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: Place the following in order of Increasing magnitude of lattice energy.MgO NaI BaOa. Nal < MgO < BaOb.  MgO < Nal < BaOc. MgO < BaO < Nald. BaO < MgO < Nale. Nal < BaO <


Place the following in order of Increasing magnitude of lattice energy.


a. Nal < MgO < BaO

b.  MgO < Nal < BaO

c. MgO < BaO < Nal

d. BaO < MgO < Nal

e. Nal < BaO < MgO 


We are being asked to rank the given compounds in increasing magnitude of lattice energy. To estimate the lattice energy (or ionic bond energy) of an ionic compound, we will use the following equation:

Radius = period number

To determine the cation and anion charge, recall that some elements have common charges based on what group they belong to on the periodic table:

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