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
Sections
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: Based on electronegativities, which of the following would you expect to be most ionic?A. CF4B. CaF2C. CH4D. N2E. CO2

Problem

Based on electronegativities, which of the following would you expect to be most ionic?

A. CF4

B. CaF2

C. CH4

D. N2

E. CO2

Solution

Establish how to find the electronegative difference and determine which among the compounds is most ionic


Recall that dipole moment refers to the electronegativity difference in a bond/molecule. This means the molecule with the largest dipole moment has the largest electronegativity difference.



Recall that bonds can be classified acc. to their EN difference as:

   __________________________________________________

Electronegativity Difference        

              (ΔEN)                                     Bond Classification
   __________________________________________________

Zero (0.0)                                          Pure Covalent
Small (0.1 – 0.4)                                Nonpolar Covalent
Intermediate (0.4  – 1.7)                    Polar Covalent
Large (Greater than 1.7)                  Ionic               


By calculating the electronegative difference, we can determine which bond/compound has the most ionic. The higher the EN difference, the more ionic it is

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