Question

calculate the lattice energy of CsCl using a Born-Haber cycle.

Answer #1

Draw the Born-Haber cycle for the formation of CaH2, and
calculate the value for lattice energy? (You will have to look up
the required thermodynamic data)

Construct a Born-Haber cycle to calculate the lattice energy of
MgCl2.
The CRC Handbook of Chemistry and Physics lists the
MgCl2 lattice energy as 2540 kJ mol-1. How does your answer compare
to the literature value?

Construct a Born-Haber cycle diagram that would be used to
determine the lattice energy for RbBr. You will need to draw a
clear diagram with arrows show each step transition. Each step
should clearly have any states and charges noted. There are no
calculations for this question

Construct a Born-Haber cycle for the formation of the
hypothetical compound NaCl2, where the sodium ion has a 2+ charge
(the 2nd ionization energy for sodium is given in Table 7.2 in the
textbook).
Part B
If we were to estimate the lattice energy of NaCl2 to be roughly
equal to that of MgCl2 (2326 kJ/mol from Table 8.2 in the
textbook), what value would you obtain for the standard enthalpy of
formation, ΔH∘f, of NaCl2?
Express your answer using...

Use the Born-Haber cycle, and the following data to
calculate the bond dissociation energy of F2.
Na(g) → Na+(g) + e-(g) ΔrH = IE1 =
500 kJ mol-1
Na(s) → Na(g) ΔsubH = 107 kJ
mol-1
F-(g) → F(g) + e-(g) ΔrH = EA1 = 329
kJ mol-1
Na(s) + 1/2 F2(g) → NaF(s) ΔfH =
-569 kJ mol-1
Na+(g) + F-(g) → NaF(s) ΔlattH =
-928 kJ mol-1

Which pair of compounds is listed in order of increasing (more
exothermic) lattice energy?
LiF < LiI
NaCl < KCl
MgO < CsCl
CaO < BaCl2
LiF < MgO

1. Which of the following transition(s) is/are necessary to
construct a Born Haber Cycle for the formation of NaCl solid?
Multiple answers: You can select more than one option
A) Na(s) → Na(l)
B) Na(s) → Na(g)
C) Na(g) → Na^++(g) + e^-−
D) Cl_22(g) → 2Cl(g)
E) Na(s) + ½ Cl_22(g) →NaCl(s)
2. Which of these transitions are exothermic processes? Multiple
answers are accepted.
A) Na(g) → Na(l)
B) Na(s) → Na(g)
C) Na(g) → Na^++(g) + e^-−
D)...

Using the thermochemical data and an estimated value of -2235.2
kJ/mol for the lattice energy for potassium oxide, calculate the
value for the second electron affinity of oxygen
[O− + e- → O2−]. (The answer is 748.5
kJ/mol)
Quantity
Numerical Value
(kJ/mol)
Enthalpy of atomization of K
89
Ionization energy of K
418.8
Enthalpy of formation of solid K2O
-363
Enthalpy of formation of O(g) from O2(g)
249.1
First electron attachment enthalpy of O -141.0

1. Sketch energy dispersion relations for:-
(i) a linear monoatomic lattice,
(ii) a linear diatomic lattice.

calculate the percent ionic character of the interatomic bonds
for the following materials: CsCl , CsBr

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