/mol, and the Li—F distance is 200.8 pm. NaF crystallizes in the same structure as LiF but with a Na—F distance of 231 pm. Which of the following values most closely approximates the lattice energy of NaF: 510, 890, 1023, 1175, or 4090 kJ/mol? Explain your choice.
Arrange the following series of compounds in order of increasing lattice energies. (a) NaBr, NaCl, KBr (b) MgO, CaO, CaCl2 (c) LiF, BeF2, BeO
Which compound in each of the following pairs has the larger lattice energy? Note: Mg2+ and Li+ have similar radii; O2 and F have similar radii. Explain your choices. (a) MgOorMgSe (b) LiForMgO (c) Li2OorLiCl (d) Li2SeorMgO
The lattice energy of LiF is 1023 kJ/mol, and the LiF 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.
For each of the following, write an equation that corresponds to the energy given. a. lattice energy of NaCl b. lattice energy of NH4Br c. lattice energy of MgS d. O9O double bond energy beginning with O2(g) as a reactant
Which compound in each of the following pairs of ionic substances has the most negative lattice energy? Justify your answers. a. LiF, CsF b. NaBr, NaI c. BaCl2, BaO d. Na2SO4, CaSO4 e. KF, K2O f. Li2O, Na2S
Calculate H for the following process: K(g)+Br(g)KBr(s) The lattice energy of KBr is 689 kJ/mol, and the ionization energy of K is 419 kJ/mol. The electron affinity of Br is given in Table 8.4. See Problem 8.119.

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Which ionic solid do you expect to have the most negative lattice energy? MgO CaCl2 Cas NaCl