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Intermolecular Forces

Intermolecular Forces. Amneet Sihota , Crystal Johnsa , Gabriel Wach , Jacob Wells. Dipole-Dipole Forces. Description: forces between positive and negative ends of two polar molecules. Types of Molecules: Positive and negative polar molecules (Permanent net dipoles)

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Intermolecular Forces

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  1. Intermolecular Forces AmneetSihota, Crystal Johnsa, Gabriel Wach, Jacob Wells

  2. Dipole-Dipole Forces • Description: forces between positive and negative ends of two polar molecules. • Types of Molecules: Positive and negative polar molecules (Permanent net dipoles) • Relative Strength: From 5 to 20 kJ per mole • Effect on Properties: Large dipole movements create solids • Real Life Example: Water, Hydrochloric Acid • Other Important effects: Partial charge bonds it together.

  3. Hydrogen Bonding • Description: Electromagnetic attractive interaction of a polar hydrogen atom in a molecule/chemical & electronegative atom from another molecule/chemical. • Types of Molecules: Hydrogen atom and either oxygen, fluorine, or nitrogen. • Relative strength: 5x stronger than dipole-dipole. • Effect on properties: Causes a high boiling point • Real-life example: H2O sticking to clothes • Other important facts: Partly responsible in the formation of proteins and amino acids.

  4. Dispersion • Description: A very weak attraction force acting between partials of matter • Types: Exist in all molecules especially non-polar • Relative Strength: The weakest force • Effects on properties: Liquefied can cause a non polar autumns’ or molecules to condense into liquids and solids as the temperatures lowers. • Important Facts : LDF – London Dispersion force causes non- polar substances to condense to liquids & freeze into solids.

  5. Ion Dipole • Description: an attractive force that results from electrostatic attraction between an ion and a neutral molecule that has a dipole. • Types: Polar Molecules • Relative Strength: Weak compared to intramolecular forces but stronger than hydrogen bonds. • Effects on properties: Cations attract the partially negative or neutral end of a polar molecule. Anions attract the partially positive or neutral end of a polar molecule • Important Facts : Ion-Dipole attractions become stronger as either the charge on the ion increases, or as the magnitude of the dipole of the polar molecule increases.

  6. Bibliography • 1. Handbook of Nanostructured Materials and Nanotechnology; Nalwa, H.S., Ed.; Academic Press: New York, NY, USA, 2000; Volume 5, pp. 501-575 • 2.http://www.elmhurst.edu/~chm/vchembook/161Ahydrogenbond.html • 3.http://www.chem.purdue.edu/gchelp/liquids/dipdip.html • 4.http://www.chem.purdue.edu/gchelp/liquids/iondip.html

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