VSEPR Theory Atoms in a molecule try to spread out from one another as much as possible.

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Presentation transcript:

VSEPR Theory Atoms in a molecule try to spread out from one another as much as possible

methane, CH4 You might think this is the farthest that the hydrogens can get away from each other 109.5° 90° In 3 dimensions, this shape actually causes less repulsion between the bonding pairs of electrons

Here are the STEPS for determining molecular geometry: 1. Draw a Lewis structure 2. Count the # of bonds and # of lone pairs around the central atom (these are called “domains”) Single, Double and Triple bonds count as ONE domain (bonding domains) Each lone pair counts as ONE domain (non-bonding domains) 3. Determine shape Name of molecule shape is based on position of atoms (not domains)

How many “domains” around each central atom?

VSEPR Example

VSEPR Example

VSEPR Example

NOTE: Lone pairs also want to be next to each other if they can be.

Now, Let’s Combine VSEPR with Polarity…..

If two atoms share electrons, but don’t share them equally, we call it a polar bond or “dipole moment” Electrons are pulled closer to the more electronegative atom One end of the molecule develops a partial negative charge because it has a higher electron density

Dipole Moments ALL molecules with a lone pair on the central atom are polar. Double bonds, even resonance, will lead to polarity

Water is Polar It has polar H-O bonds Its geometry is “bent” So the molecule is polar It has a dipole

BF3 is Non-polar It has polar B-F bonds Its geometry is “trigonal planar” So the molecule is non-polar It does NOT have a dipole All the fluorines “cancel”