11. Bonding & Molecular Structure

Born Haber Cycle

Born Haber Cycle, Basic Introduction, Lattice Energy, Hess Law & Enthalpy of Formation - Chemistry

Use the Born–Haber cycle and data from Appendix IIB, Chapter 8
and this chapter to calculate the lattice energy of KCl. (ΔHsub for
potassium is 89.0 kJ>mol.)

Constructing Born - Haber Cycles | A-level Chemistry | OCR, AQA, Edexcel

Lattice Energy and the Born-Haber Cycle

Given the following values for steps in the formation of CaO(s) from its elements, draw a Born–Haber cycle similar to that shown in Figure 6.7.
Eea1 for O1g2 = -141 kJ/mol 
Eea2 for O1g2 = 745.1 kJ/mol 
Heat of sublimation for Ca1s2 = 178 kJ/mol 
Ei1 for Ca1g2 = 590 kJ/mol Ei1 for Ca1g2 = 1145 kJ/mol 
Bond dissociation energy for O21g2 = 498 kJ/mol 
Lattice energy for CaO1s2 = 3401 kJ/mol <img src="https://lightcat-files.s3.amazonaws.com/problem_images/59d6081a4b7ac8d3-1670348493797.jpg" alt="" />

List the individual steps used in constructing a Born–Haber 
cycle for the formation of BaI2 from the elements. Which of 
the steps would you expect to be exothermic?

Solubility and the Born-Haber Cycle

Construct a Born–Haber cycle for the formation of the hypothetical
compound NaCl2, where the sodium ion has a 2+
charge (the second ionization energy for sodium is given in
Table 7.2). (a) How large would the lattice energy need to be
for the formation of NaCl2 to be exothermic?

Use data from Appendix C, Figure 7.10, and Figure 7.12 to calculate
the lattice energy of RbCl.

Given the following information, construct a Born–Haber cycle to calculate the lattice energy of CaCl2 1s2. (LO 6.13) <img src="https://lightcat-files.s3.amazonaws.com/problem_images/defd5e0ab67e3803-1670334541747.jpg" alt="" />
(a) 2603 kJ/mol
(b) 2254 kJ/mol
(c) 2481 kJ/mo
(d) l663 kJ/mol

The estimated lattice energy for CsF21s2 is +2347 kJ/mol. Use the data given in Problem 6.86 to calculate an overall energy change in kilojoules per mole for the formation of CsF21s2 from its elements. Does the overall reaction absorb energy or release it? In light of your answer to Problem 6.86, which compound is more likely to form in the reaction of cesium with fluorine, CsF or CsF2?<img src="https://lightcat-files.s3.amazonaws.com/problem_images/3d086e5d178d1d3d-1670436020587.jpg" alt="" />

Use the Born–Haber cycle and data from Appendix IIB and 
Table 9.3 to calculate the lattice energy of CaO. (ΔHsub for calcium 
is 178 kJ>mol; IE1 and IE2 for calcium are 590 kJ>mol and 
1145 kJ>mol, respectively; EA1 and EA2 for O are -141 kJ>mol 
and 744 kJ>mol, respectively.)

CHEMISTRY 101 - Born Haber Cyle and relative lattice energies

Calculate the lattice energy for the following formation equation:<img src="https://static.studychannel-prd.pearsonprd.tech/courses/general-chemistry/thumbnails/images/a97cac70"class="fr-fic fr-dii"><img src="https://lightcat-files.s3.amazonaws.com/problem_images/5a243f34f8199490-1608584035913.jpg"class="fr-fic fr-dii">

8.1b Born Haber Cycle | General Chemistry

Using the Born-Haber Cycle, demonstrate the formation of cesium chloride, CsCl, and calculate its enthalpy of formation.<img src="https://static.studychannel-prd.pearsonprd.tech/courses/general-chemistry/thumbnails/images/dd0f7e9d"class="fr-fic fr-dii">

Born Haber Cycle Example 1

(b) Using data from Appendix C, Figure 7.11, Figure 7.13, and the value of the second ionization energy for Ca, 1145 kJ>mol, calculate the lattice energy of CaCl2.

Use the following information plus the data given in Tables 6.2 and 6.3 to calculate the second electron affinity, Eea2, of oxygen. Is the O2-ion stable in the gas phase? Why is it stable in solid MgO?
Heat of sublimation for Mg1s2 = +147.7 kJ/mol 
Bond dissociation energy for O21g2 = +498.4 kJ/mol 
Eea1 for O1g2 = -141.0 kJ/mol 
Net energy change for formation of MgO(s) from its elements = -601.7 kJ/mol

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[BOOK CHEM] Clutch Version

Lewis Dot Structures: Neutral Compounds

Lewis Dot Structures or Electron Dot Structures&nbsp;are diagrams that show how elements in a molecule use their valence electrons to form bonds.&nbsp;

Average Bond Order

Average Bond Order represents the average number of chemical bonds between a pair of bond elements.

Lewis Dot Structures: Ions

Lewis Dot Structures of Ions involves losing or gaining valence electrons to draw the most likely structure.&nbsp;

Octet Rule

The&nbsp;Octet Rule states that main-group elements will generally form enough bonds to obtain 8 electrons in their valence shell.&nbsp;

Lewis Dot Symbols

Lewis Dot Symbols represent the outer shell electrons of an element.&nbsp;

Lewis Dot Structures: Sigma & Pi Bonds

Sigma Bonds directly connect element together, while Pi Bonds provide insulation and protection for those bonds.&nbsp;

Lewis Dot Structures: Exceptions

Lewis Dot Structure Exceptions&nbsp;happen when the central element violates the Octet Rule.

In the Born-Haber Cycle, ionic solids are created through the ionization and eventual combination of elements.&nbsp;

Coulomb's Law

Coulomb's Law is used to determine the forces experienced by charged particles.&nbsp;

Chemical Bonds

A chemical bond is the connection&nbsp;of different elements through the sharing, transferring or pooling of electrons.&nbsp;

Resonance Structures

Resonance Structures are used to represent the different possible bonding arrangements of a molecule.

Lewis Dot Structures: Acids

Drawing the Lewis Dot Structure of Acids&nbsp;involves first drawing the polyatomic anion and then attaching the H+ ion.&nbsp;

Formal Charge

Formal Charge is the charge given to an element within a molecule when assuming equal sharing of electrons between bonded elements.&nbsp;

Bond Energy

Bond Energy is the amount of energy stored within a chemical bond.

Lattice Energy

Lattice Energy&nbsp;is the estimate for the strength of ionic bonds.&nbsp;

Dipole Moment

Dipole arrows are used anytime a molecule possesses a dipole moment, which happens when a molecule is polar.&nbsp;

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