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POLARITY

POLARITY. POLAR BONDS Bonds between atoms POLAR MOLECULES Polarity between molecules Occurs when polar bonds create a dipole moment. Bond Polarity. HCl is POLAR because it has a positive end and a negative end. Cl has a greater share in bonding electrons than does H.

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POLARITY

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  1. POLARITY • POLAR BONDS • Bonds between atoms • POLAR MOLECULES • Polarity between molecules • Occurs when polar bonds create a dipole moment

  2. Bond Polarity HCl is POLAR because it has a positive end and a negative end. Cl has a greater share in bonding electrons than does H. Cl has slight negative charge (-d) and H has slight positive charge (+ d)

  3. Bond Polarity Which bond is more polar (or DIPOLAR)? O—H O—F  3.5 - 2.1 3.5 - 4.0  1.4 0.5 OH is more polar than OF and polarity is “reversed.”

  4. Figure 9.15 Molecular Polarity Molecules—such as HCl and H2O— can be POLAR (or dipolar). They have a DIPOLE MOMENT. The polar HCl molecule will turn to align with an electric field.

  5. Molecular Polarity Molecules will be polar if a) bonds are polar AND b) the molecule is NOT “symmetric” All above are NOT polar

  6. Polar or Nonpolar? Compare CO2 and H2O. Which one is polar?

  7. Polar or Nonpolar? • Consider AB3 molecules: BF3, Cl2CO, and NH3.

  8. Molecular Polarity, BF3 B atom is positive and F atoms are negative. B—F bonds in BF3 are polar. But molecule is symmetrical and NOT polar

  9. Molecular Polarity, HBF2 B atom is positive but H & F atoms are negative. B—F and B—H bonds in HBF2 are polar. But molecule is NOT symmetrical and is polar.

  10. Is Methane, CH4, Polar?

  11. Is CH3F Polar?

  12. BONDING/FORCES • INTRAMOLECULAR FORCES • Ionic • Covalent • Metallic • INTERMOLECULAR FORCES • Van der Waal’s Forces • London dispersion • Dipole-Dipole • Hydrogen Bonding

  13. Bonding, Intermolecular Forces (IMF) • IMF < intramolecular forces (covalent, metallic, ionic bonds) • IMF strength: solids > liquids > gases • Boiling points and melting points are good indicators of relative IMF strength.

  14. Summary of IMF Van der Waals forces

  15. Types of Crystalline Solids

  16. Ice Carbon dioxide (dry ice) Sucrose

  17. SiO2 Graphite Diamond

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