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Inorganic Chemistry Lattice Energy Calculations

This document contains 8 problems related to inorganic chemistry concepts like lattice energies, crystal structures, and densities. Problem 1 asks to calculate lattice energies for 4 ionic compounds using the Kapustinskii equation. Problem 2 asks about the crystal structure and bonding of RbCaF3. Problem 3 asks to calculate the density of nickel given its cubic close packing structure and unit cell edge length. The remaining problems ask to calculate various properties related to crystal structures, lattice energies, and densities for additional ionic compounds.

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383 views1 page

Inorganic Chemistry Lattice Energy Calculations

This document contains 8 problems related to inorganic chemistry concepts like lattice energies, crystal structures, and densities. Problem 1 asks to calculate lattice energies for 4 ionic compounds using the Kapustinskii equation. Problem 2 asks about the crystal structure and bonding of RbCaF3. Problem 3 asks to calculate the density of nickel given its cubic close packing structure and unit cell edge length. The remaining problems ask to calculate various properties related to crystal structures, lattice energies, and densities for additional ionic compounds.

Uploaded by

retno sari
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© © All Rights Reserved
We take content rights seriously. If you suspect this is your content, claim it here.
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Inorganic Chemistry 2

1. Use the Kapustinskii equation to determine the lattice energies for the following: (a)
RbCl; (b) NaI; (c) MgCl2 ; (d) LiF.
2. RbCaF3 has the perovskite structure with the Ca in the center of the unit cell. What is the
electrostatic bond character of each of the Ca-F bonds? How many fluoride ions must
2+
surround each Ca ion? What is the electrostatic bond character of each Rb–F bond? How
- +
many F ions surround each Rb ?.
3. The nickel crystal has a cubic close packing arrangement with an edge length of 352,4
nm. Using this information, calculate the density of nickel.
4. Potassium fluoride crystallizes in a sodium chloride lattice. The length of the edge of the
unit cell (sometimes called the cell or lattice constant) has the value 267 pm for KF:
a. Calculate the attraction between that exists for 1 mole of KF.
b. Using the Kapustinskii equation, calculate the lattice energy for KF. The ionic radii
+ -
are 138 and 133 pm, respectively, for K and F .
c. Explain why the values in parts (a) and (b) are different.
d. Use the results obtained in parts (a) and (b) to evaluate the appropriate value of n in
the Born-Landé.
5. Predict the crystal type for each of the following using the radius ratio: (a) K2S (b) NH4
Br (c) CoF2 (d) TiF2 (e) FeO.
6. KBr crystallizes in a sodium chloride lattice arrangement with a cell edge length of 314
pm.
a. Calculate the total attraction in 1 mole of KBr.
b. Calculate the actual lattice energy by means of the Kapustinskii equation or a
thermochemical cycle.
c. Explain why the values determined in parts (a) and (b) are different.
d. Using the results from (a) and (b), evaluate the value of n that is correct in this case
according to:
N Ae2  1
U 0
1  
r  n
-10 1/2 3/2 -1
Note: e =4,8x10 esu and 1 esu =1 g cm sec .
7. The edge of the unit cell in a crystal is sometimes called the lattice or cell constant. The
structure known as antifluorite is the structure of K 2O and its cell constant is 644 pm.
Determine the value for each of the following:
+
(a) The distance between K ions.
+ 2-
(b) The distance between K and O ions.
2-
(c) The distance between O ions .
(d) The density of K2O.
-1
8. The lattice energy of AgBr is 895 KJ mol . Predict the Lattice energy of the isomorphous
AgI using Born Lande equation. The value of r c + ra is 321pm for AgBr and 342pm for
AgI

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