Explore van der Waals forces, hydrogen bonding, and ion-dipole interactions affecting boiling points and material properties. Analyze London dispersion forces, polarizability effects, and molecular weight correlations from noble gases to complex alcohols. Interactive R analysis reveals intermolecular force patterns in CoCalc.
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Advanced Chemical Bonding with R in CoCalc - Chapter 5
Intermolecular Forces and Material Properties
This notebook contains Chapter 5 from the main Advanced Chemical Bonding with R in CoCalc notebook.
For the complete course, please refer to the main notebook: Advanced Chemical Bonding with R in CoCalc.ipynb
Chapter 5: Intermolecular Forces and Material Properties
5.1 Types of Intermolecular Forces (IMFs)
Van der Waals Forces
London Dispersion Forces: Temporary dipole interactions (all molecules)
Dipole-Dipole Forces: Permanent dipole attractions (polar molecules)
Dipole-Induced Dipole: Polar molecule induces dipole in nonpolar
Hydrogen Bonding
Requirements: H bonded to N, O, or F interacting with lone pair
Strength: 10-40 kJ/mol (stronger than typical IMFs)
Examples: H₂O, NH₃, HF, DNA base pairs
Ion-Dipole Forces
Context: Ions in polar solvents
Strength: 40-600 kJ/mol
Example: Na⁺ and Cl⁻ in water
5.2 IMF Strength Order
Ion-Dipole > H-bonding > Dipole-Dipole > London Dispersion
5.3 Impact on Physical Properties
Boiling/Melting Points: Stronger IMFs = Higher temperatures
Solubility: "Like dissolves like" principle
Viscosity: Stronger IMFs = Higher viscosity
Surface Tension: Cohesive forces at interfaces
`geom_smooth()` using formula = 'y ~ x'
🌡️ Intermolecular Force Analysis:
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# A tibble: 3 × 6
primary_imf count avg_bp avg_mw avg_dipole bp_range
<chr> <int> <dbl> <dbl> <dbl> <dbl>
1 H-bonding 4 38 21.8 1.71 133
2 Dipole-Dipole 3 -62.3 81.8 0.783 50
3 London 13 -151. 41.0 0.01 268
🔗 H-bonding Effect Analysis:
Average BP with H-bonding: 38.0°C
Average BP without H-bonding (MW<50): -162.8°C
H-bonding elevation: 200.8°C
💡 Hydrogen bonding dramatically increases boiling points!
---## From Intermolecular Forces and Material Properties to Real-World Applications and Modern FrontiersWe've explored intermolecular forces and material properties, understanding how these fundamental concepts shape our understanding of molecular interactions and chemical behavior.But how do these principles extend to real-world applications and modern frontiers?In Chapter 6, we'll discover how the concepts we've just learned provide the foundation for understanding even more complex chemical phenomena. You'll see how the principles of bonding and molecular structure directly influence the properties and behaviors we observe in real-world applications.### Journey ForwardThe transition from chapter 5 to chapter 6 represents a natural progression in chemical understanding. The foundational knowledge you've gained here will illuminate the advanced concepts ahead.Continue to Chapter 6: Real-World Applications and Modern Frontiers →orReturn to Main Notebook