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Polarity and Intermolecular Forces Mr. Krstovic
CHEMSITRY 11 Polarity and Intermolecular Forces Mr. Krstovic
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Polar and nonpolar covalent bonds
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Nonpolar - EQUAL sharing of e-
Polar - UNEQUAL sharing of e- Use E.N. values to predict polarity between two atoms 0 – 0.7 nonpolar 0.7 – 1.7 polar 1.7 + ionic
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Guidelines for Polar Molecules
Usually any diatomic compounds (HCl, HBr, CO) Any molecules with OH at one end (CH3OH) Any molecules with O at one end (OCl2) Any molecule with an N at one end (NH3)
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Guidelines for Nonpolar molecules
All diatomic elements (Cl2, N2) Most carbon compounds in the form of CxAy
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Polar or Non-polar???? CH5N CH4O C2H2 NaCl HF CO32-
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Intermolecular Forces
Ionic and covalent bonds are INTRAmolecular forces INTERmolecular forces are forces between molecules
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Intermolecular Forces
Ion-dipole: an attractive force between ions from ionic compoounds and polar molecules (Example: NaCl in Water)
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Dipole-dipole: an attractive force acting between all polar molecules (Example: between HCl molecules)
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Hydrogen Bonding (A special Case of Dipole-Dipole)
A relatively strong force between a POSITIVE hydrogen atom of one molecule and a highly electronegative atom (F,O, or N) in another molecule.
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L.D.: an attractive force acting between ALL molecules, including nonpolar molecules.
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