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
Problem

Where, approximately, is the negative pole on each of these molecules?

Which molecule should have higher dipole moment, and why?

a. COF2 because it contains more F atoms.

b. COFH because the polar bonds in COF 2 nearly cancel each other out.

c. COF2 because it contains more lone pairs.

Solution

We’re asked to determine the approximate location of the negative pole on each of these molecules and to select and explain which has a higher dipole moment.

Remember that the dipole moment between the two elements is dependent on the electronegativity (EN), and its magnitude is related to their difference in EN.

Additionally, its direction is indicated as an arrow:

Least EN element  Most EN element


The EN values for the involved elements in both molecules are:

H = 2.2, C = 2.5, O = 3.5, F = 4.


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