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Properties of Polar Molecular Compounds

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by

Viji Shanthikumar

on 21 September 2012

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Transcript of Properties of Polar Molecular Compounds

2 or more nonmetal atoms bonded
form molecules. What is a molecular
compound? Polar Molecular Compounds Viewing Models Molecules form by shared
electrons Atoms are bonded to form a water molecule Molecules attract other molecules Hydrogen Bonding Intermolecular Forces Dipole Dipole Hydrogen and Dipole Comparison Shape of the molecule
Polarity of the bonds Charge Seperations Attractions Polar molecules attracted by dipole dipole attraction. What is Dipole Dipole Attraction? Attractive force between positive end of one and negative end of other Predicting Molecules Lewis dot structure for ammonia NH3 Triagonal Pyramid 3D model of Ammonia Electronegativity of Elements Properties of Polar Molecules Electric Conductivity Solubility in water Malleability/Ductility/Brittleness Melting/Boiling Points Polar molecules are soluble in water
General rule – “ Like dissolves like” Not good conductors of electricity
Bonds block the flow of electrons Difficult to assume general rules for properties of polar molecules Cannot be calculated for polar molecules
Can only exist for metals strongest intermolecular force of attraction between the hydrogen of one molecule What is Hydrogen Bonding? Example 1. - a F-H, N-H or O-H bond must be on one molecule in order for a hydrogen bond to occur - F, O and N have high electronegativites so they pull the bonding pair of electrons towards themselves leaving hydrogen to be slightly positive. Example 2. Factors Affecting Hydrogen Bonding electronegativity; an atom with a low EN will not bond - F, O and N have high electronegativites so they pull the bonding pair of electrons towards themselves leaving hydrogen to be slightly positive.
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