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INTERMOLECULAR FORCES OF ATTRACTION

INTERMOLECULAR FORCES OF ATTRACTION. Attraction existing between molecules in a given substance Responsible for the phase of the substance at a given temperature; for example, strong IMFA – solid at room temperature; weak IMFA – gas at room temperature.

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INTERMOLECULAR FORCES OF ATTRACTION

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  1. INTERMOLECULAR FORCES OF ATTRACTION Attraction existing between molecules in a given substance Responsible for the phase of the substance at a given temperature; for example, strong IMFA – solid at room temperature; weak IMFA – gas at room temperature

  2. COMPARISON OF MOLECULAR MASS, BOILING POINT

  3. TYPES OF IMFA (weakest to strongest) 1. VAN DER WAAL’S FORCES a. London dispersion force – caused by the movement of the electrons around the nucleus - effect is very temporary - present in all substances and only force present in non-polar molecules

  4. LONDON DISPERSION FORCE

  5. Induced dipole– temporary charges due to presence of electrons from neighboring atoms

  6. BOILING POINTS OF HALOGENS The higher the number of electrons, the stronger is the London dispersion force.

  7. SHAPE OF THE MOLECULE AFFECTS BOILING POINT

  8. b. dipole-dipole interaction – present only in polar covalent molecules - caused by the dipole moment (differences in the electronegativy of the elements present)

  9. Ethanol is Polar

  10. F O N c. Hydrogen bonding - present in polar covalent compounds where hydrogen is directly attached to Fluorine, Oxygen and Nitrogen ( the three most electronegative elements)

  11. Hydrogen bonding only occurs if H is attached to F, O and N.

  12. Hydrogen bonding in water

  13. H bonding in ice

  14. 2. IONIC BONDING – • present only in ionic compounds. • Electrostatic force of attraction.

  15. An ionic compound dissolved in water.

  16. FORMULA TO DETERMINE THE NUMBER OF RINGS AND/OR DOUBLE AND TRIPLE BONDS ρ = where C = number of carbon atoms N = number of nitrogen atoms H = number of hydrogen atoms X = number of halogen (Group 17) atoms 2 + 2C + N – H – X 2

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