Ch.9 - Bonding & Molecular StructureWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds
Chemical Bonds
Lattice Energy
Lattice Energy Application
Born Haber Cycle
Dipole Moment
Lewis Dot Structure
Octet Rule
Formal Charge
Resonance Structures
Additional Practice
Bond Energy

Solution: What is the enthalpy of sublimation for K, in kJ/mol?Given:Lattice energy of KCl = 699 kJ/molFirst ionization energy of K = 418.7 kJ/molElectron affinity of Cl = 349 kJ/molBond energy of Cl-Cl = 242.7


What is the enthalpy of sublimation for K, in kJ/mol?


Lattice energy of KCl = 699 kJ/mol

First ionization energy of K = 418.7 kJ/mol

Electron affinity of Cl = 349 kJ/mol

Bond energy of Cl-Cl = 242.7 kJ/mol

Enthalpy of formation of KCl = -435.87 kJ/mol


We’re being asked to calculate the heat of sublimation of potassium (K), given the lattice energy of KCl. 

Recall that lattice energy is the energy required to combine two gaseous ions into a solid ionic compound:

Mx+(g) + Ny–(g)  MyNx(s)

To calculate for lattice energy, we need to do the Born-Haber cycle for KCl

We start with the corresponding formation equation for KCl:

K(s) + ½ Cl2(g)  KCl(s), ΔH˚f

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